The oxidation number of Fe in [Fe(CN)\(_6\)]\(^{3-}\) is

In the compound [Fe(CN)\(_6\)]\(^{3-}\), the overall charge of the compound is negative 3 (\(^{3-}\)), which means the sum of the oxidation states of all the atoms in the compound must equal negative 3. We can start by looking at the cyanide ion (CN\(^-\)), which has a known oxidation state of negative 1 (\(-1\)). There are six of them in the compound, giving a total charge of negative 6 (\(-1 \times 6 = -6\)). To find the oxidation state of iron (Fe), we can use the fact that the sum of the oxidation states of all the atoms in a compound is equal to the overall charge of the compound. Let x be the oxidation state of iron (Fe). Therefore, x + (-6) = -3 Solving for x, we get: x = +3 Therefore, the oxidation state of iron (Fe) in [Fe(CN)\(_6\)]\(^{3-}\) is +3.