Chemistry A (H032, H432)
H432/01, Periodic table, elements and physical
chemistry (AS/A level), June 2024
Neil Bechley
Please note that you may see slight differences between
this paper and the original.
Duration: 135 mins
Candidates answer on the Question paper.
OCR supplied materials:
Additional resources may be supplied with this paper.
Other materials required:
• Pencil
• Ruler (cm/mm)
INSTRUCTIONS TO CANDIDATES
• Write your name, centre number and candidate number in the boxes above. Please write clearly and in capital letters.
• Use black ink. HB pencil may be used for graphs and diagrams only.
• Answer all the questions, unless your teacher tells you otherwise.
• Read each question carefully. Make sure you know what you have to do before starting your answer.
• Where space is provided below the question, please write your answer there.
• You may use additional paper, or a specific Answer sheet if one is provided, but you must clearly show your candidate
number, centre number and question number(s).
INFORMATION FOR CANDIDATES
• The quality of written communication is assessed in questions marked with either a pencil or an asterisk. In History and
Geography a Quality of extended response question is marked with an asterisk, while a pencil is used for questions in
which Spelling, punctuation and grammar and the use of specialist terminology is assessed.
• The number of marks is given in brackets [ ] at the end of each question or part question.
• The total number of marks for this paper is 100.
• The total number of marks may take into account some 'either/or' question choices.
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, 1 Oxygen has the electron configuration 1s22s22p4.
How are the electrons in an atom of oxygen arranged in the p-orbitals?
A
B
C
D
Your answer [1]
2 Water has the anomalous properties below.
• Water has relatively high melting and boiling points.
• Ice is less dense than water.
Which statement explains these anomalous properties?
A The covalent bonding within water molecules.
B The hydrogen bonding between water molecules.
C The induced dipole-dipole interactions (London forces) between water molecules.
D The ionic bonding between water molecules.
Your answer [1]
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, 3 Which chemical process is the most sustainable in terms of the atom economy of the iron produced?
A Fe2O3 + 3CO → 2Fe + 3CO2
B Fe2O3 + 3H2 → 2Fe + 3H2O
C 2Fe2O3 → 4Fe + 3O2
D 2Fe2O3 + 3C → 4Fe + 3CO2
Your answer [1]
4 Which compounds of magnesium can be used as ‘antacids’?
A Chlorides
B Hydroxides
C Nitrates
D Sulfates
Your answer [1]
5 Which statement explains the trend in boiling points down the halogens group?
A The bond enthalpy of the covalent bonds increases.
B The halogens become less electronegative.
C The induced dipole-dipole interactions (London forces) become stronger.
D The reactivity of the halogens decreases.
Your answer [1]
6 Which equation does not represent a disproportionation reaction?
A Cl2 + H2O → HClO + HCl
B Cl2 + 2NaOH → NaClO + NaCl + H2O
C 4KClO3 → KCl + 3KClO4
D 4HCl + MnO2 → MnCl2 + Cl2 + 2H2O
Your answer [1]
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, 7 The equation for the reaction of sulfuric acid with potassium hydroxide is shown below.
H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)
25 cm3 of 1.00 mol dm–3 H2SO4 is reacted with excess KOH.
The energy given out is 2.8 kJ.
What is the enthalpy change of neutralisation, in kJ mol–1?
A –56
B –70
C –112
D –224
Your answer [1]
8 Which row in the table explains how a catalyst affects the activation energy (Ea) and the proportion of molecules
with energy > Ea?
How the activation energy Proportion of molecules with energy > Ea
changes
A decreases decreases
B decreases increases
C increases decreases
D increases increases
Your answer [1]
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, 9 A graph of ln(k) is plotted against 1 / T for a reaction.
(k = rate constant, T = temperature in K.)
The gradient has the numerical value of –16 000.
What is the activation energy, in kJ mol–1, for this reaction?
A +1.92
B +133
C +1920
D +133 000
Your answer [1]
10 A reaction is zero order with respect to a reactant.
Which rate-concentration graph for the reactant is the correct shape?
A
B
C
D
Your answer [1]
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, 11 The reversible reaction between hydrogen and iodine to form hydrogen iodide is H2(g) + I2(g) ⇋ 2HI(g)
The graph shows how the concentrations of the reactants and product change as the reaction reaches a
dynamic equilibrium.
At which point on the graph is the equilibrium reached?
Your answer [1]
12 Which solution can be added to CH3COOH(aq) to make a buffer solution?
A CH3COONa(aq)
B HCOOH(aq)
C HCl (aq)
D NaCl (aq)
Your answer [1]
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, 13 A student analyses a solution of a salt.
The results are shown below.
Test Observation
Reaction with NaOH(aq) Green precipitate
Reaction with Ba(NO3)2(aq) White precipitate
What is the formula of the salt?
