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Double Science (Chemistry) Retrospective Revision guide

Last updated over 1 year ago

130 questions

Note from the author:

Instructions

1 Principles of chemistry

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2 Inorganic chemistry

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3 Physical chemistry

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4 Organic chemistry

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The iGCSE Edexcel Double Award Science (Chemistry) syllabus for students to RAG rate to aid with revision

(a) States of matter

Question 1

1.

Question 2

2.

Question 3

3.

Question 4

4.

(b) Elements, compounds and mixtures

Question 5

5.

Question 6

6.

Question 7

7.

Question 8

8.

Question 9

9.

Question 10

10.

(c) Atomic structure

Question 11

11.

Question 12

12.

Question 13

13.

Question 14

14.

(d) The Periodic Table

Question 15

15.

Question 16

16.

Question 17

17.

Question 18

18.

Question 19

19.

Question 20

20.

Question 21

21.

(e) Chemical formulae, equations and calculations

Question 22

22.

Question 23

23.

Question 24

24.

Question 25

25.

Question 26

26.

Question 27

27.

Question 28

28.

Question 29

29.

Question 30

30.

Question 31

31.

(f) Ionic bonding

Question 32

32.

Question 33

33.

Question 34

34.

Question 35

35.

Question 36

36.

Question 37

37.

Question 38

38.

(g) Covalent bonding

Question 39

39.

Question 40

40.

Question 41

41.

Question 42

42.

Question 43

43.

Question 44

44.

Question 45

45.

Question 46

46.

(a) Group 1 (alkali metals) – lithium, sodium and potassium

Question 47

47.

Question 48

48.

Question 49

49.

(b) Group 7 (halogens) – chlorine, bromine and iodine

Question 50

50.

Question 51

51.

Question 52

52.

(c) Gases in the atmosphere

Question 53

53.

Question 54

54.

Question 55

55.

Question 56

56.

Question 57

57.

Question 58

58.

(d) Reactivity series

Question 59

59.

Question 60

60.

Question 61

61.

Question 62

62.

Question 63

63.

Question 64

64.

Question 65

65.

(e) Acids, alkalis and titrations

Question 66

66.

Question 67

67.

Question 68

68.

Question 69

69.

Question 70

70.

f) Acids, bases and salt preparations

Question 71

71.

Question 72

72.

Question 73

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Question 74

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Question 75

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Question 76

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Question 77

77.

(g) Chemical tests

Question 78

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Question 79

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Question 80

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Question 81

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Question 82

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Question 83

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Question 84

84.

(a) Energetics

Question 85

85.

Question 86

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Question 87

87.

Question 88

88.

Question 89

89.

(b) Rates of reaction

Question 90

90.

Question 91

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Question 92

92.

Question 93

93.

Question 94

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Question 95

95.

Question 96

96.

(c) Reversible reactions and equilibria

Question 97

97.

Question 98

98.

(a) Introduction

Question 99

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Question 100

100.

Question 101

101.

Question 102

102.

Question 103

103.

Question 104

104.

(b) Crude oil

Question 105

105.

Question 106

106.

Question 107

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Question 108

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Question 109

109.

Question 110

110.

Question 111

111.

Question 112

112.

Question 113

113.

Question 114

114.

Question 115

115.

Question 116

116.

(c) Alkanes

Question 117

117.

Question 118

118.

Question 119

119.

Question 120

120.

(d) Alkenes

Question 121

121.

Question 122

122.

Question 123

123.

Question 124

124.

Question 125

125.

Question 126

126.

(e) Synthetic polymers

Question 127

127.

Question 128

128.

Question 129

129.

Question 130

130.

1.1 
understand the three states of matter in terms of the arrangement, movement and 
energy of the particles

I know none of this

I know some of this

I am confident in this

1.2 
understand the interconversions between the three states of matter in terms of:
• the names of the interconversions
• how they are achieved
• the changes in arrangement, movement and energy of the particles.

