Five units of roughly even duration, covering the basics of structure and quantitative chemistry, supported by a Practical Scheme of Work (PSOW)

• Unit 1 - Counting matters
• Unit 2 - Atoms, elements and the periodic table
• Unit 3 - Making matter
• Unit 4 - Molecules and compounds
• Unit 5 - Energy change

Five units covering more applied chemistry, once again supported by a Practical Scheme of Work (PSOW)

• Unit 6 - Rates of reaction
• Unit 7 - Reversible processes
• Unit 8 - Proton transfer reactions
• Unit 9 - Electron transfer reactions
• Unit 10 - Electron sharing reactions

Kinetic theory and quantitative chemistry

• • Structure 1.1.2 - The kinetic molecular theory
• • Structure 1.1.1 - Elements
• • Structure 1.1.3 - Temperature and energy
• • Structure 1.4.1 - The mole
• • Structure 1.4.2 - Masses of atoms
• • Structure 1.4.3 - Molar mass
• • Structure 1.4.4 - The empirical formula
• • Structure 1.4.5 - The molar concentration
• • Structure 1.4.6 - Avogadro’s law
• Self-tests and teaching resources - Counting particles by mass

• The gas laws
• • Structure 1.5.1 - Ideal gases
• • Structure 1.5.2 - Real gases
• • Structure 1.5.3 - The molar volume of an ideal gas
• • Structure 1.5.4 - Ideal gas equations
• Self-tests and teaching resources - Ideal gases

• Chemical reactions
• • Reactivity 2.1.1 - Chemical equations
• • Reactivity 2.1.2 - Stoichiometry
• • Reactivity 2.1.3 - Limiting reactant
• • Reactivity 2.1.4 - Percentage yield
• • Reactivity 2.1.5 - Atom economy
• Self-tests and teaching resources - The amount of chemical change

• • Experiment E101 - Acid base titration
• • Experiment E102 - Analysis of white vinegar
• • Experiment E103 - Analysis of an unknown carbonate
• • Experiment E104 - Water of crystallisation by titration
• • Experiment E105 - Water of crystallisation by gravimetry
• • Experiment E106 - Relative mass of a gas by direct weighing
• • Experiment E107 - Relative mass of reactive metals
• • Experiment E108 - Relative mass by decomposition
• • Experiment E109 - Formula of magnesium oxide
• • Experiment E110 - Relative mass of a volatile liquid (virtual)
• • Experiment E111 - Relative mass of a metal oxide (virtual)

• Kinetics and rates of reaction
• • Reactivity 2.2.1 - Reaction rate
• • Reactivity 2.2.2 – Collision theory
• • Reactivity 2.2.3 - Factors influencing reaction rate
• • Reactivity 2.2.4 - Activation energy
• • Reactivity 2.2.5 – Catalysts
• • Reactivity 2.2.6 – Stepwise reactions (HL)
• • Reactivity 2.2.7 - Energy profiles (HL)
• • Reactivity 2.2.8 - The molecularity (HL)
• • Reactivity 2.2.9 - Rate equations (HL)
• • Reactivity 2.2.10 - The order of a reaction (HL)
• • Reactivity 2.2.11 - The rate constant (HL)
• • Reactivity 2.2.12 - The Arrhenius equation (HL)
• • Reactivity 2.2.13 - The Arrhenius factor (HL)
• Self-tests and teaching resources - Kinetics

• • Experiment E601 - The effect of concentration on reaction rate
• • Experiment E602 - The effect of temperature on reaction rate
• • Experiment E603 - The effect of surface area on reaction rate
• • Experiment E604 - Determining the order of a reaction (HL)
• • Experiment E605 - The activation energy of a catalysed reaction

• Atomic theory
• • Structure 1.2.1 - Atomic structure
• • Structure 1.2.2 - Isotopes
• • Structure 1.2.3 - Mass spectrometry (HL)
• • Structure 1.3.1 - Emission spectra
• • Structure 1.3.2 - The hydrogen spectrum
• • Structure 1.3.3 - Atomic energy levels
• • Structure 1.3.4 - Atomic sub-levels
• • Structure 3.1.1 - The periodic table
• • Structure 3.1.2 - The period number
• • Structure 1.3.5 - Orbitals
• • Structure 1.3.6 - The convergence limit (HL)
• • Structure 1.3.7 - Successive ionization energies (HL)
• Self-tests and teaching resources - Atomic theory and periodicity

