AQA Chemistry · Unit 1

Physical chemistry quizzes

43 ready‑made quiz sets for Unit 1: Physical chemistry, one for every lesson, in course order. Pick one, put it on the board and host it live — students answer on their own devices.

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Each set covers one lesson of Unit 1: Physical chemistry in the AQA Chemistry (7405), with 20 multiple-choice questions on a timed countdown. Open a set to read its revision notes, host it straight away or save it to your library.

43 lesson sets in Unit 1: Physical chemistry

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3.1.1.1 Fundamental particles
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3.1.1.2 Mass number and isotopes
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3.1.1.3 Electron configuration
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3.1.2.1 Relative atomic mass and relative molecular mass
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3.1.2.2 The mole and the Avogadro constant
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3.1.2.3 The ideal gas equation
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3.1.2.4 Empirical and molecular formula
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3.1.2.5 Balanced equations and associated calculations
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3.1.3.1 Ionic bonding
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3.1.3.2 Nature of covalent and dative covalent bonds
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3.1.3.3 Metallic bonding
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3.1.3.4 Bonding and physical properties
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3.1.3.5 Shapes of simple molecules and ions
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3.1.3.6 Bond polarity
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3.1.3.7 Forces between molecules
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3.1.4.1 Enthalpy change
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3.1.4.2 Calorimetry
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3.1.4.3 Applications of Hess’s law
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3.1.4.4 Bond enthalpies
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3.1.5a Kinetics
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3.1.5.1 Collision theory
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3.1.5.2 Maxwell–Boltzmann distribution
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3.1.5.3 Effect of temperature on reaction rate
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3.1.5.4 Effect of concentration and pressure
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3.1.5.5 Catalysts
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3.1.6a Chemical equilibria, Le Chatelier’s principle and Kc
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3.1.6.1 Chemical equilibria and Le Chatelier's principle
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3.1.6.2 Equilibrium constant Kc for homogeneous systems
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3.1.7 Oxidation, reduction and redox equations
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3.1.8.1 Born–Haber cycles
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3.1.8.2 Gibbs free-energy change, ∆G, and entropy change, ∆S
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3.1.9.1 Rate equations
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3.1.9.2 Determination of rate equation
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3.1.10 Equilibrium constant Kp for homogeneous systems (A-level
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3.1.11a Electrode potentials and electrochemical cells
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3.1.11.1 Electrode potentials and cells
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3.1.11.2 Commercial applications of electrochemical cells
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3.1.12.1 Brønsted–Lowry acid–base equilibria in aqueous solution
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3.1.12.2 Definition and determination of pH
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3.1.12.3 The ionic product of water, Kw
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3.1.12.4 Weak acids and bases Ka for weak acids
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3.1.12.5 pH curves, titrations and indicators
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3.1.12.6 Buffer action
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43 lesson sets in Unit 1: Physical chemistry

3.1.1.1 Fundamental particles

3.1.1.2 Mass number and isotopes

3.1.1.3 Electron configuration

3.1.2.1 Relative atomic mass and relative molecular mass

3.1.2.2 The mole and the Avogadro constant

3.1.2.3 The ideal gas equation

3.1.2.4 Empirical and molecular formula

3.1.2.5 Balanced equations and associated calculations

3.1.3.1 Ionic bonding

3.1.3.2 Nature of covalent and dative covalent bonds

3.1.3.3 Metallic bonding

3.1.3.4 Bonding and physical properties

3.1.3.5 Shapes of simple molecules and ions

3.1.3.6 Bond polarity

3.1.3.7 Forces between molecules

3.1.4.1 Enthalpy change

3.1.4.2 Calorimetry

3.1.4.3 Applications of Hess’s law

3.1.4.4 Bond enthalpies

3.1.5a Kinetics

3.1.5.1 Collision theory

3.1.5.2 Maxwell–Boltzmann distribution

3.1.5.3 Effect of temperature on reaction rate

3.1.5.4 Effect of concentration and pressure

3.1.5.5 Catalysts

3.1.6a Chemical equilibria, Le Chatelier’s principle and Kc

3.1.6.1 Chemical equilibria and Le Chatelier's principle

3.1.6.2 Equilibrium constant Kc for homogeneous systems

3.1.7 Oxidation, reduction and redox equations

3.1.8.1 Born–Haber cycles

3.1.8.2 Gibbs free-energy change, ∆G, and entropy change, ∆S

3.1.9.1 Rate equations

3.1.9.2 Determination of rate equation

3.1.10 Equilibrium constant Kp for homogeneous systems (A-level

3.1.11a Electrode potentials and electrochemical cells

3.1.11.1 Electrode potentials and cells

3.1.11.2 Commercial applications of electrochemical cells

3.1.12.1 Brønsted–Lowry acid–base equilibria in aqueous solution

3.1.12.2 Definition and determination of pH

3.1.12.3 The ionic product of water, Kw

3.1.12.4 Weak acids and bases Ka for weak acids

3.1.12.5 pH curves, titrations and indicators

3.1.12.6 Buffer action