A CuCl2
B CuSO4
C FeCl2
D FeSO4
Your answer [1]
14 Chlorine has the electron configuration [Ne]3s23p5.
Which statement(s) about chlorine is/are correct when it reacts in redox reactions?
1 It can gain one electron to form 1– ions.
2 It can lose its 3s2 electrons to form 2+ ions.
3 It can lose its 3p5 electrons to form 5+ ions.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]
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, 15 Which statement(s) about elements in the periodic table is/are correct?
1 The position of an element is determined by its relative atomic mass.
2 The elements in a group have similar chemical properties.
3 Transition elements are used as catalysts in the manufacture of chemicals.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]
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, 16(a) This question is about energy changes.
Hydrogen peroxide decomposes as shown in Reaction 16.1.
Reaction 16.1
The table shows enthalpy changes of formation and entropies.
ΔHfe/kJ mol1 Se / J K–-1 mol–1
H2O2(l) –188 110
H2O(l) –286 70.0
O2(g) 0 205
i. Calculate the free-energy change, ΔG, in kJ mol–1, of Reaction 16.1 at 25 °C.
Give your answer to 3 significant figures.
ΔG = .............................................. kJ mol–1 [4]
ii. The decomposition of hydrogen peroxide shown in Reaction 16.1 is feasible.
Suggest why Reaction 16.1 does not take place at 25 °C despite being feasible.
[1]
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, (b) The rate of decomposition of hydrogen peroxide shown in Reaction 16.1 can be increased by adding a small
amount of powdered manganese(IV) oxide, MnO2.
The MnO2 acts as a catalyst.
i. Complete the enthalpy profile diagram for Reaction 16.1 using formulae for the reactants and products.
• Use Ea to label the activation energy without MnO2.
• Use Ec to label the activation energy with MnO2.
• Use ΔH to label the enthalpy change of reaction.
[3]
ii. Explain why MnO2 is described as a heterogeneous catalyst for this reaction.
[1]
iii. Mn3O4 is a compound in which Mn has two different oxidation states. The two oxidation states are different
from the Mn in MnO2.
Suggest the two oxidation states of manganese in Mn3O4.
[1]
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H432/01, Periodic table, elements and physical
chemistry (AS/A level), June 2024
Neil Bechley
Please note that you may see slight differences between
this paper and the original.
Duration: 135 mins
Candidates answer on the Question paper.
OCR supplied materials:
Additional resources may be supplied with this paper.
Other materials required:
• Pencil
• Ruler (cm/mm)
INSTRUCTIONS TO CANDIDATES
• Write your name, centre number and candidate number in the boxes above. Please write clearly and in capital letters.
• Use black ink. HB pencil may be used for graphs and diagrams only.
• Answer all the questions, unless your teacher tells you otherwise.
• Read each question carefully. Make sure you know what you have to do before starting your answer.
• Where space is provided below the question, please write your answer there.
• You may use additional paper, or a specific Answer sheet if one is provided, but you must clearly show your candidate
number, centre number and question number(s).
INFORMATION FOR CANDIDATES
• The quality of written communication is assessed in questions marked with either a pencil or an asterisk. In History and
Geography a Quality of extended response question is marked with an asterisk, while a pencil is used for questions in
which Spelling, punctuation and grammar and the use of specialist terminology is assessed.
• The number of marks is given in brackets [ ] at the end of each question or part question.
• The total number of marks for this paper is 100.
• The total number of marks may take into account some 'either/or' question choices.
© OCR 2025. You may photocopy this page. 1 of 65 Created in ExamBuilder
, 1 Oxygen has the electron configuration 1s22s22p4.
How are the electrons in an atom of oxygen arranged in the p-orbitals?
A
B
C
D
Your answer [1]
2 Water has the anomalous properties below.
• Water has relatively high melting and boiling points.
• Ice is less dense than water.
Which statement explains these anomalous properties?
A The covalent bonding within water molecules.
B The hydrogen bonding between water molecules.
C The induced dipole-dipole interactions (London forces) between water molecules.
D The ionic bonding between water molecules.
Your answer [1]
© OCR 2025. You may photocopy this page. 2 of 65 Created in ExamBuilder
, 3 Which chemical process is the most sustainable in terms of the atom economy of the iron produced?
A Fe2O3 + 3CO → 2Fe + 3CO2
B Fe2O3 + 3H2 → 2Fe + 3H2O
C 2Fe2O3 → 4Fe + 3O2
D 2Fe2O3 + 3C → 4Fe + 3CO2
Your answer [1]
4 Which compounds of magnesium can be used as ‘antacids’?
A Chlorides
B Hydroxides
C Nitrates
D Sulfates
Your answer [1]
5 Which statement explains the trend in boiling points down the halogens group?
A The bond enthalpy of the covalent bonds increases.
