Standard reduction potentials of the half reactions are given below
`{:(F_(2(g))+2e^(-) rarr 2F^(-)""_((aq)),,E^(@)=+2.85V), (Cl_(2(g))+2e^(-) rarr 2Cl^(-)""_((aq)),, E^(@)=+1.36V), (Br_(2(l))+2e^(-) rarr 2Br^(-)""_((aq)),,E^(@)=+1.06V), (l_(2(s))+2e^(-) rarr 2l^(-)""_((aq)),, E^(@)=+0.53V):}`
The strongest oxidising and reducing agents respectively are

Options

A. `F_(2)" and "l^(-)`
B. `Br_(2)" and "Cl^(-)`
C. `Cl_(2)" and "Br^(-)`
D. `Cl_(2)" and "l_(2)`

Answer

To determine the strongest oxidizing and reducing agents from the given standard reduction potentials, we can follow these steps:

### Step 1: Understand Standard Reduction Potentials
Standard reduction potentials (E°) indicate the tendency of a species to gain electrons (be reduced). The higher the E° value, the stronger the oxidizing agent. Conversely, the lower the E° value, the stronger the reducing agent.

### Step 2: Identify the Highest and Lowest E° Values
From the given half-reactions and their standard reduction potentials:
- \( \text{F}_2(g) + 2e^- \rightarrow 2\text{F}^-(aq) \), \( E° = +2.85 \, \text{V} \)
- \( \text{Cl}_2(g) + 2e^- \rightarrow 2\text{Cl}^-(aq) \), \( E° = +1.36 \, \text{V} \)
- \( \text{Br}_2(l) + 2e^- \rightarrow 2\text{Br}^-(aq) \), \( E° = +1.06 \, \text{V} \)
- \( \text{I}_2(s) + 2e^- \rightarrow 2\text{I}^-(aq) \), \( E° = +0.53 \, \text{V} \)

### Step 3: Determine the Strongest Oxidizing Agent
The strongest oxidizing agent corresponds to the half-reaction with the highest E° value. Here, \( \text{F}_2 \) has the highest E° value of +2.85 V, making it the strongest oxidizing agent.

### Step 4: Determine the Strongest Reducing Agent
The strongest reducing agent corresponds to the half-reaction with the lowest E° value. Here, \( \text{I}^- \) (from the half-reaction involving \( \text{I}_2 \)) has the lowest E° value of +0.53 V, making it the strongest reducing agent.

### Conclusion
Thus, the strongest oxidizing agent is \( \text{F}_2 \) and the strongest reducing agent is \( \text{I}^- \).

### Final Answer
- Strongest oxidizing agent: \( \text{F}_2 \)
- Strongest reducing agent: \( \text{I}^- \)

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