Unit 1: Periodic Table Part 1: Basic Structure of the Periodic Table Underline the correct spelling. Can you put the chemica l symbol in this column? Is the element a metal or non-metal? Hydrogen Hidrogen Hydrogon Lithium Litheum Lithiun Sodum Sodiume Sodium Potassium Pottasium Potasium Silver Sliver Silvur Guld Geld Gold Kalcium Calcum Calcium Oxegen Oxigen Oxygen Sulphor Sulpher Sulphur Magenesium Magnesium Magneciu m Carban Carben Carbon Helium Heelium Hellium Aluminium Alumium Aluminum Copper Coper Coppur Nickle Nickil Nickel Starter Task
Transcript
Unit 1: Periodic Table Part 1: Basic Structure of the Periodic Table
Underline the correct spelling.
Can you put the chemical symbol in this column?
Is the element a metal or non-metal?
Hydrogen Hidrogen Hydrogon
Lithium Litheum Lithiun
Sodum Sodiume Sodium
Potassium Pottasium Potasium
Silver Sliver Silvur
Guld Geld Gold
Kalcium Calcum Calcium
Oxegen Oxigen Oxygen
Sulphor Sulpher Sulphur
Magenesium Magnesium Magnecium
Carban Carben Carbon
Helium Heelium Hellium
Aluminium Alumium Aluminum
Copper Coper Coppur
Nickle Nickil Nickel
Starter Task
Periodic Table
The idea of the Periodic Table is to arrange the elements in a way that enables chemists to understand patterns in the properties of elements, but some reminders first.
An ATOM is the smallest particle of a substance which can have its own characteristic properties, BUT atoms are built up of even more fundamental sub-atomic particles - the electron, proton and neutron and the structure of an atom ultimately determines its properties.
An ELEMENT is a pure substance made up of only one type of atom, 92 of the elements in the Periodic Table (part of which is shown above) naturally occur, from hydrogen H (element 1) to uranium U (element 92).
Note that each element has symbol which is a single capital letter like H or U or a capital letter + small letter e.g. cobalt Co, chlorine Cl or sodium Na.
The majority of elements are readily divided into two types with common characteristic physical and chemical properties.
Most elements on the left are METALS e.g. elements 3 to 4 (lithium to beryllium), elements 11 to 13 (sodium to aluminium), elements 19 to 31 (potassium to gallium), elements 37 to 50 (rubidium to tin).
The elements on the right are NON-METALS e.g. elements 1 to 2 (hydrogen to helium), elements 5 to 10 (boron to neon), elements 15 to 18 (phosphorus to argon), elements 35 to 36 (bromine to krypton).
BUT a few elements are referred to as SEMI-METALS which have mixed metal/non-metal character and not so easy to classify, They occur in a diagonal band (down and L to R) e.g. silicon (14Si), germanium (32Ge), arsenic (33As) and tellurium (52Te).
The elements are laid out in order of Atomic (proton) Number
Many of the similarities and differences in the properties of elements can be explained by the electronic structure of the atoms (electron configuration = electron arrangement in shells or energy levels, so watch out the varying phrases used!).
The idea of the Periodic Table is to arrange the elements in a way that enables chemists to understand patterns in the properties of elements.
The main structural features of the periodic table are ...
to produce columns of similar elements called Groups.
They are usually similar chemically and physically BUT there are often important trends in physical properties and chemical reactivity up/down a group.
The resulting complete horizontal rows are called Periods and usually consist of a range of elements of different character.
There are important trends from left to right across a period e.g. the most important overall change is from metallic ==> non-metallic element character.
Certain 'horizontal blocks' of elements within a period, which have specific chemical features in common, may be known as a particular block or series e.g. from 21Sc to 30Zn are called the 1st Transition Metal Series within period 4.
The ideas of Group and Period are totally connected with electron structure
Task: PATTERNS IN THE PERIODIC TABLE
1) On the Periodic Table below, shade the metals in one colour and the non-metals in a different colour. Fill in the key to show which is which.
Key
2) On the Periodic Table below, shade the following in different colours: Group 1, Group 7, Group 0 and the transition metals. Fill in the key.
Key
3) On the Periodic Table below, write the atomic number of the first 36 elements in their boxes.
4) The first 20 elements in the Periodic Table are shown below (with the rest of the Table including the transition metals left out). Fill in the electronic structure of each element in the boxes.
