Page | 1

Topic Page

Titrations 2

Organic Practicals 16

Other Practicals 29

Elements and Periodic Table 43

Atomic Structure 44

Electronic structure of atoms 50

Ionic and Covalent Bonding 59

Shapes of Molecules and Intermolecular Forces

64

Oxidation and Reduction 68

Radioactivity 72

Gas Laws and the Mole 77

Acids and Bases 81

pH 84

Calculations based on Chemical equations

88

Hydrocarbons & Thermochemistry

93

Organic Chemistry 101

Rates of Reaction 113

Chemical Equilibrium 119

Water 126

Page | 2

Titrations

2018 Water

Page | 3

2017 Redox

Page | 4

2016 Acid / base

Page | 5

2015 Redox

Page | 6

2014 Acid / Base

Page | 7

2013 Water

Page | 8

2012 Acid /Base

Page | 9

2011 Redox

Page | 10

2010 Water

2009 Redox

Page | 11

2008 Acid / Base

2007 Redox

Page | 12

2006 Acid / Base

Page | 13

2005 Water

Page | 14

2004 Water

2003 Redox

Page | 15

2002 Acid /Base

Page | 16

Organic Practicals

2018

Page | 17

2017

Page | 18

2016

Page | 19

2015

Page | 20

2014

Page | 21

2013

2012

Page | 22

2011

2010

Page | 23

2009

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2008

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2007

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2006

2005

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2004

2003

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2002

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Other Experiments

2018

Page | 30

2017

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2016

Page | 32

2015

Page | 33

2014

2013

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2012

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2011

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2010

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2009

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2008

2007

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2006

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2005

2004

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2003

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2002

Page | 43

Elements and the periodic Table

2018

No question

2017

4(a) Why did Mendeleev place tellurium before iodine in his periodic table of the elements?

2015

2013 Q5

2011 Q5

Page | 44

2010

Q4 (b) State two differences between Mendeleev’s periodic table and the modern periodic table

of the elements.

2008 Q4

2006 Q4

(f) What contribution did Newlands make to the systematic arrangement of the elements known to

him?

2005 Q4

(d) What contribution did Dobereiner make to the systematic arrangement of the elements?

Atomic Structure

2018 Q4

Page | 45

2017 Q10

Page | 46

2016 Q4

2015 Q4

2014 Q4

(b) Describe the structure of Thomson’s ‘plum pudding’ model of the atom.

Page | 47

Q10

2013 Q4

2012 Q4

(c) Define relative atomic mass.

Q11

Page | 48

2011 Q5

(a) Define (i) atomic number, (ii) relative atomic mass.

Q10

2010

2009 Q4

Q10

Page | 49

2007 Q11

2006 Q10

2004 Q4

(a) Define relative atomic mass.

Page | 50

Electronic Structure of Atoms

2018 Q4

(b) State and give the reason for the trend in atomic radii across the second period

of the periodic table.

(c) Write the electron configuration (s, p, etc) for an iron atom.

Page | 51

2017

Q4 (b) Identify the main energy levels involved in the electron transition that gives rise to the first

(red) line of the Balmer series in the emission spectrum of the hydrogen atom.

Page | 52

2016

Q4

Q5

Page | 53

2015

Q4

Q5

2014

Q4

Page | 54

2013 Q4

Q5

Page | 55

Q11

2012 Q4

(a) State the number of (i) sub-levels (subshells), (ii) orbitals, occupied by electrons in an argon atom

in its ground state.

Q5

2011 Q5

Page | 56

2010

Q4

(a) Write the electron configuration (s, p, etc.) of the oxygen (oxide) ion (O2–).

Q5

2009 Q4

Q5

Page | 57

2008 Q4

Q10

2007 Q5

2006 Q4

(a) Write the electron configuration (s, p, etc.) of a chromium atom in its

ground state.

Q5

Page | 58

2005 Q5

Q10

2004 Q5

Page | 59

Q10

Ionic and Covalent Bonding

2018 Q11

2017 Q4

Page | 60

Q11

2016 Q4

2015

Q11

Page | 61

2014

Q4 How many (i) sigma bonds, (ii) pi bonds, result from sharing of the valence electrons between the

atoms in a molecule of nitrogen?

