Question

Ge (II) compounds are powerful reducing agents whereas Pb (IV) compounds are strong oxidants. It can be because:

• A. Pb is more electropositive than Ge
• B. Ionisation potential of lead is less than that of Ge.
• C. Ionic radii of Pb\(^{2+}\) and Pb\(^{4+}\) are larger than that of Ge\(^{2+}\) and Ge\(^{4+}\).
• D. More pronounced inert pair effect in lead has.

Hint:

The inert pair effect increases down a group, particularly for heavier elements like lead, making them more likely to form lower oxidation states.

Answer 1

The Correct Option is D

The inert pair effect refers to the tendency of the s-electrons to remain non-bonding or less reactive in heavier elements. Lead (Pb), being a heavier element, exhibits a more pronounced inert pair effect than germanium (Ge). This effect makes Pb(II) more stable and less likely to undergo oxidation to Pb(IV), whereas Pb(IV) is more prone to reduction. In contrast, Ge(II) compounds are more reactive and easily oxidized to Ge(IV), making them powerful reducing agents. The inert pair effect is the dominant reason for the contrasting behavior of Ge and Pb in their respective oxidation states.