Please use the table below to keep track of your revision.
Revision complete?
Questions completed?
Marks in first try
% in first try
Marks in second try
% in second try
C2.1
C2.2
C2.3
C2.4
C2.5
C2.6
Use the grade boundaries below as a guide to the grade you are achieving:
% Grade 90 A*
80 A
70 B 60 C
50 D <50 U
3
C2.1 Specification statements
C2 Specification
Cu
rren
t R
AG
Revised
1 2 3
Top
ic 1
: A
tom
ic S
tru
ctu
re &
th
e P
eri
od
ic T
able
1.1 Explain how Mendeleev: a arranged the elements, known at that time, in a periodic table by using properties of these elements and their compounds b used his table to predict the existence and properties of some elements not then discovered
1.2 Classify elements as metals or non-metals according to their position in the periodic table
1.3 Describe the structure of an atom as a nucleus containing protons and neutrons, surrounded by electrons in shells (energy levels)
1.4 Demonstrate an understanding that the nucleus of an atom is very small compared to the overall size of the atom
1.5 Describe atoms of a given element as having the same number of protons in the nucleus and that this number is unique to that element
1.6 Recall the relative charge and relative mass of: a a proton b a neutron c an electron
1.7 Demonstrate an understanding that atoms contain equal numbers of protons and electrons
1.8 Explain the meaning of the terms a atomic number b mass number c relative atomic mass
1.9 Describe the arrangement of elements in the periodic table such that: a elements are arranged in order of increasing atomic number, in rows called periods b elements with similar properties are placed in the same vertical column, called groups
1.12 Apply rules about the filling of electron shells (energy levels) to predict the electronic configurations of the first 20 elements in the periodic table as diagrams and in the form 2.8.1
1.13 Describe the connection between the number of outer electrons and the position of an element in the periodic table
4
C2.1 Exam Questions- 34 marks, 34 minutes.
Questions Q1.
(a) Complete the sentence by putting a cross ( ) in the box next to your answer. The particles in atoms are electrons, neutrons and protons. The mass of an electron is
(1)
A greater than the mass of a neutron
B the same as the mass of a proton
C smaller than the mass of a proton
D the same as the mass of a neutron (b) The atomic number of oxygen is 8.
The mass number of an atom of oxygen is 17. Describe the number and type of particles in the nucleus of this atom.
(a) The diagram shows an atom of lithium. (i) A proton has been labelled.
Complete the diagram by labelling the other two particles shown. (2)
(ii) Complete the sentence by putting a cross ( ) in the box next to your answer. The atomic number of lithium is
(1)
A 3
B 6
C 7
D 10 (b) (i) Which row of the table shows the charge on a proton and the charge on an electron?
Put a cross ( ) in the box next to your answer. (1)
%%% proton electron
A positive positive
B negative negative
C negative positive
D positive negative
(ii) Use a number from the box to complete the sentence. (1)
The relative mass of a proton is . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
(c) The electronic configuration of lithium is 2.1. The electronic configuration of sodium is 2.8.1. (i) Explain, in terms of their electronic configurations, why lithium and sodium are both in group 1 of the periodic table.
(a) Some of the elements in this list are also in group 1 of the modern periodic table. Which element is in the list above and also in group 1 of the modern periodic table?
Put a cross ( ) in the box next to your answer. (1)
A gold
B silver
C copper
D sodium (b) The element francium is now included in group 1 of the modern periodic table but did not appear anywhere in Mendeleev’s periodic table. Suggest why francium was not in Mendeleev’s periodic table.
*(e) An atom of beryllium has an atomic number of 4 and a mass number of 9. Describe the numbers and arrangements of the protons, neutrons and electrons in this atom.
