Which of the following species, do not show disproportionation reaction and why ?
`ClO^(-) , ClO_(2)^(-) , ClO_(3)^(-) ` and `ClO_(4)^(-)`
Also write reaction for each of the species that disproportionates.

Explanation

To determine which of the given species do not show disproportionation reactions and to write the reactions for those that do, we will analyze the oxidation states of chlorine in each species.

### Step 1: Identify the oxidation states of chlorine in each species.

1. **For ClO⁻ (Hypochlorite ion)**:
- Let the oxidation state of Cl be \( x \).
- The equation becomes: \( x + (-2) = -1 \) (since O has an oxidation state of -2).
- Therefore, \( x = +1 \).
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