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Question

The reducing power of divalent species decreases in the order

A
Ge2+>Sn2+>Pb2+
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B
Sn2+>Ge2+>Pb2+
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C
Pb2+>Sn2+>Ge2+
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D
None of these
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Solution

The correct option is A Ge2+>Sn2+>Pb2+
Inert pair effect may be defined as inertness of inner ns sub-shell towards chemical reaction. It is seen in group 3A and 4A group especially (5s and 6s electrons). Therefore, Pb shows mainly +2 oxidation state frequently as compared to +4 oxidation state. Carbon and silicon mostly show +4 oxidation state. Germanium forms stable compounds in +4 state and only few compounds in +2 state. Tin forms compounds in both oxidation states.
So as we move down the group, due to inert pair effect lower oxidation state become more stable.
So,
The stability of + 2 O.S. follows the order
Pb2+>Sn2+>Ge2+
Higher the stability of +2 oxidation states, lesser will be its reducing power.
Therefore, order of reducing power is
Ge+2>Sn+2>Pb+2

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