Question

Assertion :$Cl{O}_4^{-}$ does not show disproportionation reaction. Reason: In $Cl{O}_4^{-}$, chlorine is present in its highest oxidation state.

• A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
• B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
• C. Assertion is correct but Reason is incorrect
• D. Both Assertion and Reason are incorrect

Answer 1

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

In $Cl{O}_4^{-}$, chlorine has an oxidation state of $+7$ which is its maximum oxidation state. Now to reduce other compound, it has to gain electrons. But $Cl{O}_4^{-}$ cannot gain $e^{-}$ as it has reached maximum oxidation state of chlorine. Hence, it cannot act as reducing agent. In disproportionation, it is necessary that $Cl{O}_4^{-}$gets oxidised as well as reduced , which is not possible.