Cambridge International Examinations Cambridge...

The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level1/Level 2 Certificate.

This document consists of 15 printed pages and 1 blank page.

IB14 06_0620_11/2RP © UCLES 2014 [Turn over

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Cambridge International Examinations Cambridge International General Certificate of Secondary Education

CHEMISTRY 0620/11

Paper 1 Multiple Choice May/June 2014

45 Minutes Additional Materials: Multiple Choice Answer Sheet Soft clean eraser Soft pencil (type B or HB is recommended)

READ THESE INSTRUCTIONS FIRST

Write in soft pencil.

Do not use staples, paper clips, glue or correction fluid.

Write your name, Centre number and candidate number on the Answer Sheet in the spaces provided unless this has been done for you.

DO NOT WRITE IN ANY BARCODES.

There are forty questions on this paper. Answer all questions. For each question there are four possible answers A, B, C and D.

Choose the one you consider correct and record your choice in soft pencil on the separate Answer Sheet.

Read the instructions on the Answer Sheet very carefully.

Each correct answer will score one mark. A mark will not be deducted for a wrong answer.

Any rough working should be done in this booklet.

A copy of the Periodic Table is printed on page 16.

Electronic calculators may be used.

2

© UCLES 2014 0620/11/M/J/14

1 The diagram shows the result of dropping a purple crystal into water.

water

purplecrystal

after five hourspurplesolution

Which processes take place in this experiment?

chemical reaction

diffusing dissolving

A � � �

B � � �

C � � �

D � � �

2 The four pieces of apparatus shown below are used in chemical experiments.

burette measuringcylinder

pipette thermometer

Which statement about the apparatus is correct?

A The burette measures the volume of liquid added in a titration.

B The measuring cylinder measures the mass of a substance used in an experiment.

C The pipette measures the volume of gas given off in a reaction.

D The thermometer measures the density of a solution.

3

© UCLES 2014 0620/11/M/J/14 [Turn over

3 Alcohol and water are completely miscible. This means when mixed together they form only one liquid layer.

Which method is used to separate alcohol from water?

A crystallisation

B filtration

C fractional distillation

D precipitation 4 The diagram shows the structure of an atom of element X.

5p6n

e e

e e

ekeye = electronn = neutronp = proton = nucleus

What is X?

A boron

B carbon

C sodium

D sulfur

4

© UCLES 2014 0620/11/M/J/14

5 The diagrams show four particles.

1

key

= an electron

= a neutron

= a proton

2p2n

= nucleus

ee

e

2

3p3n

ee

e

3

3p3n

ee

ee

4

3p4n

ee

e

e

n

p

Which two diagrams show atoms that are isotopes of each other?

A 1 and 2 B 1 and 3 C 2 and 3 D 2 and 4 6 The ‘lead’ in a pencil is made of a mixture of graphite and clay.

‘lead’

When the percentage of graphite is increased, the pencil slides across the paper more easily.

Which statement explains this observation?

A Graphite has a high melting point.

B Graphite is a form of carbon.

C Graphite is a lubricant.

D Graphite is a non-metal.

5


7 Element X is in Group I of the Periodic Table. X reacts with element Y to form an ionic compound.

Which equation shows the process that takes place when X forms ions?

A X + e– → X+

B X – e– → X–

C X + e– → X–

D X – e– → X+ 8 Solid F is an element. Solid G is a compound. Neither solid conducts electricity but G conducts electricity when dissolved in water.

These properties suggest that F is ……1…… and that G is ……2…… with ……3…… bonds.

Which words correctly complete gaps 1, 2 and 3?

1 2 3

A diamond AgCl covalent

B diamond NaCl ionic

C graphite AgCl ionic

D graphite NaCl covalent

9 A compound contains one atom of calcium, two atoms of hydrogen and two atoms of oxygen.

What is the correct chemical formula of the compound?

A CaO2H2 B HOCaOH C H2CaO2 D Ca(OH)2 10 In athletics, banned drugs such as nandrolone have been taken illegally to improve performance.

Nandrolone has the molecular formula C18H26O2.

What is the relative molecular mass, Mr, of nandrolone?

(Relative atomic mass: H = 1; C = 12; O = 16)

A 46 B 150 C 274 D 306 11 Which substance will not conduct electricity?

A aluminium

B copper

C plastic

D steel

6

© UCLES 2014 0620/11/M/J/14

12 Which products are formed at the anode and cathode when electricity is passed through molten

lead(II) bromide?

anode (+) cathode (–)

A bromide ions lead ions

B bromine molecules lead atoms

C lead atoms bromine molecules

D lead ions bromide ions

13 Some reactions are endothermic.

How does the temperature and energy change in an endothermic reaction?

temperature change energy change

A decreases energy taken in

B decreases energy given out

C increases energy taken in

D increases energy given out

14 Two chemical processes are described below.

● In the combustion of methane, energy is ......1...... .

● In the electrolysis of molten lead(II) bromide, energy is ......2...... .

Which words correctly complete gaps 1 and 2?

1 2

A given out given out

B given out taken in

C taken in given out

D taken in taken in

15 Which equation shows an oxidation reaction?

A C + O2 → CO2

B CaCO3 → CaO + CO2

C CaO + 2HCl → CaCl 2 + H2O

D N2O4 → 2NO2

7


16 In separate experiments, a catalyst is added to a reaction mixture and the temperature of the mixture is decreased.

What are the effects of these changes on the rate of the reaction?

catalyst added

temperature decreased

A faster faster

B faster slower

C slower faster

D slower slower

17 An experiment is carried out to investigate the rate of reaction when calcium carbonate is reacted

with hydrochloric acid.

The volume of carbon dioxide gas given off is measured at different intervals of time.

The diagram shows pieces of apparatus used to collect gases.

1downward delivery

2gas measuring

syringe

3over water in

graduated tube

Which apparatus is suitable to collect and measure the volume of the carbon dioxide?

A 1, 2 and 3 B 2 and 3 only C 1 only D 3 only

8

© UCLES 2014 0620/11/M/J/14

18 The equation shows a reaction that is reversed by changing the conditions. forward reaction

CuSO4.5H2O CuSO4 + 5H2O

How can the forward reaction be reversed?

by adding water by heating

A � �

B � �

C � �

D � �

19 Which statements about alkalis are correct?

1 When reacted with an acid, the pH of the alkali increases.

2 When tested with litmus, the litmus turns blue.

3 When warmed with an ammonium salt, ammonia gas is given off.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only

20 Only two elements are liquid at 20 °C. One of these elements is shiny and conducts electricity.

This suggests that this element is a ......1...... and therefore its oxide is ......2...... .


1 2

A metal acidic

B metal basic

C non-metal acidic

D non-metal basic

21 Which acid reacts with ammonia to produce the salt ammonium sulfate?

A hydrochloric

B nitric

C phosphoric

D sulfuric

9


22 Aqueous sodium hydroxide is added to solid X and the mixture is heated.

A green precipitate is formed and an alkaline gas is given off.

Which ions are present in X?

A NH4

+ and Fe2+

B NH4

+ and Fe3+

C OH– and Fe2+

D OH– and Fe3+ 23 Which statement about the Periodic Table is correct?

A Elements in the same period have the same number of outer electrons.

B The elements on the left are usually gases.

C The most metallic elements are on the left.

D The relative atomic mass of the elements increases from right to left. 24 Why is argon gas used to fill electric lamps?

A It conducts electricity.

B It glows when heated.

C It is less dense than air.

D It is not reactive.

25 An element melts at 1455 °C, has a density of 8.90 g / cm3 and forms a green chloride.

Where in the Periodic Table is this element found?

C

B

D

A

10

© UCLES 2014 0620/11/M/J/14

26 The diagrams show two items that may be found in the home. Each item contains zinc.

zinc plated bucket brass door-knocker

In which is zinc used as an alloy?

bucket door-knocker

A � �

B � �

C � �

D � �

27 In an experiment, three test-tubes labelled X, Y and Z were half-filled with dilute hydrochloric

acid. A different metal was added to each test-tube. After a few minutes the following observations were made.

In tube X, bubbles slowly rose to the surface.

In tube Y, there was a rapid release of bubbles.

In tube Z, no bubbles were produced.

Which three metals match the observations?

tube X tube Y tube Z

A copper zinc iron

B magnesium iron copper

C zinc magnesium copper

D zinc magnesium iron

11


28 The table shows properties of four metals.

Which metal is the most suitable for aircraft construction?

density strength resistance to

corrosion

A high high low

B high low low

C low high high

D low low high

29 The diagram shows a blast furnace.

In which part is iron ore changed to iron?

A

B

CD

30 The diagram shows some uses of water in the home.

1 2 3

For which uses is it important for the water to have been treated?

A 1 only B 2 only C 3 only D 1, 2 and 3

12

© UCLES 2014 0620/11/M/J/14

31 Four steel paper clips are treated as described before being placed in a beaker of water.

Which paper clip rusts most quickly?

A coated with grease

B dipped in paint and allowed to dry

C electroplated with zinc

D washed with soap and rinsed 32 Which compound contains two of the three essential elements needed for a complete fertiliser?

A ammonium chloride

B ammonium nitrate

C ammonium phosphate

D ammonium sulfate 33 When compound X is heated, it changes colour from green to black. Compound Y is formed and

a gas is given off which turns limewater milky.

What are X and Y?

X Y

A calcium carbonate calcium oxide

B copper carbonate carbon

C copper carbonate copper oxide

D copper sulfate copper oxide

34 Acid rain is formed when sulfur dioxide and oxides of nitrogen dissolve in rain water.

Which problem is not caused by acid rain?

A breathing difficulties

B dying trees

C erosion of statues

D lowered pH of lakes

13


35 Which pollutant gas is produced by the decomposition of vegetation?

A carbon monoxide

B methane

C nitrogen oxide

D sulfur dioxide 36 Which type of compound is shown?

H C

H

H

H

H

C

H

H

C OH

A alcohol

B alkane

C alkene

D carboxylic acid 37 The table shows the composition of four different types of petroleum (crude oil).

fraction Arabian Heavy

/ % Arabian Light

/ % Iranian Heavy

/ % North Sea

/ %

gasoline 18 21 21 23

kerosene 11.5 13 13 15

diesel oil 18 20 20 24

fuel oil 52.5 46 46 38

Which type of petroleum is best for the motor vehicle industry?

A Arabian Heavy

B Arabian Light

C Iranian Heavy

D North Sea

14

© UCLES 2014 0620/11/M/J/14

38 Alkenes are manufactured by cracking hydrocarbons obtained from petroleum.

alkane X obtainedfrom petroleum alkene Y

cracking

Which row describes the process of cracking?

size of X

molecules size of Y

molecules catalyst required

temperature required

A large small no low

B large small yes high

C small large no low

D small large yes high

39 X, Y and Z are three hydrocarbons.

X CH2=CH2 Y CH3–CH=CH2 Z CH3–CH2–CH=CH2

What do compounds X, Y and Z have in common?

1 They are all alkenes.

2 They are all part of the same homologous series.

3 They all have the same boiling point.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 40 Which statements about ethanol are correct?

1 It can be made by fermentation.

2 It is an unsaturated compound.

3 It burns in air and can be used as a fuel.


15

© UCLES 2014 0620/11/M/J/14

BLANK PAGE

16

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Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.

© UCLES 2014 0620/11/M/J/14

Gro

up

140

Ce

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PrP

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144

Nd

Neo

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PmP

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150

SmS

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62

152

EuE

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63

157

Gd

Gad

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64

159

Tb Terb

ium

65

162

Dy

Dys

pros

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66

165

Ho

Hol

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Er Erb

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68

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Tm Thul

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YbY

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56 Fe Iron

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This document consists of 16 printed pages.

IB14 06_0620_12/2RP © UCLES 2014 [Turn over

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CHEMISTRY 0620/12















2

© UCLES 2014 0620/12/M/J/14

1 Two gas jars each contain a different gas. The gas jars are connected and the cover slips are removed.

The diagram shows what happens to the particles of the gases.

cover slips

Which process has occurred?

A chemical reaction

B condensation

C diffusion

D evaporation 2 A liquid is heated until it boils.

thermometer

test-tube

25 cm3 liquid

ethanol

spirit burner

Which result shows that the liquid in the test-tube is pure water?

A Condensation forms at the top of the test-tube.

B Steam is produced.

C The thermometer reads 100 °C.

D There is nothing left behind in the test-tube.

3


3 Which two methods can be used to separate a salt from its solution in water?

1 crystallisation

2 decanting

3 distillation

4 filtration

A 1 and 2 B 1 and 3 C 2 and 3 D 3 and 4

4 Which statements about a phosphorus atom, P31

15, are correct?

1 The nucleon number is 16.

2 The number of outer electrons is 5.

3 The proton number is 15.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 5 The diagrams show four particles.

1

key

= an electron

= a neutron

= a proton

2p2n

= nucleus

ee

e

2

3p3n

ee

e

3

3p3n

ee

ee

4

3p4n

ee

e

e

n

p



4

© UCLES 2014 0620/12/M/J/14

6 The ‘lead’ in a pencil is made of a mixture of graphite and clay.

‘lead’






D Graphite is a non-metal. 7 The electronic structures of two atoms, X and Y, are shown.

X Y

X and Y combine together to form a compound.

What is the type of bonding in the compound and what is the formula of the compound?

type of bonding formula

A covalent X2Y

B covalent XY2

C ionic XY2

D ionic X2Y

5


8 The structure of an organic compound, X, is shown.

C C

C C

C C C

H

H H

HH

H H

H

H H H

H

What is the molecular formula of X?

A C6H9 B C6H12 C C7H12 D C7H14

9 What is the relative molecular mass, M r, of nitrogen dioxide?

A 15 B 23 C 30 D 46 10 Electrical cables are made from either ……1……, because it is a very good conductor of

electricity, or from……2……, because it has a low density. Overhead cables have a ……3…… core in order to give the cable strength.


1 2 3

A aluminium copper magnesium

B copper aluminium magnesium

C copper aluminium steel

D magnesium copper steel

11 What will be produced at the anode and at the cathode, if molten potassium chloride is

electrolysed?

anode (+) cathode (-)

A chlorine hydrogen

B chlorine potassium

C hydrogen chlorine

D potassium chlorine

6

© UCLES 2014 0620/12/M/J/14

12 Solutions of two chemicals are mixed.

A reaction occurs and the temperature change is measured.

Which statement is correct?

A If the reaction is endothermic, the temperature decreases and energy is taken in.

B If the reaction is endothermic, the temperature increases and energy is given out.

C If the reaction is exothermic, the temperature decreases and energy is given out.

D If the reaction is exothermic, the temperature increases and energy is taken in. 13 Power stations produce electrical energy from different fuels.

Which fuel causes least pollution to the atmosphere?

A coal

B fuel oil

C natural gas

D radioactive isotopes 14 A student was investigating the reaction between marble chips and dilute hydrochloric acid.

bung

marblechips

25 cm3 dilutehydrochloric acid

gas syringe

Which changes would reduce the rate of reaction?

temperature

of acid concentration

of acid surface area

of marble chips

A decrease decrease decrease

B decrease decrease increase

C increase decrease decrease

D increase increase increase

7



A C + O2 → CO2



D N2O4 → 2NO2

16 In separate experiments, a catalyst is added to a reaction mixture and the temperature of the

mixture is decreased.


catalyst added


A faster faster

B faster slower

C slower faster

D slower slower

17 Different plants grow best under different pH conditions.

Which plant grows best in alkaline soil?

plant grows best in soil at

pH

A cabbage 6-8

B potato 4-7

C strawberry 5-7

D wheat 6-7

8

© UCLES 2014 0620/12/M/J/14

18 The equation shows a reaction that is reversed by changing the conditions. forward reaction




A � �

B � �

C � �

D � �

19 Element X forms an oxide, XO, that neutralises sulfuric acid.

Which row describes X and XO?

element X nature of oxide, XO

A metal acidic

B metal basic

C non-metal acidic

D non-metal basic

20 Copper carbonate reacts with dilute sulfuric acid to make copper sulfate.

CuCO3(s) + H2SO4(aq) → CuSO4(aq) + CO2(g) + H2O(l)

Which row gives the correct order of steps for making copper sulfate crystals?

step 1 step 2 step 3 step 4

A

add excess acid to the copper carbonate

filter

evaporate filtrate to point of crystallisation

leave to cool

B

add excess acid to the copper carbonate

filter

evaporate to dryness

leave to cool

C

add excess copper carbonate to the acid

evaporate to point of crystallisation

leave to cool

filter

D

add excess copper carbonate to the acid

filter

evaporate filtrate to point of crystallisation

leave to cool

9


21 Element X is a non-metal.

In which position of the Periodic Table could element X be found?

