Complete the electronic structures of a calcium atom, $\text{1s}^2\text{2s}^2\text{2p}^6\,\ldots\ldots\ldots\ldots\ldots\ldots\ldots\ldots$ and of a calcium ion with a $+2$ oxidation state, $\text{1s}^2\text{2s}^2\text{2p}^6\,\ldots\ldots\ldots\ldots\ldots\ldots$.
Calcium nitrate, $\text{Ca(NO}_3)_2$, is used in fertilisers and can be made by an acid-base reaction. Write an equation showing the preparation of calcium nitrate by an acid-base reaction.
When anhydrous calcium nitrate is heated strongly, it decomposes and leaves a white solid. Identify this solid and suggest one additional observation for the reaction.
The ease with which the Group II nitrates undergo thermal decomposition falls down the group. Explain this trend.
What does the term standard enthalpy change of hydration, $\Delta H^{\theta}_{\text{hyd}}$, mean?
Use the data below to calculate the lattice energy, $\Delta H^{\theta}_{\text{latt}}$, of calcium nitrate, $\text{Ca(NO}_3)_2\text{(s)}$. It may help to draw an energy cycle.
The standard enthalpy change of hydration for $\text{Ba}^{2+}$, $\Delta H^{\theta}_{\text{hyd}}(\text{Ba}^{2+}\text{(g)})$, is $-1305\,\text{kJ mol}^{-1}$. Suggest an explanation for why the $\Delta H^{\theta}_{\text{hyd}}$ of the $\text{Ba}^{2+}$ ion is less exothermic than the $\Delta H^{\theta}_{\text{hyd}}$ of the $\text{Ca}^{2+}$ ion.