The species which does not undergo disproportionation reaction is:
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Disproportionation reactions typically occur with species that are in intermediate oxidation states and have higher or lower oxidation states they can transition into.
A disproportionation reaction occurs when a species is simultaneously oxidized and reduced, yielding two distinct products. Considering the provided species:- \( \text{ClO}_2^- \) and \( \text{ClO}_3^- \) can undergo disproportionation, producing \( \text{ClO}_3^- \) and \( \text{ClO}_2 \), respectively.- \( \text{ClO}_4^- \) does not participate in disproportionation reactions because chlorine exists in its highest oxidation state (chlorine(V)), precluding further oxidation.Therefore, \( \text{ClO}_4^- \) is identified as the species that does not undergo disproportionation.
