The Oxidation State of Transition Metals in Compounds,What’s the oxidation state of the transition metal in the following compounds? (i) Na3[FeCl6] (ii) Cr(OH2)6

The Oxidation State of Transition Metals in Compounds

The oxidation state of transition metals in compounds can vary significantly depending on the elements that are present and the oxidation states of those elements (FuseSchool, 2020). For example, the oxidation state of iron in Na3[FeCl6] is +3, because the net charge of the compound is zero and the sodium and chloride ions both have an oxidation state of +1. Iron is the only transition metal in this compound, so it must balance out the charge of the other elements with a +3 oxidation state. Similarly, the oxidation state of chromium in Cr(OH2)6 is +3. This is because the compound has a net charge of zero, and the oxygens have an oxidation state of -2 (Chemistry LibreTexts, 2019). Because chromium is the only transition metal, it must balance out the charge of the other elements with a +3 oxidation state. In summary, the oxidation state of a transition metal in a compound can be determined by examining the oxidation states of the other elements present, and ensuring that the net charge of the compound is zero. For example, the oxidation state of iron in Na3[FeCl6] is +3, and the oxidation state of chromium in Cr(OH2)6 is +3. These examples demonstrate how the oxidation state of transition metals in compounds can be determined. Cont…

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