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AQA Level 1/2 Certificate
CHEMISTRY
Paper 1
Thursday 19 May 2016
Morning
Time allowed: 1 hour 30 minutes
Materials
For this paper you must have:
 a ruler
 a calculator
 the periodic table (enclosed).
Instructions





Use black ink or black ball-point pen.
Fill in the boxes at the top of this page.
Answer all questions.
You must answer the questions in the spaces provided. Do not write outside the box around each
page or on blank pages.
Do all rough work in this book. Cross through any work you do not want to be marked.
Information





The marks for questions are shown in brackets.
The maximum mark for this paper is 90.
You are expected to use a calculator where appropriate.
You are reminded of the need for good English and clear presentation in your answers.
Question 7(c) should be answered in continuous prose.
In this question you will be marked on your ability to:
– use good English
– organise information clearly
– use specialist vocabulary where appropriate.
Advice

In all calculations, show clearly how you work out your answer.
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Answer all questions in the spaces provided.
1
This question is about air and rusting.
1 (a)
Air is a mixture of gases.
1 (a) (i)
What is the approximate percentage of the air that is oxygen?
[1 mark]
Tick () one box.
20%
50%
80%
1 (a) (ii) Air contains carbon dioxide.
What is the test for carbon dioxide?
[2 marks]
Test ________________________________________________________________________________
_____________________________________________________________________________________
Result ______________________________________________________________________________
1 (b)
An oxidation reaction happens when iron is heated in air.
The word equation for the reaction is:
iron + oxygen
1 (b) (i)
iron oxide
Why is the reaction described as oxidation?
[1 mark]
_____________________________________________________________________________________
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1 (b) (ii) Complete and balance the symbol equation for this reaction.
[2 marks]
____
1 (c)
Fe + __________
Fe3O4
Iron reacts with two substances to form rust.
Name the two substances.
[2 marks]
_____________________________________________________________________________________
_____________________________________________________________________________________
1 (d)
Zinc blocks are attached to ships to help prevent rusting.
1 (d) (i)
Name the method of rust prevention when zinc blocks are attached to ships.
[1 mark]
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1 (d) (ii) Explain how zinc prevents iron from rusting.
[2 marks]
_____________________________________________________________________________________
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2
This question is about metals.
2 (a)
Transition metals have different properties from the alkali metals.
Tick () two typical properties of transition metals.
[2 marks]
High density
Low boiling points
Soft
Strong
Very reactive
2 (b)
Lithium reacts with water. The equation for the reaction is:
2Li(s) + 2H2O(l)
2LiOH(aq) + H2(g)
A piece of lithium was added to water, as shown in Figure 1.
Figure 1
Piece of lithium
Water containing
universal indicator
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The lithium floated on the surface.
Give three other observations. Use the equation and Figure 1 to help you.
[3 marks]
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2 (c)
The electronic structures of lithium and potassium are shown in Figure 2.
Figure 2
Lithium
Potassium
Potassium is more reactive than lithium. Explain why, in terms of electronic structure.
[3 marks]
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3 (a)
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Figure 3 shows the displayed structures of four compounds.
Figure 3
A
B
H
H
C
C
H
H
H
C
H
H
H
C
C
H
Br
H
D
H
H
C
C
H
H
O
H
H
H
H
H
C
C
C
H
H
H
H
Use the correct letter, A, B, C or D, to answer each question.
3 (a) (i)
Which compound has the formula C3H8?
[1 mark]
3 (a) (ii) Which compound contains a halogen?
[1 mark]
3 (a) (iii) Which compound is an alcohol?
[1 mark]
3 (a) (iv) Which compound is unsaturated?
[1 mark]
3 (a) (v) Which compound is an alkane?
[1 mark]
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3 (b)
Hydrocarbons can be cracked to produce alkenes and alkanes.
3 (b) (i)
