Which of the following does not show a dispro | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) disproportionation reaction is a type of redox reaction in which the same element is simultaneously oxidized and reduced.For an element to undergo

Vedclass · Accepted Answer

$ClO_4^{-}$

Vedclass · Answer

(C) disproportionation reaction is a type of redox reaction in which the same element is simultaneously oxidized and reduced.For an element to undergo disproportionation,it must be in an intermediate oxidation state.In $ClO_4^{-}$,the oxidation state of $Cl$ is calculated as: $x + 4(-2) = -1$,which gives $x = +7$.Since $+7$ is the maximum possible oxidation state for chlorine (as it has $7$ valence electrons),it cannot be further oxidized.Therefore,$ClO_4^{-}$ cannot undergo a disproportionation reaction.

Which of the following does not show a disproportionation reaction?

Similar Questions

What is meant by 'disproportionation' of an oxidation state? Give an example.

Fluorine reacts with ice and results in the change: $H_2O_{(s)} + F_{2(g)} \to HF_{(g)} + HOF_{(g)}$. Justify that this reaction is a redox reaction.

An example of a disproportionation reaction is

Which species among the following does not show disproportionation reactions?

Which of the following is a disproportionation redox reaction?

Vedclass Test Series

Exam Paper Generator

Online Exam Module