2.1 Demonstrate an understanding that atoms of different elements can combine to form compounds by the formation of new chemical bonds
2.2 Describe how ionic bonds are formed by the transfer of electrons to produce cations and anions
2.3 Describe an ion as an atom or group of atoms with a positive or negative charge
2.4 Describe the formation of sodium ions, Na+, and chloride ions, Cl-, and hence the formation of ions in other ionic compounds from their atoms, limited to compounds of elements in groups 1, 2, 6 and 7
2.5 Demonstrate an understanding of the use of the endings –ide and –ate in the names of compounds
2.6 Deduce the formulae of ionic compounds (including oxides, hydroxides, halides, nitrates, carbonates and sulfates) given the formulae of the constituent ions
2.8 Describe the properties of ionic substances including sodium chloride and magnesium oxide, limited to: a melting points and boiling points b whether they conduct electricity as solids, when molten and in aqueous solution
2.9 Recall the general rules which describe the solubility of common types of substances in water: a all common sodium, potassium and ammonium salts are soluble b all nitrates are soluble c common chlorides are soluble except those of silver and lead d common sulfates are soluble except those of lead, barium and calcium e common carbonates and hydroxides are insoluble except those of sodium, potassium and ammonium
2.10 Demonstrate an understanding that insoluble salts can be formed as precipitates by the reaction of suitable reagents in solution
2.11 Demonstrate an understanding of the method needed to prepare a pure, dry sample of an insoluble salt
2.12 Prepare an insoluble salt by precipitation
2.13 Use solubility rules to predict whether a precipitate is formed when named solutions are mixed together and to name the precipitate
2.14 Recall that the insoluble salt, barium sulfate, is given as a ‘barium meal’ to X-ray patients because a it is opaque to X-rays b it is safe to use as, although barium salts are toxic, its insolubility prevents it entering the blood
C2 Specification
Cu
rren
t R
AG
Rev
ised
1
Rev
ised
2
Rev
ised
3
9
2.15 Describe tests to show the following ions are present in solids or solutions: a Na+, K+, Ca2+, Cu2+ using flame tests b CO3 2- using dilute acid and identifying the carbon dioxide evolved c SO4 2- using dilute hydrochloric acid and barium chloride solution d Cl- using dilute nitric acid and silver nitrate solution
2.16 Recall that chemists use spectroscopy (a type of flame test) to detect the presence of very small amounts of elements and that this led to the discovery of new elements, including rubidium and caesium
(b) This is an X-ray photograph of part of a patient's body. Before the photograph was taken a suspension of barium sulfate was introduced into his body to show the required part.
Many barium salts are toxic. Barium sulfate is insoluble in water. Explain why it is safe for the patient to have barium sulfate in his body.
*(c) Barium sulfate is prepared by reacting barium chloride with sodium sulfate. The barium sulfate is formed as a precipitate. Describe an experiment to prepare a pure, dry sample of barium sulfate, starting with barium chloride crystals and sodium sulfate crystals.
(c) Complete the sentence by putting a cross ( ) in the box next to your answer. Ionic compounds
(1)
A conduct electricity when solid
B do not conduct electricity when molten
C have low boiling points
D have high melting points
12
Q3.
Magnesium flares provide a bright light in an emergency. When the magnesium burns it reacts with oxygen to form magnesium oxide. (a) Explain why magnesium oxide is a compound.
(b) When magnesium reacts with oxygen, one magnesium atom and one oxygen atom form one magnesium ion and one oxide ion. These diagrams show the arrangement of electrons in a magnesium atom and in a magnesium ion.
(i) In the diagram below the arrangement of electrons in an oxygen atom is given. Draw the arrangement of electrons in the oxide ion.
(1)
(ii) Explain, in terms of their electrons, how a magnesium atom, Mg, and an oxygen atom, O, react together to form a magnesium ion, Mg2+, and an oxide ion, O2–.
(iii) Magnesium oxide is an ionic compound. Which of these is a property of solid magnesium oxide?
Put a cross ( ) in the box next to your answer. (1)
A it has a high melting point
B it has a low boiling point
C it conducts electricity
D it is malleable
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*(c) You are given two solid sodium salts, which are unlabelled. One of the solids is sodium chloride. The other solid is sodium carbonate. Describe how you could carry out a flame test to show that they are both sodium salts and describe another test to identify one of the salts completely.
(a) Calcium chloride solution reacts with silver nitrate solution. Solid silver chloride and calcium nitrate solution are formed.