I know none of this

I know some of this

I am confident in this

1.3 
understand how the results of experiments involving the dilution of coloured solutions 
and diffusion of gases can be explained

I know none of this

I know some of this

I am confident in this

1.4 
know what is meant by the terms:
• solvent
• solute
• solution
• saturated solution.

I know none of this

I know some of this

I am confident in this

1.8 
understand how to classify a substance as an element, compound or mixture

I know none of this

I know some of this

I am confident in this

1.9 
understand that a pure substance has a fixed melting and boiling point, but that a 
mixture may melt or boil over a range of temperatures

I know none of this

I know some of this

I am confident in this

1.10 
describe these experimental techniques for the separation of mixtures:
• simple distillation
• fractional distillation
• filtration
• crystallisation
• paper chromatography.

I know none of this

I know some of this

I am confident in this

1.11 
understand how a chromatogram provides information about the composition of a 
mixture

I know none of this

I know some of this

I am confident in this

1.12 
understand how to use the calculation of Rf values to identify the components of a 
mixture

I know none of this

I know some of this

I am confident in this

1.13 
practical: investigate paper chromatography using inks/food colourings

I know none of this

I know some of this

I am confident in this

1.14 
know what is meant by the terms atom and molecule

I know none of this

I know some of this

I am confident in this

1.15 
know the structure of an atom in terms of the positions, relative masses and relative 
charges of sub-atomic particles

I know none of this

I know some of this

I am confident in this

1.16 
know what is meant by the terms atomic number, mass number, isotopes and relative 
atomic mass (Ar)

I know none of this

I know some of this

I am confident in this

1.17 
be able to calculate the relative atomic mass of an element (Ar) from isotopic 
abundances

I know none of this

I know some of this

I am confident in this

1.18 
understand how elements are arranged in the Periodic Table:
• in order of atomic number
• in groups and periods.

I know none of this

I know some of this

I am confident in this

1.19 
understand how to deduce the electronic configurations of the first 20 elements from 
their positions in the Periodic Table

I know none of this

I know some of this

I am confident in this

1.20 
understand how to use electrical conductivity and the acid-base character of oxides to 
classify elements as metals or non-metals

I know none of this

I know some of this

I am confident in this

1.21 
identify an element as a metal or a non-metal according to its position in the Periodic 
Table

I know none of this

I know some of this

I am confident in this

1.22 
understand how the electronic configuration of a main group element is related to its 
position in the Periodic Table

I know none of this

I know some of this

I am confident in this

1.23 
understand why elements in the same group of the Periodic Table have similar 
chemical properties

I know none of this

I know some of this

I am confident in this

1.24 
understand why the noble gases (Group 0) do not readily react

I know none of this

I know some of this

I am confident in this

1.25 
write word equations and balanced chemical equations (including state symbols): 
• for reactions studied in this specification
• for unfamiliar reactions where suitable information is provided

I know none of this

I know some of this

I am confident in this

1.26 
calculate relative formula masses (including relative molecular masses) (Mr) from 
relative atomic masses (Ar)

I know none of this

I know some of this

I am confident in this

1.27 
know that the mole (mol) is the unit for the amount of a substance

I know none of this

I know some of this

I am confident in this

1.28 
understand how to carry out calculations involving amount of substance, relative 
atomic mass (Ar) and relative formula mass (Mr)

I know none of this

I know some of this

I am confident in this

1.29 
calculate reacting masses using experimental data and chemical equations

I know none of this

I know some of this

I am confident in this

1.30 
calculate percentage yield

I know none of this

I know some of this

I am confident in this

1.31 
understand how the formulae of simple compounds can be obtained experimentally, 
including metal oxides, water and salts containing water of crystallisation

I know none of this

I know some of this

I am confident in this

1.32 
know what is meant by the terms empirical formula and molecular formula

I know none of this

I know some of this

I am confident in this

1.33 
calculate empirical and molecular formulae from experimental data

I know none of this

I know some of this

I am confident in this

1.36 
practical: know how to determine the formula of a metal oxide by combustion 
(e.g. magnesium oxide) or by reduction (e.g. copper(II) oxide)

I know none of this

I know some of this

I am confident in this

1.37 
understand how ions are formed by electron loss or gain

I know none of this

I know some of this

I am confident in this

1.38 know the charges of these ions:
• metals in Groups 1, 2 and 3
• non-metals in Groups 5, 6 and 7
• Ag+, Cu2+, Fe2+, Fe3+, Pb2+, Zn2+
• hydrogen (H+), hydroxide (OH–), ammonium (NH4+), carbonate (CO32–), nitrate 
(NO3-), sulfate (SO42–).