B The halogens become less electronegative.
C The induced dipole-dipole interactions (London forces) become stronger.
D The reactivity of the halogens decreases.
Your answer [1]
6 Which equation does not represent a disproportionation reaction?
A Cl2 + H2O → HClO + HCl
B Cl2 + 2NaOH → NaClO + NaCl + H2O
C 4KClO3 → KCl + 3KClO4
D 4HCl + MnO2 → MnCl2 + Cl2 + 2H2O
Your answer [1]
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, 7 The equation for the reaction of sulfuric acid with potassium hydroxide is shown below.
H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)
25 cm3 of 1.00 mol dm–3 H2SO4 is reacted with excess KOH.
The energy given out is 2.8 kJ.
What is the enthalpy change of neutralisation, in kJ mol–1?
A –56
B –70
C –112
D –224
Your answer [1]
8 Which row in the table explains how a catalyst affects the activation energy (Ea) and the proportion of molecules
with energy > Ea?
How the activation energy Proportion of molecules with energy > Ea
changes
A decreases decreases
B decreases increases
C increases decreases
D increases increases
Your answer [1]
© OCR 2025. You may photocopy this page. 4 of 65 Created in ExamBuilder
, 9 A graph of ln(k) is plotted against 1 / T for a reaction.
(k = rate constant, T = temperature in K.)
The gradient has the numerical value of –16 000.
What is the activation energy, in kJ mol–1, for this reaction?
A +1.92
B +133
C +1920
D +133 000
Your answer [1]
10 A reaction is zero order with respect to a reactant.
Which rate-concentration graph for the reactant is the correct shape?
A
B
C
D
Your answer [1]
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, 11 The reversible reaction between hydrogen and iodine to form hydrogen iodide is H2(g) + I2(g) ⇋ 2HI(g)
The graph shows how the concentrations of the reactants and product change as the reaction reaches a
dynamic equilibrium.
At which point on the graph is the equilibrium reached?
Your answer [1]
12 Which solution can be added to CH3COOH(aq) to make a buffer solution?
A CH3COONa(aq)
B HCOOH(aq)
C HCl (aq)
D NaCl (aq)
Your answer [1]
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, 13 A student analyses a solution of a salt.
The results are shown below.
Test Observation
Reaction with NaOH(aq) Green precipitate
Reaction with Ba(NO3)2(aq) White precipitate
What is the formula of the salt?
A CuCl2
B CuSO4
C FeCl2
D FeSO4
Your answer [1]
14 Chlorine has the electron configuration [Ne]3s23p5.
Which statement(s) about chlorine is/are correct when it reacts in redox reactions?
1 It can gain one electron to form 1– ions.
2 It can lose its 3s2 electrons to form 2+ ions.
3 It can lose its 3p5 electrons to form 5+ ions.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]
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, 15 Which statement(s) about elements in the periodic table is/are correct?
1 The position of an element is determined by its relative atomic mass.
2 The elements in a group have similar chemical properties.
3 Transition elements are used as catalysts in the manufacture of chemicals.
A 1, 2 and 3
B Only 1 and 2
C Only 2 and 3
D Only 1
Your answer [1]
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, 16(a) This question is about energy changes.
Hydrogen peroxide decomposes as shown in Reaction 16.1.
Reaction 16.1
The table shows enthalpy changes of formation and entropies.
ΔHfe/kJ mol1 Se / J K–-1 mol–1
H2O2(l) –188 110
H2O(l) –286 70.0
O2(g) 0 205
i. Calculate the free-energy change, ΔG, in kJ mol–1, of Reaction 16.1 at 25 °C.
Give your answer to 3 significant figures.
ΔG = .............................................. kJ mol–1 [4]
ii. The decomposition of hydrogen peroxide shown in Reaction 16.1 is feasible.
Suggest why Reaction 16.1 does not take place at 25 °C despite being feasible.
[1]
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, (b) The rate of decomposition of hydrogen peroxide shown in Reaction 16.1 can be increased by adding a small
amount of powdered manganese(IV) oxide, MnO2.
The MnO2 acts as a catalyst.
i. Complete the enthalpy profile diagram for Reaction 16.1 using formulae for the reactants and products.
• Use Ea to label the activation energy without MnO2.
• Use Ec to label the activation energy with MnO2.
• Use ΔH to label the enthalpy change of reaction.
[3]
ii. Explain why MnO2 is described as a heterogeneous catalyst for this reaction.
[1]
iii. Mn3O4 is a compound in which Mn has two different oxidation states. The two oxidation states are different
from the Mn in MnO2.
Suggest the two oxidation states of manganese in Mn3O4.
[1]
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