(i) Complete the sentence by putting a cross ( ) in the box next to your answer. The formula of a salt is Ca(NO3)2. The name of this salt is
(1)
A calcium nitride
B calcium nitrate
C calcium chloride
D silver nitrate Q5. Solid compounds
(a) The table shows the melting points, solubility in water and relative electrical conductivity of a solution in water for five substances. The properties of each substance can be used to decide the type of structure of the substance, shown in the last column. The structure of solid X is not shown.
substance melting point / °C
solubility in water
relative electrical conductivity, when dissolved in water
type of structure
sodium nitrate 307 soluble good ionic
silicon(IV) oxide 1610 insoluble does not dissolve in water
(b) Complete the sentence by putting a cross ( ) in the box next to your answer. A flame test was carried out on another solid. A flame test can be used to show the presence of
(1)
A carbon dioxide
B methane
C nitrate ions
D sodium ions (c) Calcium chloride contains calcium ions and chloride ions. Describe how a calcium atom, Ca, forms a calcium ion, Ca2+.
(d) Lead chloride is an insoluble salt. It can be produced as a precipitate by mixing sodium chloride solution with a solution of a lead salt. Complete the word equation for the reaction that takes place when sodium chloride solution is mixed with a solution of your chosen lead salt.
(2) sodium chloride +........................................ → lead chloride +........................................
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C2.3 Specification statements C2 Specification
Cu
rren
t
RA
G
Re
vise
d
1
R
evi
sed
2
Re
vise
d
3
Top
ic 3
: Co
vale
nt
Co
mp
ou
nd
s an
d S
epar
atio
n T
ech
niq
ues
3.1 Describe a covalent bond as a pair of electrons shared between two atoms
3.2 Recall that covalent bonding results in the formation of molecules
3.3 Explain the formation of simple molecular, covalent substances using dot and cross diagrams, including: a hydrogen b hydrogen chloride c water d methane
3.4 Classify different types of elements and compounds by investigating their melting points and boiling points, solubility in water and electrical conductivity (as solids and in solution) including sodium chloride, magnesium sulfate, hexane, liquid paraffin, silicon(IV) oxide, copper sulfate, and sucrose (sugar)
3.5 Describe the properties of typical simple molecular, covalent compounds, limited to: a low melting points and boiling points, in terms of weak forces between molecules b poor conduction of electricity
3.6 Demonstrate an understanding of the differences between the properties of simple molecular, covalent substances and those of giant molecular, covalent substances, including diamond and graphite
3.8 Describe the separation of two immiscible liquids using a separating funnel
3.9 Describe the separation of mixtures of miscible liquids by fractional distillation, by referring to the fractional distillation of liquid air to produce nitrogen and oxygen
3.10 Describe how paper chromatography can be used to separate and identify components of mixtures, including colouring agents in foodstuffs
3.11 Evaluate the information provided by paper chromatograms, including the calculation of Rf values, in a variety of contexts, such as the food industry and forensic science
16
C2.3 Exam Questions- 28 marks, 28 minutes.
Questions Q1.
Hydrogen chloride is a gas at room temperature. The diagram shows the outer shell electrons in a molecule of hydrogen chloride.
(i) Give the name of the type of bond between the hydrogen and chlorine atoms in the molecule.
(1)
.............................................................................................................................................. (ii) Give the formula of a molecule of hydrogen chloride.
(iii) Complete the sentence by putting a cross ( ) in the box next to your answer. A property of hydrogen chloride is that it
(1)
A conducts electricity
B has a high melting point
C has a low boiling point
D exists as a giant structure Q2.
Phosphorus oxide is a compound that contains covalent bonds. (i) Describe what is meant by a covalent bond.
(2)
.............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (ii) The formula of a molecule of phosphorus oxide is P4O10
The separating funnel can be used to separate two immiscible liquids, such as oil and water. Describe how you would use a separating funnel to separate two immiscible liquids.
(a) Some food colourings are a mixture of coloured substances. Paper chromatography can be used to separate the coloured substances in food colourings. Charles carried out a chromatography experiment to test which food colouring was present in a coloured drink. He used samples of three food colourings, X, Y and Z. He also tested a sample of the colouring in the drink. Charles obtained this chromatogram.
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(i) Charles looked at the chromatogram to find out which food colourings contained more than one coloured substance. State all the food colourings that contain more than one coloured substance.