I know none of this

I know some of this

I am confident in this

1.39 
write formulae for compounds formed between the ions listed above

I know none of this

I know some of this

I am confident in this

1.40 
draw dot-and-cross diagrams to show the formation of ionic compounds by electron 
transfer, limited to combinations of elements from Groups 1, 2, 3 and 5, 6, 7 
only outer electrons need be shown

I know none of this

I know some of this

I am confident in this

1.41 
understand ionic bonding in terms of electrostatic attractions

I know none of this

I know some of this

I am confident in this

1.42 
understand why compounds with giant ionic lattices have high melting and boiling points

I know none of this

I know some of this

I am confident in this

1.43 
know that ionic compounds do not conduct electricity when solid, but do conduct 
electricity when molten and in aqueous solution

I know none of this

I know some of this

I am confident in this

1.44 
know that a covalent bond is formed between atoms by the sharing of a pair of 
electrons

I know none of this

I know some of this

I am confident in this

1.45 
understand covalent bonds in terms of electrostatic attractions

I know none of this

I know some of this

I am confident in this

1.46 
understand how to use dot-and-cross diagrams to represent covalent bonds in:
• diatomic molecules, including hydrogen, oxygen, nitrogen, halogens and hydrogen 
halides
• inorganic molecules including water, ammonia and carbon dioxide 
• organic molecules containing up to two carbon atoms, including methane, ethane, 
ethene and those containing halogen atoms.

I know none of this

I know some of this

I am confident in this

1.47 
explain why substances with a simple molecular structures are gases or liquids, or 
solids with low melting and boiling points
the term intermolecular forces of attraction can be used to represent all forces 
between molecules

I know none of this

I know some of this

I am confident in this

1.48 
explain why the melting and boiling points of substances with simple molecular 
structures increase, in general, with increasing relative molecular mass

I know none of this

I know some of this

I am confident in this

1.49 
explain why substances with giant covalent structures are solids with high melting and 
boiling points

I know none of this

I know some of this

I am confident in this

1.50 
explain how the structures of diamond, graphite and C60 fullerene influence their 
physical properties, including electrical conductivity and hardness

I know none of this

I know some of this

I am confident in this

1.51 
know that covalent compounds do not usually conduct electricity

I know none of this

I know some of this

I am confident in this

2.1 
understand how the similarities in the reactions of these elements with water provide 
evidence for their recognition as a family of elements

I know none of this

I know some of this

I am confident in this

2.2 
understand how the differences between the reactions of these elements with air and 
water provide evidence for the trend in reactivity in Group 1

I know none of this

I know some of this

I am confident in this

2.3 
use knowledge of trends in Group 1 to predict the properties of other alkali metals

I know none of this

I know some of this

I am confident in this

2.5 
know the colours, physical states (at room temperature) and trends in physical 
properties of these elements

I know none of this

I know some of this

I am confident in this

2.6 
use knowledge of trends in Group 7 to predict the properties of other halogens

I know none of this

I know some of this

I am confident in this

2.7 
understand how displacement reactions involving halogens and halides provide 
evidence for the trend in reactivity in Group 7

I know none of this

I know some of this

I am confident in this

2.9 
know the approximate percentages by volume of the four most abundant gases in dry 
air

I know none of this

I know some of this

I am confident in this

2.10 
understand how to determine the percentage by volume of oxygen in air using
experiments involving the reactions of metals (e.g. iron) and non-metals
(e.g. phosphorus) with air

I know none of this

I know some of this

I am confident in this

2.11 
describe the combustion of elements in oxygen, including magnesium, hydrogen and
sulfur

