#5.2.1a
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 2.2.2b–c)
Definition required.
#5.2.1b
use of the lattice enthalpy of a simple ionic solid (e.g. NaCl, MgCl2) and relevant energy terms for:
(i) the construction of Born–Haber cycles
(ii) related calculations
Relevant energy terms: enthalpy change of formation, ionisation energy, enthalpy change of atomisation and electron affinity.
Definition required for first ionisation energy (see also 3.1.1c) and enthalpy change of formation (see also 3.2.1d) only.
#5.2.1c
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)
Definitions required.
Details of infinite dilution not required.
#5.2.1d
use of the enthalpy change of solution of a simple ionic solid (e.g. NaCl, MgCl2) and relevant energy terms (enthalpy change of hydration and lattice enthalpy) for:
(i) the construction of enthalpy cycles
(ii) related calculations
#5.2.1e
qualitative explanation of the effect of ionic charge and ionic radius on the exothermic value of a lattice enthalpy and enthalpy change of hydration.