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Question

Ge(II) compounds are powerful reducing agents where as Pb(IV) compounds are strong oxidants. It can be due to:

A
Pb is more electronegative than Ge
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B
Ionisation potential of lead is less than that of Ge
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C
Ionic radii of Pb2+ and Pb4+ are larger than those of Ge2+ and Ge4+
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D
More pronounced inert pair effect in lead than in Ge
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Solution

The correct option is D More pronounced inert pair effect in lead than in Ge
The pair of electrons in valence sorbital is reluctant to take part in bond formation due to poor shielding effect of d and f electron in heavier elements. This is known as inert pair effect.
It is generally observed in post transition metal compounds.
More pronounced inert pair effect is in lead than in Ge.
So, Pb tends to be in +2 oxidation state where as Ge is stable in +4 oxidation state.
Hence, Pb(IV) compounds are reduced to Pb(II) and acts as strong oxidants.
Ge(II) compounds are oxidised to Ge(IV) and acts as powerful reducing agents.

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