Learning objectives
Define enthalpy change of atomisation, first electron affinity and lattice energy (gaseous ions forming one mole of an ionic solid), and explain the trends in electron affinity in Groups 16 and 17
Construct Born–Haber cycles for ionic solids with 1+ or 2+ cations and 1− or 2− anions, and calculate a lattice energy or any other missing term from them
Define enthalpy changes of hydration and of solution, and use the cycle ΔHsol = ΣΔHhyd − ΔHlatt to calculate any one of the three quantities
Explain why smaller, more highly charged ions give more exothermic lattice energies and hydration enthalpies, e.g. MgO compared with NaCl
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