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Question

Germanium (II) compounds are powerful reducing agents whereas lead (IV) compounds are strong oxidising agents. It is due to:

A
Pb is more electronegative than Ge
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B
The ionisation energy of Pb is less than that of Ge
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C
The ionic radii of Pb2+ and Pb4+ are less than those of Ge2+ and Ge4+
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D
More pronounced inert pair effect in Pb than in Ge
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Solution

The correct option is D More pronounced inert pair effect in Pb than in Ge
Inert pair effect increases in group 14 as the atomic number increases, i.e., the stability of divalent state increases from Ge2+ to Pb2+. Hence, germanium (II) compounds are powerful reducing agents as they are more stable in +4 state and can be easily converted to Ge(IV) and Pb(IV) compounds are strong oxidising agent as they can be easily converted to Pb2+.

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