Electronic Structure and the periodic table
Which of the elements Magnesium or Neon is the most stable?, give a reason for your answer.
Most of the chemistry of an element is about what the outer electrons can do, or can't, as the case maybe.
and the atoms of other elements try to attain this sort of electron structure when reacting to become more stable.
Metals in the Periodic Table
Metals makeup more than 75% of the elements in the periodic table. Metals are characterized by the following physical properties.
1. They are ______.
2. They are usually ________ at room temperature.
3. They are malleable. Malleable means that ____________________________________________________________________________________________________________________
4. They are ductile, this means that_________________________________________________________________________
5. They are good conductors of ______ and ________.
What is an alloy?______________________________________________________________________________________________________________________________________________________
Explain why metals are often used in the form of alloys?.
Describe the Periodic Table as a method of classifying elements and its use to predict properties of elements.
Describe the change from metallic to non-metallic character across a Period
Describe the relationship between Group number, number of valency electrons and metallic/non-metallic character.
Unit 1: Periodic Table Part 2: Alkali Metals (Group 1)
The alkali metals are in Group I of the Periodic Table. They increase in reactivity as they increase in relative atomic mass.
Properties of Group 1 Metals. (Task- Fill in the gaps)
Good conductors of _______. Good conductors of ____________. Very _______ when first cut, although they ________ quickly in
air.
Unlike most everyday metals, they are
Very _______ and can be easily cut with a knife. Have ______ densities and can ________ on water. Have relatively _______ melting and boiling points.
Burning Group I metals in Air.
Group I metals are so reactive they have to be stored in oil to stop them from reacting with air or water.
Group I metals react with oxygen in the air to form the metal oxide. The oxide of a metal is a powdery compound.
metal + oxygen metal oxide
When lithium burns in air you see a bright red flame.
lithium + oxygen lithium oxide
4Li (s) + O2 (g) 2Li2O (s)
Flame tests
It's possible to test a compound to detect the presence of an alkali metal ion.
A cleaned, moistened flame test wire is dipped into a solid sample of the compound and then put into a blue Bunsen flame. The flame colour indicates which alkali metal ion is present in the compound.Flame colours and the alkali metal ion they represent
Flame colour
Ion present
red lithium
orange sodium
lilac potassium
Reactions with Water.
Group I metals react with water to form metal hydroxides. Hydrogen gas is given off in this reaction.
Sodium + water sodium hydroxide + hydrogen
2Na(s) + 2H2O(l) 2NaOH (aq) + H2(g)
Sodium hydroxide dissolves in water and the solution is a strong alkali. All Group I metals form alkalis in water, which is why they are called Alkali Metals.
Task
1) Complete the table below (parts have been done for you already).
Element Symbol
Atomic
number
Density
(g/cm3)
Melting point (ºC)
Boiling
point (ºC)
State at
25ºC
State at
100ºC
Lithium 0.53 181 1342
Sodium 0.97 98 883
Potassium
0.86 63 780 Liquid
Rubidium
1.53 39 684
Caesium 1.88 29 669 Solid
2) Water has a density of 1g/cm3. If an object has a density greater than this, it will sink.
a) Which group 1 elements will float on water, and which will sink?
b) What can you say, in general, about the densities of the group 1 metals?
3) Underline the correct words in each bold pair or trio in the following sentences:
Lithium, sodium and potassium are very easy / difficult to cut with a scalpel. Lithium / potassium sets on fire easily when it reacts with water. When these metals react with water, they make a gas called oxygen / hydrogen / carbon dioxide. We test for this gas using a lighted / glowing splint which relights / pops. At the end of experiment, the universal indicator in the water is red / green / purple. When these metals react with water, they make acidic / alkaline / neutral solutions.
4) When lithium reacts with water, it makes lithium hydroxide and hydrogen.
The word equation for this reaction is:
lithium + water lithium hydroxide + hydrogen
a) Sodium reacts with water in a similar way. Complete the word equation:
sodium + ______ sodium hydroxide + __________
b) Potassium also reacts with water in a similar way. Write the word and symbol equation:
5) Plot a graph of melting point (vertical axis) against atomic number (horizontal axis). Describe your graph in a much detail as you can – what does it show you about how the melting points of the group 1 metals change as the atomic number increases?
