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(A) An oxidising agent is a substance that gains electrons and undergoes reduction,meaning its oxidation state must be able to decrease.In $I^{-}$,the

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$I^{-}$

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(A) An oxidising agent is a substance that gains electrons and undergoes reduction,meaning its oxidation state must be able to decrease.In $I^{-}$,the iodine atom is in its lowest possible oxidation state of $-1$. Therefore,it cannot lose electrons to be reduced further; it can only act as a reducing agent by losing electrons to become $I_2$.Conversely,$S_{(s)}$,$NO_3^{-}$,and $Cr_2O_7^{2-}$ contain elements in oxidation states that can be reduced further.

Which one of the following cannot function as an oxidising agent?

Similar Questions

The main reason for the brown ring test of $NO_3^-$ is:

Acidified permanganate solution $(MnO_4^-)$ does not oxidize which of the following ions?

In the reaction $Cr_2O_7^{2-} + X \xrightarrow{H^+} Cr^{3+} + H_2O + \text{Oxidized product of } X$,which of the following cannot be $X$?

In the following reaction,which substance acts as a reducing agent?
$14H^+ + Cr_2O_7^{2-} + 3Ni \to 2Cr^{3+} + 7H_2O + 3Ni^{2+}$

Acidified permanganate solution does not oxidize:

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