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1
AQA Level 1/2 Certificate
June 2014
2
3
Chemistry
8402/1
4
5
Paper 1
6
Thursday 15 May 2014
9.00 am to 10.30 am
7
For this paper you must have:
 a ruler
 a calculator
 the periodic table (enclosed).
8
9
10
Time allowed
 1 hour 30 minutes
A
TOTAL
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 4 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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8402/1
2
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Answer all questions in the spaces provided.
1 (a)
Figure 1 shows an atom of element G.
Figure 1
A
Proton
B
Draw a ring around the correct answer to complete each sentence.
1 (a) (i)
Label A shows
[1 mark]
an electron
an ion
a nucleus
1 (a) (ii) The particle labelled B is
[1 mark]
an isotope
a molecule
a neutron
1 (a) (iii) The mass number of element G is
[1 mark]
5
6
11
1 (a) (iv) Use the periodic table to identify element G.
[1 mark]
Element G is
boron
(02)
carbon
sodium
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1 (b)
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Figure 2 shows a compound of G and hydrogen.
Figure 2
H
H
G
H
Draw a ring around the correct answer to complete each sentence.
1 (b) (i)
The formula of the compound in Figure 2 is
[1 mark]
GH3
G3H
3HG
1 (b) (ii) The type of bonding shown in Figure 2 is
[1 mark]
covalent
ionic
metallic
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6
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2
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Lead nitrate solution reacts with potassium iodide solution.
The reaction produces a solid.
Figure 3 shows the reaction occurring.
Figure 3
2 (a) (i)
Give the name of this type of reaction.
Tick () one box.
[1 mark]
Combustion
Neutralisation
Precipitation
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2 (a) (ii) Write the missing state symbols in the chemical equation.
[2 marks]
Pb(NO3)2(aq)
+
2KI(......)
PbI2(......)
+
2KNO3(aq)
2 (a) (iii) Complete the word equation for the reaction.
[2 marks]
lead iodide + ........................................
lead nitrate + ........................................
2 (a) (iv) How is solid lead iodide separated from the solution?
Draw a ring around the correct answer.
[1 mark]
Distillation
Electrolysis
Filtration
Question 2 continues on the next page
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2 (b)
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A group of students investigated the movement of particles.
The students filled a container with water.
The students added a crystal of lead nitrate at position X and a crystal of potassium
iodide at position Y, as shown in Figure 4.
Figure 4 – view from above
Crystal of
lead nitrate
Y
X
Crystal of
potassium
iodide
Water
After 3 minutes solid lead iodide started to form at the position shown in Figure 5.
Figure 5 – view from above
X
Y
Solid lead iodide
2 (b) (i)
Tick () the correct box to complete the sentence.
[1 mark]
Lead ions and iodide ions move through the water by
diffusion.
evaporation.
neutralisation.
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2 (b) (ii) What conclusion can you make about the speed of movement of lead ions compared
with iodide ions?
Give a reason for your answer.
[2 marks]
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2 (b) (iii) The students repeated the experiment at a higher temperature.
The solid lead iodide formed after a shorter period of time.
Explain why, in terms of particles.
[2 marks]
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3 (a)
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The symbols for seven different elements are shown in Figure 6.
Figure 6
He
Be
Na
S
Ca
Ar
Fe
Choose the correct symbol from Figure 6 to answer each question.
You may use each symbol once, more than once or not at all.
Write the symbol that represents:
3 (a) (i)
a Group 1 element
[1 mark]
............................................................
3 (a) (ii) a transition metal
[1 mark]
............................................................
3 (a) (iii) an element with electrons in the same number of energy levels as an atom of argon (Ar)
[1 mark]
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3 (a) (iv) an element which forms an oxide that dissolves in water to form an acidic solution
[1 mark]
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3 (a) (v) an element that forms a chloride with the formula XCl
[1 mark]
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3 (b)
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A teacher put a cube of sodium metal into water containing universal indicator, as
shown in Figure 7.
Figure 7
Sodium metal
Water with
universal indicator
The equation for the reaction is:
3 (b) (i)
2Na(s)
+
2H2O(l)
2NaOH(aq)
+
H2(g)
sodium
+
water
sodium
hydroxide
+
hydrogen
The sodium floated on the surface of the water. The universal indicator turned purple.
Give three other observations that would be seen during the reaction.
[3 marks]
1 .........................................................................................................................................
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2 .........................................................................................................................................
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3 .........................................................................................................................................