References
IGCSE Chemistry pages 149-152
Learning Objectives
Candidates should be able to:
• Describe the properties and reactivity of lithium, sodium and potassium in Group 1
• Use the trends within the group to predict the properties of other elements.
Unit 1: Periodic Table Part 3: Reactivity Series
Least reactiveAuGold
AgSilver
CuCopper
H**Hydrogen
PbLead
FeIron
ZnZinc
C**Carbon
Al*Aluminium
MgMagnesium
CaCalcium
NaSodium
*Aluminiumseems unreactive in water and acidic solutions because it has a thin, tough layer of aluminiumoxide on its surface.**Two non-metals are in this series. This helps you to understand the making of metals by reduction using carbon and how metals react with acids and water.
Most reactiveKPotassium
SymbolElement
Reactivity series of metals
This is a list of metals (and often the non-metals carbon and hydrogen) in order of their chemical reactivity. The most reactive is at the top and the least is at the bottom.
How metals react with oxygen
Metals react with the oxygen in air, forming oxides. This can often be made clearer by reacting the metal with pure oxygen.
magnesium + oxygen → magnesium oxide
Here magnesium metal has reacted with the oxygen in the air and has been oxidised. This means that oxygen has joined to the magnesium making a compound from the elements. The compound is called magnesium oxide.
In general: metal + oxygen + metal oxide.
zinc + oxygen → zinc oxide
copper + oxygen → copper oxide
calcium + oxygen → calcium oxide
There are a few metals that do not react with oxygen in the air. They include the very unreactive metals gold, platinum and silver.
How metals react with water
Metals above hydrogen in the reactivity series will react with water. The metals below hydrogen - like copper, silver and gold - do not react with water or steam.
Lithium, sodium, and potassium all react well (fast, vigorously) with cold water. These metals react and dissolve, producing an alkaline solution - a metal hydroxide solution which turns Universal Indicator purple. While reacting, hydrogen (which is a flammable gas) is given off, making a fizzing noise.
lithium + water→ lithium hydroxide + hydrogen
potassium + water→ potassium hydroxide + hydrogen
sodium + water→ sodium hydroxide + hydrogen
Magnesium is less reactive than these three. Therefore it only reacts slowly with cold water. It will react vigorously with steam. The products are slightly different as the oxide is formed.
Once the magnesium has become very hot it starts to react with the steamin a very exothermic reaction. The magnesium, which was silver in colour, becomes pure white and a flammable gas - hydrogen - is formed. This is set on fire. The word equation is:
magnesium + water (steam) → magnesium oxide + hydrogen
How metals react with acids
Metals above hydrogen in the reactivity series react with dilute acids. The reaction involves the metal dissolving and fizzing as hydrogen gas is formed.
The test tube gets warm because the reaction produces thermal energy - i.e. it is exothermic.
The general word equation is: acid + metal → hydrogen gas + a salt
A salt is a compound made from an acid when a metal has replaced the hydrogen. The table below gives you the names of the salts formed when using each acid.
Sulphates(e.g. Magnesium sulphate
Sulphuric acid
Nitrates(e.g. Calcium nitrate)
Nitric Acid
Chlorides(e.g. Sodium chloride)
Hydrochloric acid
Name of salt (+ example)Acid
Sulphates(e.g. Magnesium sulphate
Sulphuric acid
Nitrates(e.g. Calcium nitrate)
Nitric Acid
Chlorides(e.g. Sodium chloride)
Hydrochloric acid
Name of salt (+ example)Acid
Below are some examples of reaction between metals and acids:
Take a lighted splint or spill and place it in the gas. If there is a squeaky pop - and often the splint or spill is blown out - then the gas is hydrogen.
Reactivity of Metals- Summarized
Displacement reactions
A displacement reaction happens between a reactive metal and a solution of a less reactive metal compound. The more reactive metal will displace the less reactive metal from its compound in solution.
Here's what you observe (see, hear, feel) in this type of reaction:
The more reactive metal will dissolve.
The less reactive metal will appear at the bottom of the tube or plate on the more reactive metal.
The solution may change colour.
These reactions are exothermic, so the tube gets warm.
iron + copper sulphate solution→ iron sulphate solution + copper
Reactivity Series Questions
1. For each of the following experiments, decide whether a reaction will occur.
If you think there will be no reaction, write down why you think this.
