aqa chemistry h - collins...gcse chemistry h for this paper you must have: • a ruler • a...

Name:

11©HarperCollinsPublishers 2018 Chemistry Set B - Paper 1

GCSE

Chemistry H

For this paper you must have:

• a ruler • a calculator • the Periodic Table (found at the end of the paper).

Materials

Advice

• In all calculations, show clearly how you work out your answer.

Information

• There are 100 marks available on this paper.• The marks for questions are shown in brackets.• You are expected to use a calculator where appropriate.• You are reminded of the need for good English and clear presentation in your answers.• When answering questions 02.4 and 06.2 you need to make sure that your answer: – is clear, logical, sensibly structured – fully meets the requirements of the question – shows that each separate point or step supports the overall answer.

Instructions

• Answer all questions in the spaces provided.• Do all rough work in this book. Cross through any work you do not want to be marked.

Time allowed: 1 hour 45 minutes

SET B – Paper 1 Higher TierAuthor: Jill Faircloth

AQA

82721_Chem_H_Set B_P1_RP1.indd 182721_Chem_H_Set B_P1_RP1.indd 1 20/11/2018 11:4520/11/2018 11:45

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2 ©HarperCollinsPublishers 2018Chemistry Set B - Paper 1

01 An atom of fluorine has the symbol 199F

01.1 How many neutrons are in one atom of fluorine?

Tick one box.

0

9

10

19 [1 mark]

01.2 Draw the electronic structure of a single atom of fluorine on Figure 1.1

Figure 1.1

[2 marks]


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3Chemistry Set B - Paper 1©HarperCollinsPublishers 2018

01.3 Chlorine has two stable isotopes.

Table 1.1 gives some information about chlorine isotopes.

Table 1.1

Relative mass of isotope Relative abundance35 337 1

Calculate the relative atomic mass of chlorine.

Give the answer to 1 decimal place.

[2 marks]

01.4 Chlorine and fluorine are both members of Group 7

Name two physical properties of the elements of Group 7 that increase as you look

down the group.

1.

2. [2 marks]

Turn over >


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02.1 Describe what happens when atoms bond covalently.

Include the effect on each atom’s outer shell.

[2 marks]

02.2 Ammonia has the formula NH3

One nitrogen atom and three hydrogen atoms bond covalently to make a molecule of

ammonia.

Draw a dot and cross diagram that shows the bonds in a molecule of ammonia.

You need only show the outer electrons.

[2 marks]

02.3 Most molecules that are bonded covalently are liquid or gas at room temperature.

Diamond and graphite are both solid.

What makes diamond and graphite different from covalently bonded molecules?

Tick one box.

They are giant covalent structures.

Each atom is held in four covalent bonds.

They are bonded by delocalised electrons.

There are strong bonds between each small molecule. [1 mark]


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02.4 Diamond and graphite are both made of carbon atoms.

Table 2.1 shows some of the properties.

Table 2.1

Carbon allotrope Electrical conductivity Physical state

diamond poor hard solid

graphite good solid with greasy feel

Explain the differences in the properties of diamond and graphite.

Use your knowledge of their bonding and structure.

[6 marks]

Turn over >


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03 Metals are held together by a distinctive type of bonding called metallic bonding.

03.1 What is meant by the term metallic bonding?

[3 marks]

03.2 Which of the following properties are the result of metallic bonding?

Tick three boxes.

High solubility

High malleability

Low boiling point

High boiling point

Low thermal conductivity

High electrical conductivity [3 marks]

03.3 When alkali metals are put into water they produce a characteristic fizzing.

Write a balanced equation for the reaction that happens when potassium reacts with water

to make potassium hydroxide and hydrogen.

Include state symbols.

[3 marks]


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03.4 Unlike potassium, iron reacts very slowly with water.

Explain why you could predict this from the position of iron the Periodic Table.

[1 mark]

03.5 Suggest a method of speeding up the reaction between iron and water.

You do not need to include details of equipment or techniques used.

[1 mark]

Turn over >


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04 Metals can be arranged in a reactivity series.

04.1 Calcium, lithium and sodium all react with water to give off hydrogen.

A student is given small strips of each metal. All strips are the same size, and have the same

surface area.

