The correct statements with respect to halides of group 14 elements are I. Both $\mathrm{CCl}_4$ and…
The correct statements with respect to halides of group 14 elements are
I. Both $\mathrm{CCl}_4$ and $\mathrm{SiCl}_4$ undergo hydrolysis
II. $\mathrm{GeX}_4$ is more stable than $\mathrm{GeX}_2$
III. $\mathrm{PbX}_4$ is less stable than $\mathrm{PbX}_2$
IV. Stability of dihalides decreases down the group.
I, IV only
II, IV only
II, III only
III, IV only
Solution
$\mathrm{CCl}_4$ does not undergo hydrolysis since $\mathrm{C}$ does not have 'd' orbital to accept the electrons from donor.
$\therefore \quad$ (I) is incorrect.
GP. 14 elements have 4 electrons in their valence shells.
So, $(+4)$ and $(+2)$ are the common oxidate states (O.S.)
for $\mathrm{C}$ to $\mathrm{Pb}$. However, the stability of $(+4)$ O.S. decreases from $\mathrm{Ge}$ to $\mathrm{Pb}(\mathrm{Ge} < \mathrm{Sn} < \mathrm{Pb})$ due to inert pair effect.
Therefore, Ge forms stable compound in $(+4)$ O.S. and $\mathrm{Pb}$ in $(+2)$ O.S. $\therefore$ (II) $\&$ (III) are correct.
Stability of dihalides increases down the group.
$\therefore \quad$ (IV) is incorrect.