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(D) In $NaNO_2$ (Sodium nitrite),the oxidation state of nitrogen $(N)$ is $+3$. Nitrogen can be oxidized to a higher oxidation state (e.g.,$+5$ in $NO

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$NaNO_2$

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(D) In $NaNO_2$ (Sodium nitrite),the oxidation state of nitrogen $(N)$ is $+3$. Nitrogen can be oxidized to a higher oxidation state (e.g.,$+5$ in $NO_3^-$) or reduced to a lower oxidation state (e.g.,$+2, +1, 0, -3$). Therefore,$NaNO_2$ can act as both an oxidizing agent and a reducing agent. In $NaNO_3$,$N$ is in its maximum oxidation state $(+5)$,so it acts only as an oxidizing agent. In $Na_2O$,$O$ is in its minimum oxidation state $(-2)$,so it acts only as a reducing agent. In $Na_2O_2$,$O$ is in $-1$ state,which can be oxidized to $0$ or reduced to $-2$,but $NaNO_2$ is the classic example of a substance showing dual behavior due to the intermediate oxidation state of nitrogen.

Which of the following substances acts as both an oxidizing agent and a reducing agent?

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$P_4 + 3NaOH + 3H_2O \to 3NaH_2PO_2 + PH_3$ is an example of

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