A at the bottom of Group I

B at the top of Group 0

C at the top of Group I

D in the transition elements 22 Aqueous sodium hydroxide is added to solid X and the mixture is heated.



A NH4

+ and Fe2+

B NH4

+ and Fe3+

C OH– and Fe2+

D OH– and Fe3+ 23 A student carried out an experiment to find the order of reactivity of five metals. They were tested with cold water, hot water and steam and the results recorded in a table.

metal cold water hot water steam

V no reaction reacts slowly vigorous reaction

W no reaction no reaction slow reaction

X reacts slowly vigorous reaction not attempted

Y no reaction no reaction no reaction

Z vigorous reaction explosive reaction not attempted

What is the order of reactivity of these metals?

most reactive least reactive

A V W Y X Z

B W X Z V Y

C Z X V W Y

D Z X Y W V

10

© UCLES 2014 0620/12/M/J/14

24 Why is argon gas used to fill electric lamps?




D It is not reactive.



C

B

D

A




bucket door-knocker

A � �

B � �

C � �

D � �

11


27 Which object is likely to be made from stainless steel?

bicycle chain

A

car body

B

can of beans

C

teaspoon

D

28 Four reactions that take place in the blast furnace to produce iron are shown.

Which reaction is used to keep the furnace hot?

A C + O2 → CO2

B CO2 + C → 2CO

C Fe2O3 + 3C → 2Fe + 3CO

D Fe2O3 + 3CO → 2Fe + 3CO2

12

© UCLES 2014 0620/12/M/J/14



A

B

CD


1 2 3


A 1 only B 2 only C 3 only D 1, 2 and 3 31 A piece of uncoated iron and three pieces of iron with various coatings were left exposed to the

air.

Which piece of iron would rust?

A the painted piece

B the tin-coated piece

C the uncoated piece

D the zinc-coated piece

13


32 Which compound would not be an effective fertiliser?

A ammonium nitrate, NH4NO3

B calcium oxide, CaO

C calcium phosphate, Ca3(PO4)2

D potassium nitrate, KNO3 33 Sulfur dioxide, SO2, nitrogen dioxide, NO2, and carbon monoxide, CO, are air pollutants.

Which row correctly shows their major source?

motor car engines power stations

A CO NO2, SO2

B NO2, CO SO2

C SO2, NO2 CO

D SO2 NO2, CO

34 Which process does not produce carbon dioxide?

A combustion of methane

B fermentation of sugar

C polymerisation of ethene

D respiration 35 Which pollutant gas is produced by the decomposition of vegetation?

A carbon monoxide

B methane

C nitrogen oxide

D sulfur dioxide

14

© UCLES 2014 0620/12/M/J/14

36 Which diagram shows the structure of pentanoic acid?

H C

H

H

H

H

H

H

H

H

H

H

C C C C O H

A

H

H

H

O

H

H

H

H

H

C C C C C

H

H

O

B

H C

H

H

H

H

H

H H

H

H

C C C C

C

H C

H

H

H

H

H

H

H

H

O

C C C C

HO

D

H

H

37 The table shows the composition of four different types of petroleum (crude oil).


/ % Arabian Light

/ % Iranian Heavy

/ % North Sea

/ %


kerosene 11.5 13 13 15


fuel oil 52.5 46 46 38


A Arabian Heavy

B Arabian Light

C Iranian Heavy

D North Sea

15

© UCLES 2014 0620/12/M/J/14

38 The diagram shows the cracking of substance X.

Y

water

cotton woolsoaked in X catalyst

heat

Which type of organic compound is found in Y, which is not present in X?

A acid

B alcohol

C alkane

D alkene 39 In which reaction could one of the products belong to the same homologous series as the organic

reactant?

A addition of steam to ethene

B combustion of an alkane

C cracking of an alkane

D polymerisation of ethene 40 Ethanol is produced from either ethene or sugar.

Which type of chemical reaction is used in each case?

ethene → ethanol sugar → ethanol

A addition fermentation

B addition fractional distillation

C distillation fermentation

D distillation fractional distillation

16



© UCLES 2014 0620/12/M/J/14

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



IB14 06_0620_13/FP © UCLES 2014 [Turn over

*8978722695*


CHEMISTRY 0620/13















2

© UCLES 2014 0620/13/M/J/14

1 The diagram shows the result of dropping a purple crystal into water.

water

purplecrystal

after five hourspurplesolution

Which processes take place in this experiment?

chemical reaction

diffusing dissolving

A � � �

B � � �

C � � �

D � � �

2 Alcohol and water are completely miscible. This means when mixed together they form only one

liquid layer.

Which method is used to separate alcohol from water?

A crystallisation

B filtration

C fractional distillation

D precipitation

3


3 The four pieces of apparatus shown below are used in chemical experiments.

burette measuringcylinder

pipette thermometer

Which statement about the apparatus is correct?

A The burette measures the volume of liquid added in a titration.

B The measuring cylinder measures the mass of a substance used in an experiment.

C The pipette measures the volume of gas given off in a reaction.

D The thermometer measures the density of a solution. 4 The diagram shows the structure of an atom of element X.

5p6n

e e

e e

ekeye = electronn = neutronp = proton = nucleus

What is X?

A boron

B carbon

C sodium

D sulfur

4

© UCLES 2014 0620/13/M/J/14

5 The ‘lead’ in a pencil is made of a mixture of graphite and clay.

‘lead’






D Graphite is a non-metal. 6 The diagrams show four particles.

1

key

= an electron

= a neutron

= a proton

2p2n

= nucleus

ee

e

2

3p3n

ee

e

3

3p3n

ee

ee

4

3p4n

ee

e

e

n

p



5


7 Solid F is an element. Solid G is a compound. Neither solid conducts electricity but G conducts electricity when dissolved in water.

These properties suggest that F is ……1…… and that G is ……2…… with ……3…… bonds.


1 2 3

A diamond AgCl covalent

B diamond NaCl ionic

C graphite AgCl ionic

D graphite NaCl covalent

8 In athletics, banned drugs such as nandrolone have been taken illegally to improve performance.

Nandrolone has the molecular formula C18H26O2.

What is the relative molecular mass, Mr, of nandrolone?

(Relative atomic mass: H = 1; C = 12; O = 16)

A 46 B 150 C 274 D 306 9 A compound contains one atom of calcium, two atoms of hydrogen and two atoms of oxygen.

What is the correct chemical formula of the compound?

A CaO2H2 B HOCaOH C H2CaO2 D Ca(OH)2 10 Element X is in Group I of the Periodic Table. X reacts with element Y to form an ionic compound.

Which equation shows the process that takes place when X forms ions?

A X + e– → X+

B X – e– → X–

C X + e– → X–

D X – e– → X+ 11 Which substance will not conduct electricity?

A aluminium

B copper

C plastic

D steel

6

© UCLES 2014 0620/13/M/J/14

12 Two chemical processes are described below.

● In the combustion of methane, energy is ......1...... .

● In the electrolysis of molten lead(II) bromide, energy is ......2...... .


1 2

A given out given out

B given out taken in

C taken in given out

D taken in taken in


A C + O2 → CO2



D N2O4 → 2NO2

14 Some reactions are endothermic.

How does the temperature and energy change in an endothermic reaction?

temperature change energy change

A decreases energy taken in

B decreases energy given out

C increases energy taken in

D increases energy given out

15 Which products are formed at the anode and cathode when electricity is passed through molten

lead(II) bromide?

anode (+) cathode (–)

A bromide ions lead ions

B bromine molecules lead atoms

C lead atoms bromine molecules

D lead ions bromide ions

7


16 An experiment is carried out to investigate the rate of reaction when calcium carbonate is reacted with hydrochloric acid.

The volume of carbon dioxide gas given off is measured at different intervals of time.

The diagram shows pieces of apparatus used to collect gases.

1downward delivery

2gas measuring

syringe

3over water in

graduated tube

Which apparatus is suitable to collect and measure the volume of the carbon dioxide?

A 1, 2 and 3 B 2 and 3 only C 1 only D 3 only 17 In separate experiments, a catalyst is added to a reaction mixture and the temperature of the

mixture is decreased.


catalyst added


A faster faster

B faster slower

C slower faster

D slower slower

18 Which statements about alkalis are correct?

1 When reacted with an acid, the pH of the alkali increases.

2 When tested with litmus, the litmus turns blue.

3 When warmed with an ammonium salt, ammonia gas is given off.


8

© UCLES 2014 0620/13/M/J/14

19 Which acid reacts with ammonia to produce the salt ammonium sulfate?

A hydrochloric

B nitric

C phosphoric

D sulfuric 20 The equation shows a reaction that is reversed by changing the conditions. forward reaction




A � �

B � �

C � �

D � �

21 Only two elements are liquid at 20 °C. One of these elements is shiny and conducts electricity.

This suggests that this element is a ......1...... and therefore its oxide is ......2...... .


1 2

A metal acidic

B metal basic

C non-metal acidic

D non-metal basic

9




C

B

D

A

23 Why is argon gas used to fill electric lamps?




D It is not reactive. 24 Which statement about the Periodic Table is correct?

A Elements in the same period have the same number of outer electrons.

B The elements on the left are usually gases.

C The most metallic elements are on the left.

D The relative atomic mass of the elements increases from right to left. 25 Aqueous sodium hydroxide is added to solid X and the mixture is heated.



A NH4

+ and Fe2+

B NH4

+ and Fe3+

C OH– and Fe2+

D OH– and Fe3+

10

© UCLES 2014 0620/13/M/J/14

26 In an experiment, three test-tubes labelled X, Y and Z were half-filled with dilute hydrochloric acid. A different metal was added to each test-tube. After a few minutes the following observations were made.

In tube X, bubbles slowly rose to the surface.

In tube Y, there was a rapid release of bubbles.

In tube Z, no bubbles were produced.

Which three metals match the observations?

tube X tube Y tube Z

A copper zinc iron

B magnesium iron copper

C zinc magnesium copper

D zinc magnesium iron




bucket door-knocker

A � �

B � �

C � �

D � �

11



1 2 3


A 1 only B 2 only C 3 only D 1, 2 and 3 29 The table shows properties of four metals.

Which metal is the most suitable for aircraft construction?

density strength resistance to

corrosion

A high high low

B high low low

C low high high

D low low high



A

B

CD

12

© UCLES 2014 0620/13/M/J/14

31 Acid rain is formed when sulfur dioxide and oxides of nitrogen dissolve in rain water.

Which problem is not caused by acid rain?

A breathing difficulties

B dying trees

C erosion of statues

D lowered pH of lakes 32 Which compound contains two of the three essential elements needed for a complete fertiliser?

A ammonium chloride

B ammonium nitrate

C ammonium phosphate

D ammonium sulfate 33 Four steel paper clips are treated as described before being placed in a beaker of water.

Which paper clip rusts most quickly?

A coated with grease

B dipped in paint and allowed to dry

C electroplated with zinc

D washed with soap and rinsed 34 When compound X is heated, it changes colour from green to black. Compound Y is formed and

a gas is given off which turns limewater milky.

What are X and Y?

X Y

A calcium carbonate calcium oxide

B copper carbonate carbon

C copper carbonate copper oxide

D copper sulfate copper oxide

13


35 Which type of compound is shown?

H C

H

H

H

H

C

H

H

C OH

A alcohol

B alkane

C alkene

D carboxylic acid 36 The table shows the composition of four different types of petroleum (crude oil).


/ % Arabian Light

/ % Iranian Heavy

/ % North Sea

/ %


kerosene 11.5 13 13 15


fuel oil 52.5 46 46 38


A Arabian Heavy

B Arabian Light

C Iranian Heavy

D North Sea 37 Which pollutant gas is produced by the decomposition of vegetation?

A carbon monoxide

B methane

C nitrogen oxide

D sulfur dioxide

14

© UCLES 2014 0620/13/M/J/14

38 X, Y and Z are three hydrocarbons.

X CH2=CH2 Y CH3–CH=CH2 Z CH3–CH2–CH=CH2

What do compounds X, Y and Z have in common?

1 They are all alkenes.

2 They are all part of the same homologous series.

3 They all have the same boiling point.

A 1, 2 and 3 B 1 and 2 only C 1 and 3 only D 2 and 3 only 39 Alkenes are manufactured by cracking hydrocarbons obtained from petroleum.

alkane X obtainedfrom petroleum alkene Y

cracking

Which row describes the process of cracking?

size of X

molecules size of Y

molecules catalyst required

temperature required

A large small no low

B large small yes high

C small large no low

D small large yes high

40 Which statements about ethanol are correct?

1 It can be made by fermentation.

2 It is an unsaturated compound.

3 It burns in air and can be used as a fuel.


15

© UCLES 2014 0620/13/M/J/14

BLANK PAGE

16



© UCLES 2014 0620/13/M/J/14

Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents

This document consists of 17 printed pages and 3 blank pages.

[Turn overIB14 06_0620_21/2RP© UCLES 2014

*1339612500*


Write your Centre number, candidate number and name in the spaces at the top of this page.Write in dark blue or black pen.You may use an HB pencil for any diagrams or graphs.Do not use staples, paper clips, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.

Answer all questions.Electronic calculators may be used.A copy of the Periodic Table is printed on page 20.You may lose marks if you do not show your working or if you do not use appropriate units.

At the end of the examination, fasten all your work securely together.The number of marks is given in brackets [ ] at the end of each question or part question.

CHEMISTRY 0620/21

Paper 2 May/June 2014

1 hour 15 minutes

Candidates answer on the Question Paper.

No Additional Materials are required.

Cambridge International ExaminationsCambridge International General Certifi cate of Secondary Education

The syllabus is approved for use in England, Wales and Northern Ireland as a Cambridge International Level 1/Level 2 Certifi cate.

2

0620/21/M/J/14© UCLES 2014

1 (a) Choose from the list of substances below to answer the following questions.

calcium oxidecarbon dioxide

carbon monoxidecopper

hydrogenmagnesium

methaneoxygenwater

Each substance may be used once, more than once or not at all.

Which substance:

(i) releases hydrogen when it reacts with steam,

....................................................................................................................................... [1]

(ii) is produced at the cathode when concentrated aqueous sodium chloride is electrolysed,

....................................................................................................................................... [1]

(iii) is a product of the incomplete combustion of carbon,

....................................................................................................................................... [1]

(iv) is used in electrical wiring,

....................................................................................................................................... [1]

(v) is manufactured by heating limestone?

....................................................................................................................................... [1]

(b) Complete the following sentences about the Periodic Table of elements using words from the list below.

argon colour density sodium

one similarity trend seven

Chlorine, bromine and iodine are elements in Group ......................... of the Periodic Table.

These elements show a ......................... in ......................... down the group.

They all react rapidly with ......................... to form ionic compounds. [4]

[Total: 9]

3

0620/21/M/J/14© UCLES 2014 [Turn over

2 In 1904, J. J. Thomson suggested a model of the atom. He called this the ‘plum pudding’ model. This model of an atom, containing 14 electrons, is shown below.

sphere of positive chargewhich is spread out

electrons

(a) Describe how Thomson’s model of the atom differs from our present ideas of the structure of an atom.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(b) Lithium has two naturally-occurring isotopes. These can be written as:

63Li 7

3Liand

(i) Describe the difference between these isotopes.

....................................................................................................................................... [1]

(ii) Isotopes can be radioactive or non-radioactive. State one industrial use of radioactive isotopes.

