Course Outline

Paper 4 (alternative to practical, 1 h) replaces Paper 3 for candidates who cannot sit a practical exam. Internally assessed coursework is not used.

Four-option MCQ. Marks are not deducted for wrong answers — attempt every question. Questions test recall, interpretation of data, and applying chemical principles. Common traps: confusing elements with compounds, misreading state symbols, and sign errors in energy questions.

Section A: compulsory structured questions. Section B: choice of two from three extended questions. Show all working in calculations — method marks apply. Equations must be balanced with correct state symbols where asked.

Paper 3: hands-on lab work — titrations, salt preparation, qualitative analysis tests. Paper 4: data-based questions that simulate experimental work (drawing graphs, identifying errors, suggesting improvements).

1 — Particulate Nature of Matter

Kinetic particle theory · states of matter · diffusion · changes of state

2 — Experimental Techniques

Filtration, distillation, chromatography · purity and melting/boiling points · safe handling and measurement

3 — Atoms, Elements and Compounds

Atomic structure (protons, neutrons, electrons) · isotopes · electron configuration · periodic table (groups, periods, trends) · ionic and covalent bonding · metallic bonding · giant vs simple molecular structures

4 — Stoichiometry

Relative atomic and formula masses · mole concept · empirical and molecular formulae · percentage composition · reacting masses and volumes · concentration · yield and purity calculations

5 — Electricity and Chemistry (Electrochemistry)

Electrolytes and non-electrolytes · electrolysis of molten and aqueous solutions · half-equations · products at electrodes · electroplating · extraction of aluminium

6 — Chemical Energetics

Exothermic and endothermic reactions · bond energies · activation energy · energy profile diagrams

7 — Rates of Reaction

Effect of concentration, temperature, pressure, surface area, and catalysts · collision theory

8 — Equilibrium

Reversible reactions · Le Chatelier's principle · Haber process · Contact process

9 — Inorganic Chemistry — Metals

Reactivity series · extraction methods · reactions of metals with oxygen, water, and acids · alloys · rusting and its prevention

10 — Inorganic Chemistry — Non-metals

Properties and uses of hydrogen, oxygen, nitrogen, and chlorine · industrial processes

11 — Organic Chemistry

Homologous series · alkanes and alkenes (reactions, isomerism) · alcohols · carboxylic acids · esters · addition and condensation polymers · cracking

Check Cambridge's published grade threshold documents for the exact values for your series.

• State symbols (s, l, g, aq) cost marks when omitted — practise writing them automatically.
• Calculations: always show the mole calculation in two clear lines (moles → mass or volume), and include units.
• Electrochemistry half-equations: practise writing oxidation and reduction separately, then balance electrons before combining.
• In Paper 1, eliminate obviously wrong options first; if unsure between two, pick and move on — no penalty.