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.