I know none of this

I know some of this

I am confident in this

2.12 
describe the formation of carbon dioxide from the thermal decomposition of metal 
carbonates, including copper(II) carbonate

I know none of this

I know some of this

I am confident in this

2.13 
know that carbon dioxide is a greenhouse gas and that increasing amounts in the 
atmosphere may contribute to climate change

I know none of this

I know some of this

I am confident in this

2.14 
practical: determine the approximate percentage by volume of oxygen in air using a 
metal or a non-metal

I know none of this

I know some of this

I am confident in this

2.15 
understand how metals can be arranged in a reactivity series based on their reactions 
with:
• water
• dilute hydrochloric or sulfuric acid.

I know none of this

I know some of this

I am confident in this

2.16 
understand how metals can be arranged in a reactivity series based on their 
displacement reactions between:
• metals and metal oxides
• metals and aqueous solutions of metal salts.

I know none of this

I know some of this

I am confident in this

2.17 
know the order of reactivity of these metals: potassium, sodium, lithium, calcium, 
magnesium, aluminium, zinc, iron, copper, silver, gold

I know none of this

I know some of this

I am confident in this

2.18 
know the conditions under which iron rusts

I know none of this

I know some of this

I am confident in this

2.19 
understand how the rusting of iron may be prevented by:
• barrier methods
• galvanising 
• sacrificial protection.

I know none of this

I know some of this

I am confident in this

2.20 
 the terms:
• oxidation
• reduction
• redox
• oxidising agent
• reducing agent
in terms of gain or loss of oxygen and loss or gain of electrons.

I know none of this

I know some of this

I am confident in this

2.21 
practical: investigate reactions between dilute hydrochloric and sulfuric acids and 
metals (e.g. magnesium, zinc and iron)

I know none of this

I know some of this

I am confident in this

2.28 
describe the use of litmus, phenolphthalein and methyl orange to distinguish between 
acidic and alkaline solutions

I know none of this

I know some of this

I am confident in this

2.29 
understand how to use the pH scale, from 0–14, can be used to classify solutions as 
strongly acidic (0–3), weakly acidic (4–6), neutral (7), weakly alkaline (8–10) and 
strongly alkaline (11–14)

I know none of this

I know some of this

I am confident in this

2.30 
describe the use of universal indicator to measure the approximate pH value of an 
aqueous solution

I know none of this

I know some of this

I am confident in this

2.31 
know that acids in aqueous solution are a source of hydrogen ions and alkalis in a 
aqueous solution are a source of hydroxide ions

I know none of this

I know some of this

I am confident in this

2.32 
know that alkalis can neutralise acids

I know none of this

I know some of this

I am confident in this

2.34 
know the general rules for predicting the solubility of ionic compounds in water:
• common sodium, potassium and ammonium compounds are soluble
• all nitrates are soluble
• common chlorides are soluble, except those of silver and lead(II)
• common sulfates are soluble, except for those of barium, calcium and lead(II)
• common carbonates are insoluble, except for those of sodium, potassium and 
ammonium
• common hydroxides are insoluble except for those of sodium, potassium and 
calcium (calcium hydroxide is slightly soluble).

I know none of this

I know some of this

I am confident in this

2.35 
understand acids and bases in terms of proton transfer

I know none of this

I know some of this

I am confident in this

2.36 
understand that an acid is a proton donor and a base is a proton acceptor

I know none of this

I know some of this

I am confident in this

2.37 
describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals, 
bases and metal carbonates (excluding the reactions between nitric acid and metals) 
to form salts

I know none of this

I know some of this

I am confident in this

2.38 
know that metal oxides, metal hydroxides and ammonia can act as bases, and that 
alkalis are bases that are soluble in water

I know none of this

I know some of this

I am confident in this

2.39 
describe an experiment to prepare a pure, dry sample of a soluble salt, starting from 
an insoluble reactant 

I know none of this

I know some of this

I am confident in this

2.42 
practical: prepare a sample of pure, dry hydrated copper(II) sulfate crystals starting 
from copper(II) oxide

I know none of this

I know some of this

I am confident in this

2.44 
describe tests for these gases:
• hydrogen
• oxygen
• carbon dioxide
• ammonia
• chlorine.