Dodecane (C12H26) can be cracked to produce butene and an alkane.
Complete the balanced equation for this reaction.
[2 marks]
C12H26
_______________
+ _______________
3 (b) (ii) Alkenes can form polymers.
Disposal of these polymers can cause problems.
Explain one problem caused by the disposal of these polymers.
[2 marks]
_____________________________________________________________________________________
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3 (b) (iii) Describe the colour change seen when bromine water reacts with an alkene.
[2 marks]
_____________________________________________________________________________________
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Question 3 continues on the next page
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3 (c)
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Table 1 shows the boiling points and melting points for five alkenes.
Table 1
Number of
carbon atoms
Boiling point
in °C
Melting point
in °C
Ethene
2
–104
–169
Propene
3
– 47
–185
Butene
4
–6
– 85
Pentene
5
+30
Hexene
6
+63
Name of alkene
3 (c) (i)
– 40
These alkenes have simple molecular structures.
Describe and explain the trend in boiling point shown in Table 1.
[3 marks]
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3 (c) (ii) It is not possible to use the data in Table 1 to predict the melting point of pentene.
Suggest why.
[1 mark]
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4 (a)
An atom of lithium has the symbol 37 Li
4 (a) (i)
How many protons are in one atom of lithium?
[1 mark]
Tick () one box.
3
4
7
4 (a) (ii) Complete the sentence.
[1 mark]
The nucleus of a lithium atom contains protons and _________________________________ .
4 (a) (iii) Lithium has two different atoms, 37 Li and 36 Li
What name is given to different atoms of the same element?
[1 mark]
_____________________________________________________________________________________
4 (b)
Figure 4 shows the electronic structures of three atoms, A, B and C.
Figure 4
A
B
C
Which two of the atoms, A, B and C, are in the same group of the periodic table?
[1 mark]
_____________________________________________________________________________________
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4 (c)
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Figure 5 shows the electronic structures of an atom of magnesium and an
atom of fluorine.
Figure 5
Magnesium
Fluorine
Magnesium reacts with fluorine to produce the ionic compound magnesium fluoride.
4 (c) (i)
Describe what happens, in terms of electrons, when magnesium reacts with fluorine to
produce magnesium fluoride (MgF2).
[3 marks]
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4 (c) (ii) The melting point of magnesium fluoride is 1263 °C.
Explain why ionic compounds have high melting points.
[3 marks]
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4 (d)
The equation for the reaction of magnesium with fluorine is:
Mg + F2
4 (d) (i)
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MgF2
In one reaction, the theoretical yield of magnesium fluoride was 3.20 g.
The mass of magnesium fluoride obtained was 2.50 g.
Calculate the percentage yield of magnesium fluoride in this reaction.
Give your answer to 3 significant figures.
[2 marks]
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_____________________________________________________________________________________
Percentage yield = ___________________________ %
4 (d) (ii) In another reaction, 1.20 g of magnesium reacted with fluorine.
Calculate the mass of fluorine needed to react with 1.20 g of magnesium.
Relative atomic masses (Ar): F = 19; Mg = 24
[3 marks]
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Mass of fluorine = ____________________ g
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5
This question is about reactions of hydrochloric acid.
5 (a)
Figure 6 shows what happens when magnesium, iron, copper and zinc are added to
hydrochloric acid of the same concentration.
Figure 6
Magnesium
Iron
Copper
Zinc
Hydrogen
Complete the order of reactivity of these four metals. Use the information in Figure 6.
[1 mark]
Most reactive
________________________
________________________
________________________
Least reactive
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Copper
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5 (b)
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A student made a solution of copper chloride.
This is the method he used.
5 (b) (i)