Q11 (a)

2012

Q4 (d) Distinguish between sigma (σ) and pi (π) covalent bonding

Q5

Page | 62

2011 Q11

2010 Q4

(g) Distinguish between sigma (σ) and pi (π) covalent bonding.

Q10

2008 Q5

Page | 63

2007

Q5 (b)

2006 Q5 (b)

2005 Q5

2004 Q5

Page | 64

Shapes of Molecules and Intermolecular forces

2018 Q11

2017

Q4(g) Identify, in ammonia, the type of (i) intramolecular bonding, (ii) intermolecular forces,

present.

2016

Page | 65

2015

Q4

Q8

2014

Q11(a)

2013 Q4

Q10

Page | 66

2012 Q5

2011 Q4

(b) Give two possible shapes for a covalent molecule of general formula AB2.

2010 Q10

Q4

(c) What are the two possible shapes of molecules of general formula QX2?

2009 Q11 (b)

Page | 67

2008

Q4 (g) Account for the difference in bond angle between water (104.5 º) and methane (109.5 º).

Q5

2007 Q5

2005 Q4

(b) What are the possible shapes for molecules of general formula AB2?

2004 Q5

Page | 68

Oxidation and Reduction

2018 Q4

2017 Q4

2016 Q10

2015 Q10

Page | 69

2014 Q10

2013 Q10

2012 Q4

(h) Name (i) the gas, (ii) the ion, formed at the negative electrode when aqueous sodium sulfate

solution is electrolysed.

2012 Q10

Page | 70

2011 Q4

2010 Q10

Q11

2009 Q10

Page | 71

2008 Q10

2007 Q10

2006 Q10

2005 Q11

Page | 72

2004 Q4

(g) What is the oxidation number (i) of oxygen in H2O2 and (ii) of bromine in KBrO3?

(i) State and explain the colour observed at the negative electrode in the electrolysis of aqueous

potassium

iodide, containing a little phenolphthalein indicator, using inert electrodes.

Radioactivity

2018 Q5

2017 Q4

Page | 73

Q10

2016 Q10

Page | 74

2015 Q4

Q5

2014 Q4

2013 Q10

2012

Q4 (b) Write a balanced nuclear reaction for the beta particle decay of iodine-131.

Q11

Page | 75

2011

Q4

(a) Give two properties of cathode rays.

Q10

2010 Q11

2009 Q4

(b) What change occurs in the nucleus of an atom when it undergoes beta emission?

Page | 76

2007 Q11

2005 Q5

2004 Q11

Page | 77

Gas Laws and the Mole

2018 Q4

(d) Give two reasons why real gases deviate from ideal behaviour at high pressures and low temperatures.

2017 Q4

(e) State Avogadro’s law.

2016 Q4

(f) What was Gay-Lussac’s observation about reactions involving gaseous reactants and

products?

(g) The structure of the cinnamaldehyde molecule is shown.

How many moles of cinnamaldehyde are there in 1.65 g

of the pure compound?

2015 Q4

2014 Q4

Page | 78

2013 Q4

2012 Q4

(f) State Avogadro’s law.

2011 Q4

(c) State Avogadro’s law.

(d) Define the mole, the SI unit of chemical amount

2010 Q4

(h) What is an ideal gas?

2009 Q10

Page | 79

2008 Q11

2007 Q10

2006 Q11

Page | 80

2005 Q11

2004 Q10

Page | 81

Acids and Bases

2018 Q4

Q11

2017

2016 Q4

Page | 82

2015 Q9

2014 Q7

2013

2012 Q10

Page | 83

2011 Q7

2010 Q8

2009 Q4

(d) Define a conjugate pair according to the Brønsted-Lowry theory.

2007 Q7

2006 Q4

(e) What is (i) the conjugate acid and (ii) the conjugate base of H2O?

2005 Q8

2004 Q4

Page | 84

pH

2018 Q11

2017 Q9

Page | 85

2016 Q10

2015 Q9

Page | 86

2014 Q7

2013 Q11

2012 Q10

2011 Q7

Page | 87

2010 Q8

2009

Q4 (f) Calculate the pH of a 0.025 M solution of nitric acid.

