Question

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

Answer 1

Relative stability of +2 oxidation state progressively increases for heavier elements. Thus, Germanium forms stable compounds in +4 state and only few compounds in +2 state.
Ge(II) tends to acquire Ge (IV) state by loss of electrons. Hence it is reducing in nature. Pb shows mainly +2 oxidation state frequently as compared to +4 oxidation state. This is due to the inert pair effect. Pb (IV) tends to acquire Pb (II) O.S. by gain of electrons. Hence it is oxidising in nature.
Thus, option (d) is correct.