If you think a reaction will happen:· write down why you think it will happen,· what you expect to see, and· the word equation to go with it.
a) iron into copper(II) sulphate solution……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….
b) tin into magnesium sulphate solution……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….
c) copper dipped into silver nitrate solution.............................................................................................................................................................................................................................................................................................................................................................................................................................
d) zinc dipped into lead nitrate solution……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
Competition reactions
“If a reactive metal is heated with the oxide of a less reactive metal it will remove the oxygen from it”.
For example, if zinc powder is mixed with copper(II) oxidepowder, and heated on a tin lid, there is a vigorous exothermicreaction which produces zinc oxide and copper. This is becausezinc is more reactive than copper, and so will “steal” the oxygenaway from the copper(II) oxide.
The word equation is:zinc + copper(II) oxide→zinc oxide + copper
2. For each of the following experiments, decide whether a reaction will occur.
If you think there will be no reaction, write down why you think this.If you think a reaction will happen:· write down why you think it will happen,· what you expect to see, and· the word equation to go with it.
a) iron heated with copper(II) oxide.............................................................................................................................................................................................................................................................................................................................................................................................................................
b) aluminium heated with iron oxide………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
c) copper heated with iron oxide……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
The table below shows the elements on the third period. Sample of each of the elements were burnt in oxygenand the oxides formed were tested to see whether they were acids or bases.
11Na
sodium23
12Mg
magnesium24
13A1
aluminium27
14Si
silicon28
15P
phosphorus31
16S
sulphur32
17C1
chlorine35.5
18Ar
argon40
(a) (i) How many electron shells does the third period have?……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….…[1]
(ii) The element with atomic number 10 is neon. Explain in terms of electron arrangement why a new period starts after neon.………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………[2]
(b)(i) Which three elements in the third period are metals?
• Describe the properties and reactivity of lithium, sodium and potassium in Group 1
• Use the trends within the group to predict the properties of other elements.
Unit 1: Periodic Table Part 4: Using the reactivity series
Starter A student is given some solid nickel nitrate and several small pieces of magnesium, zinc, iron, copper and silver. Describe and explain how he can find the position of nickel in the reactivity series given above. .............................................................................................................................. .............................................................................................................................. ..............................................................................................................................
The reactivity series of metals is an important concept in chemistry and has implications for corrosion chemistry and its prevention, metal extraction, storage of reactive metals.
The higher the metal in the series, the more reactive it is and you usually observe a more vigorous - faster and more exothermic (heat releasing) reaction with oxygen, water or an acid.
At a more theoretical level, the more reactive a metal, the greater tendency it has to form a positive ion in the context of a chemical reaction (e.g. Na ==> Na+ or Fe ==> Fe2+).
This also implies that the reverse reaction becomes more difficult i.e. the more reactive a metal, the more difficult it is to extract the metal from its ore and the metal is also more susceptible to corrosion with oxygen and water.
The reactivity series can be established by observation of the reaction of metals with water, oxygen or acids (and also from simple cell experiments).
The apparent unreactivity of Aluminium
The surface of aluminium goes white when strongly heated in air/oxygen to form white solid aluminium oxide. Theoretically its quite a reactive metal but an oxide layer is readily formed even at room temperature and this has quite an inhibiting effect on its reactivity.
Even when scratched, the oxide layer rapidly reforms, which is why it appears to be less reactive than its position in the reactivity series of metals would predict but the oxide layer is so thin it is transparent, so aluminium surfaces look metallic and not a white matt surface.
This property makes it a useful metal for out-door purposes e.g. aluminium window frames, greenhouse frames.
aluminium + oxygen ==> aluminium oxide
4Al(s) + 3O2(g) ==> 2Al2O3(s)
Aluminium oxide is insoluble with water.
Under 'normal circumstances' in the school laboratory aluminium has virtually no reaction with water, not even when heated in steam due to a protective aluminium oxide layer of Al2O3. The metal chromium behaves chemically in the same way, forming a protective layer of chromium(III) oxide, Cr2O3, and hence its anti-corrosion properties when used in stainless steels and chromium plating. Although this again illustrates the 'under-reactivity' of aluminium, the Thermit Reaction (Unit 7) shows its rightful place in the reactivity series of metals.
