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8402/1G/KL/101792/Jun14/E4(Jun148402101)
AQA Level 1/2 Certificate
June 2014
Chemistry 8402/1
Paper 1
Thursday 15 May 2014 9.00 am to 10.30 am
For this paper you must have: a ruler a calculator the periodic table (enclosed).
Time allowed 1 hour 30 minutes
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.
Centre Number Candidate Number
Surname
Other Names
Candidate Signature
For Examiner’s Use
Examiner’s Initials
Question Mark
1
2
3
4
5
6
7
8
9
10
TOTALA
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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 carbon sodium
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1 (b) Figure 2 shows a compound of G and hydrogen.
Figure 2
G
H
H 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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2 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 nitrate + ........................................ lead iodide + ........................................
2 (a) (iv) How is solid lead iodide separated from the solution?
Draw a ring around the correct answer.[1 mark]
Distillation Electrolysis Filtration
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2 (b) 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
X
Water
Crystal ofpotassiumiodide
Crystal oflead nitrate Y
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) The symbols for seven different elements are shown in Figure 6.
Figure 6
Be
He
ArS
Ca Fe
Na
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]
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3 (a) (ii) a transition metal[1 mark]
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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) A teacher put a cube of sodium metal into water containing universal indicator, as shown in Figure 7.
Figure 7
Sodium metal
Water withuniversal indicator
The equation for the reaction is:
2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
sodium + water sodium hydroxide
+ hydrogen
3 (b) (i) 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]
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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) 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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4 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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5 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
Magnesium
Heat
Unreacted steamand hydrogen outSteam in
Glass tube
5 (a) (i) The hydrogen produced was collected.
Describe how to test the gas to show that it is hydrogen.[2 marks]
Test ....................................................................................................................................
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Result .................................................................................................................................
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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) MgO(s) + H2(g)
5 (b) (i) 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 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
Pure water
Electrodes
Conductivity meter
d.c. power supply
–+
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
Relative conductivity of solution
0 01 1002 1203 3104 4005 5106 5907 7108 800
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6 (a) (i) 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
2 3 400
100
200
300
400
500
600
700
800
1Number of drops of sodium chloride added
Relativeconductivityof solution
5 6 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 .................................................................____10
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7 Figure 13 shows the displayed structures of five organic compounds,A, B, C, D and E.
Figure 13
DH
CH
H
H
C
H
H
EH
CH
H
C
O H
O
AH
CH
H
H
C
H
O H
CBH
C
H
CH H
H
H
C
H
H
C
H
O
C O
H
H
C
H
7 (a) 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 3C2H4 + C8H18
7 (b) (i) 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 ....................................................................................................................................
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Result .................................................................................................................................
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7 (d) Compound B is ethene.
Complete the equation to show the formation of poly(ethene) from ethene.[3 marks]
H
Cn
H
H
C
H____14
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8 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
H
Li Be B C N O F
Na Mg Al Si P S Cl
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) 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 2KBr + I2
8 (b) (i) 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 elementin Group 7.
[3 marks]
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9 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 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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