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Calculate the oxidation number of the underlined atom in the following species. K_(4)ul(Fe)(CN)_(6) |
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Answer» Solution :`K_(4)Fe(CN)_(6)` : Suppose the oxidation number of Fe in this molecule is x. The oxidation number of each K (alkali metal) atom is +1. `CN^(-)` is an ION and bears a CHARGE equal to -1. Therefore, the sum of oxidation numbers of all atoms present in `CN^(-)` ion is equal to -1. Since `K_(4)Fe(CN)_(6)` is a neutral molecule, the sum of oxidation numbers of all atoms present in it will be equal to zero. Therefore, `(+1)xx4+(x)+(-1)xx6=0` or `x=+6-4=+2` Hence, the oxidation number of Fe in `K_(4)Fe(CN)_(6)` is +2. |
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