Uses of Aluminium
Aluminum has the following properties:
Light Weight Corrosion Resistance Electrical and Thermal Conductivity Reflectivity Recyclabilit
Task- Considering the properties of Aluminium, suggest how the metal is often used and why.(5 uses)
Unit 1: Periodic Table Part 5: Metal Extraction (Blast Furnace)
Principles of metal extraction
1) The occurrence of metals in the Earth's crust
Metals are found in the Earth's crust. The least reactive metals are found as elements (i.e. native, e.g. silver, gold), but most metals are found in compounds, usually oxides or sulphides.
Rocks that contain a high enough percentage of a metal to be extracted commercially are known as ores (what percentage is required depends on the value of the metal).
Aluminium and iron are the most abundant metals in the Earth's crust, and they are widely distributed around the world, which explains why they are so widely used.
There are some other commonly used metals, such as Ni and Cu that are scarce in the Earth's crust, but occur in high grade ores in a few locations.
2) Methods of extraction
Most compounds are found as oxides or sulphides, but the sulphides are usually converted to oxides before extraction.
The extraction of metals involves reduction, usually of metal oxides.
This reduction of the metal compound is usually done in one of three main ways:
1)………………………………………………………………………………………………………………………
2)…………………………………………………………………………………………………………………….
3)……………………………………………………………………………………………………………………
Which method is used depends on:
1)………………………………………………………………………………………………………………………
2)…………………………………………………………………………………………………………………….
3)……………………………………………………………………………………………………………………
Reduction of metal oxides with carbon
Use of carbon reduction
Nearly all metals can be extracted this way, but many are not because:
1)………………………………………………………………………………………………………………………
2)…………………………………………………………………………………………………………………….
The Blast Furnace Extraction of Iron
Inset the correct lables…..
Task
Under each of the steps below write word and symbol equations for the reactions taking place
1) Coke (a form of carbon) is burned in hot air, producing CO2 and a lot of heat (needed for all the other reactions)
……………………………………………………...............
……………………………………………………………………
…………………………………………………………………..
2) In the high temperatures in the furnace, more coke is reacted with the carbon dioxide produced, forming CO.
5) The calcium oxide (a base) reacts with acidic impurities such as sand (silicon dioxide), producing a molten mixture of compounds, mainly calcium silicate, called slag which floats on the iron – slag is used in construction (e.g. road making, cement making).
Pollution problems arise from using carbon, giving CO2 (a greenhouse gas) and CO (toxic)
Roasting of sulphide ores to give oxides leads to SO2 pollution, leading to acid rain.
Steel making
Steel is an alloy of iron and other elements, including carbon, nickel and chromium.
The iron produced in (cast or pig iron) has impurities such as C (making it very brittle), P and S.
In the Basic Oxygen Process, the excess carbon is burnt off in a converter and the correct amount of carbon added to make steel. Other metals (e.g. chromium) can be added to make specialist steels.
1) …………………………………………..
2) …………………………………………..
3) …………………………………………..
4) …………………………………………..
Types of Steel
Type Propertie Uses
MILD easily pressed into shape
chains and pylons
LOW CARBON soft, easily shaped
HIGH CARBON strong but brittle chisels, razor blades, saws
STAINLESS hard, resistant to corrosion
(contains chromium and
nickel)
tools, sinks, cutlery
Metal extraction Questions
1) The diagram represents a blast furnace used for extracting iron from iron ore.
P
hot gases
hot air
X
a) i) Name an iron ore used in the blast furnace (1)
………………………………………………………………………………
ii) Name two substances that are mixed with iron ore and fed into the blast furnace at point P. (2)
…………………………………………………………………………………………………………….
b) What substance is removed from the blast furnace at X? (1)
……………………………………………………………………………………………………………
c) Name one of the gases leaving the blast furnace. (1)
………………………………………………………………………………………………………………
d) Name two substances which react together to produce most of the energy required to heat the furnace to 1400C
(2)
…………………………………………………………………………………………………………….
e) Explain why the extraction of iron is a reduction reaction.(1)
…………………………………………………………………………………………………………….
f) The iron ores which are used contain sandy impurities. Explain how the limestone enables the furnace to run continuously without becoming blocked up with these impurities. (3)
……………………………………………………………………………………………………………
2) In the manufacture of iron from iron (III) oxide, reduction of the oxide by carbon monoxide occurs.