Describe an experiment to establish their relative reactivity.

Include any safety precautions.

[3 marks]

04.2 Suggest how the student could adapt the experiment to include copper, iron, magnesium

and zinc.

[2 marks]

04.3 The student decides to check her results using displacement reactions.

She sets up three test tubes.

• The first contains 20 cm3 of copper nitrate solution

• The second contains 20 cm3 of iron nitrate solution

• The third contains 20 cm3 of zinc nitrate solution.

A 2 cm strip of magnesium is added to each one. The contents of each test tube are

observed.

The experiment is then repeated using strips of copper, iron and zinc.


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Table 4.1 shows her results.

Table 4.1

The metal strip displaces the metal in solution from

Metal coppernitrate

ironnitrate

magnesiumnitrate

zincnitrate

copper no no no

iron yes no no

magnesium yes yes yes

zinc yes yes no

Put the metals in order of reactivity, from most reactive to least reactive.

(most reactive)

(least reactive) [2 marks]

04.4 Explain the relative reactivity of potassium, lithium and magnesium in terms of their

electronic structure.

You may use the Periodic Table provided.

[3 marks]

04.5 Write an ionic equation to show the displacement of copper ions by magnesium metal.

Both copper and magnesium ions have a 2+ charge.

[1 mark]

Turn over >


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05 A student is investigating the reaction between marble chips and dilute hydrochloric

acid (HCl).

Marble chips are calcium carbonate (CaCO3).

The products are calcium chloride (CaCl2), water and carbon dioxide.

05.1 Complete the equation below to give a balanced equation for the reaction.

State symbols are not required.

+ CaCl2 + +

[1 mark]

05.2 What is the name of the scientific law that means chemical equations must always balance?

[1 mark]

05.3 Calculate the relative formula masses of CaCO3 and CaCl2


CaCO3

CaCl2

[2 marks]


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05.4 Four students want to compare the mass of the reactants and products in the reaction of

calcium carbonate with hydrochloric acid.

Each student uses a beaker with a mass of 150 g

They each measure in 10 g of dilute hydrochloric acid and 10 g of calcium carbonate.

Table 5.1 shows their results.

Table 5.1

Student Mass of beaker and product when reaction has finished (g)

1 163.02

2 162.73

3 162.15

4 161.98

Calculate the mean mass of the products once the reaction has finished.

Mean mass: g [2 marks]

05.5 Calculate the percentage uncertainty of the results.

Percentage uncertainty: % [2 marks]

Question 5 continues on the next page


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05.6 What has caused the reduction in mass of the beaker and contents during the reaction?

Tick one box.

Some water has evaporated.

The carbon dioxide produced has escaped.

The carbon dioxide produced has no mass.

The products are lighter than the reactants. [1 mark]

05.7 A student burnt 50 g of calcium in oxygen.

Write a balanced equation for the reaction.


[1 mark]

05.8 Calculate the mass of product that will be produced by burning 50 g of calcium in oxygen.

Mass of product: g [2 marks]


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06 Some students are investigating the reaction between sulfuric acid and sodium hydroxide

solution.

06.1 Write a balanced equation for the reaction between sulfuric acid (H2SO4) and sodium

hydroxide (NaOH).

The products are sodium sulfate (Na2SO4) and water.


[1 mark]



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06.2 Some of the students have the apparatus as shown in Figure 6.1

They also have a pipette and a funnel.

Figure 6.1

They want to find out how much sulfuric acid is required to neutralise 30 cm3 of sodium

hydroxide solution.

They want to obtain accurate results, and as safely as possible.

Describe the method, and the indicator, to use.

[6 marks]


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06.3 Two students worked together. They used a pH probe and plotted the change in pH as

sulfuric acid was added to 30 cm3 sodium hydroxide solution of concentration 0.15 mol/dm3

Figure 6.2 shows the students’ graph.

The end point is at pH 7

The neutralising volume of sulfuric acid was found from the graph at the end point of the

titration, when just sufficient acid has been added to neutralise the alkali.

Figure 6.2

Calculate the concentration of the sulfuric acid.

