ZIMSEC · Form 5 · Lower 6
Chemistry
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- Atomic structure and electron configuration Electrons occupy s, p, d and f sub-shells. An orbital holds up to two electrons of opposite spin. Order of filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p.
- Chemical bonding, shapes and intermolecular forces Ionic (electrostatic attraction between ions), covalent (shared pairs, including dative bonds where both electrons come from one atom, e.g. NH₄⁺) and metallic.
- Stoichiometry and the mole The reactant that runs out first determines the amount of product.
- Chemical energetics ΔH is negative for exothermic and positive for endothermic reactions. Standard conditions: 298 K, 100 kPa (or 1 atm), 1 mol dm⁻³.
- Chemical equilibria and acid–base chemistry In a closed system, forward and reverse rates are equal and concentrations remain constant.
- The periodic table: periodicity, groups and transition elements Reactivity increases down the group. Hydroxides become more soluble and sulfates less soluble down the group; carbonates and nitrates become more thermally stable down the group (larger cations polarise the anion less).
- Organic chemistry: hydrocarbons and halogenoalkanes Homologous series, functional groups, IUPAC naming and isomerism: structural (chain, position, functional group) and stereoisomerism (geometric cis/trans around C=C; optical, with a chiral carbon bonded to four different groups).