AQA A-LEVEL CHEMISTRY – PRACTICE
EXAMINATION PAPER 1 JUNE 2026 | FULLY
SOLVED PAPER + EXPERT MARKING TIPS |
GUARANTEED TOP GRADES PACK”
Paper 1 – Inorganic and Physical Chemistry
Time allowed: 2 hours
Total marks: 91
Instructions
• Use black ink or black ball-point pen.
• Fill in the boxes at the top of the page.
• Answer all questions.
• You must show all your working.
• The marks for questions are shown in brackets.
• The maximum mark for this paper is 91.
Data Sheet (Summary)
• Avogadro constant = 6.02 × 10²³ mol⁻¹
• Gas constant R = 8.31 J mol⁻¹ K⁻¹
• Faraday constant F = 96500 C mol⁻¹
• Standard conditions = 298 K, 100 kPa
,Section A
Q1 Atomic Structure (4 marks)
(a) Define the term relative atomic mass. (2)
Weighted mean mass of an atom compared with 1/12 of carbon-12.
(b) State why isotopes have identical chemical properties. (2)
Same electron configuration.
Q2 Periodicity (4 marks)
(a) Explain the trend in atomic radius across Period 3. (2)
Increasing nuclear charge, same shielding → stronger attraction → smaller radius.
(b) Predict which has the highest first ionisation energy: Na, Mg, Al. Explain. (2)
Mg; Al lower due to electron removed from 3p orbital.
Q3 Bonding (5 marks)
(a) Define electronegativity. (2)
Ability of an atom to attract bonding electrons.
(b) Explain why H₂O has a higher boiling point than H₂S. (3)
Hydrogen bonding in H₂O vs weaker van der Waals in H₂S.
Q4 Structure & Properties (5 marks)
Explain why graphite conducts electricity but diamond does not. (5)
Graphite has delocalised electrons; diamond has no free electrons.
Q5 Energetics (6 marks)
, Given:
ΔHf° (CO₂) = –393 kJ mol⁻¹
ΔHf° (CO) = –110 kJ mol⁻¹
Calculate ΔH for:
CO + ½O₂ → CO₂
(6)
ΔH = –393 – (–110) = –283 kJ mol⁻¹
Common Mistake
Students often forget Hess cycle signs—always reverse sign when reversing
equation.
Q6 Enthalpy Cycles (5 marks)
Explain why lattice enthalpy values differ from theoretical values. (5)
Polarisation/covalent character not accounted for.
Q7 Kinetics (6 marks)
(a) Define rate of reaction. (2)
Change in concentration per unit time.
(b) A reaction has rate = k[A]²[B].
State order with respect to A and B and overall order. (2)
A = 2, B = 1, total = 3.
(c) Suggest units of k. (2)
dm⁶ mol⁻² s⁻¹
Q8 Maxwell–Boltzmann (4 marks)
EXAMINATION PAPER 1 JUNE 2026 | FULLY
SOLVED PAPER + EXPERT MARKING TIPS |
GUARANTEED TOP GRADES PACK”
Paper 1 – Inorganic and Physical Chemistry
Time allowed: 2 hours
Total marks: 91
Instructions
• Use black ink or black ball-point pen.
• Fill in the boxes at the top of the page.
• Answer all questions.
• You must show all your working.
• The marks for questions are shown in brackets.
• The maximum mark for this paper is 91.
Data Sheet (Summary)
• Avogadro constant = 6.02 × 10²³ mol⁻¹
• Gas constant R = 8.31 J mol⁻¹ K⁻¹
• Faraday constant F = 96500 C mol⁻¹
• Standard conditions = 298 K, 100 kPa
,Section A
Q1 Atomic Structure (4 marks)
(a) Define the term relative atomic mass. (2)
Weighted mean mass of an atom compared with 1/12 of carbon-12.
(b) State why isotopes have identical chemical properties. (2)
Same electron configuration.
Q2 Periodicity (4 marks)
(a) Explain the trend in atomic radius across Period 3. (2)
Increasing nuclear charge, same shielding → stronger attraction → smaller radius.
(b) Predict which has the highest first ionisation energy: Na, Mg, Al. Explain. (2)
Mg; Al lower due to electron removed from 3p orbital.
Q3 Bonding (5 marks)
(a) Define electronegativity. (2)
Ability of an atom to attract bonding electrons.
(b) Explain why H₂O has a higher boiling point than H₂S. (3)
Hydrogen bonding in H₂O vs weaker van der Waals in H₂S.
Q4 Structure & Properties (5 marks)
Explain why graphite conducts electricity but diamond does not. (5)
Graphite has delocalised electrons; diamond has no free electrons.
Q5 Energetics (6 marks)
, Given:
ΔHf° (CO₂) = –393 kJ mol⁻¹
ΔHf° (CO) = –110 kJ mol⁻¹
Calculate ΔH for:
CO + ½O₂ → CO₂
(6)
ΔH = –393 – (–110) = –283 kJ mol⁻¹
Common Mistake
Students often forget Hess cycle signs—always reverse sign when reversing
equation.
Q6 Enthalpy Cycles (5 marks)
Explain why lattice enthalpy values differ from theoretical values. (5)
Polarisation/covalent character not accounted for.
Q7 Kinetics (6 marks)
(a) Define rate of reaction. (2)
Change in concentration per unit time.
(b) A reaction has rate = k[A]²[B].
State order with respect to A and B and overall order. (2)
A = 2, B = 1, total = 3.
(c) Suggest units of k. (2)
dm⁶ mol⁻² s⁻¹
Q8 Maxwell–Boltzmann (4 marks)