Put 25 cm3 of dilute hydrochloric acid into a beaker.

Add one spatula of solid copper oxide.

Heat until all the copper oxide has reacted.
What two further steps should the student do to make sure that all the hydrochloric acid
had reacted and to obtain only copper chloride solution?
[2 marks]
Step 1 ______________________________________________________________________________
_____________________________________________________________________________________
Step 2 ______________________________________________________________________________
_____________________________________________________________________________________
5 (b) (ii) What technique could the student use to obtain solid copper chloride from a solution of
copper chloride?
[1 mark]
Tick () one box.
Chromatography
Crystallisation
Precipitation
Question 5 continues on the next page
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5 (c)
Hydrochloric acid neutralises potassium hydroxide, as shown in the equation.
HCl(aq) + KOH(aq)
5 (c) (i)
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KCl(aq) + H2O(l)
Write the ionic equation for a neutralisation reaction.
[1 mark]
_____________________________________________________________________________________
5 (c) (ii) Calculate the percentage by mass of potassium in potassium hydroxide (KOH).
Relative atomic masses (Ar): H=1; O=16; K=39
[2 marks]
_____________________________________________________________________________________
_____________________________________________________________________________________
Percentage = _________________________%
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DO NOT WRITE ON THIS PAGE
ANSWER IN THE SPACES PROVIDED
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6
This question is about reversible reactions.
6 (a)
When blue crystals of copper sulfate are heated, they produce white anhydrous copper
sulfate and water.
The equation for this reversible reaction is:
CuSO4.5H2O
6 (a) (i)
CuSO4 + 5H2O
What is the name of CuSO4.5H2O?
[1 mark]
Tick () one box.
Aqueous copper sulfate
Hydrated copper sulfate
Copper sulfate solution
6 (a) (ii) How is this reversible reaction used to test for the presence of water?
[2 marks]
_____________________________________________________________________________________
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6 (a) (iii) What physical property can be used to show that a liquid is pure water?
[1 mark]
_____________________________________________________________________________________
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6 (b)
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Two gases exist in equilibrium.
N2O4(g)
2NO2(g)
The enthalpy change, ∆H, for the forward reaction is + 57 kJ per mole.
6 (b) (i)
Give the enthalpy change for the reverse reaction.
[1 mark]
_________________________
kJ per mole
6 (b) (ii) What happens to a reaction at equilibrium?
[1 mark]
Tick () one box.
The amounts of reactants and products are equal.
The forward and reverse reactions occur at equal rates.
The forward and reverse reactions have both stopped.
6 (b) (iii) A mixture of N2O4 and NO2 is at equilibrium.
N2O4 is colourless and NO2 is brown.
When the mixture is heated the colour becomes darker brown.
Explain why.
[2 marks]
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_____________________________________________________________________________________
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6 (b) (iv) A mixture of N2O4 and NO2 is at equilibrium.
N2O4(g)
2NO2(g)
What happens to the position of the equilibrium when the pressure is decreased?
Give a reason for your answer.
[2 marks]
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7
Hydrogen, chlorine and sodium hydroxide solution are produced when sodium chloride
solution is electrolysed.
7 (a) (i)
State one use of sodium hydroxide.
[1 mark]
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7 (a) (ii) State one use of chlorine.
[1 mark]
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7 (b)
The electronic structure of a hydrogen atom and a chlorine atom are shown
in Figure 7.
Figure 7
Hydrogen
Chlorine
Describe what happens, in terms of electrons, when a hydrogen atom bonds with a
chlorine atom to form a molecule of hydrogen chloride.
[2 marks]
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7 (c)
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In this question you will be assessed on using good English, organising
information clearly and using specialist terms where appropriate.
Figure 8 shows the electrolysis of sodium chloride solution, NaCl(aq).
Figure 8
Chlorine gas, Cl2
Hydrogen gas, H2
Solution containing
sodium hydroxide,
NaOH(aq)
Positive electrode
(anode)
Negative electrode
(cathode)
–
+
d.c. power
supply
–
–
Sodium chloride solution contains Na+, Cl , H+ and OH ions.
Describe and explain how the products

hydrogen

chlorine

sodium hydroxide solution
are formed during the electrolysis of sodium chloride solution.
[6 marks]
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Extra space _________________________________________________________________________
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8
This question is about the metal titanium.
8 (a)
Describe the structure of a metal.
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[3 marks]
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8 (b)
Titanium(IV) chloride (TiCl4) reacts with sodium to produce titanium.
8 (b) (i)
Balance the symbol equation.
[1 mark]
TiCl4
+
Na
Ti
+
NaCl
8 (b) (ii) In the reaction, Ti4+ ions are reduced to produce titanium.
Complete the half equation.
[1 mark]
Ti4+
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Ti
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8 (c)
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Titanium(IV) chloride (TiCl4) is one chloride of titanium.
A different chloride of titanium acts as a catalyst in the production of poly(propene).
8 (c) (i)
The titanium chloride in the catalyst contains 0.932 g of titanium and
2.068 g of chlorine.
Calculate the empirical formula of this titanium chloride.
Relative atomic masses (Ar): Cl = 35.5; Ti = 48
You must show all of your working to get full marks.
[4 marks]
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Empirical formula = _________________________
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8 (c) (ii) Explain how a catalyst increases the rate of a chemical reaction.
[2 marks]
_____________________________________________________________________________________
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8 (c) (iii) Complete the equation to show the formation of poly(propene) from propene.
[3 marks]
n
H
H
C
C
H
CH3
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END OF QUESTIONS
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