Question

$Ge(II)$ compounds are more powerful reducing agents whereas $Pb(IV)$ compounds are strong oxidants. It can be due to

• A. $Pb$ is more electropositive than $Ge$
• B. ionisation potential of lead is less than that of $Ge$
• C. ionic radii of $P{b}^{2+}$ and $P{b}^{4+}$ are larger than those of $G{e}^{2+}$ and $G{e}^{4+}$
• D. more pronounced inert pair effect in lead than in Ge

Answer 1

Answer: (D)

$Ge(IV)$ is more stable than $Ge(II)$ . Therefore, $Ge(II)$ compounds are powerful reducing agents. $Pb(IV)$ is less stable than $Pb(II)$ . Therefore, $Pb(IV)$ compounds are powerful oxidising agents. This is due to inert pair effect, due to which the +2 oxidation state becomes more stable on moving down the group.