2008 Q8

2007 Q7

2006 Q8

Page | 88

2005 Q8

2004 Q11

Calculations based on chemical equations

2018 Q10

Page | 89

2017 Q11

2016 Q11

2015 Q4

Page | 90

Q10

2014 Q11

2013 Q4

Page | 91

Q10

2012 Q10

2011 Q4

(e) When 4.10 g of hydrated magnesium sulfate, MgSO4•xH2O, were heated strongly, 2.00 g of

anhydrous magnesium sulfate were obtained.

Calculate the value of x, the degree of hydration of the crystals.

2006 Q11(a)

2005

Q4 (h) When 3.175 g of copper reacts with chlorine gas 6.725 g of copper chloride is formed.

Find by calculation the empirical formula of the chloride.

Page | 92

Q10

2004 Q10

Page | 93

Hydrocarbons and Thermochemistry

2018

Page | 94

2017

2016

Page | 95

2015

Page | 96

2014 Q4

(i) Give two structural features of hydrocarbons with high octane numbers.

2013

Page | 97

2012 Q4

(i) Define bond energy

2011 Q4

(i) What is a homologous series of organic compounds?

Q6

Page | 98

2010 Q6

2009

Q4 (d) Define bond energy.

Q6

Page | 99

2008 Q6

2007 Q6

Page | 100

2006 Q6

2005 Q6

Page | 101

2004 Q6

Organic Chemistry

2018 Q4

(h) State and explain the effect of adding a little tetraethyllead to an equimolar mixture of

methane and chlorine exposed to weak sunlight.

Page | 102

Q10

2017

Q4 (h) The structure of eugenol is shown.

(i) Write the molecular formula of eugenol.

(ii) Name a spectroscopic technique that could help

confirm the identity of a sample of eugenol.

Page | 103

Q10

Page | 104

2016

Page | 105

2015

Q4

2014

Page | 106

Q10

2013 Q4

2012 Q8

Page | 107

Q10

2011 Q2

Q4 (j) What is the principle involved in the separation of a mixture by chromatography?

Q8

Q10

Page | 108

2010 Q4

(j) Draw the structural formulae of any two molecules with the molecular formula C3H6O2.

Q10

2009 Q4

Page | 109

Q8

2008 Q9

Q11 (a)

Page | 110

2007 Q8

Q11

2006 Q9

Page | 111

Q10

2005 Q7

Page | 112

2004 Q7

Page | 113

Rates of Reaction

2018

2017 No question

2016 Q4

(i) What is meant by the activation energy of a reaction?

Page | 114

2015

2014 Q9

Page | 115

2013 Q4

2012 Q4

(g) Why does raising the temperature generally increase the rates of chemical reactions?

Page | 116

2011

Q4 (h) Define the activation energy of a chemical reaction.

Q10

2009

Page | 117

2008 Q4

2007 Q9

Page | 118

2006 Q7

2004 Q8

Page | 119

Chemical Equilibrium

2018

Page | 120

2017

2016 Q7

Page | 121

2015 Q11

2014 Q9

Page | 122

2013 Q9

2012 Q11

Page | 123

2011 Q9

2010 Q7

Page | 124

2009 Q11

2008 Q7

2007 Q10

Page | 125

2006 Q11

2005 Q9

2004 Q9

Page | 126

Water

2018 Q4

(j) Explain the term biochemical oxygen demand.

2017 Q4

(j) How does boiling remove any temporary hardness, caused by the presence of calcium

hydrogencarbonate, in a water sample?

2016 Q9

2015 Q4

2014 Q4

(j) State two processes that are carried out during the primary treatment of sewage.

2013 Q4

Page | 127

2012 Q4

(j) What happens during the secondary treatment of sewage?

Q7

2011 Q4

(g) Give two methods for removing all of the hardness in a water sample

Q11

2010 Q4

(i) What happens during the secondary stage of sewage treatment?

2009 Q4

(g) When water that contains temporary hardness is boiled in a kettle, scale is formed on the heating

element. Identify the chemical that is the main component of this scale.

Page | 128

Q7

2008 Q8

Q10

Page | 129

2007 Q7

2006 Q8

2005 Q8

2004

Q4 (f) How are heavy metals, e.g. mercury, removed from industrial waste before it is discharged

into rivers, lakes or the sea?