The redusing power of divalent species decreases in the order
1) Ge > Sn > Pb
2) Sn > Ge > Pb
38 Pb >3 > Ge
4) Non of these
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3
Answer:
Option A
Ge > Sn > Pb
ReAsOn :
Reduction involves increases in the oxidation state of the reducing agent. The stability of +2 state increases down the group-most stable in case of lead and least stable in case of Ge. So, the reducing power of divalent spcies decreases in the order Ge gt Sn gt Pb.
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The reducing power of divalent species decreases in the order
Ge > Sn > Pb
Explaination :
The tendency to show the +2 oxidation state increases as we move down the group. This is due to the inert pair effect which causes the inability of ns² electrons of valence shell to participate in bonding.
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