The number of ions from the following that are expected to behave as oxidising agent is :
$$\mathrm{Sn}^{4+}, \mathrm{Sn}^{2+}, \mathrm{Pb}^{2+}, \mathrm{Tl}^{3+}, \mathrm{Pb}^{4+}, \mathrm{Tl}^{+}$$
Solution
<p>Due to inert pair effect $\mathrm{Pb}^{2+}$ is more stable than $\mathrm{Pb}^{4+}$ and $\mathrm{Tl}^{+}$ is more stable than $\mathrm{Tl}^{3+}$. Therefore, $\mathrm{Pb}^{4+}$ and $\mathrm{T}^{3+}$ will function as oxidising agents and easily get reduced to $\mathrm{Pb}^{2+}$ and $\mathrm{TI}^{+}$ respectively.</p>
About this question
Subject: Chemistry · Chapter: Redox Reactions · Topic: Oxidation States
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