Write an equation for the thermal decomposition of strontium hydrogencarbonate, $\text{Sr(HCO}_3\text{)}_2$.
Explain why the thermal stability of Group 2 carbonates rises down the group.
The hydroxides and fluorides of Group 2 elements show similar solubility patterns. Describe the pattern in the solubility of the fluorides of calcium, strontium and barium. Explain your answer.
Define $\Delta H_{\mathrm{hyd}}$, the enthalpy change of hydration.
State the main factors that influence the size of enthalpy change of hydration. Explain your answer.
Table 1.1 gives several energy changes. Use data from Table 1.1 to calculate the enthalpy change of solution, $\Delta H_{\mathrm{sol}}$, for $\text{MgF}_2$(s). Drawing a labelled energy cycle may help. Show your working.
Mercury(I) fluoride, Hg$_2$F$_2$, is only sparingly soluble in water. In Hg$_2$F$_2$, the cation is the diatomic ion Hg$_2^{2+}$ with a covalent Hg-Hg bond. Write the solubility product expression, $K_{\mathrm{sp}}$, for Hg$_2$F$_2$. Include the units.
At 298 K, the solubility of Hg$_2$F$_2$ is $9.20 \times 10^{-3}\ \mathrm{mol\ dm^{-3}}$. Calculate $K_{\mathrm{sp}}$ for Hg$_2$F$_2$ at 298 K.