(a) explanation of the term lattice enthalpy (formation of 1 mol of ionic lattice from gaseous ions, ∆LEH) and use as a measure of the strength of ionic bonding in a giant ionic lattice (see also 2.2.2 b–c)

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(b) use of the lattice enthalpy of a simple ionic solid (e.g. NaCl, MgCl 2) and relevant energy terms for:

              (i) the construction of Born–Haber cycles

              (ii) related calculations

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(c) explanation and use of the terms:

              (i) enthalpy change of solution (dissolving of 1 mol of solute, ∆solH)

              (ii) enthalpy change of hydration (dissolving of 1 mol of gaseous ions in water, ∆hydH)

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(d) use of the enthalpy change of solution of a simple ionic solid (e.g. NaCl, MgCl 2) and relevant energy terms (enthalpy change of hydration and lattice enthalpy) for:

(i) the construction of enthalpy cycles

(ii) related calculations

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(e) qualitative explanation of the effect of ionic charge and ionic radius on the exothermic value of a lattice enthalpy and enthalpy change of hydration.