Question:
Which of the following tetrahalides does not exist?
Which of the following tetrahalides does not exist?
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Due to inert pair effect, the stability of the \(+4\) oxidation state decreases down Group 14. Heavy elements like lead prefer the \(+2\) oxidation state.
Updated On: Jun 15, 2026
- \(\mathrm{CCl_4}\)
- \(\mathrm{SiCl_4}\)
- \(\mathrm{PbCl_4}\)
- \(\mathrm{PbI_4}\)
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The Correct Option is D
Solution and Explanation
Step 1: Understand the stability of Group 14 tetrahalides.
Group 14 elements form tetrahalides in the \(+4\) oxidation state. However, the stability of the \(+4\) oxidation state decreases down the group because of the inert pair effect.
Step 2: Analyze lead tetrahalides.
Lead commonly shows the \(+2\) oxidation state more stable than the \(+4\) state.
Among lead tetrahalides, \(\mathrm{PbCl_4}\) can exist under controlled conditions, but \(\mathrm{PbI_4}\) is unstable because iodide ion is a strong reducing agent.
Step 3: Explain decomposition of \(\mathrm{PbI_4}\).
\(\mathrm{Pb^{4+}}\) oxidizes \(\mathrm{I^-}\) to iodine and itself gets reduced to \(\mathrm{Pb^{2+}}\).
\[ \mathrm{PbI_4\rightarrow PbI_2+I_2} \]
Hence, \(\mathrm{PbI_4}\) does not exist as a stable compound.
Step 4: Final conclusion.
Therefore, the tetrahalide that does not exist is
\[ \boxed{\mathrm{PbI_4}} \]
Group 14 elements form tetrahalides in the \(+4\) oxidation state. However, the stability of the \(+4\) oxidation state decreases down the group because of the inert pair effect.
Step 2: Analyze lead tetrahalides.
Lead commonly shows the \(+2\) oxidation state more stable than the \(+4\) state.
Among lead tetrahalides, \(\mathrm{PbCl_4}\) can exist under controlled conditions, but \(\mathrm{PbI_4}\) is unstable because iodide ion is a strong reducing agent.
Step 3: Explain decomposition of \(\mathrm{PbI_4}\).
\(\mathrm{Pb^{4+}}\) oxidizes \(\mathrm{I^-}\) to iodine and itself gets reduced to \(\mathrm{Pb^{2+}}\).
\[ \mathrm{PbI_4\rightarrow PbI_2+I_2} \]
Hence, \(\mathrm{PbI_4}\) does not exist as a stable compound.
Step 4: Final conclusion.
Therefore, the tetrahalide that does not exist is
\[ \boxed{\mathrm{PbI_4}} \]
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