(a(i))[2]
Define the term lattice energy, $\Delta H_{\text{latt}}$.
(a(ii))[1]
Define the enthalpy change of solution, $\Delta H_{\text{sol}}$.
(b)[1]
The enthalpy change of hydration may be written as $\Delta H_{\text{hyd}}$. Write the mathematical expression for the $\Delta H_{\text{sol}}$ of NaCl in terms of $\Delta H_{\text{latt}}(\text{NaCl})$, $\Delta H_{\text{hyd}}(\text{Na}^+)$ and $\Delta H_{\text{hyd}}(\text{Cl}^-)$.
(c)[3]
Complete the Born-Haber cycle in Fig. 8.1 for the ionic solid NaCl. Add the state symbols for the relevant species.
(d)[2]
Predict which ion, $\text{Cl}^-$ or $\text{NO}_3^-$, has the more negative enthalpy change of hydration. Explain your reasoning.