Find out the oxidation states of two types of Fe atoms in `Fe_(4)[Fe(CN)_(6)]_(3)` and reqrite the formula in stock notation form

Explanation

From our knowledge of coordinate complex we know that the species `Fe_(4)` which lies outside the complex ion I.e `[Fe(CN)_(6)]_(3)` is the +ve part while the complex ion itself is the -ve part in other words the +ve charge on 4 fe atoms ouside the ocordination spher is balanced by the -ve charge on the complex ion since fe has two oxidation states i.e +2 and +3 and oxidation number of `CN^(-)=-1 therefore`
Fe in the complex ions has an O.N of +2 while the fe atoms outside the coordination spere have an O.N of +3 thus the stock notation for `Fe_(4)[Fe(CN)_(6)]_(3)` is `Fe_(4)[Fe^(II)(CN)_(6)]_(3)`