I know none of this

I know some of this

I am confident in this

2.45 
describe how to carry out a flame test

I know none of this

I know some of this

I am confident in this

2.46 
know the colours formed in flame tests for these cations:
• Li+ is red 
• Na+ is yellow
• K+ is lilac
• Ca2+ is orange-red
• Cu2+ is blue-green.

I know none of this

I know some of this

I am confident in this

2.47 
describe tests for these cations:
• NH4+ using sodium hydroxide solution and identifying the gas evolved
• Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution.

I know none of this

I know some of this

I am confident in this

2.48 
describe tests for these anions:
• Cl–, Br– and I– using acidified silver nitrate solution
• SO42– using acidified barium chloride solution
• CO32– using hydrochloric acid and identifying the gas evolved.

I know none of this

I know some of this

I am confident in this

2.49 
describe a test for the presence of water using anhydrous copper(II) sulfate

I know none of this

I know some of this

I am confident in this

2.50 
describe a physical test to show whether a sample of water is pure

I know none of this

I know some of this

I am confident in this

3.1 
know that chemical reactions in which heat energy is given out are described as 
exothermic, and those in which heat energy is taken in are described as endothermic

I know none of this

I know some of this

I am confident in this

3.2 
describe simple calorimetry experiments for reactions such as combustion,
displacement, dissolving and neutralisation

I know none of this

I know some of this

I am confident in this

3.3 
calculate the heat energy change from a measured temperature change using the 
expression Q = mcΔT

I know none of this

I know some of this

I am confident in this

3.4 
calculate the molar enthalpy change (ΔH) from the heat energy change, Q

I know none of this

I know some of this

I am confident in this

3.8 
practical: investigate temperature changes accompanying some of the following types 
of change:
• salts dissolving in water
• neutralisation reactions
• displacement reactions
• combustion reactions.

I know none of this

I know some of this

I am confident in this

3.9 
describe experiments to investigate the effects of changes in surface area of a solid, 
concentration of a solution, temperature and the use of a catalyst on the rate of a 
reaction

I know none of this

I know some of this

I am confident in this

3.10 
describe the effects of changes in surface area of a solid, concentration of a solution, 
pressure of a gas, temperature and the use of a catalyst on the rate of a reaction

I know none of this

I know some of this

I am confident in this

3.11 
explain the effects of changes in surface area of a solid, concentration of a solution, 
pressure of a gas and temperature on the rate of a reaction in terms of particle 
collision theory

I know none of this

I know some of this

I am confident in this

3.12 
know that a catalyst is a substance that increases the rate of a reaction, but is 
chemically unchanged at the end of the reaction

I know none of this

I know some of this

I am confident in this

3.13 
know that a catalyst works by providing an alternative pathway with lower activation 
energy

I know none of this

I know some of this

I am confident in this

3.15 
practical: investigate the effect of changing the surface area of marble chips and of 
changing the concentration of hydrochloric acid on the rate of reaction between 
marble chips and dilute hydrochloric acid

I know none of this

I know some of this

I am confident in this

3.16 
practical: investigate the effect of different solids on the catalytic decomposition of 
hydrogen peroxide solution

I know none of this

I know some of this

I am confident in this

3.17 
know that some reactions are reversible and this is indicated by the symbol ⇌ in 
equations

I know none of this

I know some of this

I am confident in this

3.18 
describe reversible reactions such as the dehydration of hydrated copper(II) sulfate 
and the effect of heat on ammonium chloride

I know none of this

I know some of this

I am confident in this

4.1 
know that a hydrocarbon is a compound of hydrogen and carbon only

I know none of this

I know some of this

I am confident in this

4.2 
understand how to represent organic molecules using empirical formulae, molecular 
formulae, general formulae, structural formulae and displayed formulae

I know none of this

I know some of this

I am confident in this

4.3 
know what is meant by the terms homologous series, functional group and isomerism

