The ion(s) that act/s as oxidizing agent in solution is/are

Options

A. `Tl^(+)` and `Al^(3+)`
B. `B^(3+)` and `Al^(3+)`
C. `Tl^(3+)` only
D. `B^(3+)` only

Explanation

To determine the ion(s) that act as oxidizing agents in solution, we need to analyze the oxidation states and stability of the given ions. Here’s a step-by-step solution:

### Step 1: Identify the Ions
We are given several ions: Tellurium (Te), Aluminum (Al), Boron (B), Gallium (Ga), and Indium (In). We need to assess their oxidation states and stability.

### Step 2: Analyze Tellurium
Tellurium can exist in multiple oxidation states, but the +1 oxidation state is particularly stable due to the inner pair effect. This means that in the +1 state, Tellurium is less likely to be reduced further, making it a good candidate for acting as an oxidizing agent.

### Step 3: Analyze Aluminum
Aluminum typically exists in the +3 oxidation state. Once it achieves this state, it has a stable electron configuration and does not easily get reduced further. Therefore, it does not act as an oxidizing agent.

### Step 4: Analyze Boron
Boron in the +3 oxidation state is also stable and has achieved a stable electron configuration by losing three electrons. Thus, it will not act as an oxidizing agent.

### Step 5: Analyze Gallium and Indium
Gallium and Indium can also exist in multiple oxidation states, but like Aluminum and Boron, their higher oxidation states are stable. Therefore, they do not act as oxidizing agents.

### Step 6: Conclusion
The only ion that acts as an oxidizing agent in solution is Tellurium in the +3 oxidation state. This is because it can be reduced to its +1 state, allowing it to oxidize other species.

### Final Answer
The ion that acts as an oxidizing agent in solution is Tellurium (Te) in the +3 oxidation state.

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