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  • In which one of the following sets all species show disproportionation reaction?Option: 1 <img alt="\mathrm{ClO}_{4}^{-}, \mathrm{MnO}_{4}^{-}, \mathrm{ClO}_{2}^{-}$and $\mathrm{F}_{2}" src="https://entrancecorner.codecogs.com/gif.latex?%5Cmat

In which one of the following sets all species show disproportionation reaction?
Option: 1 \mathrm{ClO}_{4}^{-}, \mathrm{MnO}_{4}^{-}, \mathrm{ClO}_{2}^{-}$and $\mathrm{F}_{2}
Option: 2 \mathrm{ClO}_{2}^{-}, \mathrm{Cl}_{2}$ and $\mathrm{Mn}^{3+}
Option: 3 \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}, \mathrm{MnO}_{4}^{-}, \mathrm{ClO}_{2}^{-}$and $\mathrm{Cl}_{2}
Option: 4 \mathrm{ClO}_{2}^{-}, \mathrm{F}_{2}, \mathrm{MnO}_{4}^{-}$and $\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}

Answers (1)

best_answer

As we have learnt,

\mathrm{-MnO_{4}^{-}\: and \: Cr_{2}O_{7}^{2-}} cannot disproportionate because the metals are present in their highest oxidation state.

\mathrm{-F_{2}}  cannot disproportionate as it cannot have a positive oxidation state

\mathrm{-ClO_{2}^{-},Cl_2\: and \: Mn^{3+}}  show disproportionation reaction

Hence, the correct answer is option (2)

Posted by

sudhir.kumar

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