`Cl_(2` is stronger `…………………..` agent then `Br_(2)` and `I_(2)` as its reduction potential is `………………………` than that of `Br_(2)` and `I_(2)`

Explanation

To solve the question, we need to fill in the blanks regarding the strength of chlorine (Cl₂) as an oxidizing agent compared to bromine (Br₂) and iodine (I₂), based on their reduction potentials.

### Step-by-Step Solution:

1. **Identify the Strength of Oxidizing Agents**:
- Oxidizing agents are substances that can gain electrons and, in the process, cause another substance to be oxidized. The strength of an oxidizing agent is determined by its reduction potential. A higher reduction potential indicates a stronger oxidizing agent.

2. **Know the Reduction Potentials**:
- We need to know the standard reduction potentials for Cl₂, Br₂, and I₂:
- Cl₂ + 2e⁻ → 2Cl⁻; E° = +1.36 V
- Br₂ + 2e⁻ → 2Br⁻; E° = +1.06 V
- I₂ + 2e⁻ → 2I⁻; E° = +0.54 V

3. **Compare the Reduction Potentials**:
- From the values:
- Cl₂ has a reduction potential of +1.36 V.
- Br₂ has a reduction potential of +1.06 V.
- I₂ has a reduction potential of +0.54 V.
- It is clear that Cl₂ has the highest reduction potential among the three.

4. **Fill in the Blanks**:
- Since Cl₂ has a higher reduction potential than both Br₂ and I₂, we can conclude:
- Cl₂ is a stronger **oxidizing** agent than Br₂ and I₂.
- Its reduction potential is **more** than that of Br₂ and I₂.

### Final Answers:
- Cl₂ is a stronger **oxidizing** agent than Br₂ and I₂ as its reduction potential is **more** than that of Br₂ and I₂.