Question

Germanium $\left(II\right)$ compounds are powerful reducing agents whereas lead $\left(IV\right)$ compounds are strong oxidising agents. It is due to:

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

Answer 1

The correct option is D More pronounced inert pair effect in $Pb$ than in $Ge$

Inert pair effect increases in group $14$ as the atomic number increases, i.e., the stability of divalent state increases from $G{e}^{2+}$ to $P{b}^{2+}$. Hence, germanium $\left(II\right)$ compounds are powerful reducing agents as they are more stable in $+4$ state and can be easily converted to $Ge\left(IV\right)$ and $Pb\left(IV\right)$ compounds are strong oxidising agent as they can be easily converted to $P{b}^{2+}$.