Question

The number of ions from the following that are expected to behave as oxidising agent is: $\text{Sn}^{4+}, \, \text{Sn}^{2+}, \, \text{Pb}^{2+}, \, \text{Tl}^{3+}, \, \text{Pb}^{4+}, \, \text{Tl}^{+}$

• A. 3
• B. 4
• C. 1
• D. 2

Answer 1

The Correct Option is D

To determine the ions that can behave as oxidizing agents, we need to understand the concept of oxidation states and the role of oxidizing agents:

• Oxidizing agents are species that can accept electrons, thereby getting reduced themselves while oxidizing another species.
• In general, a higher oxidation state of an element is more likely to accept electrons, making it a potential oxidizing agent.

Now, let's analyze the given ions:

1. \(\text{Sn}^{4+}\): Tin in the +4 oxidation state. It can potentially accept electrons to reduce to \(\text{Sn}^{2+}\), hence can act as an oxidizing agent.
2. \(\text{Sn}^{2+}\): Tin in the +2 oxidation state. It is already in a lower oxidation state and more likely to act as a reducing agent instead by losing electrons.
3. \(\text{Pb}^{2+}\): Lead in the +2 oxidation state. Similar to \(\text{Sn}^{2+}\), it is more likely to lose electrons and act as a reducing agent.
4. \(\text{Tl}^{3+}\): Thallium in the +3 oxidation state. It can gain electrons to reduce to \(\text{Tl}^+\), serving as an oxidizing agent.
5. \(\text{Pb}^{4+}\): Lead in the +4 oxidation state. It can accept electrons to reduce to \(\text{Pb}^{2+}\), thus can act as an oxidizing agent.
6. \(\text{Tl}^{+}\): Thallium in the +1 oxidation state. It is in a lower oxidation state and more likely to lose electrons, acting as a reducing agent.

Based on the above analysis, the ions that can act as oxidizing agents are:

• \(\text{Sn}^{4+}\)
• \(\text{Pb}^{4+}\)

Thus, the number of ions expected to behave as oxidizing agents is 2.

Therefore, the correct answer is 2.

Answer 2

Due to the inert pair effect, \(\text{Tl}^{3+}\) and \(\text{Pb}^{4+}\) can behave as oxidising agents.
Thus the correct answer is Option 4.