Use the balanced equation in question 06.1 and the data from the students’ graph.

[4 marks]

Turn over >


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07 An electrolytic cell is set up as shown in Figure 7.1

Figure 7.1

07.1 In an electrolytic cell, some parts are positively charged and others are negatively charged.

Draw four lines (one line from each part to its charge).

Part Charge

ions attracted to the anode

anode positive

ions attracted to the cathode negative

cathode

[2 marks]

07.2 The electrolyte is a solution of sodium chloride.

Identify all of the positive and negative ions in the solution.

[2 marks]


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07.3 What will be produced at each electrode when the power supply is turned on?

[2 marks]

07.4 Explain why some of the ions in the sodium chloride solution are discharged while

others remain in solution.

[2 marks]

07.5 Write the half equation for the reduction that occurs in this electrolysis.

[1 mark]

07.6 The experiment is repeated using a solution of copper sulfate as the electrolyte.

Write the half equation for the reduction that occurs in this electrolysis.

[2 marks]

Turn over >


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08 A group of students want to make magnesium sulfate by reacting magnesium with sulfuric acid.

They plan to remove unreacted magnesium by filtration, to concentrate the remaining solution,

and leave it to crystallise.

08.1 Some students use strips of magnesium, and some use powdered magnesium.

Which method will give the faster reaction?

Explain your answer.

[1 mark]

08.2 Some students warm the sulfuric acid, and some leave it at room temperature.

Which method will give the faster reaction?


[1 mark]

08.3 Write a balanced equation for this reaction.

[1 mark]


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08.4 Calculate the percentage atom economy for this reaction to make magnesium sulfate.


Percentage atom economy: % [3 marks]

08.5 Magnesium sulfate can also be made by reacting magnesium carbonate with sulfuric acid.

MgCO3 + H2SO4 MgSO4 + H2O + CO2

Based on atom economy only, decide which of the two methods, using magnesium or using

magnesium carbonate, is the most efficient.

Explain your decision.

[2 marks]

08.6 Name two other factors that could be considered when deciding on the best method.

1.

2. [1 mark]



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08.7 Calculate the theoretical yield of magnesium sulfate from 4 g of magnesium and

sulfuric acid.

Assume that magnesium is the limiting factor.

Theoretical yield: g [2 marks]

08.8 To compare the reactions, students also made magnesium sulfate from magnesium

carbonate and sulfuric acid.

They used 14 g of magnesium carbonate.

They were told that the theoretical yield was 20 g

The mean yield achieved by the group was 18.8 g

What was their percentage yield?

Percentage yield: % [2 marks]


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09 A student sets up a simple cell as shown in Figure 9.1

Figure 9.1

As the electrodes are put into the electrolyte, the voltmeter registers a current.

09.1 Explain how the current is produced.

[3 marks]

09.2 State which metal is oxidised and which reduced in this cell.

Oxidised:

Reduced: [1 mark]



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09.3 The students have several electrodes available.

The electrodes are all the same size but are made of different metals.

The students want to make a single cell with a higher voltage than the one in Figure 9.1

Describe a change they could make.


[2 marks]

09.4 Table 9.1 shows the voltages achieved when different metals are used as electrodes.

Table 9.1

chromium lead aluminium magnesium

chromium 0

lead –0.6 0

aluminium –0.9 –1.5 0

magnesium –1.6 –2.3 –0.9 0


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Using Table 9.1 and your knowledge of the reactivity series, put the four metals into order

of reactivity from most to least reactive.

Explain why you chose this order.

(most reactive)

(least reactive)

Explanation:

[3 marks]

09.5 Fuel cells operate using hydrogen as fuel, a catalyst and oxygen from the air.

Describe the two reactions that allow electricity to be generated without heat.

For each reaction, write down the half equation.

