Chemistry › Revision posters
A-level Chemistry revision posters
One page per topic: the diagrams, the processes and the handful of points worth remembering. Made to be printed, put on a wall, or saved to a phone. Click a poster to open it full size, or download it to keep; the title goes to the lesson it came from.
Working in the laboratory
Atomic structure
Amount of substance
Bonding and structure
Energetics
Kinetics
Chemical equilibria
Redox
Thermodynamics
Rate equations
Electrochemistry
Acids and bases
Periodicity and Period 3
Group 2 and Group 7
Transition metals
Ions in aqueous solution
Introduction to organic chemistry
Alkanes and halogenoalkanes
Alkenes and alcohols
Organic analysis
Carbonyls and carboxylic acids
Aromatic chemistry and amines
Organic synthesis
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![Revision poster: Rate equations, orders of reaction and the rate constant. rate = k[A]^m[B]^n; overall order is m + n. Orders come from experiment, not the equation. Double [A]: order 0 ×1, order 1 ×2, order 2 ×4. Units of k: rearrange, substitute, cancel. k changes with temperature, not concentration.](/chemistry/assets/posters/rate-equations-and-orders.png)





![Revision poster: Brønsted–Lowry acids and bases, pH and strong acids. An acid donates H⁺; a base accepts H⁺. A conjugate pair differs by exactly one proton. Strong means fully dissociated, not concentrated. pH = −log[H⁺]; one unit is a factor of ten. Mixing: find the excess, divide by the total volume.](/chemistry/assets/posters/bronsted-lowry-and-ph.png)
![Revision poster: Weak acids, Ka and pKa; Kw and strong bases. Kw = [H⁺][OH⁻] = 1.00 × 10⁻¹⁴ at 298 K. Neutral means [H⁺] = [OH⁻], not pH 7. Strong base: [H⁺] = Kw ÷ [OH⁻]. Weak acid: [H⁺] = √(Ka × [HA]). Smaller pKa, stronger acid.](/chemistry/assets/posters/weak-acids-and-ka.png)

![Revision poster: Buffer solutions and buffer calculations. A buffer resists pH change; it does not prevent it. Weak acid + its conjugate base, both in large amounts. Added H⁺ meets A⁻; added OH⁻ meets HA. [H⁺] = Ka × [HA] / [A⁻] Blood: H₂CO₃ / HCO₃⁻ holds pH 7.35 to 7.45.](/chemistry/assets/posters/buffers.png)







![Revision poster: Transition metal characteristics and complex formation. Transition metal: stable ion with part-filled d subshell. Sc³⁺ is 3d⁰ and Zn²⁺ is 3d¹⁰, so neither counts. Ions lose 4s before 3d: Fe³⁺ is [Ar] 3d⁵. A ligand donates a lone pair: a coordinate bond. CO binds the Fe²⁺ of haem more strongly than O₂.](/chemistry/assets/posters/transition-metals-and-complexes.png)
![Revision poster: Ligands, the shapes of complexes, isomerism and ligand substitution. H₂O and NH₃: six ligands, octahedral, 90°. Cl⁻ is larger: four ligands, tetrahedral, 109.5°. Cisplatin is square planar; [Ag(NH₃)₂]⁺ is linear. Chelate effect: more particles, ΔS up, ΔG down. Cis 90°, trans 180°; three en ligands: optical.](/chemistry/assets/posters/ligands-shapes-and-substitution.png)



![Revision poster: Metal-aqua ions and the acidity of their solutions. Six water ligands: [M(H₂O)₆]²⁺ or [M(H₂O)₆]³⁺. The aqua ion loses H⁺ to water: a weak acid. 3+ ions: higher charge/size, O–H more polarised. 3+ solutions: pH about 1.7 (Fe³⁺) to 3 (Al³⁺). Carbonate: 3+ fizzes, 2+ gives MCO₃ and no gas.](/chemistry/assets/posters/metal-aqua-ions-and-acidity.png)



























