JEE Main 2023 — Redox Reactions Question with Solution

To find the sum of the oxidation states of the metals in ${\mathrm{Fe}(\mathrm{CO})}_5$, ${\mathrm{VO}}^{2+}$, and ${\mathrm{WO}}_3$, we first need to find the oxidation states of the metals in each compound.

1. ${\mathrm{Fe}(\mathrm{CO})}_5$: The compound $\mathrm{CO}$ is a neutral ligand, so it does not contribute to the oxidation state of the metal. Hence, the oxidation state of Fe in ${\mathrm{Fe}(\mathrm{CO})}_5$ is 0.




2. ${\mathrm{VO}}^{2+}$: The compound $\mathrm{O}$ has an oxidation state of -2, and since the overall charge of the compound is +2, the oxidation state of V must be +4 to balance this out.




3. ${\mathrm{WO}}_3$: The compound $\mathrm{O}$ has an oxidation state of -2, and since there are three oxygen atoms, the total oxidation state contributed by oxygen is -6. To balance this out, the oxidation state of W must be +6.

Therefore, the sum of the oxidation states of the metals in these three compounds is $0+4+6=10$.