Write the equation for the decomposition of strontium hydrogencarbonate, $\mathrm{Sr(HCO_3)_2}$.
Thermal stability of Group 2 carbonates rises down the group. Explain this pattern.
The hydroxides and fluorides of Group 2 elements follow similar solubility patterns. Describe how the solubility of the fluorides of calcium, strontium and barium changes. Explain your answer.
Define enthalpy change of hydration, $\Delta H_{\mathrm{hyd}}$.
State the main factors that influence the size of the enthalpy change of hydration. Explain your answer.
Table 1.1 lists several energy changes. Use the data in Table 1.1 to work out the enthalpy change of solution, $\Delta H_{\mathrm{sol}}$, for $\mathrm{MgF_2(s)}$. Drawing a labelled energy cycle may help. Show your working.
Mercury(I) fluoride, $\mathrm{Hg_2F_2}$, has only limited solubility in water. In $\mathrm{Hg_2F_2}$ the cation is the diatomic ion $\mathrm{Hg_2^{2+}}$, which contains a covalent $\mathrm{Hg{-}Hg}$ bond. Write the solubility product expression, $K_{sp}$, for $\mathrm{Hg_2F_2}$. Include the units.
The solubility of $\mathrm{Hg_2F_2}$ is $9.20 \times 10^{-3}\ \mathrm{mol\ dm^{-3}}$ at $298\ \mathrm{K}$. Calculate the value of $K_{sp}$ for $\mathrm{Hg_2F_2}$ at $298\ \mathrm{K}$.