....................................................................................................................................... [1]

(c) Lithium is in Group I of the Periodic Table. The table shows some properties of the Group I elements.

metal melting point / °C atomic radius / nm

lithium 0.157

sodium 98 0.191

potassium 63

rubidium 39 0.250

caesium 29 0.272

Deduce:

the melting point of lithium, ........................................................................... °C

the atomic radius of potassium .................................................................... nm [2]

4

0620/21/M/J/14© UCLES 2014

(d) Lithium reacts with water. An alkaline solution and a colourless gas are formed.

(i) Complete the word equation for this reaction.

lithium + water → .......................... .......................... + ..........................[2]

(ii) What is the most likely pH of the alkaline solution? Put a ring around the correct answer.

pH 2 pH 5 pH 7 pH 13[1]

(e) Draw the electronic structure of a potassium atom.

[2]

[Total: 12]

5


3 The table shows some fractions obtained from the distillation of petroleum.

fraction number ofcarbon atoms

boiling point ofthe fraction / °C

refi nery gas 1 – 4 under 40

gasoline 5 – 10 40 – 160

kerosene 10 – 16 160 – 250

diesel 16 – 20 250 – 300

fuel oil 20 – 30 300 – 350

(a) What is the relationship between the number of carbon atoms and the boiling points of the fractions?

.............................................................................................................................................. [1]

(b) State the names of two petroleum fractions not given in the table.

................................................................... and ................................................................... [2]

(c) Two of the compounds present in refi nery gas are methane and ethane.

(i) Draw the structure of ethane. Show all atoms and bonds.

[1]

(ii) Complete the dot and cross diagram of methane to show all the electrons.

H

HH C

H

[2]

6

0620/21/M/J/14© UCLES 2014

(d) Refi nery gas also contains propane. Propane can be cracked in the presence of a catalyst to form hydrogen.

(i) Complete the symbol equation for this reaction.

C3H8 → ............... + H2[1]

(ii) A catalyst is one condition needed to crack an alkane.

State one other condition needed to crack an alkane.

....................................................................................................................................... [1]

[Total: 8]

7


4 The diagram shows the changes of state when tin vapour is cooled slowly to room temperature.

tinvapour

liquidtin

solidtin

condensation solidification(freezing)

(a) Explain what happens to the arrangement and motion of the atoms during these changes.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [4]

(b) Tin is a metal in Group IV of the Periodic Table. How many electrons does tin have in its outer shell?

.............................................................................................................................................. [1]

(c) State one physical property of tin.

.............................................................................................................................................. [1]

(d) The table below describes the reaction of some metals with dilute hydrochloric acid.

iron bubbles of gas produced and temperature of the mixture rises slowly

magnesium many bubbles of gas produced rapidly and temperature of the mixture rises rapidly

silver no bubbles of gas given off and no temperature change

tin a few bubbles of gas given off slowly and temperature of the mixture rises very slowly

Put these metals in order of their reactivity.

least reactive most reactive

[2]

8

0620/21/M/J/14© UCLES 2014

(e) Tin is extracted by heating tin(IV) oxide with carbon.


SnO2 + .......C → Sn + .......CO[2]

(ii) State one adverse effect of carbon monoxide on health.

....................................................................................................................................... [1]

[Total: 11]

9


5 The diagram shows a blast furnace for extracting iron.

mixture ofiron ore

and coke

(a) On the diagram above, write:

● the letter A to show where the air blast enters the furnace,

● the letter W to show where the waste gases exit the furnace.[2]

(b) Which one of the following is an ore of iron? Put a ring around the correct answer.

calcite fl uorite hematite halite[1]

(c) In the furnace, the coke burns to form carbon dioxide. This reaction is exothermic.

(i) What is meant by the term exothermic ?

....................................................................................................................................... [1]

(ii) Describe a test for carbon dioxide.

test ......................................................................................................................................

result ............................................................................................................................. [2]

(d) In the blast furnace, carbon dioxide reacts with more coke to form carbon monoxide. The carbon monoxide reduces iron(III) oxide to iron.

Fe2O3 + 3CO → 2Fe + 3CO2

How does this equation show that iron(III) oxide is being reduced?

.............................................................................................................................................. [1]

[Total: 7]

10

0620/21/M/J/14© UCLES 2014

6 The structure of ethanol is shown below.

H C C

H

H

O

H

H

H

(a) On the structure above, put a ring around the alcohol functional group. [1]

(b) Ethanol can be made by fermentation.

(i) Complete the word equation for fermentation.

............................ → ethanol + ............................ ............................[2]

(ii) What type of catalysts are used in fermentation? Put a ring around the correct answer.

acids carbonates enzymes metals[1]

(c) Ethanol can also be made by hydration. Complete the symbol equation for this reaction.

............................ + H2O → C2H5OH[1]

(d) The diagram below shows how the rate of fermentation changes with temperature.

0 10 20 30temperature / °C

40 50 60

rate

Describe how the rate of fermentation changes with temperature.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

11


(e) The table shows some properties of different alcohols.

alcohol formula melting point/ °C

boiling point/ °C

densityin g / cm3

methanol CH4O – 94 65

ethanol C2H6O –117 79 0.789

propanol C3H8O –126 98 0.804

butanol C4H10O – 89 117 0.810

pentanol C5H12O – 79 138 0.815

(i) Describe how density changes with the number of carbon atoms in the alcohol.

....................................................................................................................................... [1]

(ii) Which one of these alcohols has the lowest melting point?

....................................................................................................................................... [1]

(iii) Is pentanol a solid, liquid or gas at room temperature? Explain your answer.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [1]

[Total: 10]

12

0620/21/M/J/14© UCLES 2014

7 A student used chromatography to separate the dyes in the blue ink from a ball-point pen. She used the equipment shown in the diagrams below.

solvent large watchglass chromatography tankchromatography paper

(a) Complete the diagram below to show how she set up the apparatus.

[3]

(b) Describe how chromatography could be used by the student to separate the dyes.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(c) The student used water as a solvent. Suggest a different solvent that she could use.

.............................................................................................................................................. [1]

13


(d) The diagram below shows the results of the chromatography using the blue ink, B, and several pure dyes, W, X, Y and Z.

B W X Y Z

(i) Which of the dyes, W, X, Y and Z, were in the blue ink?

....................................................................................................................................... [1]

(ii) How many dyes in the ink had been separated by this chromatography?

....................................................................................................................................... [1]

(e) The diagram shows the ball-point pen used in the experiment.

alloy tippoly(ethene) cap

ink

(i) The cap of the pen is made of poly(ethene). Describe the formation of poly(ethene) from ethene. In your answer, include the words:

● monomer, ● polymer.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) The tip of the pen is made from an alloy. What is meant by the term alloy ?

.............................................................................................................................................

....................................................................................................................................... [1]

14

0620/21/M/J/14© UCLES 2014

(f) The table shows some properties of four alloys.

alloy strength/ GPa

densityin g / cm3

thermalconductivityin W / m / K

low strength steel 250 7.70 60

high strength steel 300 7.90 56

low strength aluminium 70 2.72 170

high strength aluminium 220 2.80 100

(i) How does the strength of the steel and aluminium alloys vary with their thermal conductivity?

....................................................................................................................................... [1]

(ii) Which one of these alloys is the best one to use to make the body of an aircraft? Give two reasons for your answer.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

[Total: 16]

15


8 Zinc can be extracted from zinc sulfi de ore in three steps.

(a) In the fi rst step, zinc sulfi de is heated in air to produce zinc oxide.


2ZnS + ....O2 → 2ZnO + .....SO2[2]

(ii) The product sulfur dioxide, SO2, is harmful to the environment. Explain why it is harmful to the environment and state one effect it has on buildings.

.............................................................................................................................................

....................................................................................................................................... [2]

(b) In the second step, zinc oxide reacts with sulfuric acid to form zinc sulfate.

zinc oxide + sulfuric acid → zinc sulfate + water

Zinc sulfate is soluble in water. Some insoluble impurities in the zinc oxide do not react with the sulfuric acid. Suggest how these insoluble impurities are removed from the zinc sulfate solution.

.............................................................................................................................................. [1]

(c) In the third step, zinc is extracted from zinc sulfate by electrolysis using the cell shown below.

+ –lead rod aluminium rod

aqueous zinc sulfate

(i) Which word best describes the aluminium rod? Put a ring around the correct answer.

anion anode cathode cation electrolyte product[1]

16

0620/21/M/J/14© UCLES 2014

(ii) Suggest which statement about this electrolysis is completely correct. Tick one box.

Zinc is formed at the positive electrode and hydrogen at the negative electrode.

Zinc is formed at the positive electrode and oxygen at the negative electrode.

Zinc is formed at the negative electrode and hydrogen at the positive electrode.

Zinc is formed at the negative electrode and oxygen at the positive electrode.

[1]

[Total: 7]

17

0620/21/M/J/14© UCLES 2014

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18

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19

0620/21/M/J/14© UCLES 2014

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20

0620/21/M/J/14© UCLES 2014

Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Everyreasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included the publisher will be pleased to make amends at the earliest possible opportunity.


Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

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(r.t.p

.).

a Xb

a =

rela

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atom

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X =

atom

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b =

prot

on (a

tom

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r

Key

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71 L

anth

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90-1

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Elem

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*6390889396*





CHEMISTRY 0620/22


1 hour 15 minutes





2

0620/22/M/J/14© UCLES 2014

BLANK PAGE

3


1 The diagram shows part of the Periodic Table. Only some of the elements are shown.

H

Li C N O

Na Al

K Fe Co Ni Cu Zn

Rb

Cs Pb

(a) Answer the following questions using only the elements shown in the diagram. Each element may be used once, more than once or not at all.

(i) Which element has a giant covalent structure? ............................................................ [1]

(ii) Which element has the highest relative atomic mass? ................................................. [1]

(iii) Which two elements are formed when molten aluminium oxide is electrolysed?

...................... and ...................... [1]

(iv) Which element in Group I reacts most rapidly with water? ........................................... [1]

(v) Which element oxidises in the presence of water to form rust? ................................... [1]

(vi) Which element burns in oxygen to form water? ........................................................... [1]

(b) Rubidium reacts with oxygen to form rubidium oxide, Rb2O. Complete the symbol equation for this reaction.

....Rb + ...... → 2Rb2O[2]

(c) Lead compounds are atmospheric pollutants. State one adverse effect of lead compounds on health.

.............................................................................................................................................. [1]

[Total: 9]

4

0620/22/M/J/14© UCLES 2014

2 Carbon dioxide can be prepared in the laboratory using the apparatus shown below.

hydrochloric acid

A

carbondioxide

B

marble chips(calcium carbonate)

(a) State the names of the pieces of apparatus labelled A and B.

A ................................................................................................................................................

B ................................................................................................................................................[2]

(b) Complete the word equation for this reaction.

calciumcarbonate + hydrochloric

acid →.....................

.....................+ carbon

dioxide + .....................

[2]

(c) Carbon dioxide is slightly soluble in water. What effect will this have on the volume of carbon dioxide collected? Tick one box.

The volume is lower than expected.

The volume is higher than expected.

The volume is the same as expected.

No carbon dioxide is collected.[1]

5


(d) A burning candle is lowered into a beaker of carbon dioxide.

beaker

candle

(i) The fl ame goes out. Explain why the fl ame goes out.

....................................................................................................................................... [1]

(ii) After 20 seconds, the candle is removed and relit. It is then lowered into the same beaker again. The fl ame goes out again. What does this tell you about the density of carbon dioxide compared to air?

....................................................................................................................................... [1]

(iii) After 40 minutes, the candle is removed and relit. It is then lowered into the same beaker again. The candle stays alight. Explain why the candle stays alight.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 9]

6

0620/22/M/J/14© UCLES 2014

3 River water contains a variety of ions and gases, and insoluble materials such as soil particles.

(a) Describe how you could remove the insoluble materials from a sample of river water. Include a labelled diagram.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [4]

(b) The table shows the ions present in a sample of river water.

name of ion formula of ion concentration in mg / dm3

calcium Ca2+ 0.6

chloride Cl – 14.0

hydrogen carbonate HCO3– 1.5

iron(III) Fe3+ 0.5

magnesium Mg2+ 1.0

potassium K+ 3.0

sodium Na+ 11.0

SO42– 0.4

(i) Which ion with a charge of 2+ is present in the highest concentration?

....................................................................................................................................... [1]

(ii) State the name of the ion with the formula SO42–.

....................................................................................................................................... [1]

7


(iii) Calculate the total mass of ions present in 1 dm3 of river water.

.................. mg [1]

(iv) Use your answer to part (iii) to calculate the total mass of ions in 50 cm3 of river water.

.................. mg [1]

(v) A student evaporated the sample of river water to leave a solid containing a number of different compounds.

Use the information in the table to suggest the name of the compound present in the greatest amount.

....................................................................................................................................... [1]

8

0620/22/M/J/14© UCLES 2014

(c) The table shows the solubility of oxygen in river water at different temperatures.

temperature / °C 0 10 20 30 40 50 60

solubility in mg / dm3 11.0 8.8 7.2 6.0 4.9 4.2 3.6

(i) On the axes below, plot a graph to show how the solubility of oxygen changes with temperature. Draw a curve of best fi t through the points.

12

10

8

6

4

2

00 10 20 30

temperature / °C

solubilityin mg / dm3

40 50 60

[3]

(ii) Deduce the solubility of oxygen in river water at 25 °C.

....................................................................................................................................... [1]

(iii) State the approximate percentage of oxygen in the air.

....................................................................................................................................... [1]

[Total: 14]

9


4 The alkanes are a homologous series of hydrocarbons.

(a) Name another homologous series of hydrocarbons.

.............................................................................................................................................. [1]

(b) The graph below shows how the melting points of the fi rst eight alkanes vary with the number of carbon atoms.

1 2 3 4 5

number of carbon atoms

6 7 8 9 10

0

–50

–100

–150

–200

meltingpoint / °C

(i) Describe how the melting points of these alkanes vary with the number of carbon atoms.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) On the graph above, continue the line to show the melting points of the hydrocarbons having 9 and 10 carbon atoms. [2]

(c) The fi rst member of the alkane homologous series is methane.

(i) State one source of the methane in the atmosphere.

....................................................................................................................................... [1]

(ii) State one adverse effect of methane in the atmosphere.

....................................................................................................................................... [1]

(d) Complete the symbol equation to show the complete combustion of methane.

CH4 + ....O2 → ........ + 2H2O[2]

[Total: 9]

10

0620/22/M/J/14© UCLES 2014

5 Iron from a blast furnace contains carbon, sulfur, silicon and phosphorus as impurities.

(a) Iron is converted into steel in a basic oxygen converter. The impurities undergo oxidation. What is meant by the term oxidation?

.............................................................................................................................................. [1]

(b) Carbon is oxidised to carbon dioxide. Sulfur is oxidised to sulfur dioxide. Explain why these oxides are easily removed from the molten iron.

.............................................................................................................................................. [1]

(c) Phosphorus is converted to phosphorus(V) oxide.


.....P + 5O2 → 2P2O5[1]

(ii) Is phosphorus(V) oxide an acidic or basic oxide? Give a reason for your answer.

.............................................................................................................................................

....................................................................................................................................... [1]

(d) Phosphorus(V) oxide is a solid. Explain how this oxide is removed from the molten iron.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(e) Steel is an alloy.

(i) State one use of:

mild steel, ...........................................................................................................................

stainless steel. ....................................................................................................................[2]

11


(ii) Which diagram, A, B, C or D, best represents an alloy? Put a ring around the correct answer.

A B C D[1]

(f) The table shows the composition of some different brasses.

composition of the brass strength/ 108

Pa% zinc % copper

10 90 2.6

20 80 3.0

30 70 3.3

40 60 3.6

How does the composition of brass affect its strength?

.............................................................................................................................................. [1]

(g) A student dissolved a sample of brass in concentrated nitric acid. Nitrogen dioxide, NO2, was released.

Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O

(i) Write a word equation for this reaction.