(1)
.............................................................................................................................................. (ii) Food colouring Y is banned. Explain how Charles can tell that the drink that he tested did not contain the banned food colouring.
(2)
.............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (iii) Calculate the Rf value for the coloured substance in food colouring X.
Rf = . . . . . . . . . . . . . . . . . . . . . *(b) Describe in detail how the experiment should be carried out to produce the chromatogram shown in (a).
(c) The drink contained water. Complete the dot and cross diagram for water by adding the electrons of the hydrogen atoms.
(1)
(Total for Question is 12 marks)
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Q5. Structures
The diagram shows part of the structure of diamond.
(a) How many bonds does a typical carbon atom in diamond form?
(1)
.............................................................................................................................................. (b) Complete the sentences by putting a cross ( ) in the box next to your answer.
(i) The bonds between carbon atoms in diamond contain (1)
A protons
B neutrons
C electrons
D ions (ii) The structure of diamond is
(1)
A simple molecular, covalent
B giant molecular, covalent
C ionic
D metallic (c) Hexane and water are immiscible. The diagram shows a piece of apparatus being used to separate a mixture of hexane and water.
4.1 Classify elements as alkali metals (group 1), halogens (group 7), noble gases (group 0) and transition metals based on their position in the periodic table
4.2 Describe the structure of metals as a regular arrangement of positive ions surrounded by a sea of delocalised electrons
4.3 Describe and explain the properties of metals, limited to malleability and the ability to conduct electricity
4.4 Recall that most metals are transition metals and that their typical properties include: a high melting point b the formation of coloured compounds
4.5 Demonstrate an understanding that elements and compounds can be classified as a ionic, b simple molecular covalent, c giant molecular covalent, d metallic and that each type of substance has different physical properties, including relative melting point and boiling point, relative solubility in water and ability to conduct electricity (as solids and in solution)
4.6 Describe alkali metals as a soft metals b metals with comparatively low melting points
4.7 Describe the reactions of lithium, sodium and potassium with water to form hydroxides which are alkaline, and hydrogen gas
4.8 Describe the pattern in reactivity of the alkali metals lithium, sodium and potassium with water and use this pattern to predict the reactivity of other alkali metals and explain the pattern
4.9 Recall the colours and physical states of the halogens at room temperature
4.10 Describe the reaction of halogens with metals to form metal halides
4.11 Recall that halogens react with hydrogen to produce hydrogen halides which dissolve in water to form acidic solutions
4.12 Investigate displacement reactions of halogens reacting with halide ions in solution
4.13 Describe the relative reactivity of the halogens as shown by their displacement reactions with halide ions in aqueous solution
4.14 Describe the noble gases as chemically inert, compared with the other elements and demonstrate an understanding that this lack of reactivity can be explained by the electronic arrangements in their atoms
4.15 Demonstrate an understanding that the discovery of the noble gases was due to chemists: a noticing that the density of nitrogen made in a reaction differed from that of nitrogen obtained from air b developing a hypothesis about the composition of the air c performing experiments to test this hypothesis and show the presence of the noble gases
4.16 Relate the uses of the noble gases to their properties, including: a inertness (including providing an inert atmosphere for welding and in filament lamps) b low density (including filling balloons) c non-flammability
4.17 Use the pattern in a physical property of the noble gases, such as boiling point or density, to estimate an unknown value foranother member of the group
22
C2.4 Exam Questions- 28 marks, 28 minutes.
Questions Q1.
Potassium reacts with water. In a class demonstration, a teacher drops a piece of potassium on to water.
(i) The teacher ties back her hair and wears a laboratory coat and goggles. Suggest another safety precaution that the teacher should take.
(1)
.............................................................................................................................................. .............................................................................................................................................. (ii) The word equation for this reaction is given below. Two of the state symbols have been given. Write the other two state symbols in the spaces provided.
(iii) Describe what you see when potassium is added to water. (2)
.............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. .............................................................................................................................................. (iv) Balance the equation for the reaction between potassium and water by putting numbers in the spaces provided.
