The table shows the values for all but one of the enthalpy changes relevant to this cycle.

Enthalpy change	Value/$\mathrm{kJ} {\mathrm{mol}}^{-1}$
lattice energy	$-2327$
enthalpy change of hydration of ${\mathrm{Mg}}^{2+}$ ion	$-1920$
enthalpy change of hydration of ${\mathrm{I}}^{-}$ ion	$-314$

Use the values in the table to calculate the value for the enthalpy change of solution of magnesium iodide. (Only give the value without units)

Draw a diagram to show how water molecules are arranged around a magnesium ion.

The lattice energy of magnesium bromide, ${\mathrm{MgBr}}_2$ can be calculated using the enthalpy changes shown in the table.

State the meaning of the term lattice energy.

The lattice energy of magnesium bromide, ${\mathrm{MgBr}}_2$ can be calculated using the enthalpy changes shown in the table.

State the meaning of the term second ionisation energy.

The lattice energy of magnesium bromide, ${\mathrm{MgBr}}_2$ can be calculated using the enthalpy changes shown in the table.

Draw and label a Born-Haber cycle to calculate the lattice energy of magnesium bromide and calculate the lattice energy of magnesium bromide.

For the pair $\mathrm{NaCl}$ and $\mathrm{KBr}$, state with reasons, which one you would expect to have the higher lattice energy.

For the pair $\mathrm{KCl}$ and $\mathrm{SrS}$, state with reasons, which one you would expect to have the higher lattice energy.

In some crystal lattices, some of the ions are polarised. State the meaning of the term ion polarisation.