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3 (b) (ii) Name the ion that made the universal indicator turn purple.
[1 mark]
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3 (c)
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Figure 8 represents the electronic structure of a sodium atom.
Figure 8
In the space below, draw the electronic structure of a sodium ion. Include the charge
on the ion.
[2 marks]
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ANSWER IN THE SPACES PROVIDED
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4
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In this question you will be assessed on using good English, organising
information clearly and using specialist terms where appropriate.
A group of students had four different colourless solutions in beakers 1, 2, 3 and 4,
shown in Figure 9.
Figure 9
1
2
3
4
The students knew that the solutions were




sodium chloride
sodium iodide
sodium carbonate
potassium carbonate
but did not know which solution was in each beaker.
The teacher asked the class to plan a method that could be used to identify each
solution.
She gave the students the following reagents to use:


dilute nitric acid
silver nitrate solution.
The teacher suggested using a flame test to identify the positive ions.
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Outline a method the students could use to identify the four solutions.
You should include the results of the tests you describe.
[6 marks]
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Extra space ........................................................................................................................
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5
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Magnesium reacts with steam to produce hydrogen gas and magnesium oxide.
A teacher demonstrated the reaction to a class. Figure 10 shows the apparatus the
teacher used.
Figure 10
Glass tube
Magnesium
Unreacted steam
and hydrogen out
Steam in
Heat
5 (a) (i)
The hydrogen produced was collected.
Describe how to test the gas to show that it is hydrogen.
[2 marks]
Test ....................................................................................................................................
............................................................................................................................................
Result .................................................................................................................................
............................................................................................................................................
5 (a) (ii) Explain why the magnesium has to be heated to start the reaction.
[2 marks]
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5 (b)
The equation for the reaction is:
Mg(s) + H2O(g)
5 (b) (i)
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MgO(s) + H2(g)
The teacher used 1.00 g of magnesium.
Use the equation to calculate the maximum mass of magnesium oxide produced.
Give your answer to three significant figures.
Relative atomic masses (Ar): O = 16; Mg = 24
[3 marks]
............................................................................................................................................
............................................................................................................................................
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Maximum mass = ........................................ g
5 (b) (ii) The teacher’s demonstration produced 1.50 g of magnesium oxide.
Use your answer from part (b)(i) to calculate the percentage yield.
If you could not answer part (b)(i), use 1.82 g as the maximum mass of
magnesium oxide. This is not the answer to part (b)(i).
[2 marks]
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Percentage yield = ........................................ %
5 (b) (iii) Give one reason why the percentage yield is less than 100%.
[1 mark]
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6
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A student investigated the conductivity of different concentrations of sodium chloride
solution.
The student set the apparatus up as shown in Figure 11.
Figure 11
d.c. power supply
Conductivity meter
–
+
Electrodes
Pure water
The student measured the conductivity of the pure water with a conductivity meter.
The reading on the conductivity meter was zero.
6 (a)
The student:



added sodium chloride solution one drop at a time
stirred the solution
recorded the reading on the conductivity meter.
The student’s results are shown in Table 1.
Table 1
Number of drops of
sodium chloride solution
added
(16)
Relative conductivity
of solution
0
0
1
100
2
120
3
310
4
400
5
510
6
590
7
710
8
800
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6 (a) (i)
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The student plotted the results on the grid shown in Figure 12.
Plot the four remaining results.
Draw a line of best fit, ignoring the anomalous result.
[3 marks]
Figure 12
800
700
600
500
Relative
conductivity 400
of solution
300
200
100
0
0
1
2
3
4
5
6
Number of drops of sodium chloride added
7
8
6 (a) (ii) One of the points is anomalous.
Suggest one error that the student may have made to cause the anomalous result.
[1 mark]
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6 (a) (iii) The student wanted to compare the conductivity of sodium chloride solution with the
conductivity of potassium chloride solution.
State one variable he should keep constant when measuring the conductivity of the two
solutions.
[1 mark]
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6 (b) (i)
Explain, in terms of bonding, why pure water does not conduct electricity.
[2 marks]
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6 (b) (ii) Explain why sodium chloride solution conducts electricity.
[2 marks]
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6 (b) (iii) After he had added sodium chloride solution, the student noticed bubbles of gas at the
negative electrode.
Complete the sentence.
[1 mark]
The gas produced at the negative electrode is .................................................................
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Turn over for the next question
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ANSWER IN THE SPACES PROVIDED
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7
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Figure 13 shows the displayed structures of five organic compounds,
A, B, C, D and E.
