The number of ions from the following that are expected to behave as oxidising agent is: $\text{Sn}^{4+}, \, \text{Sn}^{2+}, \, \text{Pb}^{2+}, \, \text{Tl}^{3+}, \, \text{Pb}^{4+}, \, \text{Tl}^{+}$
To identify potential oxidizing agents among the given ions, we must first define oxidation states and the function of oxidizing agents:
Oxidizing agents are chemical species that receive electrons. In this process, they are reduced while causing another species to be oxidized.
Elements in higher oxidation states generally exhibit a greater tendency to accept electrons, which qualifies them as potential oxidizing agents.
We will now examine each ion:
\(\text{Sn}^{4+}\): Tin is in the +4 oxidation state. This ion can accept electrons, reducing to \(\text{Sn}^{2+}\), and therefore functions as an oxidizing agent.
\(\text{Sn}^{2+}\): Tin is in the +2 oxidation state. Being in a lower oxidation state, it is more inclined to lose electrons and act as a reducing agent.
\(\text{Pb}^{2+}\): Lead is in the +2 oxidation state. Analogous to \(\text{Sn}^{2+}\), this ion is more prone to losing electrons and acting as a reducing agent.
\(\text{Tl}^{3+}\): Thallium is in the +3 oxidation state. This ion can accept electrons, reducing to \(\text{Tl}^+\), and thus acts as an oxidizing agent.
\(\text{Pb}^{4+}\): Lead is in the +4 oxidation state. This ion can accept electrons, reducing to \(\text{Pb}^{2+}\), and therefore functions as an oxidizing agent.
\(\text{Tl}^{+}\): Thallium is in the +1 oxidation state. In this lower oxidation state, it is more likely to lose electrons and act as a reducing agent.
Based on this assessment, the ions that can function as oxidizing agents are:
\(\text{Sn}^{4+}\)
\(\text{Pb}^{4+}\)
Consequently, there are 2 ions expected to act as oxidizing agents.
The correct answer is 2.
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