Which of the following explanation is incorrect for ClO 4-species?

Question

Which of the following explanation is incorrect for ClO 4-species? (A) ClO 4-shows disproportionation reaction (B) ClO 4-does not show disproportionation reaction (C) The oxidation number of Cl is +7 in ClO 4- (D) ClO 4-is basic in nature

Tardigrade Admin · Accepted Answer

ClO 4-does not show disproportionation reaction because oxoanion of chlorine is present in its highest oxidation state, i.e. +7, so it does not further increase its oxidation number.

Q. Which of the following explanation is incorrect for $Cl O_{4}^{-}$ species?

$Cl O_{4}^{-}$ shows disproportionation reaction

$Cl O_{4}^{-}$ does not show disproportionation reaction

$T h e$ oxidation number of $Cl$ is $+ 7$ in $Cl O_{4}^{-}$

$Cl O_{4}^{-}$ is basic in nature

$Cl O_{4}^{-}$ does not show disproportionation reaction because oxoanion of chlorine is present in its highest oxidation state, i.e. $+ 7$ , so it does not further increase its oxidation number.

Q. Which of the following explanation is incorrect for ClO4−​species?

ClO4−​shows disproportionation reaction

ClO4−​does not show disproportionation reaction

The oxidation number of Cl is +7 in ClO4−​

ClO4−​is basic in nature