(a) Complete the sentence by putting a cross ( ) in the box next to your answer. The periodic table is a table of
(1)
A mixtures
B elements
C compounds
D solutions
(b) Complete the sentence by putting a cross ( ) in the box next to your answer. Group 1 in the periodic table contains
(1)
A transition metals
B noble gases
C halogens
D alkali metals (c) The table shows some of the gases in group 0 and some of their properties. The gases are shown in the order in which they appear in group 0.
(i) Fill in the three spaces in the table.
(ii) Some light bulbs contain a metal filament.
These light bulbs are filled with argon. Explain why argon, instead of air, is used inside these light bulbs.
(d) The table shows some solids and some properties of solids. Draw one straight line from each solid to properties of that solid.
Q3. Group 7
(a) The elements fluorine, chlorine, bromine and iodine are all in group 7 of the periodic table. (i) State the name given to the elements in group 7.
(1)
.............................................................................................................................................. (ii) Give the symbol for an atom of bromine.
(1)
.............................................................................................................................................. (b) The table shows the states and colours of three of these elements at room temperature. The information for chlorine is missing.
element state at room temperature colour at room temperature
fluorine gas pale yellow
chlorine
bromine liquid dark red
iodine solid grey
Use the information in the table to describe the appearance of chlorine at room temperature. (2)
*(c) When chlorine is added to a solution of potassium bromide, a colour change is seen. When chlorine is added to a solution of potassium fluoride, no colour change is seen. Explain how these observations provide evidence for the order of reactivity of bromine, chlorine and fluorine.
5.1 Measure temperature changes accompanying some of the following types of change: a salts dissolving in water b neutralisation reactions c displacement reactions d precipitation reactions
5.2 Define an exothermic change or reaction as one in which heat energy is given out, including combustion reactions or explosions
5.3 Define an endothermic change or reaction as one in which heat energy is taken in, including photosynthesis or dissolving ammonium nitrate in water
5.4 Describe the breaking of bonds as endothermic and the making of bonds as exothermic
5.5 Demonstrate an understanding that the overall heat energy change for a reaction is a exothermic if more heat energy is released making bonds in the products than is required to break bonds in the reactants b endothermic if less heat energy is released making bonds in the products than is required to break bonds in the reactants
5.7 Investigate the effect of temperature, concentration and surface area of a solid on the rate of a reaction such as hydrochloric acid and marble chips
5.8 Recall that the rates of chemical reactions vary from very fast, explosive reactions to very slow reactions
5.9 Describe the effect of changes in temperature and concentration on the rate of reaction
5.10 Describe how reactions can occur when particles collide
5.12 Recall the effect of a catalyst on the rate of reaction
5.13 Demonstrate an understanding that catalytic converters in cars: a have a high surface area, to increase the rate of reaction of carbon monoxide and unburnt fuel from exhaust gases with oxygen from the air to produce carbon dioxide and water b work best at high temperatures
28
C2.5 Exam Questions- 34 marks, 34 minutes.
Questions Q1.
Some people use a hand warmer to warm their hands in winter.
(a) A chemical reaction takes place in the hand warmer. This reaction gives out heat energy. Give the name for reactions that give out heat energy.
(1)
.............................................................................................................................................. (b) In the hand warmer, iron reacts with oxygen. Complete the word equation for this reaction.
(c) Some hand warmers contain sodium chloride mixed with the reactants. If sodium chloride is present, it is not used up but the chemical reaction is faster.
Complete the sentence by putting a cross ( ) in the box next to your answer. In this reaction the sodium chloride is acting as
(1)
A a precipitate
B a catalyst
C an element
D an alkali metal (d) When ammonium nitrate crystals are dissolved in water, heat energy is taken in. A student puts some water in a beaker. He puts a thermometer in the water. He adds some ammonium nitrate crystals and stirs the mixture. Describe what the student would see.
(e) In an experiment, the time taken for some potassium chloride crystals to dissolve in water has been measured. A student is given the same mass of potassium chloride to dissolve in the same volume of water. State one change that could be made to the potassium chloride crystals and one change that could be made to the water to make the dissolving faster.
(2) change made to the potassium chloride crystals
Zinc is a metal. Zinc reacts with dilute hydrochloric acid to produce zinc chloride and hydrogen. (a) Write the word equation for the reaction of zinc with dilute hydrochloric acid.
