Post on 11-Mar-2020
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
Page | 24
2008
Page | 25
2007
Page | 26
2006
2005
Page | 27
2004
2003
Page | 28
2002
Page | 29
Other Experiments
2018
Page | 30
2017
Page | 31
2016
Page | 32
2015
Page | 33
2014
2013
Page | 34
2012
Page | 35
2011
Page | 36
2010
Page | 37
2009
Page | 38
2008
2007
Page | 39
2006
Page | 40
2005
2004
Page | 41
2003
Page | 42
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?