• • Experiment E201 - Flame tests
• • Experiment E202 - The radius of an atom

• The equilibrium state
• • Reactivity 2.3.1 - Dynamic equilibrium
• • Reactivity 2.3.2 - The equilibrium law
• • Reactivity 2.3.3 - The equilibrium constant
• • Reactivity 2.3.4 - Le Châtelier’s principle
• • Reactivity 2.3.5 - The reaction quotient, Q, (HL)
• • Reactivity 2.3.6 – Using the equilibrium law (HL)
• • Reactivity 2.3.7 – Determining the equilibrium constant (HL)
• Self-tests and teaching resources - Equilibrium

• • Experiment E701 - Determination of an equilibrium constant (HL)

• Models of bonding and structure - giant lattices
• • Structure 2.3.1 - Metallic bonding
• • Structure 3.1.6 - Oxidation state
• • Structure 3.1.3 - Periodicity
• • Structure 2.3.2 - Metallic bond strength
• • Structure 2.3.3 - Transition elements (HL)
• • Structure 3.1.4 - Trends in properties of elements
• • Structure 3.1.5 - Metallic and non-metallic properties
• • Structure 3.1.7 - 1st ionization energies (HL)
• • Structure 3.1.8 - Transition elements (HL)
• • Structure 3.1.9 - Variable oxidation state (HL)
• • Structure 2.4.3 - Alloys
• • Structure 2.1.1 - Ions
• • Structure 2.1.2 - Ionic bonding
• • Structure 2.1.3 - Ionic structure
• • Structure 3.1.10 - Complex ions (HL)
• • Structure 1.4.5 - (revisit)
• Self-tests and teaching resources - Metallic, ionic bonding and periodicity

• • Experiment E301 - Properties of covalent liquids

• Acids and bases
• • Reactivity 3.1.1 - Brønsted–Lowry theory
• • Reactivity 3.1.2 - Conjugate acid–base pairs
• • Reactivity 3.1.3 – Amphiprotic species
• • Reactivity 3.1.4 - The pH scale
• • Reactivity 3.1.5 - The ion product constant of water
• • Reactivity 3.1.6 - Strong and weak acids and bases
• • Reactivity 3.1.7 - Neutralization reactions
• • Reactivity 3.1.8 - pH curves for neutralization reactions
• • Reactivity 3.1.9 - The pOH scale (HL)
• • Reactivity 3.1.10 - Strength of weak acids and bases (HL)
• • Reactivity 3.1.11 - Ka × Kb = Kw (HL)
• • Reactivity 3.1.12 - The pH of a salt solution (HL)
• • Reactivity 3.1.13 - pH curves of weak acids and bases (HL)
• • Reactivity 3.1.14 - Acid–base indicators (HL)
• • Reactivity 3.1.15 - Appropriate indicator (HL)
• • Reactivity 3.1.16 - Buffer solutions (HL)
• • Reactivity 3.1.17 - The pH of a buffer solution (HL)
• Self-tests and teaching resources - Acids, bases and salts

• • Experiment E801 - The reactions of acids
• • Experiment E802 - pH of weak acids
• • Experiment E803 - ka by half-equivalence

• Models of bonding and structure - covalency
• • Structure 2.2.1 - The covalent bond
• • Reactivity 1.2.1 - Bond energy
• • Structure 2.2.2 - Multiple bonds
• • Structure 2.2.3 - The coordination bond
• • Reactivity 3.4.8 - Coordination bonds in complex ions (HL)
• • Structure 2.2.4 - Valence shell electron pair repulsion
• • Structure 2.2.5 - Bond polarity
• • Structure 2.2.6 - Molecular polarity
• • Structure 2.2.7 - Macromolecules
• Self-tests and teaching resources - Covalent bonding

• Organic compounds
• • Structure 3.2.1 - Organic compounds
• • Structure 3.2.2 - Functional groups
• • Structure 3.2.3 - Homologous series
• • Structure 3.2.5 - IUPAC nomenclature
• • Structure 3.2.6 - Structural isomers
• • Structure 3.2.7 - Stereoisomers
• Self-tests and teaching resources - Organic structure

• • Structure 3.2.8 - Structural determination - MS
• • Structure 3.2.9 - Structural determination - IR
• • Structure 3.2.10 - Structural determination - NMR
• • Structure 3.2.11 - Structural determination - NMR splitting
• • Structure 3.2.12 - Structural determination overview
• Self-tests and teaching resources - Determination of structure

• • Structure 2.2.8 - Intermolecular forces
• • Structure 3.2.4 - Trends in physical properties
• • Structure 2.2.9 - Relative intermolecular force strength
• • Structure 2.2.10 - Chromatography
• Self-tests and teaching resources - Interparticular forces