[4 marks]

END OF QUESTIONS


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Hh

yd

rog

en

34

56

71

2

0 o

r 8

Non-m

eta

ls

Meta

ls

Key

1 17 Li

lith

ium

3

9 Be

be

rylli

um

4

23

Na

so

diu

m

11

39 K

po

tassiu

m

19

85

Rb

rub

idiu

m

37

133

Cs

ca

esiu

m

55

[223]

Fr

fra

nc

ium

87

24

Mg

ma

gn

esiu

m

12

40

Ca

ca

lciu

m

20

88

Sr

str

on

tiu

m

38

137

Ba

ba

riu

m

56

[226]

Ra

rad

ium

88

45

Sc

sc

an

diu

m

21

89 Y

ytt

riu

m

39

139

La*

lan

tha

nu

m

57

[227]

Ac*

ac

tin

ium

89

48 Ti

tita

niu

m

22

91

Zr

zirc

on

ium

40

178

Hf

ha

fniu

m

72

[261]

Rf

ruth

erford

ium

104

51 V

va

na

diu

m

23

93

Nb

nio

biu

m

41

181

Ta

tan

talu

m

73

[262]

Db

du

bn

ium

105

52

Cr

ch

rom

ium

24

96

Mo

moly

bd

enum

42

184

Wtu

ng

ste

n

74

[266]

Sg

se

ab

org

ium

106

55

Mn

ma

ng

an

ese

25

[98]

Tc

tec

hn

etiu

m

43

186

Re

rhe

niu

m

75

[264]

Bh

bo

hriu

m

107

56

Fe

iro

n

26

101

Ru

ruth

en

ium

44

190

Os

osm

ium

76

[277]

Hs

ha

ssiu

m

108

59

Co

co

ba

lt

27

103

Rh

rho

diu

m

45

192

Iririd

ium

77

[268]

Mt

me

itn

eriu

m

109

59

Ni

nic

ke

l

28

106

Pd

pa

llad

ium

46

195

Pt

pla

tin

um

78

[271]

Ds

darm

stad

tium

110

63.5

Cu

co

pp

er

29

108

Ag

silv

er

47

197

Au

go

ld

79

[272]

Rg

roe

ntg

en

ium

111

65

Zn

zin

c

30

112

Cd

ca

dm

ium

48

201

Hg

me

rcu

ry

80

11 B

bo

ron

5 27

Al

alu

min

ium

13

70

Ga

ga

lliu

m

31

115

Inin

diu

m

49

204

Tl

tha

lliu

m

81

12 C

ca

rbo

n

6 28

Si

sili

co

n

14

73

Ge

ge

rma

niu

m

32

119

Sn

tin

50

207

Pb

lea

d

82

14 N

nitro

ge

n

7 31 P

ph

osp

ho

rus

15

75

As

ars

en

ic

33

122

Sb

an

tim

on

y

51

209

Bi

bis

mu

th

83

16 O

oxyg

en

8 32 S

su

lfu

r

16

79

Se

se

len

ium

34

128

Te

tellu

riu

m

52

[209]

Po

po

lon

ium

84

19 F

flu

orin

e

9

35.5

Cl

ch

lorin

e

17

80

Br

bro

min

e

35

127 I

iod

ine

53

[210]

At

asta

tin

e

85

20

Ne

ne

on

10

40

Ar

arg

on

18

84

Kr

kry

pto

n

36

131

Xe

xe

no

n

54

[222]

Rn

rad

on

864 He

he

lium

2

*The lanth

anid

es (

ato

mic

num

bers

58–71)

and

the a

ctinid

es (

ato

mic

num

bers

90–103)

have b

een o

mitte

d.

The r

ela

tive a

tom

ic m

asses o

f cop

per

and

chlo

rine h

ave n

ot b

een r

ound

ed

to the n

eare

st w

hole

num

ber.

Na

me

Ato

mic

/pro

ton

nu

mb

er

Ato

mic

sy

mb

ol

Re

lati

ve

ato

mic

ma

ss

[294]

Uu

ou

nu

no

ctiu

m

118

[285]

Cn

co

pe

rnic

ium

112

[286]

Uu

tu

nu

ntr

ium

113

[289]

Fl

fle

roviu

m

114

[289]

Uu

pu

nu

np

en

tiu

m

115

[293]

Lv

live

rmo

riu

m

116

[294]

Uu

su

nu

nse

ptiu

m

117

The Periodic Table


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aqa chemistry h - collins...gcse chemistry h for this paper you must have: • a ruler • a...

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