Import Question JSON

$\text{Hint: Due to inert pair effect, } \text{Pb}^{2+} \text{ is more stable than } \text{Pb}^{4+} \text{ and } \text{Tl}^{+} \text{ is more stable than } \text{Tl}^{3+}.$ $\text{Due to inert pair effect, } \text{Pb}^{2+} \text{ is more stable than } \text{Pb}^{4+} \text{ and } \text{Tl}^{+} \text{ is more stable than } \text{Tl}^{3+}. \text{ Therefore, } \text{Pb}^{4+} \text{ and } \text{Tl}^{3+} \text{ only will act as oxidising agents.}$ $\bullet \ \text{Sn}^{2+}: \text{This is a relatively stable oxidation state of tin. It can act as a reducing agent, but it is not typically an oxidizing agent because it is more likely to lose electrons to form } \text{Sn}^{4+}.$ $\bullet \ \text{Sn}^{4+}: \text{This is the more stable oxidation state for tin, so } \text{Sn}^{4+} \text{ is unlikely to gain electrons further and therefore does not act as an oxidizing agent.}$ $\bullet \ \text{Pb}^{4+}: \text{Lead(IV) is relatively unstable and tends to reduce to } \text{Pb}^{2+}, \text{ so it can act as an oxidizing agent by accepting electrons.}$ $\bullet \ \text{Pb}^{2+}: \text{This is a stable oxidation state for lead, so it generally does not act as an oxidizing agent.}$ $\bullet \ \text{Tl}^{+}: \text{Thallium(I) is the more stable oxidation state of thallium, so it is unlikely to act as an oxidizing agent.}$ $\bullet \ \text{Tl}^{3+}: \text{Thallium(III) is relatively unstable and tends to reduce to } \text{Tl}^{+}, \text{ making it an oxidizing agent.}$