Fe2O3(s) + 3 CO(g) 2 Fe(l) + 3 CO2(g)
a) What mass of carbon monoxide must be used to convert 320 tonnes of iron (III) oxide into iron? (3)
……………………………………………………………………………………………………………
b) What mass of coke must be used to provide this quantity of carbon monoxide? (Assume that coke is 100% carbon and that it is all converted to carbon monoxide). (2)
……………………………………………………………………………………………………………….
3) The flowchart shows some of the stages in the manufacture of stainless steel from impure iron (pig iron) obtained from a blast furnace.
a) i) Name the main impurity present in pig iron. (1)
……………………………………………………………………………………………………………….
ii) Why is pig iron a poor material. (1)
……………………………………………………………………………………………………………….
iii) Name gas A used in steel making. (1)
……………………………………………………………………………………………………………….
iv) Explain how this gas removes the main impurity from pig iron (2)
……………………………………………………………………………………………………………….
b) Solid B also has to be added in steel making to remove other impurities.
……………………………………………………………………………………………………………….
i) What are these other impurities. (2)
……………………………………………………………………………………………………………….
ii) Name solid B. (1)
……………………………………………………………………………………………………………….
iii) Explain how blowing gas A and adding solid B removes these other impurities. (4
(2) The impure zinc oxide can be treated in two ways to extract the zinc:
(a) It is roasted in a smelting furnace with carbon (coke, reducing agent) and limestone (to remove the acidic impurities). The chemistry is similar to iron from a blast furnace.
ZnO(s) + CO(g) ==> …………. + ………… (zinc oxide reduced by CO, Zn undergoes O loss)
or direct reduction by carbon: ZnO(s) + C(s) ==> Zn(l) + CO(g) (ZnO reduced, C oxidised)
The carbon monoxide acts as the reducing agent i.e. it removes the oxygen from the oxide.
The impure zinc is then fractionally distilled from the mixture of slag and other metals like lead and cadmium out of the top of the furnace in an atmosphere rich in carbon monoxide which stops any zinc from being oxidised back to zinc oxide.
The slag and lead (with other metals like cadmium) form two layers which can be tapped off at the base of the furnace.
The zinc can be further purified by a 2nd fractional distillation or more likely by dissolving it in dilute sulphuric acid and purified by electrolysis. (this will be covered in Unit 8)
Uses of Zinc
Zinc is used to galvanise (coat) iron or steel to sacrificially protect them from corrosion. The zinc layer can be put on the iron/steel object by chemical or physically dipping it into a bath of molten zinc.
Zinc sulphate solution can be used as the electrolyte for electroplating/galvanising objects with a zinc layer.
Zinc is used as a sacrificed electrode in a zinc-carbon battery. It slowly reacts with a weakly acidic ammonium chloride paste, converting chemical energy into electrical energy.
The alloy BRASS is a mixture copper and zinc. It is a much more hard wearing metal than copper (too soft) and zinc (too brittle) but is more malleable than bronze for 'stamping' or 'cutting' it into shape
11. The process forextracting highreactivity metals
12. A compound thatcontains carbon andoxygen is called this
13. A type of reactionwhere a more reactivemetal "kicks out" a lessreactive one
15. An acid that is used tomake a chloride salt
17. A common alkali -sodium ________
18. The more common namefor iron oxide
22. In methyl orangeindicator an alkali wouldbe this colour
23. One of the "ingredients"in a blast furnace
25. The abbreviation for"reduction-oxidation"reactions
26. The type of reactionwhen oxygen is takenaway from a substance
30. Acid + metal -> _____ +water
31. Acid + ______ -> salt +hydrogen
33. During electrolysis thenon-metal forms a________ ion
35. During electrolysispositive metal ions ____electrons at the negativeelectrode
36. A substance which has apH of 7 is this
37. The waste liquid from ablast furnace is calledthe molten ____
38. Iron needs this to rust
DOWN1. This gas is given off
when an acid reacts witha carbonate
2. A substance that a metalcould be extracted from(e.g. haematite)
3. The ore that aluminiumcould be extracted from
4. The type of reactionwhen oxygen is added toa substance
6. This substance is addedto bauxite to make itsboiling point lower
7. Carbon dioxide makesthis liquid turn milky
8. The __________ seriesis a series that putsmetals in order of howmuch they react
9. Metals are good_________ conductors
10. This substance wouldhave a pH of 1-6
14. This gas would make a litsplint go "pop"
16. The only metal that coulddisplace sodium
19. A common pH indicator20. A mixture of metals is
called an ______21. Non-metals are_____
conductors of heat24. A method of stopping a
metal from rusting27. The negative electrode
is called the _______28. Reacting a base with
nitric acid wouldproduce a ________
29. The only metal that is aliquid at roomtemperature
32. Sodium is an example ofan ______ metal
34. A non-metal that canconduct electricity
35. A very unreactive metal
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Learning Objectives
Candidates should be able to:
Describe in outline, the extraction of zinc from zinc blende. Name the uses of zinc for galvanising and for making brass.