[2]

(ii) The student added aqueous ammonia to the solution formed until the ammonia was in excess.

Describe what the student would observe.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(iii) State one source of the nitrogen dioxide in the atmosphere.

....................................................................................................................................... [1]

[Total: 17]

12

0620/22/M/J/14© UCLES 2014

6 In the 1860s, John Newlands listed the elements in order of increasing atomic mass. Part of his table is shown.

H1

Li2

Be3

B4

C5

N6

O7

F8

Na9

Mg10

Al11

Si12

P13

S14

Cl15

K16

Ca17

Cr18

Ti19

Mn20

Fe21

(a) (i) Describe the differences between Newlands’ table and the Periodic Table we use today.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) What evidence is there, from Newlands’ table, that some elements with similar properties are grouped together?

.............................................................................................................................................

....................................................................................................................................... [1]

(b) The table below shows some properties of some of the halogens.

halogen melting point/ °C

boiling point/ °C colour

chlorine –101 –7 yellow-green

bromine –7 red-brown

iodine +114 +184 grey-black

astatine +302 +337

Deduce:

the colour of astatine, ................................................................................................................

the boiling point of bromine, ......................................................................................................

the state of iodine at 190 °C. ......................................................................................................[3]

13


(c) Aqueous chlorine reacts with aqueous potassium bromide.

Cl 2 + 2KBr → Br2 + 2KCl

(i) Describe the colour change you would observe in this reaction.

....................................................................................................................................... [1]

(ii) State the name of the salt formed in this reaction.

....................................................................................................................................... [1]

(iii) Explain why aqueous bromine does not react with aqueous potassium chloride.

.............................................................................................................................................

....................................................................................................................................... [1]

(iv) The halogens exist as diatomic molecules. What is meant by the term diatomic?

....................................................................................................................................... [1]

[Total: 11]

14

0620/22/M/J/14© UCLES 2014

7 Ethanol is an alcohol.

(a) Complete the structure of ethanol showing all atoms and bonds.

– C – O – H

[1]

(b) State the name of the products formed when ethanol undergoes incomplete combustion.

................................................................... and ................................................................... [2]

(c) Ethanol can be manufactured by fermentation or by the hydration of ethene.

(i) Complete the word equation for the manufacture of ethanol from ethene.

ethene + ........................ → ethanol[1]

(ii) What conditions are needed for the manufacture of ethanol from ethene? Tick two boxes.

temperature above 100 °C

room temperature

presence of inorganic catalyst

presence of yeast

presence of hydrogen[2]

15


(iii) When ethanol is prepared by fermentation, the fermentation mixture produced contains ethanol and water.

The boiling point of ethanol is 78 °C. Describe how fractional distillation can be used to separate ethanol from water. In your answer, refer to:

● the apparatus used, ● changes in state, ● differences in boiling points.

You may use a diagram.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [5]

[Total: 11]

16

0620/22/M/J/14© UCLES 2014



Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



*1126807358*





CHEMISTRY 0620/23


1 hour 15 minutes





2

0620/23/M/J/14© UCLES 2014

1 (a) Choose from the list of compounds below to answer the following questions.

aluminium oxidecalcium carbonate

calcium oxidecopper(II) sulfatehydrogen chloridepotassium bromide

sodium chloridesodium hydroxide

Each compound can be used once, more than once or not at all.

Which compound:

(i) reacts with aqueous ammonia to form a light blue precipitate,

....................................................................................................................................... [1]

(ii) is formed by the decomposition of limestone,

....................................................................................................................................... [1]

(iii) forms an acidic solution when dissolved in water,

....................................................................................................................................... [1]

(iv) when electrolysed, gives a red-brown vapour at the anode,

....................................................................................................................................... [1]

(v) is an oxide of a metal in Group III of the Periodic Table,

....................................................................................................................................... [1]

(vi) is a transition element compound?

....................................................................................................................................... [1]

(b) Complete the following sentences about compounds using words from the list below.

chemically different fi xed

mixed physically similar

A compound is a substance which consists of two or more different elements ............................ combined together.

The properties of a compound are ............................ from those of the elements from which it is formed.

In a compound, the elements are combined in ............................ proportions. [3]

[Total: 9]

3


2 (a) Calcium chloride, CaCl 2, is a salt. Suggest the name of an acid and a base that would react together to make calcium chloride.

acid ............................................................................................................................................

base ...........................................................................................................................................[2]

(b) Calcium chloride absorbs water vapour. When calcium chloride is heated, it loses its water of crystallisation. Complete the symbol equation for this reaction. Include the sign for a reversible reaction.

CaCl 2.6H2O CaCl 2 + .................[2]

(c) A student put some clean iron nails in two test-tubes, as shown in the diagram. She then left the test-tubes for several weeks.

A B

anhydrouscalcium chloride

CaCl 2

cotton wool

cotton wool

Explain why the nails in tube A did not rust but the nails in tube B rusted.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

(d) Rust is hydrated iron(III) oxide. What does the (III) in iron(III) oxide refer to? Tick one box.

the oxidation state of the oxygen

the oxidation state of the iron

the number of atoms of oxygen in a formula unit of iron(III) oxide

the number of water molecules in the hydrated iron oxide

[1]

4

0620/23/M/J/14© UCLES 2014

(e) (i) The table describes the ease of reduction of some metal oxides with carbon monoxide.

lead oxide moderate heating to about 200 °C needed

iron oxide high temperature furnace at 750 °C needed

magnesium oxide temperatures above 1000 °C needed

zinc oxide very high temperature furnace at 900 °C needed

Put these metals in order of their reactivity with carbon monoxide.

least reactive most reactive

[2]

(ii) Some metal oxides can be reduced by heating with hydrogen gas.

CuO + H2 → Cu + H2O

Explain how this equation shows that copper oxide is being reduced.

....................................................................................................................................... [1]

[Total: 10]

5


3 The diagram shows the best pH ranges for growing different plants.

4pH 5 6 7 8

beans

carrots

clover

potatoes

tomatoes

(a) (i) Which two plants grow best in acidic conditions only?

................................................................ and ............................................................... [1]

(ii) Which pH shown in the diagram above represents a neutral pH?

....................................................................................................................................... [1]

(b) (i) Explain why lime is added to acidic soils.

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Farmers fertilise soil by adding compounds containing ammonium salts. Explain why adding lime to fertilised soil may cause a loss of nitrogen from the soil.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

6

0620/23/M/J/14© UCLES 2014

(c) The graphs below show the rate of uptake of potassium and phosphate ions by plant roots at different pH values.

3 4 5 6 7pH

8 9 10

rate ofuptake

ofpotassium

3 4 5 6 7pH

8 9 10 11

rate ofuptake

ofphosphorus

(i) Describe the effect of pH on the rate of uptake of potassium by plant roots.

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) At which pH value is the rate of uptake of phosphorus by plant roots the highest?

....................................................................................................................................... [1]

[Total: 10]

7


4 Chromatography is used to separate a mixture of coloured dyes.

(a) Three different dye mixtures, A, B and C, were spotted onto a piece of chromatography paper. Two pure dyes, X and Y, were also spotted onto the same piece of paper.

The diagram below shows the results of the chromatography.

A B C X Y

solvent front

base line

(i) State the name of a piece of apparatus that could be used to spot the dyes onto the paper.

....................................................................................................................................... [1]

(ii) Suggest why the base line was drawn in pencil and not in ink.

....................................................................................................................................... [1]

(iii) Which dye mixture contains both dye X and dye Y?

....................................................................................................................................... [1]

(iv) Which dye mixture does not contain dye X or dye Y?

....................................................................................................................................... [1]

(v) In which mixture, A, B or C, has the greatest number of dyes been separated?

....................................................................................................................................... [1]

8

0620/23/M/J/14© UCLES 2014

(b) The structure of the dye chrysoidine G is shown below.

C C

C C

C CC N NNH

HH

HH

C C

C C

C

H

H

H

H HN

HH

(i) How many nitrogen atoms are there in a molecule of chrysoidine G?

....................................................................................................................................... [1]

(ii) Complete the table below to calculate the relative molecular mass of chrysoidine G.

type of atom number of atoms atomic mass

carbon 12 12 12 × 12 = 144

hydrogen

nitrogen

relative molecular mass = ............................[2]

(c) The fi bres in the chromatography paper are polymers.

(i) What is meant by the term polymer?

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) State the chemical name of the polymer formed from ethene.

....................................................................................................................................... [1]

[Total: 10]

9


5 The table shows some properties of the fi rst four carboxylic acids.

acid molecularformula

melting point/ °C

boiling point/ °C

densityin g / cm3

methanoic acid CH2O2 +10 +101 1.22

ethanoic acid C2H4O2 +17 +118 1.05

propanoic acid C3H6O2 –21 0.99

butanoic acid C4H8O2 – 4 +166

(a) (i) How does the boiling point of these carboxylic acids vary with the number of carbon atoms?

....................................................................................................................................... [1]

(ii) Suggest a value for:

the boiling point of propanoic acid, ................................................................................ °C

the density of butanoic acid. .................................................................................... g / cm3

[2]

(iii) Is butanoic acid a solid, liquid or gas at room temperature? Use the data in the table to explain your answer.

.............................................................................................................................................

....................................................................................................................................... [1]

(b) Complete the diagram below to show the structure of ethanoic acid. Show all atoms and bonds.

H C

H

H

C

[1]

10

0620/23/M/J/14© UCLES 2014

(c) The concentration of ethanoic acid can be determined by titration using the apparatus shown below.

AB

ethanoicacid

(i) State the name of the piece of glassware labelled A.

....................................................................................................................................... [1]

(ii) Liquid B is an alkali. Which one of the following compounds is also an alkali? Put a ring around the correct answer.

calcium carbonate

calcium sulfate

sodium chloride

sodium hydroxide[1]

(iii) Describe how you would carry out this titration.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 9]

11


6 Lead(II) bromide is a white solid. Part of the structure of lead(II) bromide is shown below.

Br –

Br –

Br –

Br –Pb2+

Br –

Br –

Br –

Br –Pb2+

Br – Br –

Pb2+

Br – Br –

Pb2+

Pb2+ Pb2+

(a) Deduce the simplest formula for lead(II) bromide.

.............................................................................................................................................. [1]

(b) A student electrolysed lead(II) bromide in a fume cupboard using the apparatus shown below.

anode cathode

lead(II) bromide

(i) Why is heat needed for this electrolysis?

....................................................................................................................................... [1]

(ii) Suggest the name of a substance that could be used for the electrodes.

....................................................................................................................................... [1]

(iii) State the name of the products of electrolysis at:

the anode, ...........................................................................................................................

the cathode. .................................................................................................................. [1]

12

0620/23/M/J/14© UCLES 2014

(c) Items can be electroplated with silver using the apparatus shown below.

B

CA

D

rod of silveralloy rod

electrolyte

+–

(i) On the diagram, which letter, A, B, C or D, is the cathode?

....................................................................................................................................... [1]

(ii) What would you observe during the experiment at the:

positive electrode,

.............................................................................................................................................

negative electrode?

.............................................................................................................................................[2]

(iii) The electrolyte used is aqueous silver cyanide, AgCN. Calculate the relative formula mass of silver cyanide. You must show all your working.

[2]

[Total: 9]

13


7 Dmitri Mendeleev published his fi rst Periodic Table in 1869. Part of this table is shown below.

Ti = 50 V = 51 Cr = 52 Mn = 55 Fe = 56 Co = 59 H = 1 Cu = 63.4 Be = 9.4 Mg = 24 Zn = 65.2 B = 11 Al = 27.4 ? C = 12 Si = 28 ? N = 14 P = 31 As = 75 O = 16 S = 32 Se = 79.4 F = 19 Cl = 35.5 Br = 80 Li = 7 Na = 23 K = 39 Rb = 85.4

(a) (i) What differences are there between Mendeleev’s table and the Periodic Table we use today?

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [4]

(ii) State the names of any two elements in the table above which exist as diatomic molecules.

................................................................ and ............................................................... [1]

(b) Titanium is a transition element. Sodium is a metal in Group I of the Periodic Table. State three differences in the physical properties of titanium and sodium.

1 .................................................................................................................................................

2 .................................................................................................................................................

3 .................................................................................................................................................[3]

14

0620/23/M/J/14© UCLES 2014

(c) Titanium(IV) oxide reacts with a mixture of chlorine and carbon. The products are titanium(IV) chloride, TiCl 4, and a gas which turns limewater milky. Complete the symbol equation for this reaction.

TiO2 + .....Cl 2 + C → TiCl 4 + ...............[2]

(d) Titanium is extracted from titanium(IV) chloride by reduction with molten sodium in the presence of argon.

Suggest why this reaction is carried out in the presence of argon.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 12]

15


8 Sodium sulfate is a solid with a high melting point. Sodium sulfate conducts electricity when molten but not when solid.

(a) What type of structure is sodium sulfate? Tick one box.

structure of separated atoms

simple molecular structure

giant ionic structure

giant covalent structure[1]

(b) Describe a test for sulfate ions.

test .............................................................................................................................................

result ..........................................................................................................................................[2]

(c) Describe how simple distillation is used to separate water from an aqueous solution of sodium sulfate.

In your answer, refer to:

● the apparatus used, ● changes in state, ● differences in boiling points.

You may use a diagram.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [5]

16

0620/23/M/J/14© UCLES 2014

(d) What would you observe when a piece of blue cobalt chloride paper is dipped into water?

.............................................................................................................................................. [1]

(e) Describe how impure water is treated so that it can be used for drinking.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 11]

17

0620/23/M/J/14© UCLES 2014

BLANK PAGE

18

0620/23/M/J/14© UCLES 2014

BLANK PAGE

19

0620/23/M/J/14© UCLES 2014

BLANK PAGE

20

0620/23/M/J/14© UCLES 2014



Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



*3226538232*


Write your Centre number, candidate number and name on all the work you hand in.Write in dark blue or black pen.You may use an HB pencil for any diagrams or graphs.Do not use staples, paper clips, glue or correction fl uid.DO NOT WRITE IN ANY BARCODES.



CHEMISTRY 0620/31

Paper 3 (Extended) May/June 2014

1 hour 15 minutes





2

0620/31/M/J/14© UCLES 2014

1 The table below gives the composition of six particles which are either atoms or ions.

particle number of protons number of neutrons number of electrons

A 33 40 33

B 19 20 18

C 34 45 36

D 33 42 33

E 13 14 13

F 24 28 21

(a) Which particles are atoms? Explain your choice.

....................................................................................................................................................

.............................................................................................................................................. [2]

(b) Which particle is a negative ion and why has this particle got a negative charge?

....................................................................................................................................................

.............................................................................................................................................. [2]

(c) Which particles are positive ions?

.............................................................................................................................................. [1]

(d) Explain why particle A and particle D are isotopes.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 7]

3


2 (a) Water is needed for industry and in the home.

(i) Rain water is collected in reservoirs. How is it treated before entering the water supply?

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) State two industrial uses of water.

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) State two uses of water in the home.

.............................................................................................................................................

....................................................................................................................................... [1]

(b) In many regions, drinking water is obtained by the distillation of sea-water. Explain how distillation separates the water from sea-water.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 7]

4

0620/31/M/J/14© UCLES 2014

3 (a) Different gases diffuse at different speeds.

(i) What is meant by the term diffusion?

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) What property of a gas molecule affects the speed at which it diffuses?

....................................................................................................................................... [1]

(b) Helium is a gas used to fi ll balloons. It is present in the air in very small quantities. Diffusion can be used to separate it from the air.

Air at 1000 °C is on one side of a porous barrier. The air which passes through the barrier has a larger amount of helium in it.

(i) Why does the air on the other side of the barrier contain more helium?

....................................................................................................................................... [1]

(ii) Why is it an advantage to have the air at a high temperature?

.............................................................................................................................................

....................................................................................................................................... [1]

(c) Most helium is obtained from natural gas found in the USA. Natural gas contains methane and 7% helium. One possible way to obtain the helium would be to burn the methane.

(i) Write an equation for the complete combustion of methane.

