If water is added to magnesium nitride, $\text{Mg}_3\text{N}_2$, a white suspension of $\text{Mg(OH)}_2$ and an alkaline gas are formed. Write the equation for this reaction.
A sample of $2.52\,\text{g}$ of $\text{Mg}_3\text{N}_2$ is placed in excess water. Determine the mass of $\text{Mg(OH)}_2$ produced.
State and explain how the solubility of the Group 2 hydroxides changes down the group.
Magnesium hydroxide is only slightly soluble in water. The concentration of its saturated solution at $298\,\text{K}$ is $1.7 \times 10^{-4}\,\text{mol dm}^{-3}$. Write an expression for the solubility product, $K_{sp}$, of $\text{Mg(OH)}_2$.
Find the value of $K_{sp}$ for $\text{Mg(OH)}_2$ at $298\,\text{K}$ and give the units.
The temperatures at which Group 2 hydroxides and carbonates begin to decompose increase down the group. Suggest why the decomposition temperature of the Group 2 hydroxides shows this pattern.