(1)
.............................................................................................................................................. (b) A student wanted to investigate the speed of the reaction between zinc and dilute hydrochloric acid. Describe how the student could use this apparatus to obtain the results in the table.
(c) Complete each sentence by putting a cross ( ) in the box next to your answer. (i) For a reaction to take place the reacting particles must
(1)
A dissolve
B boil
C collide
D evaporate (ii) The reaction can be slowed down by
(1)
A using a bigger volume of the same acid
B cooling the hydrochloric acid
C increasing the concentration of the hydrochloric acid
D adding a catalyst (d) When zinc powder is used, instead of larger pieces of zinc, the reaction is faster. Explain, using ideas about particles, why the reaction is faster when zinc powder is used.
(a) A technician made some dilute sodium hydroxide solution by carefully adding some solid sodium hydroxide to pure water. This is the hazard symbol on a bottle of solid sodium hydroxide.
(i) State what this symbol shows about sodium hydroxide.
(c) Dilute hydrochloric acid reacts with calcium carbonate to produce carbon dioxide gas. Three different experiments were carried out using large pieces of calcium carbonate, small pieces of calcium carbonate and powdered calcium carbonate. The size of the calcium carbonate pieces was the only factor that was changed. In each experiment the volume of carbon dioxide released in five minutes was measured. The results are
Describe what this shows about the effect of the surface area of calcium carbonate on the rate of this reaction.
*(d) Hydrochloric acid reacts with magnesium metal to produce hydrogen gas. magnesium + hydrochloric acid → magnesium chloride + hydrogen
Describe how you could use magnesium ribbon and a solution of hydrochloric acid to show that decreasing the concentration of the hydrochloric acid changes the rate of this reaction.
6.1 Calculate relative formula mass given relative atomic masses
6.2 Calculate the formulae of simple compounds from reacting masses and understand that these are empirical formulae
6.3 Determine the empirical formula of a simple compound, such as magnesium oxide
6.4 Calculate the percentage composition by mass of a compound from its formula and the relative atomic masses of its constituent elements
6.6 Recall that the yield of a reaction is the mass of product obtained in the reaction
6.7 Demonstrate an understanding that the actual yield of a reaction is usually less than the yield calculated using the chemical equation (theoretical yield)
6.8 Calculate the percentage yield of a reaction from the actual yield and the theoretical yield
6.9 Demonstrate an understanding of the reasons why reactions do not give the theoretical yield due to factors, including: a incomplete reactions b practical losses during the preparation c competing, unwanted reactions
6.10 Demonstrate an understanding that many reactions produce waste products which: a are not commercially useful b can present economic, environmental and social problems for disposal
34
C2.6 Exam Questions- 16 marks, 16 minutes.
Questions Q1. In an experiment iron reacts with chlorine to produce 13.00 g of iron chloride. The theoretical yield of this reaction is calculated to be 16.25g. Calculate the percentage yield of the reaction.
Rosie used this apparatus to prepare a sample of copper oxide.
Oxygen from the air reacted with the hot copper to form copper oxide. These are Rosie's results mass of copper used = 3.2 g mass of copper oxide formed = 3.6 g Calculate the percentage of oxygen in copper oxide, CuO.
Rosie used this apparatus to prepare a sample of copper oxide.
Oxygen from the air reacted with the hot copper to form copper oxide. These are Rosie's results mass of copper used = 3.2 g mass of copper oxide formed = 3.6 g The theoretical yield for Rosie's experiment was 4.0 g of copper oxide.
She only obtained 3.6 g of copper oxide. Calculate the percentage yield of Rosie's experiment.
Calcium chloride solution reacts with silver nitrate solution. Solid silver chloride and calcium nitrate solution are formed.
(i) Complete the sentence by putting a cross ( ) in the box next to your answer. The formula of a salt is Ca(NO3)2. The name of this salt is
(1)
A calcium nitride
B calcium nitrate
C calcium chloride
D silver nitrate (ii) The mixture produced in the reaction is filtered to obtain the silver chloride. The solid silver chloride is washed with water and left to dry. The yield of dry silver chloride was 3.0 g. The theoretical yield of dry silver chloride in this experiment was 4.0 g. 1. Suggest why the yield was less than 4.0 g.