....................................................................................................................................... [1]

(ii) Suggest why this would not be a suitable method to obtain the helium.

.............................................................................................................................................

....................................................................................................................................... [1]

(iii) Suggest another method, other than diffusion, by which helium could be separated from the mixture of gases in natural gas.

....................................................................................................................................... [1]

[Total: 7]

5


4 In the Periodic Table, the elements are arranged in columns called Groups and in rows called Periods.

(a) (i) Complete the table for some of the elements in Period 3.

group number I II III IV V VI VII

symbol Na Mg Al Si P S Cl

number of valency electrons

valency

[2]

(ii) What is the relationship between the group number and the number of valency electrons?

.............................................................................................................................................

....................................................................................................................................... [1]

(iii) Explain the relationship between the number of valency electrons and the valency

for the elements Na to Al,

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

for the elements P to Cl.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................[4]

(b) Across a period, the elements change from metallic to non-metallic.

(i) Describe how the type of oxide changes across this period.

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Describe how the type of bonding in the chlorides formed by these elements changes across this period.

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 11]

6

0620/31/M/J/14© UCLES 2014

BLANK PAGE

7


5 Zinc is obtained from the ore, zinc blende, ZnS.

(a) Describe the extraction of zinc from its ore, zinc blende. Include at least one balanced equation in your description.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [5]

(b) State two major uses of zinc.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 7]

8

0620/31/M/J/14© UCLES 2014

6 Hydrogen peroxide decomposes to form water and oxygen. This reaction is catalysed by manganese(IV) oxide.

2H2O2(aq) → 2H2O(l) + O2(g)

The rate of this reaction can be investigated using the following apparatus.

aqueous hydrogen peroxideand manganese(IV) oxide

oxygen gas

40 cm3 of aqueous hydrogen peroxide was put in the fl ask and 0.1 g of small lumps of manganese(IV) oxide was added. The volume of oxygen collected was measured every 30 seconds. The results were plotted to give the graph shown below.

volume ofoxygen

time

00t1 t2 t3

(a) (i) How do the rates at times t1, t2 and t3 differ?

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Explain the trend in reaction rate that you described in (a)(i).

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

9


(b) The experiment was repeated using 0.1 g of fi nely powdered manganese(IV) oxide. All the other variables were kept the same.

(i) On the axes opposite, sketch the graph that would be expected. [2]

(ii) Explain the shape of this graph. ..........................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(c) Describe how you could show that the catalyst, manganese(IV) oxide, was not used up in the reaction. Manganese(IV) oxide is insoluble in water.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [4]

(d) In the fi rst experiment, the maximum volume of oxygen produced was 96 cm3 measured at r.t.p. Calculate the concentration of the aqueous hydrogen peroxide in mol / dm3.

2H2O2(aq) → 2H2O(l) + O2(g)

number of moles of O2 formed = .......................................................................................... [1]

number of moles of H2O2 in 40 cm3 of solution = ................................................................. [1]

concentration of the aqueous hydrogen peroxide in mol / dm3 = ................................................

.......................................... [1]

[Total: 15]

10

0620/31/M/J/14© UCLES 2014

7 One way of establishing a reactivity series is by displacement reactions.

(a) A series of experiments was carried out using the metals lead, magnesium, zinc and silver. Each metal was added in turn to aqueous solutions of the metal nitrates.

The order of reactivity was found to be:

magnesium most reactive

zinc ↓lead

silver least reactive

(i) Complete the table.

= reacts = does not react

metal

aqueous solution

leadPb

magnesiumMg

zincZn

silverAg

lead(II)nitrate

magnesiumnitrate

zincnitrate

silvernitrate

[3]

(ii) Displacement reactions are redox reactions. On the following equation, draw a ring around the reducing agent and an arrow to show

the change which is oxidation.

Zn + Pb2+ → Zn2+ + Pb[2]

(iii) Complete the following ionic equation.

Zn + 2Ag+ → ....... + .......[1]

11


(b) Another way of determining the order of reactivity of metals is by measuring the voltage and polarity of simple cells. The polarity of a cell is shown by which metal is the positive electrode and which metal is the negative electrode. An example of a simple cell is shown below.

zinc electrodelead electrode

electrolyte ofdilute acid

voltmeter

+ –

V

(i) Mark on the above diagram the direction of the electron fl ow. [1]

(ii) Explain, in terms of electron transfer, why the more reactive metal is always the negative electrode.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) The following table gives the polarity of cells using the metals zinc, lead, copper and manganese.

cell electrode 1 polarity electrode 2 polarity

A zinc – lead +

B manganese – lead +

C copper + lead –

What information about the order of reactivity of these four metals can be deduced from the table?

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(iv) What additional information is needed to establish the order of reactivity of these four metals using cells?

....................................................................................................................................... [1]

[Total: 12]

12

0620/31/M/J/14© UCLES 2014

8 Polymers are made by the polymerisation of simple molecules called monomers.

(a) (i) The structural formula of a polymer is given below.

n

CH

CH3

CH

CH3

This polymer is made by addition polymerisation. Draw the structural formula of its monomer.

[1]

(ii) The two monomers shown below form a nylon which is a condensation polymer.

NH2H2N

COOHHOOC

Draw its structural formula showing one repeat unit of the polymer.

[3]

(iii) Name the natural macromolecule which contains the same linkage as nylon.

....................................................................................................................................... [1]

(iv) Explain the difference between addition polymerisation and condensation polymerisation.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

13


(b) Many polymers are non-biodegradable.

(i) Explain the term non-biodegradable.

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) State three problems caused by the disposal of non-biodegradable polymers.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(c) Storage tanks for cold water are now made from polymers because they are cheaper than metal tanks. Suggest two other advantages of making cold water tanks from polymers.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 14]

14

0620/31/M/J/14© UCLES 2014

BLANK PAGE

15

0620/31/M/J/14© UCLES 2014

BLANK PAGE

16

0620/31/M/J/14© UCLES 2014



Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



*5879467154*





CHEMISTRY 0620/32


1 hour 15 minutes





2

0620/32/M/J/14© UCLES 2014

1 The table below gives the electron distributions of atoms of different elements.

element electron distribution

A 2 + 7

B 2 + 8 + 4

C 2 + 8 + 8 + 1

D 2 + 8 + 18 + 5

E 2 + 8 + 18 + 7

F 2 + 8 + 18 + 18 + 8

For each of the following, select an element or elements from the table that matches the description. Each element may be selected once, more than once or not at all.

(a) These two elements are in the same group.

.............................................................................................................................................. [1]

(b) This element forms a fl uoride with a formula of the type XF3.

.............................................................................................................................................. [1]

(c) This element reacts violently with cold water.

.............................................................................................................................................. [1]

(d) This element has a macromolecular structure similar to that of diamond.

.............................................................................................................................................. [1]

(e) The only oxidation state of this element is 0.

.............................................................................................................................................. [1]

(f) This element is bromine.

.............................................................................................................................................. [1]

(g) This element is a good conductor of electricity.

.............................................................................................................................................. [1]

[Total: 7]

3


2 (a) Natural gas, which is mainly methane, is a fossil fuel.

(i) What is meant by the term fuel ?

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Name two other fossil fuels.

....................................................................................................................................... [2]

(iii) Name a solid fuel which is not a fossil fuel.

....................................................................................................................................... [1]

(b) Fossil fuels are formed by the anaerobic decomposition of organic matter. Anaerobic means in the absence of oxygen.

(i) The organic matter contains hydrogen and carbon. Suggest the products that would be formed if the decomposition occurred in the presence of oxygen.

....................................................................................................................................... [2]

(ii) What are the two main disadvantages in the widespread use of fossil fuels?

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 8]

4

0620/32/M/J/14© UCLES 2014

3 Plant growth is improved by the availability of essential elements, such as nitrogen, and by the soil having a suitable pH.

(a) Nitrogen-based fertilisers are made from ammonia. Ammonia is manufactured by the Haber process.

(i) Describe the Haber process giving reaction conditions and a balanced equation. (Do not discuss reaction rate and yield.)

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [5]

(ii) Fertilisers contain nitrogen. Name the other two elements essential for plant growth commonly found in fertilisers.

....................................................................................................................................... [2]

(b) Crops do not grow well if the soil is too acidic.

(i) One cause of acidity in soil is acid rain. Explain how acid rain is formed.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(ii) Name two bases which are used to increase the pH of acidic soils.

....................................................................................................................................... [2]

[Total: 12]

5


4 Propanoic acid is a carboxylic acid. Its formula is CH3–CH2–COOH.

(a) Propanoic acid is the third member of the homologous series of carboxylic acids.

(i) Give the name and structural formula of the fourth member of this series.

name ...................................................................................................................................

formula .......................................................................................................................... [2]

(ii) Members of a homologous series have very similar chemical properties. State three other characteristics of a homologous series.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(b) Carboxylic acids can be made by the oxidation of alcohols.

(i) Draw the structural formula of the alcohol which can be oxidised to propanoic acid. Show all atoms and bonds.

[1]

(ii) Name a reagent, other than oxygen, which can oxidise alcohols to carboxylic acids.

....................................................................................................................................... [2]

6

0620/32/M/J/14© UCLES 2014

(c) Complete the following equations for some of the reactions of propanoic acid. The salts of this acid are called propanoates.

(i) zinc + propanoic acid → ........................... ........................... + hydrogen [1]

(ii) calcium + propanoic → ........................... ........................... + ........................... oxide acid [1]

(iii) LiOH + CH3CH2COOH → ............................... + ........................... [1]

(d) A piece of magnesium was added to 100 cm3 of an aqueous acid. The time taken for the metal to react completely was measured. This experiment was repeated using different aqueous acids. The same volume of acid was used in each experiment and the pieces of magnesium used were identical. In one experiment the reaction was carried out at a different temperature.

experiment acid concentrationin mol / dm3

temperature/ °C

time/ minutes

A propanoic 1.0 20 5

B propanoic 1.0 30 3

C propanoic 0.5 20 8

D hydrochloric 1.0 20 1

Explain the following in terms of collision rate between reacting particles.

(i) Why is the rate in experiment C slower than the rate in experiment A?

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Why is the rate in experiment B faster than the rate in experiment A?

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) Why is the rate in experiment D faster than the rate in experiment A?

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

[Total: 18]

7


5 Carbonyl chloride is made from carbon monoxide and chlorine.

CO(g) + Cl 2(g) COCl 2(g)

(a) Two methods of preparing carbon monoxide are from methane and oxygen, and from methane and steam.

(i) The reaction between methane and oxygen can also form carbon dioxide. How can carbon monoxide be made instead of carbon dioxide?

....................................................................................................................................... [1]

(ii) The following reaction is used to make carbon monoxide and hydrogen. The reaction is carried out at 1100 °C and normal pressure.

CH4(g) + H2O(g) CO(g) + 3H2(g)

The reaction is reversible and comes to equilibrium. Suggest why a high temperature is used.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) What is the disadvantage of using a high pressure for the reaction given in (a)(ii)?

.............................................................................................................................................

....................................................................................................................................... [2]

(b) Chlorine is made by the electrolysis of concentrated aqueous sodium chloride. Describe this electrolysis. Write ionic equations for the reactions at the electrodes and name

the sodium compound formed.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [5]

8

0620/32/M/J/14© UCLES 2014

(c) The structural formula of carbonyl chloride is given below.

C O

Cl

Cl

Draw a diagram showing the arrangement of the valency electrons around the atoms in one molecule of this covalent compound.

Use ○ to represent an electron from an oxygen atom. Use × to represent an electron from a chlorine atom. Use ● to represent an electron from a carbon atom.

[3]

[Total: 13]

6 Scandium, proton number 21, is not a typical transition element.

(a) Scandium is a low density metal which has only one oxidation state in its compounds. Scandium compounds are white solids which form colourless solutions. Titanium, the next metal in the period, is a far more typical transition element. How would the properties of titanium differ from those of scandium?

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

9


(b) Scandium fl uoride is an ionic compound. The valency of scandium in scandium fl uoride is three.

Draw a diagram which shows the formula of this compound, the charges on the ions and the arrangement of the valency electrons around the negative ions.

Use × to represent an electron from a fl uorine atom. Use ○ to represent an electron from a scandium atom.

[3]

(c) Scandium oxide is insoluble in water. Describe how you could show that it is an amphoteric oxide.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 9]

10

0620/32/M/J/14© UCLES 2014

7 The soluble salt hydrated lithium sulfate is made by titration from the soluble base lithium hydroxide.

burette filled withsulfuric acid

aqueous lithium hydroxideand a few drops of a pH indicator

conical flask

(a) The sulfuric acid is added slowly from the burette until the indicator just changes colour. The volume of sulfuric acid needed to just neutralise the lithium hydroxide is noted.

Describe how you would continue the experiment to obtain pure dry crystals of hydrated lithium sulfate.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [5]

(b) Using 25.0 cm3 of aqueous lithium hydroxide, concentration 2.48 mol / dm3, 2.20 g of hydrated lithium sulfate was obtained.

Calculate the percentage yield, giving your answer to one decimal place.

2LiOH + H2SO4 → Li2SO4 + 2H2O

Li2SO4 + H2O → Li2SO4.H2O

Number of moles of LiOH used = .......................

Number of moles of Li2SO4.H2O which could be formed = .......................

Mass of one mole of Li2SO4.H2O = 128 g

Maximum yield of Li2SO4.H2O = ....................... g

Percentage yield = .......................% [4]

11


(c) An experiment was carried out to show that the formula of the hydrated salt is Li2SO4.H2O. A sample of the hydrated salt was weighed and its mass recorded. It was then heated and the anhydrous salt was weighed. This procedure was repeated until two consecutive masses were the same. This procedure is called ‘heating to constant mass’.

(i) What is the reason for heating to constant mass?

....................................................................................................................................... [1]

(ii) The mass of the hydrated salt is m1 and the mass of the anhydrous salt is m2. Explain how you could show that the hydrated salt has one mole of water of crystallisation per mole of the anhydrous salt.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

[Total: 13]

12

0620/32/M/J/14© UCLES 2014



Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



*4182021420*





CHEMISTRY 0620/33


1 hour 15 minutes





2

0620/33/M/J/14© UCLES 2014

1 Choose a gas from the following list to answer the questions below. Each gas may be used once, more than once or not at all.

ammonia carbon dioxide carbon monoxide fl uorine

hydrogen krypton nitrogen propene sulfur dioxide

(a) It is a product of respiration. ................................................................................................ [1]

(b) It polymerises to form a poly(alkene). .................................................................................. [1]

(c) It is a noble gas. .................................................................................................................. [1]

(d) It is the main component of air. ............................................................................................ [1]

(e) It is a very reactive non-metal. ............................................................................................. [1]

(f) It is used to kill micro-organisms in fruit juice. ..................................................................... [1]

(g) It burns to form water as the only product. .......................................................................... [1]

[Total: 7]

3


2 Explain each of the following in terms of the kinetic particle theory.

(a) The rate of most reactions increases at higher temperatures.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(b) A liquid has a fi xed volume but takes up the shape of the container. A gas takes up the shape of the container but it does not have a fi xed volume.

liquid gas

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 6]

4

0620/33/M/J/14© UCLES 2014

3 (a) Biological catalysts produced by microbes cause food to deteriorate and decay.

(i) What is the name of these biological catalysts?

....................................................................................................................................... [1]

(ii) Freezing does not kill the microbes. Suggest why freezing is still a very effective way of preserving food.

.............................................................................................................................................

....................................................................................................................................... [2]

(b) Pea seeds grow in pods on pea plants.

Freshly picked pea seeds contain a sugar. The sugar can form a polymer. Give the structural formula of the polymer and name the other product of this polymerisation

reaction. You may represent the sugar by the formula:

OHHO

structural formula of the polymer

other product ....................................................................................................................... [3]

5


(c) Describe how the pea plant makes a sugar such as glucose.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 9]

4 Iron from a blast furnace contains about 5% of the impurities – carbon, silicon, phosphorus and sulfur. Most of this impure iron is used to make steels, such as mild steel, and a very small percentage is used to make pure iron.

