Question:
The correct statements with respect to halides of group 14 elements are:
\[
\text{I. Both } CCl_4 \text{ and } SiCl_4 \text{ undergo hydrolysis.}
\]
\[
\text{II. } GeX_4 \text{ is more stable than } GeX_2.
\]
\[
\text{III. } PbX_4 \text{ is less stable than } PbX_2.
\]
IV. Stability of dihalides decreases down the group.
The correct statements with respect to halides of group 14 elements are:
\[ \text{I. Both } CCl_4 \text{ and } SiCl_4 \text{ undergo hydrolysis.} \] \[ \text{II. } GeX_4 \text{ is more stable than } GeX_2. \] \[ \text{III. } PbX_4 \text{ is less stable than } PbX_2. \] IV. Stability of dihalides decreases down the group.
\[ \text{I. Both } CCl_4 \text{ and } SiCl_4 \text{ undergo hydrolysis.} \] \[ \text{II. } GeX_4 \text{ is more stable than } GeX_2. \] \[ \text{III. } PbX_4 \text{ is less stable than } PbX_2. \] IV. Stability of dihalides decreases down the group.
Show Hint
In group 14, the inert pair effect increases down the group. Hence, the \(+2\) oxidation state becomes more stable down the group, especially for lead.
Updated On: Jun 24, 2026
- I, IV only
- II, IV only
- II, III only
- III, IV only
Show Solution
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The Correct Option is C
Solution and Explanation
Step 1: Check statement I.
\[ CCl_4 \] does not undergo hydrolysis because carbon has no vacant \(d\)-orbitals and cannot expand its octet.
However, \[ SiCl_4 \] undergoes hydrolysis because silicon can accept electron pairs from water.
So, statement I is false.
Step 2: Check statement II.
For germanium, the \(+4\) oxidation state is more stable than the \(+2\) oxidation state.
Therefore, \[ GeX_4 \] is more stable than \[ GeX_2 \] So, statement II is true.
Step 3: Check statement III.
Due to inert pair effect, the stability of \(+2\) oxidation state increases down group 14.
For lead, \[ Pb^{2+} \] is more stable than \[ Pb^{4+} \] Therefore, \[ PbX_4 \] is less stable than \[ PbX_2 \] So, statement III is true.
Step 4: Check statement IV.
The stability of dihalides increases down the group due to inert pair effect.
So, statement IV is false.
Step 5: Final conclusion.
Hence, the correct statements are \[ \boxed{\text{II, III only}} \]
\[ CCl_4 \] does not undergo hydrolysis because carbon has no vacant \(d\)-orbitals and cannot expand its octet.
However, \[ SiCl_4 \] undergoes hydrolysis because silicon can accept electron pairs from water.
So, statement I is false.
Step 2: Check statement II.
For germanium, the \(+4\) oxidation state is more stable than the \(+2\) oxidation state.
Therefore, \[ GeX_4 \] is more stable than \[ GeX_2 \] So, statement II is true.
Step 3: Check statement III.
Due to inert pair effect, the stability of \(+2\) oxidation state increases down group 14.
For lead, \[ Pb^{2+} \] is more stable than \[ Pb^{4+} \] Therefore, \[ PbX_4 \] is less stable than \[ PbX_2 \] So, statement III is true.
Step 4: Check statement IV.
The stability of dihalides increases down the group due to inert pair effect.
So, statement IV is false.
Step 5: Final conclusion.
Hence, the correct statements are \[ \boxed{\text{II, III only}} \]
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