Figure 13
A
H
H
H
C
C
H
H
B
O
H
C
H
H
C
C
H
H
H
7 (a)
O
C
C
O
H
D
H
H
H
H
C
C
H
H
H
E
H
H
C
C
H
H
H
H
H
C
C
O
H
O
H
Choose which organic compound, A, B, C, D or E, matches the descriptions.
You may choose each compound once, more than once or not at all.
Write the letter of the compound that:
7 (a) (i)
is a saturated hydrocarbon
[1 mark]
7 (a) (ii) comes from a homologous series with the general formula CnH2n
[1 mark]
7 (a) (iii) has the empirical formula C2H6O
[1 mark]
7 (a) (iv) reacts with calcium carbonate to produce carbon dioxide
[1 mark]
7 (a) (v) reacts with compound A to produce compound C.
[1 mark]
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7 (b)
Compound B (C2H4) and C8H18 are produced by cracking C14H30
C14H30
7 (b) (i)
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3C2H4 + C8H18
Give two conditions for cracking.
[2 marks]
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7 (b) (ii) Explain why C8H18 has a lower boiling point than C14H30
[2 marks]
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7 (c)
Compound B is a colourless gas.
Give a chemical test and its result to show that compound B is unsaturated.
[2 marks]
Test ....................................................................................................................................
............................................................................................................................................
Result .................................................................................................................................
............................................................................................................................................
7 (d)
Compound B is ethene.
Complete the equation to show the formation of poly(ethene) from ethene.
[3 marks]
n
H
H
C
C
H
H
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8
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Use the periodic table and the information in Table 2 to help you to answer the
questions.
Table 2 shows part of an early version of the periodic table.
Table 2
Group 1
Group 2
Group 3
Group 4
Group 5
Group 6
Group 7
Li
Be
B
C
N
O
F
Na
Mg
Al
Si
P
S
Cl
H
8 (a)
Hydrogen was placed at the top of Group 1 in the early version of the periodic table.
The modern periodic table does not show hydrogen in Group 1.
8 (a) (i)
State one similarity between hydrogen and the elements in Group 1.
[1 mark]
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8 (a) (ii) State one difference between hydrogen and the elements in Group 1.
[1 mark]
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8 (b)
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Fluorine, chlorine, bromine and iodine are in Group 7, the halogens.
The reactivity of the halogens decreases down the group.
Bromine reacts with a solution of potassium iodide to produce iodine.
Br2 + 2KI
8 (b) (i)
2KBr + I2
In the reaction between bromine and potassium iodide, there is a reduction of bromine
to bromide ions.
In terms of electrons, what is meant by reduction?
[1 mark]
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8 (b) (ii) Complete the half equation for the oxidation of iodide ions to iodine molecules.
[2 marks]
2l–
8 (b) (iii) Explain, in terms of electronic structure, why fluorine is the most reactive element
in Group 7.
[3 marks]
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9
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Scientists found that a compound contained:
22.8% sodium; 21.8% boron; and 55.4% oxygen.
Use the percentages to calculate the empirical formula of the compound.
Relative atomic masses (Ar): B = 11; O = 16; Na = 23
To gain full marks you must show all your working.
[5 marks]
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Empirical formula = ............................................................
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10
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A company manufactures ethanol (C2H5OH).
The reaction for the process is:
C2H4(g) + H2O(g) C2H5OH(g)
∆H = – 45 kJ per mole
The temperature and pressure can be changed to increase the yield of ethanol
at equilibrium.
10 (a)
Explain what is meant by equilibrium.
[3 marks]
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10 (b) (i)
How would increasing the temperature change the yield of ethanol at equilibrium?
Give a reason for your answer.
[2 marks]
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10 (b) (ii) How would increasing the pressure change the yield of ethanol at equilibrium?
Give a reason for your answer.
[2 marks]
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10 (c)
A catalyst is added to increase the rate of the reaction.
Explain how adding a catalyst increases the rate of a chemical reaction.
[2 marks]
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END OF QUESTIONS
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Acknowledgement of copyright-holders and publishers
Permission to reproduce all copyright material has been applied for. In some cases, efforts to contact copyright-holders have been unsuccessful and
AQA will be happy to rectify any omissions of acknowledgements in future papers if notified.
Question 2:
photograph © Charles D. Winters/Science Photo Library
Copyright © 2014 AQA and its licensors. All rights reserved.
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