Standard Grade Revision Units 11 and 12 Q1. The box contains the names of some metals. You may wish...

Standard Grade RevisionUnits 11 and 12

Q1. The box contains the names of some metals.

You may wish to use page 8 of the data booklet.

magnesium lithium calcium

nickel aluminium potassium

(a) Identify the metal which was discovered in 1827.

(b) Identify the transition metal.

Standard Grade Chemistry

(a) Aluminium

(b) Nickel

Q2. The word box contains the names of some metals.

zinc copper iron magnesium silver sodium

(a) Identify the metal which is made in a blast furnace.

(b) Identify the two metals that do not react with acid.

(c) Identify the two metals that can be used in sacrificial

protection of iron.

(d) Identify the metal which reacts rapidly with water forming

an alkali solution.

(a) Iron

(b) Copper and silver

(c) Zinc and magnesium

(d) Sodium

Units 11 and 12 Revision

Q3. Copper can be mixed with other metals to produce alloys for different uses.


Aluminium is added to copper to make an alloy suitable for aircraft bodies.

Coins are made from a hard wearing alloy which contains copper and nickel.

Musical instruments can be made from an alloy of copper and zinc.

If tin is added to copper can be used to make ship’s propellers.

(a) Present this information in a table with suitable headings.

(b) Copper metal is a finite resource.

What is meant by the term ‘finite resource’?

(a) Metals in alloy Use of alloy

copper and aluminium aircraft bodies

copper and nickel coins

copper and zinc musical instruments

copper and tin ship’s propellers

(b) A finite resource is a material whose supply will run out some time in the future.

Units 11 and 12 Revision


Q 4. The reactivity of metals can be compared by adding them to a mixture of hydrochloric

acid and detergent.

Amy set up five test tubes each containing a different metal.

(a) Name the gas produced when a metal reacts with hydrochloric acid. (b) Suggest a name for metal X.

(You may wish to use page 7 of the data booklet). (c) Name one factor which would have to be kept the same to ensure a fair

comparison.

(a) Hydrogen.

(b) Copper or silver or gold.

(c) Concentration of acid, temperature and size of piece of metal.

Units 11 and 12 Revision.


Q5. Hot magnesium ribbon reacts vigorously with steam. It glows very brightly and the products are magnesium oxide and hydrogen gas.

(a) Write a balanced equation, using symbols and formulae, for the reaction taking

place in the test tube.

(b) The magnesium oxide which is formed will react with dilute hydrochloric acid.

Name the type of chemical reaction which takes place.

(c) Name the salt formed when magnesium oxide reacts with hydrochloric acid.

(d) Name the product formed when hydrogen burns.

(a) 2Mg + O2 2MgO

(b) Neutralisation.

(c) Magnesium chloride.

(d) Water.



Q6. The diagram shows some ways in which iron can be protected from rusting.

galvanising

painting IRON alloying

sacrificial

protection

(a) Name a metal which is suitable for the sacrificial protection of iron.

(b) Which metal is used to galvanise iron? (c) How does painting prevent the rusting of iron. (d) Alloys of iron are called steels.

Name another alloy.

(a) Magnesium or zinc.

(b) Zinc

(c) Paint stops air or water getting to the surface of the iron.

(d) Brass, bronze, solder are a few examples of alloys.



Q7. Wilma investigated the reaction of the metals R, S and T with water.

(a) Place the metals in order of reactivity (most reactive first)

(b) Identify a variable that Wilma would have kept constant.

(c) Why is it unsafe to use potassium metal in this experiment?

(d) How would Wilma test the gas to show that it was hydrogen?

hydrogen hydrogen

beaker

water

filter funnel

Metal R Metal S Metal T

(a) T R S.

(b) Water temperature, size size of metals.

(c) Potassium is too reactive –there could be an explosion.

(d) The hydrogen gas burns with a ‘pop’.



Fe2O

3 + 3CO 2Fe + 3CO

2

Fe2O

3 + 3CO 2Fe + 3CO

2

Q8. Metals and their compounds take part in many reactions.

2Mg + SiO2 2MgO + Si

2Mg + SiO2 2MgO + Si

CuCO3 CuO + CO

2

CuCO3 CuO + CO

2

2Zn + O2 2ZnO

2Zn + O2 2ZnO

A

B

C

D

Which of the reactions, A to D, shows

(a) The reaction which produces a non-metal element

(b) The reaction which takes place in the blast furnace.

Q9. (a) Calculate the percentage by mass of aluminium in aluminium oxide,

Al2O3.

