Eduqas A Level Chemistry
Eduqas A Level Chemistry Component 1: Physical and Inorganic Chemistry Exam Questions
Free Eduqas A Level Chemistry exam questions for Component 1: Physical and Inorganic Chemistry, with a mark scheme for every pack. Covers electrode potentials, redox titrations, p-block and d-block chemistry, kinetics, enthalpy, entropy, equilibrium constants and acid-base equilibria.
Component 1: Physical and Inorganic Chemistry exam questions
9 question packs of real past exam questions, each with its mark scheme. Do not stop after a few: answer as many as you can without notes, then mark every answer with the mark scheme. The more questions you do, the more quickly you will spot how examiners ask about each idea.
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A-Level Chemistry Flashcards for 2027 Onwards
Every answer is written in mark scheme wording, so you learn exactly what examiners give marks for. Then test yourself with the questions on this page.
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About Eduqas A Level Chemistry Component 1: Physical and Inorganic Chemistry
Component 1 of the Eduqas A Level Chemistry course brings together the physical and inorganic chemistry of the second year. It covers standard electrode potentials and redox reactions, the chemistry of the p-block and of the d-block transition metals, chemical kinetics, enthalpy changes for solids and solutions, entropy and feasibility, equilibrium constants and acid-base equilibria. It builds directly on the first year ideas of formulae, bonding, energetics, rates and equilibria. Examiners expect confident calculations (Kc, Kp, pH, E cell, delta G and rate constants) alongside clear explanations of inorganic trends, such as the inert pair effect and the colour of transition metal complexes.
What you need to know
- PI1 Redox and electrode potentials Standard electrode potentials are measured against the standard hydrogen electrode under standard conditions (298 K, 1 mol dm-3 solutions). E cell = E(reduction) - E(oxidation); a positive value means the reaction is feasible. Redox titrations use manganate(VII), dichromate(VI) and iodine with thiosulfate.
- PI2.1 p-block Group 3 compounds such as BCl3 and AlCl3 are electron deficient and form dative bonds (Al2Cl6). Down Groups 4 and 5 the lower oxidation state becomes more stable (inert pair effect), so PbO2 is an oxidising agent. Learn amphoteric behaviour of aluminium and lead compounds and the structures of boron nitride.
- PI2.2 d-block transition metals Transition metals have partly filled d orbitals, variable oxidation states, coloured complexes and catalytic activity. Colour arises from d orbital splitting by ligands. Learn ligand exchange (for example [Cu(H2O)6]2+ with Cl- giving yellow [CuCl4]2-) and precipitates with NaOH.
- PI3 Chemical kinetics Orders of reaction are found from initial rates or concentration time graphs. Rate equations link to the rate-determining step of a mechanism, and the Arrhenius equation links k to activation energy and temperature.
- PI4 Enthalpy and entropy Born-Haber cycles give lattice enthalpies; enthalpy of solution links lattice and hydration enthalpies. Feasibility uses delta G = delta H - T delta S, with a reaction feasible when delta G is zero or negative.
- PI5 Equilibria Kc and Kp expressions and calculations, the effect of temperature on K, then Ka, pKa, Kw, pH of strong and weak acids and strong bases, buffer action and titration curves with indicators.
Common mistakes in Component 1: Physical and Inorganic Chemistry
- Using delta S in J K-1 mol-1 with delta H in kJ mol-1 in delta G calculations. Convert to the same energy unit first.
- Writing the inert pair effect as the s electrons becoming more reactive. It is the reluctance of the ns2 pair to be used in bonding that makes the lower oxidation state more stable down the group.
- Stating that a positive E cell guarantees a reaction. Kinetics or non-standard conditions can prevent it.
- Using the weak acid formula for buffer calculations instead of [H+] = Ka x [HA] / [A-].
- Saying that catalysts or pressure change Kc or Kp. Only temperature changes the equilibrium constant.
Try three Component 1: Physical and Inorganic Chemistry exam-style questions
1. 1.00 mol ethanoic acid and 1.00 mol ethanol react to equilibrium, forming 0.667 mol ethyl ethanoate. Calculate Kc. (3 marks)
Show the mark scheme answer
At equilibrium: ester = water = 0.667 mol, acid = ethanol = 0.333 mol; Kc = (0.667 x 0.667) / (0.333 x 0.333); = 4.0 (no units, as volumes cancel).
2. Lead(IV) oxide reacts with concentrated hydrochloric acid to release chlorine. Explain this in terms of the stability of oxidation states in Group 4. (3 marks)
Show the mark scheme answer
Down Group 4 the +2 oxidation state becomes more stable than +4 (inert pair effect); so Pb(IV) is readily reduced to Pb(II); PbO2 therefore acts as an oxidising agent, oxidising chloride ions to chlorine.
3. Explain why a solution of [Cu(H2O)6]2+ changes colour when concentrated hydrochloric acid is added. (3 marks)
Show the mark scheme answer
Ligand exchange: water ligands are replaced by chloride ions to form [CuCl4]2-; the coordination number and shape change (octahedral to tetrahedral) and the ligand is different; so d orbital splitting changes and a different frequency of light is absorbed (blue to yellow/green).
Component 1: Physical and Inorganic Chemistry FAQs
What does Eduqas A Level Chemistry Component 1: Physical and Inorganic Chemistry cover?
It covers redox and electrode potentials, redox titrations, p-block and d-block chemistry, kinetics, lattice and solution enthalpies, entropy and Gibbs energy, equilibrium constants and acid-base equilibria.
How do I revise Component 1 effectively?
Split revision into calculation practice (Kc, Kp, pH, E cell, delta G, rate constants) and inorganic recall (p-block trends, transition metal colours and observations), then mix both in timed past questions.
What equations do I need for Component 1?
Key ones are E cell = E reduction - E oxidation, Kc and Kp expressions, pH = -log[H+], Ka = [H+][A-]/[HA], Kw = [H+][OH-], delta G = delta H - T delta S and the Arrhenius equation.
