Two statements are given below. Statement I: $\mathrm{SnF}_4, \mathrm{PbF}_4$ are ionic in nature Statement…
Two statements are given below.
Statement I: $\mathrm{SnF}_4, \mathrm{PbF}_4$ are ionic in nature
Statement II: $\mathrm{GeCl}_2$ is more stable than $\mathrm{GeCl}_4$
The correct answer is
Both statements I \& II are correct
Both statements I \& II are not correct
Statement I is correct, but statement II is not correct
Statement I is not correct, but statement II is correct
Solution
In group 14 , most of the $\mathrm{MX}_4$ are covalent in nature exceptions $\mathrm{SnF}_4$ and $\mathrm{PbF}_4$ because there is more electronegativity difference make the bond ionic. So statement I is correct.
Ge electronic configuration : $[\mathrm{Ar}] 3 \mathrm{~d}^{10} 4 \mathrm{~s}^2 4 \mathrm{p}^2$ and $\mathrm{Ge}^{+4}$ oxidation is more stable because its allows germanium to achieve a full valence shell, which is energetically more favorable than having an incomplete valence shell in the $\mathrm{Ge}^{+2}$ oxidation state.
'So' only statement I is correct.