(b) Explain why aluminium cannot be obtained from aluminium oxide

by heating with carbon.

(a) Reaction B (Silicon)

(b) Reaction A.

(a) 52.9%

(b) Aluminium forms very strong bonds with oxygen. Heating with carbon does not provide enough energy to break these bonds.



Q10. Some Euro coins are made from a hard-wearing alloy called Nordic Gold.

(a) What is an alloy?

(b) The composition of Nordic Gold is shown in the table.

Metal copper aluminium zinc tin

% by mass 89 5 5 1

One of the coins has a mass of 5.74 g.

(i) Calculate the mass, in grams, of aluminium in the coin.

(ii) Calculate the number of moles of aluminium in the coin.

(a) Mixture of

metals.

(b) (i) 0.287 g

(ii) 0.011 mol

Q11. Titanium is obtained from titanium(IV) chloride, TiCl4.

Given that titanium has a relative atomic mass of 48, calculate the

percentage of titanium in titanium(IV) chloride. 25.26%



Q12. Oil rigs made from iron should be protected from rusting.

Identify the two correct statements.

A Salt water slows down rusting

B Tin gives sacrificial protection to the iron.

C The rusting of iron is an example of oxidation

D Ferroxyl indicator turns blue in the presence of Fe2+ ions.

E Iron rusts faster when connected to the negative terminal of a battery.

C and D are correct statements.

Q13. Equations are used to represent chemical reactions.

A 2H2(g) + O2 (g) 2H2O(g)

B Zn(s) + FeSO4(aq) Fe(s) + ZnSO4(aq)

C Fe2+(aq) Fe3+(aq) + e-

D CH4(g) + 2O2 (g) CO2 (g) + H2O(g)

E 2H2O(l + O2 (g) + 4 e- 4OH-(aq)

F Fe2+(aq) + 2e- Fe(s)

Identify the two equations which represent a step in the rusting of iron.

C and E



Q14. Some metals are found uncombined in the Earth’s crust but others have to be extracted

from their ores.

(a) lead magnesium, mercury

Which of these metals

(i) can only be obtained by electrolysis of its molten ore?

(ii) can be obtained from its ore by heat alone?

(iii) can be obtained from its ore by heating with carbon?

(b) Iron is extracted by reacting iron(III) oxide with carbon monoxide.

(i) Name the type of industrial plant where iron is extracted.

(ii) The overall reaction taking place during the extraction of iron is given by

the equation:

Fe2O3 + 3CO 2Fe + 3CO2

Calculate the mass of iron, in tonnes, which is produced from 1600 tonnes of

iron(III) oxide.

(a) (i) magnesium

(ii) mercury

(iii) lead.

1 mole of iron(III) oxide 2 moles of iron

160g of iron(III) oxide 112 g of iron

So 1600 tonnes of iron(III) oxide 1120 tonnes of iron


Q15. Iron can be coated with different materials which provide a physical barrier

against corrosion.

A tin

B grease

C paint

D plastic

E zinc

(a) Identify the coating which also provides sacrificial protection.

(b) Identify the coating which, if scratched, would cause the iron to rust faster

than normal.

(a) E (zinc)

(b) A (tin)

Q16. Iron can be protected against corrosion by

(a) connecting to magnesium.

(b) connecting to the negative terminal of a power supply.

Explain how both these methods of protection work.

(a) Both methods involve electrons being pushed on to iron which stops it

rusting.Standard Grade Chemistry


Q.17 Siobhan carried out some experiments with four metals (W,X,Y and Z) and some of

their compounds. She made the following observations.

(a) Name the gas formed when metal Y reacts with water.

(b) Suggest names for metals W and Y.

(c) Place the metals (W,X,Y and Z) in order of reactivity

(most reactive first).

d) Name the type of chemical reaction which takes place when

a metal is extracted from its oxide.

(a) Hydrogen.

(b) W = silver or mercury.

Y = sodium, lithium,

potassium or calcium.

(c) Y, X,Z,W

(d) Reduction.Standard Grade Chemistry

The diagram shows how an object can be coated in nickel.


The following reactions take place at the electrodes

Negative electrode:- Ni2+(aq) + 2e- Ni(s)

Positive electrode:- Ni(s) Ni2+(aq) + 2e-

Identify the two correct statements.

A Nickel ions move towards the nickel electrode.

B The mass of the nickel electrode decreases.

C The process is an example of galvanising.

D Oxidation occurs at the nickel electrode.

E Electrons flow through the solution.

B and D

Standard Grade Revision Units 11 and 12 Q1. The box contains the names of some metals. You may wish...

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