• • Structure 2.2.11 - Resonance (HL)
• • Structure 2.2.12 - Benzene (HL)
• • Structure 2.2.13 - Octet expansion (HL)
• • Structure 2.2.14 - Formal charge (HL)
• • Structure 2.2.15 - Sigma bonds (HL)
• • Structure 2.2.16 - Hybridization (HL)

• • Structure 2.4.1 - The bonding continuum
• • Structure 2.4.2 - The bonding triangle
• • Structure 2.4.3 (revisit briefly) -
• Self-tests and teaching resources - Covalent bonding and structure

• • Experiment E401 - Synthesis of copper(II) sulfate
• • Experiment E402 - Determination of copper
• • Experiment E403 - Transition metal complexes (HL)

• Oxidation and reduction.
• • Reactivity 3.2.1 - Oxidation and reduction.
• • Reactivity 3.2.2 - Half-equations
• • Reactivity 3.2.3 - The relative ease of oxidation and reduction
• • Reactivity 3.2.4 - Acids react with reactive metals
• • Reactivity 3.2.5 - Electrochemical cells
• • Reactivity 3.2.6 - A primary (voltaic) cell
• • Reactivity 3.2.7 - Secondary (rechargeable) cells
• • Reactivity 3.2.8 - An electrolytic cell
• • Reactivity 3.2.9 – Oxidation of organic functional groups
• • Reactivity 3.2.10 - Reduction of organic functional groups
• • Reactivity 3.2.11 - Reduction of unsaturated compounds
• • Reactivity 3.2.12 - The hydrogen half-cell (HL)
• • Reactivity 3.2.13 - Standard cell potential (HL)
• • Reactivity 3.2.14 - Gibbs energy and standard cell potential (HL)
• • Reactivity 3.2.15 - Electrolysis of aqueous solutions (HL)
• • Reactivity 3.2.16 – Electroplating (HL)
• Self-tests and teaching resources - Oxidation and reduction

• • Experiment E901 - Redox titration - Determination of iodine
• • Experiment E902 - Voltaic cells
• • Experiment E903 - Electrolysis of sodium chloride solution

• Energetics and thermodynamics
• • Reactivity 1.1.1 - Chemical reactions
• • Reactivity 1.1.2 - Exo- and endothermic processes
• • Reactivity 1.1.3 - Relative stability
• • Reactivity 1.1.4 - The standard enthalpy change
• • Reactivity 1.2.1 - Covalent bond energy (revisit)
• • Reactivity 1.3.1 - Combustion
• • Reactivity 1.3.2 - Incomplete combustion
• • Reactivity 1.3.3 - Fossil fuels
• • Reactivity 1.2.2 - Hess’s law
• • Reactivity 1.2.3 - Standard enthalpy change of combustion (HL)
• • Reactivity 1.2.4 - An application of Hess’s law (HL)
• • Reactivity 1.2.5 - Born–Haber cycles (HL)
• • Reactivity 1.4.1 - Entropy (HL)
• • Reactivity 1.4.2 - Gibbs free energy change (HL)
• • Reactivity 1.4.3 - Spontaneity (HL)
• Self-tests and teaching resources - Energetics

• • Experiment E501 - Combustion enthalpy of fuels
• • Experiment E502 - Neutralisation enthalpy
• • Experiment E503 - Combustion enthalpy of a metal
• • Experiment E504 - Hess' law - hydration enthalpy
• • Experiment E505 - Hess' law - reaction enthalpy
• • Experiment E506 - Thermometric titration
• • Experiment E507 - Displacement enthalpy

• Organic chemistry
• • Reactivity 3.3.1 – Free-radicals
• • Reactivity 3.3.2 - Homolytic fission
• • Reactivity 3.3.3 – Free-radical substitution
• Self-tests and teaching resources - Alkanes
• • Reactivity 3.4.1 - Nucleophiles
• • Reactivity 3.4.2 - Nucleophilic substitution
• • Reactivity 3.4.3 - Heterolytic fission
• • Reactivity 3.4.4 - Electrophiles
• • Reactivity 3.4.5 - Electrophilic addition to alkenes
• • Structure 2.4.5 - Addition polymers
• • Structure 2.4.6 – Condensation polymers (HL)
• • Reactivity 3.4.9 - Nucleophilic substitution (HL)
• • Reactivity 3.4.10 - The rate of substitution (HL)
• • Reactivity 3.4.11 - Electrophilic addition (HL)
• • Reactivity 3.4.12 – Asymmetric addition (HL)
• • Reactivity 3.4.6 – Lewis acids (HL)
• • Reactivity 3.4.13 - Electrophilic substitution (HL)
• Self-tests and teaching resources - Organic chemistry

• • Experiment E001 - Free radical substitution of an alkane (demo)
• • Experiment E002 - Cracking and alkenes