The stability of the lower oxidation state increases down a group in the p-block due to the inert pair effect. Based on this principle, which of the following oxides will act as the most powerful oxidizing agent?

Step-by-step solution

The elements given belong to Group 14 of the periodic table: C, Si, Sn, Pb. The general oxidation states exhibited by Group 14 elements are +2 and +4. Down the group, the stability of the lower oxidation state (+2) increases and that of the higher oxidation state (+4) decreases due to the inert pair effect. For lead (Pb), the +2 oxidation state is much more stable than the +4 oxidation state. In PbO₂ , lead is in the +4 oxidation state, which is highly unstable. Therefore, PbO₂ readily accepts electrons to get redu