Metals Crossword
5 7
11 12
13
1517 18
2223
25 26
30 3133
3536
37 38
1 2 3 46 7
89 10
1416
19 2021
24 27
28 29 32
3435
ACROSS5. The process for
extracting middlereactivity metals
7. Oxidation is _____ ofelectrons (hint - OILRIG)
11. The process forextracting highreactivity metals
12. A compound thatcontains carbon andoxygen is called this
13. A type of reactionwhere a more reactivemetal "kicks out" a lessreactive one
15. An acid that is used tomake a chloride salt
17. A common alkali -sodium ________
18. The more common namefor iron oxide
22. In methyl orangeindicator an alkali wouldbe this colour
23. One of the "ingredients"in a blast furnace
25. The abbreviation for"reduction-oxidation"reactions
26. The type of reactionwhen oxygen is takenaway from a substance
30. Acid + metal -> _____ +water
31. Acid + ______ -> salt +hydrogen
33. During electrolysis thenon-metal forms a________ ion
35. During electrolysispositive metal ions ____electrons at the negativeelectrode
36. A substance which has apH of 7 is this
37. The waste liquid from ablast furnace is calledthe molten ____
38. Iron needs this to rust
DOWN1. This gas is given off
when an acid reacts witha carbonate
2. A substance that a metalcould be extracted from(e.g. haematite)
3. The ore that aluminiumcould be extracted from
4. The type of reactionwhen oxygen is added toa substance
6. This substance is addedto bauxite to make itsboiling point lower
7. Carbon dioxide makesthis liquid turn milky
8. The __________ seriesis a series that putsmetals in order of howmuch they react
9. Metals are good_________ conductors
10. This substance wouldhave a pH of 1-6
14. This gas would make a litsplint go "pop"
16. The only metal that coulddisplace sodium
19. A common pH indicator20. A mixture of metals is
called an ______21. Non-metals are_____
conductors of heat24. A method of stopping a
metal from rusting27. The negative electrode
is called the _______28. Reacting a base with
nitric acid wouldproduce a ________
29. The only metal that is aliquid at roomtemperature
32. Sodium is an example ofan ______ metal
34. A non-metal that canconduct electricity
35. A very unreactive metal
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Unit 1: Periodic Table
Part 6: Transition Metals
Transition means “an in between state” and the transition elements come in between Group 2 and Group 3.
Use these words to fill in the gaps on the worksheet.
Shiny Hard Heat High Blue Conductors Mercury Cu Electricity Fe Rusting Coloured
Sc
Ti VCr
Mn
Fe
Co
Ni
Cu
Zn
YZr
Nb
Mo
Tc
Ru
Pd
Ag
Cd
RhH
fTa
WRe
Os
IrAu
Hg
La
PtR
fDb
Sg
Bh
Hs
Mt
? ?Ac
?
H
LiNaKRbCsFr
BeMg G
aGe
Se
Br
Ca
Kr
InSn
Sb
Sr
TeB
aTl
Pb
BiPo
AtR
a
Al PN O
SCl
FNeAr
Rn
I
Si
Xe
He
B C
As
Gp 2 Gp 3
Transition Elements
Transition Metals are the ‘everyday’ metals, such as iron and copper. They are in a block in the middle of the Periodic Table (the bit with no Group Numbers).
Like Group I metals they are …………………, are good ………………………… of electricity and …………………….
Unlike the Group I metals, they are ………………………, tough and strong. They also have ……………………… melting points, except ………………………………….
Transition Metals as Catalysts
A catalyst is a substance that speeds up a chemical reaction without being used up.
