Calculate the oxidation number of the underlined atom in the following

1.	Calculate the oxidation number of the underlined atom in the following species. ul(Fe)(H_(2)O)_(6)Cl_(3)
Answer» Solution :`FE(H_(2)O)_(6)Cl_(3)` : Let the oxidation NUMBER of Fe in this molecule be x. The sum of oxidation numbers of atoms present in `H_(2)O` is ZERO because it is a NEUTRAL molecule. The oxidation number of each Cl atom is -1. Therefore, `(x)+(0)xx6+(-1)xx3=0` or x=+3 Hence, the oxidation number of Fe in the given molecule is +3.

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