Ge(II) compounds are strong reducing agents,w | vedclass

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(D) In group $14$ elements,the stability of the $+2$ oxidation state increases down the group due to the inert pair effect. $Ge$ is at the top of the

Vedclass · Accepted Answer

The more pronounced inert pair effect in $Pb$ compared to $Ge$.

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(D) In group $14$ elements,the stability of the $+2$ oxidation state increases down the group due to the inert pair effect. $Ge$ is at the top of the group,so $Ge(IV)$ is more stable than $Ge(II)$. Thus,$Ge(II)$ tends to lose two more electrons to reach the stable $+4$ state,acting as a strong reducing agent. Conversely,$Pb$ is at the bottom of the group,so $Pb(II)$ is more stable than $Pb(IV)$ due to the inert pair effect. Thus,$Pb(IV)$ tends to gain two electrons to reach the stable $+2$ state,acting as a strong oxidizing agent.

$Ge(II)$ compounds are strong reducing agents,whereas $Pb(IV)$ compounds are strong oxidizing agents. This is due to:

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