(a) Calcium oxide and oxygen are used to remove the impurities from the iron produced in the blast furnace.

(i) State how these chemicals are manufactured.

calcium oxide ......................................................................................................................

.............................................................................................................................................

oxygen ................................................................................................................................

.............................................................................................................................................[3]

(ii) Describe how these two chemicals remove the four impurities. Include at least one equation in your answer.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [5]

6

0620/33/M/J/14© UCLES 2014

(b) (i) Describe the structure of a typical metal such as iron. You may include a diagram.

.............................................................................................................................................

.............................................................................................................................................

[2]

(ii) Explain why pure iron is malleable.

.............................................................................................................................................

....................................................................................................................................... [2]

(iii) Mild steel is an alloy of iron and carbon. Suggest why mild steel is harder than pure iron.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 14]

7


5 Ammonia is made by the Haber process.

N2(g) + 3H2(g) 2NH3(g)

The forward reaction is exothermic. The conditions in the reaction chamber are:

● a pressure of 200 atmospheres, ● a catalyst of finely divided iron, ● a temperature of 400 to 450 °C.

(a) What are the two advantages of using a high pressure? Give a reason for both.

advantage 1 ...............................................................................................................................

reason ........................................................................................................................................

....................................................................................................................................................

advantage 2 ...............................................................................................................................

reason ........................................................................................................................................

....................................................................................................................................................[4]

(b) A higher temperature would give a faster reaction rate. Why is a higher temperature not used?

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

(c) (i) Why is the iron catalyst used as a fi ne powder?

.............................................................................................................................................

....................................................................................................................................... [1]

(ii) Give two reasons why a catalyst is used.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [2]

8

0620/33/M/J/14© UCLES 2014

(d) The equilibrium mixture leaving the reaction chamber contains 15% ammonia. Suggest how the ammonia could be separated from the mixture.

boiling point / °C

hydrogen –253

nitrogen –196

ammonia –33

....................................................................................................................................................

.............................................................................................................................................. [2]

(e) Ammonia is used to make nitrogen trifl uoride, NF3. Nitrogen trifl uoride is essential to the electronics industry. It is made by the following reaction.

H N

H

H + +F F

→F FF F

H FH FH F

NF F

F

Determine if the above reaction is exothermic or endothermic using the following bond energies and by completing the following table. The fi rst line has been done as an example.

Bond energy is the amount of energy, in kJ / mole, needed to break or make one mole of the bond.

bond bond energy in kJ / mole

N – H 390

F – F 155

N – F 280

H – F 565

bond energy change / kJ

N – H (3 × 390) = 1170

F – F

N – F

H – F

....................................................................................................................................................

.............................................................................................................................................. [4]

[Total: 16]

9


6 The alkanes are a family of saturated hydrocarbons. Their reactions include combustion, cracking and substitution.

(a) (i) What is meant by the term hydrocarbon?

....................................................................................................................................... [1]

(ii) What is meant by the term saturated ?

....................................................................................................................................... [1]

(b) (i) What is the general formula for the homologous series of alkanes?

....................................................................................................................................... [1]

(ii) Calculate the mass of one mole of an alkane with 14 carbon atoms.

.............................................................................................................................................

....................................................................................................................................... [2]

(c) The complete combustion of hydrocarbons produces carbon dioxide and water only.

(i) Write the equation for the complete combustion of nonane, C9H20.

....................................................................................................................................... [2]

(ii) 20 cm3 of a gaseous hydrocarbon was mixed with an excess of oxygen, 200 cm3. The mixture was ignited. After cooling, 40 cm3 of oxygen and 100 cm3 of carbon dioxide remained. Deduce the formula of the hydrocarbon and the equation for its combustion. All volumes were measured at r.t.p..

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

10

0620/33/M/J/14© UCLES 2014

(d) Cracking is used to obtain short-chain alkanes, alkenes and hydrogen from long-chain alkanes.

(i) Give a use for each of the three products listed above.

short-chain alkanes ............................................................................................................

alkenes ...............................................................................................................................

hydrogen ....................................................................................................................... [3]

(ii) Write an equation for the cracking of decane, C10H22, which produces two different alkenes and hydrogen as the only products.

....................................................................................................................................... [1]

(e) Chlorine reacts with propane in a substitution reaction to form 1-chloropropane.

CH3 – CH2 – CH3 + Cl 2 → CH3 – CH2 – CH2 – Cl + HCl

(i) What is the essential condition for the above reaction?

....................................................................................................................................... [1]

(ii) There is more than one possible substitution reaction between chlorine and propane. Suggest the structural formula of a different product.

....................................................................................................................................... [1]

[Total: 16]

11


7 Aluminium is obtained from purifi ed alumina, Al 2O3, by electrolysis.

(a) Alumina is obtained from the main ore of aluminium. State the name of this ore.

.............................................................................................................................................. [1]

(b) Describe the extraction of aluminium from alumina. Include the electrolyte, the electrodes and the reactions at the electrodes.

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [6]

(c) Aluminium is resistant to corrosion. It is protected by an oxide layer on its surface. The thickness of this oxide layer can be increased by anodising.

(i) State a use of aluminium due to its resistance to corrosion.

....................................................................................................................................... [1]

(ii) Anodising is an electrolytic process. Dilute sulfuric acid is electrolysed with an aluminium object as the anode. The thickness of the oxide layer is increased. Complete the equations for the reactions at the aluminium anode.

.......OH– → O2 + 2H2O + ......e–

....Al + ......... → ......... Al 2O3 [4]

[Total: 12]

12

0620/33/M/J/14© UCLES 2014



Gro

up

140

Ce

Cer

ium

58

141

PrP

rase

odym

ium

59

144

Nd

Neo

dym

ium

60

PmP

rom

ethi

um61

150

SmS

amar

ium

62

152

EuE

urop

ium

63

157

Gd

Gad

olin

ium

64

159

Tb Terb

ium

65

162

Dy

Dys

pros

ium

66

165

Ho

Hol

miu

m67

167

Er Erb

ium

68

169

Tm Thul

ium

69

173

YbY

tterb

ium

70

175

LuLu

tetiu

m71

232

Th Thor

ium

90

PaP

rota

ctin

ium

91

238 U

Ura

nium

92

Np

Nep

tuni

um93

PuP

luto

nium

94

Am

Am

eric

ium

95

Cm

Cur

ium

96

Bk

Ber

keliu

m97

Cf

Cal

iforn

ium

98

EsE

inst

eini

um99

Fm Ferm

ium

100

Md

Men

dele

vium

101

No

Nob

eliu

m10

2

LrLa

wre

nciu

m10

3

1 HH

ydro

gen

1

7 LiLi

thiu

m3

23 Na

Sod

ium

11

24 Mg

Mag

nesi

um12

40 Ca

Cal

cium

20

45 ScS

cand

ium

21

48 TiTi

tani

um22

51 VVa

nadi

um23

52 Cr

Chr

omiu

m24

55 Mn

Man

gane

se25

56 Fe Iron

26

59 Co

Cob

alt

27

59 Ni

Nic

kel

28

64 Cu

Cop

per

29

65 Zn Zinc

30

70 Ga

Gal

lium

31

27 Al

Alu

min

ium

13

11 B Bor

on5

12 CC

arbo

n6

14 NN

itrog

en7

16 OO

xyge

n8

19 FFl

uorin

e9

28 Si Sili

con

14

31 PP

hosp

horu

s15

32 S Sul

fur

16

35.5 Cl

Chl

orin

e17

40 Ar

Arg

on18

20 Ne

Neo

n10

4 He

Hel

ium

2

73 Ge

Ger

man

ium

32

75 As

Ars

enic

33

79 SeS

elen

ium

34

80 Br

Bro

min

e35

84 Kr

Kry

pton

36

39 KP

otas

sium

19

88 SrS

tront

ium

38

89 YY

ttriu

m39

91 ZrZi

rcon

ium

40

93 Nb

Nio

bium

41

96 Mo

Mol

ybde

num

42

TcTe

chne

tium

43

101

Ru

Rut

heni

um44

103

Rh

Rho

dium

45

106

PdP

alla

dium

46

108

Ag

Silv

er47

112

Cd

Cad

miu

m48

115

In Indi

um49

119

Sn Tin

50

122

SbA

ntim

ony

51

128

TeTe

lluriu

m52

127 I

Iodi

ne53

131

Xe Xen

on54

137

Ba

Bar

ium

56

139

LaLa

ntha

num

57

*

178

Hf

Haf

nium

72

181

TaTa

ntal

um73

184 W

Tung

sten

74

186

Re

Rhe

nium

75

190

Os

Osm

ium

76

192

Ir Iridi

um77

195 Pt

Pla

tinum

78

197

Au

Gol

d79

201

Hg

Mer

cury

80

204 Tl

Thal

lium

81

207

Pb Lead

82

209 Bi

Bis

mut

h83

PoP

olon

ium

84

At

Ast

atin

e85

Rn

Rad

on86

FrFr

anci

um87

227

Ac

Act

iniu

m89

9 Be

Ber

ylliu

m4

III

IIIIV

VV

IV

II0

85 Rb

Rub

idiu

m37

133

Cs

Cae

sium

55

226

Ra

Rad

ium

88

The

volu

me

of o

ne m

ole

of a

ny g

as is

24

dm3

at ro

om te

mpe

ratu

re a

nd p

ress

ure

(r.t.p

.).

a Xb

a =

rela

tive

atom

ic m

ass

X =

atom

ic s

ymbo

l

b =

prot

on (a

tom

ic) n

umbe

r

Key

* 58-

71 L

anth

anoi

d se

ries

90-1

03 A

ctin

oid

serie

s

DAT

A SH

EET

The

Perio

dic

Tabl

e of

the

Elem

ents



*5760352473*



Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.Practical notes are provided on page 8.


CHEMISTRY 0620/51

Paper 5 Practical Test May/June 2014

1 hour 15 minutes


Additional Materials: As listed in the Confi dential Instructions



For Examiner’s Use

Total

2

0620/51/M/J/14© UCLES 2014

1 You are going to investigate what happens when dilute hydrochloric acid reacts with anaqueous solution R, containing two different substances S and T.

Read all the instructions below carefully before starting the experiments.

Instructions You are going to carry out three experiments.

(a) Experiment 1

Using a measuring cylinder, pour 25 cm3 of solution R into the conical fl ask. Add fi ve drops of the phenolphthalein indicator to the fl ask.

Fill the burette with hydrochloric acid to the 0.0 cm3 mark. Using the burette, add hydrochloric acid to solution R and shake the fl ask. Continue to add hydrochloric acid to the fl ask until the colour just disappears.

Record the volume of hydrochloric acid added when the indicator changes colour. Keep the mixture in the fl ask for Experiment 2.

burette readings

fi nal volume / cm3

initial volume / cm3

difference / cm3

[3]

(b) Experiment 2

Add four drops of methyl orange indicator to the mixture in the fl ask from Experiment 1. Check that the burette reading is the same as your fi nal reading in Experiment 1. This is the

initial volume reading for Experiment 2. Using the burette, add hydrochloric acid to the mixture in the fl ask and shake the mixture. Record the volume of hydrochloric acid added when the indicator just changes colour.

burette readings

fi nal volume / cm3


difference / cm3

[4]

(c) Experiment 3

Pour about 5 cm3 of solution R into a test-tube. Using a teat pipette, add hydrochloric acid to the solution. Note any observations.

.............................................................................................................................................. [1]

3


(d) (i) When phenolphthalein indicator was used in Experiment 1 the colour changed

from ............................................................ to ............................................................. [2]

(ii) What was the colour of the indicator at the end-point in Experiment 2?

....................................................................................................................................... [1]

(e) (i) What type of substances are S and T?

....................................................................................................................................... [1]

(ii) What conclusion can you draw from Experiment 3?

....................................................................................................................................... [1]

(f) The volume of hydrochloric acid added in Experiment 1 reacted with all of substance S and half of substance T.

The volume of hydrochloric acid in Experiment 2 reacted with half of substance T.

(i) Work out the volume of hydrochloric acid which reacted with substance S.

....................................................................................................................................... [2]

(ii) Work out the volume of hydrochloric acid which reacted with substance T.

....................................................................................................................................... [1]

(iii) Compare the volumes of hydrochloric acid which reacted with substances S and T.

.............................................................................................................................................

....................................................................................................................................... [1]

(g) (i) Predict the volume of hydrochloric acid which would be added in Experiments 1 and 2 if the experiments were repeated using 100 cm3 of solution R. Explain your answer.

Experiment 1 ......................................................................................................................

Experiment 2 ......................................................................................................................

Explanation ................................................................................................................... [3]

(ii) Suggest a practical problem that would occur when carrying out these repeat experiments and how you could solve this problem.

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 22]

4

0620/51/M/J/14© UCLES 2014

2 You are provided with solid U, which is a metal salt. Carry out the following tests on U, recording all of your observations in the table. Conclusions must not be written in the table.

tests observations

tests on solid U

(a) Describe the appearance of solid U. ................................................................ [2]

(b) Place half of solid U in a test-tube. Heat the test-tube gently at fi rst and then

more strongly.

......................................................................

................................................................ [2]

(c) Add the rest of solid U to about 8 cm3 of distilled water in a test-tube.

Stopper the test-tube and shake the contents until dissolved.

Divide the solution into four equal portions in separate test-tubes and carry out the following tests.

Add several drops of aqueous sodium hydroxide to the fi rst portion of the solution and shake the test-tube.

Then add about 1 cm3 of hydrogen peroxide solution to the mixture.

Test the gas given off.

......................................................................

......................................................................

................................................................ [5]

(d) Add excess aqueous ammonia to the second portion of the solution. ................................................................ [1]

(e) Add about 1 cm3 of dilute nitric acid to the third portion of the solution followed by about 1 cm3 of barium nitrate solution. ................................................................ [2]

(f) Add about 1 cm3 of dilute nitric acid to the fourth portion of the solution followed by about 1 cm3 of silver nitrate solution. ................................................................ [1]

5


(g) What does test (f) tell you about solid U?

.............................................................................................................................................. [1]

(h) Name the gas given off in test (c).

.............................................................................................................................................. [1]

(i) What conclusions can you draw about solid U?

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 18]

6

0620/51/M/J/14

BLANK PAGE

© UCLES 2014

7

0620/51/M/J/14

BLANK PAGE

© UCLES 2014

8



0620/51/M/J/14

NOTES FOR USE IN QUALITATIVE ANALYSIS

Test for anions

anion test test result

carbonate (CO32–) add dilute acid effervescence, carbon dioxide

produced

chloride (Cl –)[in solution]

acidify with dilute nitric acid, thenadd aqueous silver nitrate

white ppt.

iodide (I–)[in solution]


yellow ppt.

nitrate (NO3–)

[in solution]add aqueous sodium hydroxidethen aluminium foil; warm carefully

ammonia produced

sulfate (SO42–)

[in solution]acidify with dilute nitric acid, thenaqueous barium nitrate

white ppt.

Test for aqueous cations

cation effect of aqueous sodium hydroxide effect of aqueous ammonia

aluminium (Al 3+) white ppt., soluble in excess givinga colourless solution

white ppt., insoluble in excess

ammonium (NH4+) ammonia produced on warming –

calcium (Ca2+) white ppt., insoluble in excess no ppt., or very slight white ppt.

copper (Cu2+) light blue ppt., insoluble in excess light blue ppt., soluble in excessgiving a dark blue solution

iron(II) (Fe2+) green ppt., insoluble in excess green ppt., insoluble in excess

iron(III) (Fe3+) red-brown ppt., insoluble in excess red-brown ppt., insoluble in excess

zinc (Zn2+) white ppt., soluble in excess givinga colourless solution

white ppt., soluble in excess givinga colourless solution

Test for gases

gas test and test results

ammonia (NH3) turns damp red litmus paper blue

carbon dioxide (CO2) turns limewater milky

chlorine (Cl 2) bleaches damp litmus paper

hydrogen (H2) ‘pops’ with a lighted splint

oxygen (O2) relights a glowing splint

© UCLES 2014



*1093878163*





CHEMISTRY 0620/52


1 hour 15 minutes






Total

2

0620/52/M/J/14© UCLES 2014

1 You are going to investigate the temperature rise produced when different lengths of magnesium ribbon react with excess dilute sulfuric acid.


