Which of following coordination compounds contains the central metal witrh the highest oxidation number ?

Options

A. `[Ru (NH_(3))_(5)(H_(2)O)] CI_(2)`
B. `[Cr(NH_(3))_(6)](NO_(3))_(3)`
C. `[Fe(CO)_(5)]`
D. `K_(4)[Fe(CN)_(6)]`

Answer

B

Explanation

Each nitrate ion has a charge of `-1`, therefore, the cation must be `[Cr(NH_(3))_(6)]^(3+) NH_(3)` is netural so the oxidation In (1), both `NH_(3)` and `H_(2)O` are netural species. Since each chloride ion carries a `1-` charge, and there are two `CI^(-)` ions, the oxidation number of Ru must be `+2` In (3), the oxidation number of Fe is zero, since the CO species are netural. In (4), each potassium ion has a charge of `1+` , therefpre, the anion is `[Fe(CN)_(6)]^(4-)` . Next we know that each cyanide group bears a charge of `1-` , so Fe must have an oxidation number of `+2` .