The solubility of the Group 2 hydroxides rises as you go down the group. Explain this pattern.
At $298\,\text{K}$, the solubility of $\text{Be(OH)}_2$ in water is $2.40 \times 10^{-6}\,\text{g dm}^{-3}$. Write the solubility product expression, $K_{sp}$, for $\text{Be(OH)}_2$ and give its units.
Calculate the numerical value of $K_{sp}$ for $\text{Be(OH)}_2$ at $298\,\text{K}$.
$\text{Be(OH)}_2$ dissolves in alkaline solutions that contain excess hydroxide ions and produces the complex ion $[\text{Be(OH)}_4]^{2-}$. Define the term complex ion.
Draw a three-dimensional diagram to show the structure of the complex ion $[\text{Be(OH)}_4]^{2-}$. Name the shape of the $[\text{Be(OH)}_4]^{2-}$ complex ion.
Explain why transition elements can form complex ions.
Complete Table 1.1 to show the coordination number of each metal ion, and the shapes and overall polarities of the complex ions listed: cis-$[\text{Pt(H}_2\text{NCH}_2\text{CH}_2\text{NH}_2)\text{Cl}_2]$, $[\text{Ag(NH}_3)_2]^+$, and $[\text{Fe(C}_2\text{O}_4)_3]^{3-}$.
Define stability constant, $K_{stab}$.
Nickel can form complexes with the ligands $en$, $\text{H}_2\text{NCH}_2\text{CH}_2\text{NH}_2$, and $tn$, $\text{H}_2\text{NCH}_2\text{CH}_2\text{CH}_2\text{NH}_2$, as shown. Equilibrium 1: $[\text{Ni(H}_2\text{O})_6]^{2+} + 3en \rightleftharpoons [\text{Ni(en)}_3]^{2+} + 6\text{H}_2\text{O}$, $K_{stab} = 6.76 \times 10^{17}$. Equilibrium 2: $[\text{Ni(H}_2\text{O})_6]^{2+} + 3tn \rightleftharpoons [\text{Ni(tn)}_3]^{2+} + 6\text{H}_2\text{O}$, $K_{stab} = 1.86 \times 10^{12}$. Construct an expression for the stability constant, $K_{stab}$, for equilibrium 1 and state its units.
Describe what the $K_{stab}$ values show about the equilibrium position for equilibrium 1 and 2. Use the $K_{stab}$ values to decide which complex, $[\text{Ni(en)}_3]^{2+}$ or $[\text{Ni(tn)}_3]^{2+}$, is more stable.