Instructions You are going to carry out fi ve experiments.

(a) Experiment 1

Using a measuring cylinder, pour 20 cm3 of dilute sulfuric acid into the beaker. Measure the initial temperature of the acid and record it in the table below. Add the 2 cm length of magnesium ribbon to the acid in the beaker, and stir the mixture with the thermometer.

Measure the highest temperature reached and record it in the table. Remove the thermometer and rinse out the beaker with water.

(b) Experiment 2

Repeat Experiment 1, using the 3 cm length of magnesium ribbon. Record the initial and highest temperatures in the table.

(c) Experiment 3

Repeat Experiment 1, using the 4 cm length of magnesium ribbon. Record the temperatures in the table.

(d) Experiment 4


(e) Experiment 5


Complete the table.

Experiment initial temperature/ °C

highest temperature/ °C

change in temperature/ °C

1

2

3

4

5

[5]

3


(f) Plot the results you have obtained on the grid below. Draw a straight line of best fi t through the points.

30

20

10

0

length of magnesium ribbon / cm

change intemperature / °C

[4]

(g) From your graph, deduce the expected change in temperature if Experiment 1 was repeated using a 5 cm length of magnesium ribbon.

Show clearly on the graph how you worked out your answer.

.............................................................................................................................................. [2]

(h) Give two observations when magnesium reacts with dilute sulfuric acid.

1 .................................................................................................................................................

2 ........................................................................................................................................... [2]

4

0620/52/M/J/14© UCLES 2014

(i) (i) Which experiment gave the greatest change in temperature?

....................................................................................................................................... [1]

(ii) Suggest why the change in temperature was greatest in this experiment.

.............................................................................................................................................

....................................................................................................................................... [1]

(j) What difference would be observed if Experiment 1 was repeated using an equal mass of magnesium powder? Explain your answer.

....................................................................................................................................................

.............................................................................................................................................. [2]

(k) Draw a diagram of apparatus you could use to collect and measure the volume of gas given off in the reaction.

[2]

(l) State one source of error in the results obtained in Experiments 1-5. Give one improvement to reduce this source of error.

error ...........................................................................................................................................

improvement ........................................................................................................................ [2]

[Total: 21]

5


2 You are provided with mixture E. E consists of two solids, F and G. Solid F is water-soluble and solid G is insoluble.

Carry out the following tests on E, recording all of your observations in the table. Conclusions must not be written in the table.

tests observations

tests on the mixture E

(a) Describe the appearance of the mixture. ................................................................ [1]

(b) Place a little of mixture E in a test-tube. Heat the mixture gently at fi rst then more

strongly for about 1 minute. After 1 minute, test the gas given off with damp pH indicator paper. Leave the test-tube to cool.

......................................................................

......................................................................

................................................................ [3]

Add the rest of mixture E to about 10 cm3 of distilled water in a boiling tube. Stopper the boiling tube and shake the contents for about a minute. Filter the contents of the boiling tube.

Keep the residue and the fi ltrate for the following tests.

tests on the fi ltrate

(c) (i) To about 1 cm3 of the fi ltrate, add about 1 cm3 of aqueous sodium hydroxide.

Gently heat the mixture. Test the gas given off with damp pH indicator paper.

(ii) Add about 1 cm3 of silver nitrate solution to the second portion of the fi ltrate followed by about 1 cm3 of dilute nitric acid.

......................................................................

................................................................ [1]

......................................................................

................................................................ [1]

6

0620/52/M/J/14© UCLES 2014

tests observations

tests on the residue

(d) Using a spatula, transfer a little of the residue from the fi lter paper to a test-tube. Using a teat pipette, add about 2 cm3 of dilute hydrochloric acid to the residue. Test the gas given off.

Add an equal volume of distilled water to the solution in the test-tube.

Shake the contents and divide into two portions.

......................................................................

......................................................................

................................................................ [2]

(e) (i) Add several drops of aqueous sodium hydroxide to the fi rst portion of the solution. Now add excess aqueous sodium hydroxide.

(ii) Add several drops of aqueous ammonia to the second portion. Now add excess aqueous ammonia.

......................................................................

................................................................ [3]

......................................................................

................................................................ [2]

(f) Explain your observations in test (b).

....................................................................................................................................................

.............................................................................................................................................. [2]

(g) What conclusions can you draw about solid F?

....................................................................................................................................................

.............................................................................................................................................. [2]

(h) What conclusions can you draw about solid G?

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 19]

7

0620/52/M/J/14

BLANK PAGE

© UCLES 2014

8



0620/52/M/J/14


Test for anions



produced



white ppt.



yellow ppt.

nitrate (NO3–)


ammonia produced

sulfate (SO42–)


white ppt.












Test for gases







© UCLES 2014



*7887217677*





CHEMISTRY 0620/53


1 hour 15 minutes






Total

2

0620/53/M/J/14© UCLES 2014

1 You are going to investigate what happens when two different solids, M and N, dissolve in water.


Instructions You are going to carry out three experiments.

(a) Experiment 1

Use a measuring cylinder to pour 25 cm3 of distilled water into the polystyrene cup. Support the cup by putting it into the 250 cm3 beaker. Measure the temperature of the water and record it in the table below.

Add all of solid M to the water, start the timer and stir the solution with the thermometer.

Measure the temperature of the solution every 30 seconds for three minutes. Record your results in the table. At the end of the experiment, pour about 4 cm3 of the solution into a test-tube for Experiment 3.

time / s 0 30 60 90 120 150 180

temperature of solution / °C

[2]

(b) Experiment 2

Empty the polystyrene cup and rinse it with water.

Use a measuring cylinder to pour 25 cm3 of distilled water into the polystyrene cup. Measure the temperature of the water and record it in the table below.

Add all of solid N to the water, start the timer and stir the solution with the thermometer.

Measure the temperature of the solution every 30 seconds for three minutes. Record your results in the table.

time / s 0 30 60 90 120 150 180

temperature of solution / °C

[2]

(c) Experiment 3

To about 4 cm3 of the solution from Experiment 1, add about 1 cm3 of dilute sulfuric acid. Record your observation.

.............................................................................................................................................. [1]

3


(d) Plot the results for Experiments 1 and 2 on the grid and draw two smooth line graphs. Clearly label your graphs.

60

50

40

30

20

10

0

time / s

temperatureof solution / °C

0 30 60 90 120 150 180

[6]

(e) (i) From your graph, deduce the temperature of the solution in Experiment 1 after45 seconds.


...................................... °C [2]

(ii) From your graph, deduce how long it takes for the initial temperature of the solution in Experiment 2 to change by 2 °C.


...................................... s [2]

4

0620/53/M/J/14© UCLES 2014

(f) From your results in Experiment 2, what type of chemical process occurs when substance N dissolves in water?

.............................................................................................................................................. [1]

(g) What conclusion can you draw from Experiment 3?

.............................................................................................................................................. [1]

(h) Suggest the effect on the results if Experiment 1 was repeated using 50 cm3 of distilled water.

....................................................................................................................................................

.............................................................................................................................................. [2]

(i) Predict the temperature of the solution in Experiment 2 after one hour. Explain your answer.

....................................................................................................................................................

.............................................................................................................................................. [2]

(j) When carrying out the experiments, what would be the advantage of taking the temperature readings every 10 seconds?

....................................................................................................................................................

.............................................................................................................................................. [1]

[Total: 22]

5


2 You are provided with two solids P and Q. Carry out the following tests on P and Q, recording all of your observations in the table. Conclusions must not be written in the table.

tests observations

tests on solid P

Use a spatula to divide solid P into two separate boiling tubes.

(a) Describe the appearance of solid P. ......................................................................

(b) (i) Add about 3 cm3 of dilute sulfuric acid to the fi rst boiling tube of P and warm the mixture for two minutes.

Allow the mixture to settle.

Decant the solution into two equal portions in separate test-tubes. Add an equal volume of distilled water to each test-tube. Carry out the following tests.

(ii) Add several drops of aqueous sodium hydroxide to the fi rst portion of the solution and shake the test-tube.

Now add excess sodium hydroxide to the test-tube.

(iii) Add aqueous potassium iodide to the second portion of the solution, shake and leave to stand for ten minutes.

................................................................ [1]

......................................................................

................................................................ [2]

......................................................................

................................................................ [2]

(c) To the second boiling tube of P add about 2 cm3 of dilute hydrochloric acid and warm the mixture for two minutes. Allow the mixture to settle.

Decant off 1 cm3 of the liquid into atest-tube. Add aqueous ammonia to the solution until no further change is seen.

................................................................ [1]

......................................................................

......................................................................

................................................................ [3]

6

0620/53/M/J/14© UCLES 2014

tests observations

tests on solid Q

(d) Describe the appearance of solid Q. ................................................................ [1]

(e) (i) Add about 3 cm3 of dilute sulfuric acid to solid Q in the boiling tube and warm the mixture for two minutes.

Allow the mixture to settle.

Decant the solution into two equal portions in separate test-tubes.

(ii) Add aqueous sodium hydroxide to the fi rst portion until there is no further change.

(iii) Add aqueous ammonia to the second portion until there is no further change.

......................................................................

................................................................ [2]

......................................................................

................................................................ [1]

......................................................................

................................................................ [2]

(f) Identify solid P.

.............................................................................................................................................. [2]

(g) Draw a conclusion about Q.

.............................................................................................................................................. [1]

[Total: 18]

7

0620/53/M/J/14

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© UCLES 2014

8



0620/53/M/J/14


Test for anions



produced



white ppt.



yellow ppt.

nitrate (NO3–)


ammonia produced

sulfate (SO42–)


white ppt.












Test for gases







© UCLES 2014





Answer all questions.Electronic calculators may be used.You may lose marks if you do not show your working or if you do not use appropriate units.


CHEMISTRY 0620/61

Paper 6 Alternative to Practical May/June 2014

1 hour





2

0620/61/M/J/14© UCLES 2014

1 A student separated a mixture of two alcohols, ethanol (boiling point 78 C) andbutanol (boiling point 118 C).

The apparatus used is shown below.

heat

mixture ofalcohols

(a) Complete the boxes to identify the pieces of apparatus labelled. [2]

(b) Label the arrows. [1]

(c) State the name of this separation process.

.............................................................................................................................................. [2]

(d) (i) Which liquid is fi rst to collect in the beaker?

....................................................................................................................................... [1]

(ii) How would the student know when all of this liquid had collected?

.............................................................................................................................................

....................................................................................................................................... [1]

3


(e) Identify and explain a possible hazard in this experiment.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 9]

2 The following paragraph was taken from a student’s notebook.

Preparation of lead chloride

10 cm3 of aqueous lead nitrate was placed in a beaker and 10 cm3 of aqueous potassium chloride added. Lead chloride, a white solid, was formed. The solid was separated from the mixture.Water was then added to the solid and the mixture boiled. A clear liquid was formed. On cooling, white crystals were deposited.

(a) What type of chemical reaction resulted in the formation of the lead chloride?

.............................................................................................................................................. [1]

(b) What is the solubility of lead chloride in

(i) cold water, ..........................................................................................................................

(ii) hot water? ..................................................................................................................... [2]

(c) What method should be used to separate the crystals from the mixture?

.............................................................................................................................................. [1]

[Total: 4]

4

0620/61/M/J/14© UCLES 2014

3 A student investigated the reaction of zinc powder with dilute hydrochloric acid using the apparatus below.

hydrochloric acid

zinc

gas syringe

The same mass of zinc was added to different volumes of hydrochloric acid at room temperature, 20 C. The total volume of hydrogen gas given off in each experiment was measured.

(a) Use the gas syringe diagrams to record the volumes of hydrogen gas in the table.

volume ofhydrochloric acid

/ cm3gas syringe diagram volume of hydrogen gas

/ cm3

0 0 10 20 30 50 6040

5 0 10 20 30 50 6040

10 0 10 20 30 50 6040

15 0 10 20 30 50 6040

20 0 10 20 30 50 6040

30 0 10 20 30 50 6040

40 0 10 20 30 50 6040

[3]

5


(b) On the grid, plot the points and draw a smooth line graph.

60

40

20

00 10 20

volume of hydrochloric acid / cm3

30 40

volume ofhydrogengas / cm3

[4]

(c) (i) Which point is inaccurate?

....................................................................................................................................... [1]

(ii) Suggest a possible reason for this inaccurate measurement.

....................................................................................................................................... [1]

(iii) Use your graph to work out the volume that would be expected to be formed. Show clearly on the grid how you got your answer.

....................................................................................................................................... [2]

(d) Explain why the volume of hydrogen gas does not increase after 30 cm3 of hydrochloric acid.

....................................................................................................................................................

.............................................................................................................................................. [2]

(e) Sketch on the grid the graph you would expect if the experiments were repeated using the same mass of zinc granules. [2]

[Total: 15]

6

0620/61/M/J/14© UCLES 2014

4 A student investigated the reaction between dilute hydrochloric acid and an aqueous alkaline solution R, containing two different substances, S and T.

Three experiments were carried out.

Experiment 1

Using a measuring cylinder, 25 cm3 of solution R was poured into a conical fl ask and fi ve drops of phenolphthalein were added to the fl ask.

A burette was fi lled with hydrochloric acid up to the 0.0 cm3 mark. Hydrochloric acid was added to the solution R and the fl ask shaken. Addition of hydrochloric acid was continued until the colour just disappeared.

The mixture in the fl ask was kept for Experiment 2.

(a) Use the burette diagram to record the fi nal volume in the table of results and complete the table.

16

17

18final burette reading

burette readings

fi nal volume / cm3


difference / cm3

[3]

Experiment 2

Five drops of methyl orange indicator were added to the mixture in the fl ask from Experiment 1. The mixture turned yellow. The initial volume reading of the burette was the same as the fi nal reading in Experiment 1. Hydrochloric acid was added from the burette to the mixture in the fl ask and the mixture shaken.

The volume of hydrochloric acid added was recorded when the indicator just changed colour.

(b) Use the burette diagram to record the fi nal volume in the table of results and complete the table.

24

25

26final burette reading

burette readings

fi nal volume / cm3


difference / cm3

[3]

7


(c) Experiment 3

Hydrochloric acid was added to about 5 cm3 of solution R in a test-tube.

Rapid effervescence was observed.

(d) When phenolphthalein indicator was used in Experiment 1 the colour changed

from pink to .......................................................................................................................... [1]

(e) In a similar experiment, methyl orange indicator was used in Experiment 1 followed by phenolphthalein in Experiment 2.

Suggest why this experiment would not work.

....................................................................................................................................................

.............................................................................................................................................. [1]

(f) What conclusion can you draw from Experiment 3?

.............................................................................................................................................. [1]

(g) The volume of hydrochloric acid added in Experiment 1 reacted with all of substance S and half of substance T.

The volume of hydrochloric acid in Experiment 2 reacted with half of substance T.

(i) Work out the volume of hydrochloric acid which reacted with substance S.

....................................................................................................................................... [2]

(ii) Work out the volume of hydrochloric acid which reacted with substance T.

....................................................................................................................................... [1]

(iii) Compare the volumes of hydrochloric acid which reacted with substances S and T.

....................................................................................................................................... [1]

(h) (i) The experiments were repeated using 100 cm3 of solution R. Predict the volume of hydrochloric acid which would be added in Experiments 1 and 2.

Explain your answer.

Experiment 1 ......................................................................................................................

Experiment 2 ......................................................................................................................

Explanation ................................................................................................................... [3]

(ii) Suggest a practical problem that would occur when carrying out these repeat experiments and how you could solve this problem.

.............................................................................................................................................

