Question

The species which does not undergo disproportionation reaction is:

• A. \( \text{ClO}_2^- \)
• B. \( \text{ClO}_4^- \)
• C. \( \text{ClO}_3^- \)
• D. \( \text{ClO}_2 \)

Hint:

Disproportionation reactions typically occur with species that are in intermediate oxidation states and have higher or lower oxidation states they can transition into.

Answer 1

The Correct Option is B

Disproportionation reactions involve a species being simultaneously oxidized and reduced to form two different products. Among the given species: - \( \text{ClO}_2^- \) and \( \text{ClO}_3^- \) can undergo disproportionation to form \( \text{ClO}_3^- \) and \( \text{ClO}_2 \), respectively. - \( \text{ClO}_4^- \) does not undergo disproportionation because it is already in its most oxidized state as a chlorine(V) species, and there is no higher oxidation state to form. Thus, the correct answer is \( \text{ClO}_4^- \), which does not undergo disproportionation.