Catalysts are hugely valuable in industry where they can save time and energy.
Many transition elements ( and their compounds) are catalysts.
Examples;
Nickle
……………………………………………………………………………………………
Iron
……………………………………………………………………………………………
Vanadium
……………………………………………………………………………………………
Titanium
……………………………………………………………………………………………
Copper
Copper’s chemical symbol is …………. It has some useful properties. It is a very good conductor of ………………………………… It is easy to bend and shape. It does not react (corrode) much with water and air.
Copper is used in electrical wires and for pipes in houses.
Iron and Steel
Iron’s chemical symbol is …………. This is because it used to be called ferrum. Steel is a form of iron.
Iron and steel have many useful properties. They are hard, tough and strong. They can be hammered and bent into many different shapes
when hot. They have very high melting points.
Unfortunately though, iron and steel corrode in water and air. This is called ……………………………….
Compounds of Transition Metals.
Transition metals react to form compounds. Unlike the alkali metals where the compounds are white, transition metal compounds are often brightly coloured.
Copper Sulphate solution is bright ……………….. Other copper compounds are also blue, but others can be green.
Iron compounds can also be green, but others are rusty brown. Rust is actually iron oxide.
Questions on Transition Metals.
1 – You have some iron sulphate and copper sulphate crystals in two unlabelled jars. How could you tell which was which?
2 – Manganese forms pink or purple compounds. Is this an alkali metal or a transition metal?
3 – Gold is an excellent conductor of electricity. Why isn’t it used in house wiring instead of copper?
4 – Give four properties you would expect a transition metal to have.
Learning Objectives
Candidates should be able to:
Name the uses of copper related to its properties; electrical wiring and in cooking utensils. Describe the transition elements as a collection of metals having high densities, high melting points and forming coloured compounds, and which, as elements and compounds, often act as catalysts.
Unit 1: Periodic Table Part 7: Revision Questions
A new metal has been discovered.It has the name mancunium with the symbol M.Mancunium reacts violently with water to form a colourless gas and an alkaline solution. The alkaline solution is mancunium hydroxide with formula MOH.Mancunium also forms a chloride salt with formula MCl.
(a) Describe a test to show that the solution formed with water was alkaline.
TEST …………………………………………………………………………………………………………………………………[1]
RESULT (2)
(b) Use the information to predict the formula of mancunium oxide.
(f) Mancunium hydroxide reacts with sulphuric acid to form a salt and water. (i) Complete the word equation by naming the salt formed in this reaction.
mancunium hydroxide + sulphuric acid __________+ water [1]
(ii) Complete the symbol equation for this reaction.
______ MOH + H2SO4 ____________________ [2]
TOTAL / 11
2) Reactions that give out a large amount of heat have many uses.A company has invented 'cook-in-the-can' meals.
A ring is pulled which ignites the chemicals surrounding the can. The chemicals react and produce heat, which cooks the food in the can.
One of the reactions used is a mixture of aluminium powder and iron(III) oxide.The aluminium used is finely powdered.
(a)(i) Complete the word equation below for this reaction:
(ii) John found a copy of the reactivity series in a chemistry textbook. It is shown below:
magnesium zinc iron silver gold
Use this information to name another metal that John could use that would react with iron(III) oxide. …………………………………………………………………………………………………………………………………
Q3 Some students were investigating the reaction between zinc metal and copper sulphate solution. They set up the apparatus as shown in the diagram below.
(a) Name a piece of apparatus that could be used to measure out 50 cm3 of copper sulphate solution.……………………………………………………………………………………………………………………………[1]
(1)
(b) Name a piece of apparatus that could be used to measure 5 g of zinc metal.
(f) The students repeated the experiment but added zinc to magnesium sulphate solution. (i) What would the students see?……………………………………………………………………………………………………………………………[1]
(ii) Explain your answer. ……………………………………………………………………………………………………………………………
(d) Which of the four metals would be found 'native'? ……………………………………………………………………………………………………………………………[1]
(1)
(e) Metal A was found to be copper. Write a word equation for the reaction of copper in air. ……………………………………………………………………………………………………………………………
…………………………………………………………………………………………………………………………[2]
(f) A student wished to try the reaction between metal D and hydrochloric acid. Explain why you should not carry out this reaction. ……………………………………………………………………………………………………………………………
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