....................................................................................................................................... [2]

[Total: 18]

8

0620/61/M/J/14© UCLES 2014

5 A solid U was analysed. U was a soluble metal sulfate. The tests on U, and some of the observations are in the following table. Complete the observations.

tests observations

tests on solid U

(a) Appearance of solid U. pink crystals

(b) Solid U was heated gently and then strongly in a test-tube. condensation droplets formed on the sides of the test-tube

(c) Solid U was added to distilled water in a test-tube and shaken until dissolved.

The solution was divided into three equal portions in separate test-tubes and the following tests carried out.

Several drops of aqueous sodium hydroxide were added to the fi rst portion of the solution and thetest-tube shaken.

Then hydrogen peroxide solution was added to the mixture and the gas given off tested.

pale brown precipitate

effervescenceglowing splint relit

(d) Dilute nitric acid was added to the second portion of the solution followed by barium nitrate solution.

............................................................................................

...................................................................................... [2]

(e) Dilute nitric acid was added to the third portion of the solution followed by silver nitrate solution. ...................................................................................... [1]

9


(f) What does test (e) tell you about solid U?

.............................................................................................................................................. [1]

(g) Name the gas given off in test (c).

.............................................................................................................................................. [1]

(h) What conclusions can you draw about solid U?

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 7]

10

0620/61/M/J/14© UCLES 2014

6 Nuts contain oil. Nuts can be burned to produce energy. The apparatus shown can be used to compare the energy produced by burning different nuts.

thermometer

water

nut

Plan an investigation to show which of three different types of nut produce the most energy. You are provided with peanuts, brazil nuts and hazelnuts.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [7]

[Total: 7]

11

0620/61/M/J/14© UCLES 2014

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12

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*9115508770*





CHEMISTRY 0620/62


1 hour





2

0620/62/M/J/14© UCLES 2014

1 A student investigated the effect of using electricity to break down a solution of concentrated hydrochloric acid using the apparatus shown.

concentratedhydrochloric acid

carbon rods

During the experiment, bubbles were observed at both carbon rods.

(a) Complete the box to identify the piece of apparatus used. [1]

(b) (i) Name the process that occurs when electricity is passed through concentrated hydrochloric acid.

....................................................................................................................................... [1]

(ii) What is the purpose of the carbon rods?

....................................................................................................................................... [1]

(c) Name one of the gases formed and state a test for this gas.

name ..........................................................................................................................................

test .............................................................................................................................................

result .................................................................................................................................... [2]

(d) Draw a diagram of different apparatus that could be used to collect the gases formed at the carbon rods.

[2]

[Total: 7]

3


2 The graph shows the change in the pH when aqueous potassium hydroxide is added to 25.0 cm3 of dilute nitric acid to form a solution of potassium nitrate. A pH meter was used.

14

12

10

8

6

4

2

00 5 10 15

volume of potassium hydroxide / cm3

20 25

pHpoint X

(a) Name a suitable piece of apparatus to measure 25.0 cm3 of dilute nitric acid.

.............................................................................................................................................. [1]

(b) What could be used instead of a pH meter in this experiment?

.............................................................................................................................................. [1]

(c) Describe how the pH of the mixture changes as the potassium hydroxide is added.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [2]

4

0620/62/M/J/14© UCLES 2014

(d) (i) What has happened at point X?

....................................................................................................................................... [1]

(ii) What volume of aqueous potassium hydroxide had been added to the mixture at point X?

....................................................................................................................................... [2]

(iii) What conclusion can you draw about the concentrations of the dilute nitric acid and the aqueous potassium hydroxide? Explain your answer.

.............................................................................................................................................

.............................................................................................................................................

....................................................................................................................................... [3]

(e) Suggest the effect of heating the solution of potassium nitrate to boiling point and then heating for a further ten minutes.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 12]

5


3 Long-chain alkanes can be cracked to form short-chain alkenes. The apparatus below was used to produce ethene.

water

ethene

aluminiumoxide

liquid alkaneon mineral fibre

(a) Which piece of apparatus is missing from the diagram?

.............................................................................................................................................. [1]

(b) Suggest why the fi rst tube of gas that is collected should be discarded.

....................................................................................................................................................

.............................................................................................................................................. [2]

(c) What is the function of the aluminium oxide?

.............................................................................................................................................. [1]

(d) Describe a chemical test to distinguish an alkane from an alkene.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 6]

6

0620/62/M/J/14© UCLES 2014

4 A student investigated the temperature rises produced when different lengths of magnesium ribbon reacted with excess dilute sulfuric acid.

Five experiments were carried out.

(a) Experiment 1

Using a measuring cylinder, 20 cm3 of dilute sulfuric acid was added to a beaker. The initial temperature of the solution was measured. A 2 cm length of magnesium ribbon was added to the acid in the beaker and the mixture stirred with a thermometer. The highest temperature reached was measured.

Use the thermometer diagrams to record the initial and highest temperatures in the table on page 7.

40

35

30

30

25

20

initial temperature highest temperature

(b) Experiment 2

Experiment 1 was repeated, using a 3 cm length of magnesium ribbon. Use the thermometer diagrams to record the initial and highest temperatures in the table.

7


(c) Experiments 3, 4 and 5

Experiment 1 was repeated, using a 4 cm length, a 6 cm length and a 7 cm length of magnesium ribbon. Use the thermometer diagrams to record the temperatures in the table.

Complete the table of results.

1

40

35

30

2

30

25

20

50

45

40

3

35

30

25

50

45

40

4

30

25

20

55

50

45

5

35

30

25

Experimentinitial

temperature/ °C

thermometerdiagram

thermometerdiagram

highesttemperature

/ °C

change intemperature

/ °C

[5]

8

0620/62/M/J/14© UCLES 2014

(d) Plot the results on the grid below. Draw a best fi t straight line graph.

30

20

10

00 1 2 3

length of magnesium ribbon / cm

4 5 6 7 8

change intemperature

/ °C

[4]

(e) From your graph, deduce the temperature change expected if Experiment 1 was repeated using an 8 cm length of magnesium ribbon.

Show clearly on the grid how you worked out your answer.

.............................................................................................................................................. [3]

(f) Give one expected observation, other than temperature rise, when magnesium reacts with dilute sulfuric acid.

.............................................................................................................................................. [1]

9


(g) (i) Which experiment gave the greatest change in temperature?

....................................................................................................................................... [1]

(ii) Suggest why the change in temperature was greatest in this experiment.

.............................................................................................................................................

....................................................................................................................................... [1]

(h) What difference would be observed if Experiment 1 was repeated using an equal mass of magnesium powder? Explain your answer.

....................................................................................................................................................

.............................................................................................................................................. [2]

(i) Suggest the temperature change expected if Experiment 1 was repeated using 40 cm3 of dilute sulfuric acid.

.............................................................................................................................................. [1]

(j) Draw a diagram of apparatus you could use to collect and measure the volume of gas given off in the reaction.

[2]

(k) State one source of error in the results obtained in the experiments. Give one improvement to reduce this source of error.

error ...........................................................................................................................................

improvement ........................................................................................................................ [2]

[Total: 22]

10

0620/62/M/J/14© UCLES 2014

5 A mixture E was analysed. E consisted of two solids, F and G. Solid F was ammonium chloride which is water-soluble and solid G was insoluble.

The tests on E and some of the observations are in the following table. Complete the observations in the table.

tests observations

tests on mixture E

(a) Appearance of mixture E. white solid

(b) Mixture E was heated gently then strongly.

The gas was tested with damp pH indicator paper and the test-tube left to cool.

............................................................................................

...................................................................................... [1]

Mixture E was added to distilled water in a boiling tube and shaken. The contents of the boiling tube were fi ltered.

tests on the fi ltrate

(c) (i) Aqueous sodium hydroxide was added to the fi ltrate.

The mixture was heated. The gas given off was tested with damp pH indicator paper.

(ii) Silver nitrate solution was added to the fi ltrate followed by about 1 cm3 of dilute nitric acid.

............................................................................................

...................................................................................... [2]

...................................................................................... [2]

11


tests observations

tests on the residue

(d) The residue was transferred from the fi lter paper into a test-tube. Dilute hydrochloric acid was added to the residue.

The gas given off was tested.

rapid effervescence

limewater turned milky

The solution in the test-tube was divided into two portions.

(e) (i) Several drops of aqueous sodium hydroxide were added to the fi rst portion of the solution.

Excess aqueous sodium hydroxide was then added to the mixture.

(ii) Several drops of aqueous ammonia were added to the second portion of the solution.

Excess aqueous ammonia was then added to the mixture.

white precipitate

precipitate dissolved

white precipitate

precipitate dissolved

(f) What conclusions can you draw about solid G?

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 7]

12

0620/62/M/J/14© UCLES 2014



6 Cerussite is an ore of lead. Cerussite is lead carbonate, PbCO3.

In the reactivity series, lead is between iron and copper.

Plan an investigation to obtain a sample of lead from a large lump of cerussite.

You are provided with common laboratory apparatus and chemicals.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [6]

[Total: 6]







CHEMISTRY 0620/63


1 hour





2

0620/63/M/J/14© UCLES 2014

1 Steam was passed over heated magnesium ribbon using the apparatus below.

ceramic wool

magnesiumribbon

Y

(a) (i) Complete the box to show the substance absorbed by the ceramic wool. [1]

(ii) Indicate on the diagram, with two arrows, where the heat is applied. [1]

(b) (i) Describe the change in the appearance of the magnesium.

....................................................................................................................................... [2]

(ii) Predict the effect of adding water and a few drops of Universal Indicator to the solid product of the reaction.

.............................................................................................................................................

....................................................................................................................................... [2]

(c) Suggest the effect of a lighted splint at point Y. Explain your suggestion.

....................................................................................................................................................

.............................................................................................................................................. [2]

[Total: 8]

3


2 A student carried out three experiments to investigate the rate of reaction between dilutehydrochloric acid and zinc powder.

Experiment 1

50 cm3 of dilute hydrochloric acid were reacted with excess zinc powder. The volume of gas produced was measured every minute for ten minutes.

Experiment 2

Experiment 1 was then repeated using 100 cm3 of the dilute hydrochloric acid. The results for these two experiments are shown below.

60

50

40

30

20

10

00 1 2 3 4 5

time / mins

6 7 8 9 10

volume ofgas / cm3

(a) Label the two lines to identify each experiment. [1]

4

0620/63/M/J/14© UCLES 2014

Experiment 3

Experiment 1 was repeated using 50 cm3 of dilute hydrochloric acid which was half as concentrated as in Experiment 1.

(b) (i) How could the student prepare a solution of dilute hydrochloric acid which was half as concentrated as the acid in Experiment 1?

.............................................................................................................................................

....................................................................................................................................... [2]

(ii) Sketch, on the grid on page 3, the result that would be expected in Experiment 3. [2]

(c) Complete the diagram to show how the gas could be collected and measured.

[2]

(d) Explain how the rate of reaction could be increased in Experiment 3 without changing the concentration of the dilute hydrochloric acid.

....................................................................................................................................................

....................................................................................................................................................

.............................................................................................................................................. [3]

[Total: 10]

5


3 A student carried out an investigation to coat a copper key with nickel. He followed these instructions.

1 Rub the copper key with sandpaper.

2 Set up the circuit as shown.

copper keynickelelectrode

electrolyte

3 Switch on the circuit for ten minutes.

4 Remove the key, wash it and dry.

(a) Name the process used to coat the copper key with nickel.

.............................................................................................................................................. [1]

(b) Why was the key rubbed with sandpaper?

....................................................................................................................................................

.............................................................................................................................................. [2]

(c) Name a possible electrolyte that could be used.

.............................................................................................................................................. [2]

(d) Give one expected observation during the ten minutes that the circuit was switched on.

.............................................................................................................................................. [1]

(e) Describe how the key would be washed and dried.

....................................................................................................................................................

.............................................................................................................................................. [1]

[Total: 7]

6

0620/63/M/J/14© UCLES 2014

4 A student investigated what happened when two different solids, M and N, dissolved in water.

Three experiments were carried out.

(a) Experiment 1

Using a measuring cylinder, 25 cm3 of distilled water were poured into a polystyrene cup. The temperature of the water was measured. Solid M was added to the water, the timer started and the mixture stirred with a thermometer. The temperature of the solution was measured every 30 seconds for three minutes.

Use the thermometer diagrams to record the results in the table.

A little of the solution was poured into a test-tube for Experiment 3.

30

25

20

time / s

temperature/ °C

thermometerdiagram

0

40

35

30

30

40

35

30

60

40

35

30

90

40

35

30

120

40

35

30

150

40

35

30

180

[2]

(b) Experiment 2

Experiment 1 was repeated using solid N. The temperature of the solution was measured every 30 seconds for three minutes. Use the thermometer diagrams to record the results in the table.

30

25

20

time / s

temperature/ °C

thermometerdiagram

0

20

15

10

30

20

15

10

60

20

15

10

90

20

15

10

120

20

15

10

150

20

15

10

180

[2]

(c) Experiment 3

Dilute sulfuric acid was added to the solution from Experiment 1.

Rapid effervescence was observed.

7


(d) Plot the results for Experiments 1 and 2 on the grid and draw two smooth line graphs. Clearly label your graphs.

40

30

20

10

00 30 60 90

time / s

120 150 180

temperature/ °C

[6]

(e) (i) From your graph, deduce the temperature of the solution in Experiment 1 after45 seconds.


..................................... C [2]

(ii) From your graph, deduce how long it takes for the initial temperature of the solution in Experiment 2 to change by 2 C.


..................................... s [2]

8

0620/63/M/J/14© UCLES 2014

(f) From the results in Experiment 2, what type of chemical process occurs when substance N dissolves in water?

....................................................................................................................................... [1]

(g) What conclusion can you draw from Experiment 3?

....................................................................................................................................... [1]

(h) Suggest the effect on the results if Experiment 1 was repeated using 50 cm3 of water.

....................................................................................................................................................

.............................................................................................................................................. [2]

(i) Predict the temperature of the solution in Experiment 2 after 1 hour. Explain your answer.

....................................................................................................................................................

.............................................................................................................................................. [2]

(j) When carrying out the experiments, what would be the advantage of taking the temperature readings every 10 seconds?

....................................................................................................................................................

.............................................................................................................................................. [1]

[Total: 21]

9


5 Two solids, P and Q, were analysed. P was a metal compound and Q was calcium iodide. Tests were carried out on P and Q and some of the observations are in the following table. Complete the observations for solid Q.

tests observations

tests on solid P

(a) Appearance of solid P. black solid

(b) (i) Dilute sulfuric acid was added to solid P and the mixture warmed.

The solution was divided into two equal portions in test-tubes.

The following tests were carried out.

(ii) Drops of aqueous sodium hydroxide were added to the fi rst portion of the solution.

Excess sodium hydroxide was then added to the mixture in the test-tube.

(iii) Aqueous ammonia was added to the second portion of the solution until no further change was seen.

the solid reacted and a blue solution was formed

blue precipitate formed

blue precipitate insoluble

blue precipitate formed which dissolvedto form a deep blue solution

10

0620/63/M/J/14© UCLES 2014

tests observations

tests on solid Q

(c) Distilled water was added to solid Q and the mixture shaken to dissolve solid Q.

The solution was divided into three equal portions in separate test-tubes.

(i) Aqueous sodium hydroxide was added to the fi rst portion until no further change was seen.

(ii) Aqueous ammonia was added to the second portion until no further change was seen.

(iii) Dilute nitric acid and aqueous silver nitrate were added to the third portion.

..........................................................................................

..................................................................................... [3]

..........................................................................................

..................................................................................... [1]

..................................................................................... [1]

(d) Identify solid P.

.............................................................................................................................................. [2]

[Total: 7]

11


6 Vinegar contains ethanoic acid. Different brands of vinegar contain different concentrations of ethanoic acid. The concentration of ethanoic acid in the vinegar can be determined by reaction with aqueous sodium hydroxide.

Plan an experiment to show which of two different brands of colourless vinegar, C and D, contain the highest concentration of ethanoic acid.

You are provided with common laboratory apparatus. You may use the space below to draw a diagram.

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

...........................................................................................................................................................

..................................................................................................................................................... [7]

[Total: 7]

12

0620/63/M/J/14© UCLES 2014



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