I know none of this

I know some of this

I am confident in this

4.4 
understand how to name compounds relevant to this specification using the rules of 
International Union of Pure and Applied Chemistry (IUPAC) nomenclature
students will be expected to name compounds containing up to six carbon atoms

I know none of this

I know some of this

I am confident in this

4.5 
understand how to write the possible structural and displayed formulae of an organic 
molecule given its molecular formula

I know none of this

I know some of this

I am confident in this

4.6 
understand how to classify reactions of organic compounds as substitution, addition 
and combustion
knowledge of reaction mechanisms is not required

I know none of this

I know some of this

I am confident in this

4.7 
know that crude oil is a mixture of hydrocarbons

I know none of this

I know some of this

I am confident in this

4.8 
describe how the industrial process of fractional distillation separates crude oil into 
fractions

I know none of this

I know some of this

I am confident in this

4.9 
know the names and uses of the main fractions obtained from crude oil:
refinery gases, gasoline, kerosene, diesel, fuel oil and bitumen

I know none of this

I know some of this

I am confident in this

4.10 
know the trend in colour, boiling point and viscosity of the main fractions

I know none of this

I know some of this

I am confident in this

4.11 
know that a fuel is a substance that, when burned, releases heat energy

I know none of this

I know some of this

I am confident in this

4.12 
know the possible products of complete and incomplete combustion of hydrocarbons 
with oxygen in the air

I know none of this

I know some of this

I am confident in this

4.13 
understand why carbon monoxide is poisonous, in terms of its effect on the capacity 
of blood to transport oxygen
references to haemoglobin are not required

I know none of this

I know some of this

I am confident in this

4.14 
know that, in car engines, the temperature reached is high enough to allow nitrogen 
and oxygen from air to react, forming oxides of nitrogen

I know none of this

I know some of this

I am confident in this

4.15 
explain how the combustion of some impurities in hydrocarbon fuels results in the
formation of sulfur dioxide

I know none of this

I know some of this

I am confident in this

4.16 
understand how sulfur dioxide and oxides of nitrogen contribute to acid rain

I know none of this

I know some of this

I am confident in this

4.17 
describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes 
by catalytic cracking (using silica or alumina as the catalyst and a temperature in the 
range of 600–700 ºC)

I know none of this

I know some of this

I am confident in this

4.18 
explain why cracking is necessary, in terms of the balance between supply and
demand for different fractions

I know none of this

I know some of this

I am confident in this

4.19 
know the general formula for alkanes

I know none of this

I know some of this

I am confident in this

4.20 
explain why alkanes are classified as saturated hydrocarbons

I know none of this

I know some of this

I am confident in this

4.21 
understand how to draw the structural and displayed formulae for alkanes with up to 
five carbon atoms in the molecule, and to name the unbranched-chain isomers

I know none of this

I know some of this

I am confident in this

4.22 
describe the reactions of alkanes with halogens in the presence of ultraviolet
radiation, limited to mono-substitution
knowledge of reaction mechanisms is not required

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4.23 
know that alkenes contain the functional group >C=C<

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4.24 
know the general formula for alkenes

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4.25 
explain why alkenes are classified as unsaturated hydrocarbons

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4.26 
understand how to draw the structural and displayed formulae for alkenes with up to 
four carbon atoms in the molecule, and name the unbranched-chain isomers
knowledge of cis/trans or E/Z notation is not required

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4.27 
describe the reactions of alkenes with bromine to produce dibromoalkanes

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4.28 
describe how bromine water can be used to distinguish between an alkane and an 
alkene

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4.44 
know that an addition polymer is formed by joining up many small molecules called 
monomers

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4.45 
understand how to draw the repeat unit of an addition polymer, including 
poly(ethene), poly(propene), poly(chloroethene) and (poly)tetrafluoroethene

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4.46 
understand how to deduce the structure of a monomer from the repeat unit of an 
addition polymer and vice versa

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4.47 
explain problems in the disposal of addition polymers, including:
• their inertness and inability to biodegrade
• the production of toxic gases when they are burned.

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