Which oxide among the following cannot act as | vedclass

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(C) reducing agent is a substance that can be oxidized,meaning its central atom must be able to increase its oxidation state.In $SO_2$,the oxidation s

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$CO_2$

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(C) reducing agent is a substance that can be oxidized,meaning its central atom must be able to increase its oxidation state.In $SO_2$,the oxidation state of $S$ is $+4$,and its maximum oxidation state is $+6$,so it can be oxidized.In $NO_2$,the oxidation state of $N$ is $+4$,and its maximum oxidation state is $+5$,so it can be oxidized.In $CO_2$,the oxidation state of $C$ is $+4$,which is its maximum group oxidation state (Group $14$). Therefore,it cannot be oxidized further and cannot act as a reducing agent.In $ClO_2$,the oxidation state of $Cl$ is $+4$,and its maximum oxidation state is $+7$,so it can be oxidized.

Which oxide among the following cannot act as a reducing agent?

Similar Questions

Which of these substances is a good reducing agent?

Which of the following may act as both an oxidising and a reducing agent?

For the reactions $(A) \ S^{2-} + 4H_2O_2 \rightarrow SO_4^{2-} + 4H_2O$ and $(B) \ Cl_2 + H_2O_2 \rightarrow 2HCl + O_2$,which statement is correct?

Which of the following acts as an oxidizing agent?

Which of the following compounds cannot act as a reducing agent?

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