Standard Grade Revision

1
Standard Grade Revision

• Units 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.

• Aluminium
• (b) Nickel

Q2. The word box contains the names of some
metals.
zinc copper iron magnesium
silver sodium

• Identify the metal which is made in a blast
  furnace.
• Identify the two metals that do not react with
  acid.
• Identify the two metals that can be used in
  sacrificial
• protection of iron.
• Identify the metal which reacts rapidly with
  water forming
• an alkali solution.

(a) Iron (b) Copper and silver (c) Zinc and
magnesium (d) Sodium
Standard Grade Chemistry
2
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 ships
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?
Standard Grade Chemistry
3
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.

• Hydrogen.
• Copper or silver or gold.
• (c) Concentration of acid, temperature and
  size of piece of metal.

Standard Grade Chemistry
4
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.

• 2Mg O2 ? 2MgO
• Neutralisation.
• Magnesium chloride.
• (d) Water.

Standard Grade Chemistry
5
Units 11 and 12 Revision.
Q6. The diagram shows some ways in which iron can
be protected from rusting.
galvanising   painting
IRON alloying   sacrifici
al 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.

• Magnesium or zinc.
• Zinc
• Paint stops air or water getting to the surface
  of the iron.
• (d) Brass, bronze, solder are a few examples
  of alloys.

Standard Grade Chemistry
6
Units 11 and 12 Revision.
Q7. Wilma investigated the reaction of the metals
R, S and T with water.
hydrogen
hydrogen
beaker water filter funnel
Metal R
Metal S
Metal T

1. Place the metals in order of reactivity (most
   reactive first)
2. Identify a variable that Wilma would have kept
   constant.
3. Why is it unsafe to use potassium metal in this
   experiment?
4. How would Wilma test the gas to show that it was
   hydrogen?

• T R S.
• Water temperature, size size of metals.
• Potassium is too reactive there could be an
  explosion.
• (d) The hydrogen gas burns with a pop.

Standard Grade Chemistry
7
Units 11 and 12 Revision.
Q8. Metals and their compounds take part in many
reactions.
A B C D

• Which of the reactions, A to D, shows
• The reaction which produces a non-metal element
• The reaction which takes place in the blast
  furnace.

(a) Reaction B (Silicon) (b) Reaction A.
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) 52.9
(b) Aluminium forms very strong bonds with
oxygen. Heating with carbon does not provide
enough energy to break these bonds.
Standard Grade Chemistry
8
Units 11 and 12 Revision.
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.
Standard Grade Chemistry
25.26
9
Units 11 and 12 Revision.
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.
Standard Grade Chemistry
C and E
10
Units 11 and 12 Revision.
Q14. Some metals are found uncombined in the
Earths 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
Standard Grade Chemistry
11
Units 11 and 12 Revision.
Q15. Iron can be coated with different materials
which provide a physical barrier
against corrosion. A tin B grease C paint D p
lastic 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.

• 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
12
Units 11 and 12 Revision.
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) Hydrogen.
• (b) W silver or mercury.
• Y sodium, lithium,
• potassium or calcium.
• (c) Y, X,Z,W
• (d) Reduction.

(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.
Standard Grade Chemistry
13
Units 11 and 12 Revision.
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