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[Fe(CN)(6)]^(4-) and [Fe(H(2)O)(6)]^(2+)...

`[Fe(CN)_(6)]^(4-)` and `[Fe(H_(2)O)_(6)]^(2+)` show different colours in dilute solution because

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In both the complexes, `Fe is in +2` state with the configuration `3d^(6)`, i.e., it has four unpaired electrons. As the ligands `H_(2)O and.`CN^(-)` posses, different crystal field splitting energy(triangle_(o))`, they absorb different components of the visible light (VIBGYOR) for d-d transition. Hence, the transmitted colours are different
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[Fe(CN)_(6)]^(4-) and [Fe(H_(2)O)_(6)]^(2+) are of different colours in dilute solutions why?

[Fe(CN)_(6)]^(4-) and [Fe(H_(2)O)_(6)]^(2+) are of different colours in dilute solutions why?

[Fe(H_(2)O)_(6)]^(2+) and [Fe(CN)_(6)]^(4-) differ in :

[Fe(H_(2)O)_(6)]^(2+) and [Fe(CN)_(6)]^(4-) differ in :

[Fe(H_(2)O)_(6)]^(3+) and [Fe(CN)_(6)]^(3-) differ in

K_(3)[Fe(CN)_(6)]+FeCl_(2) to Fe_(3)[Fe(CN)_(6)]_(2)darr

4KCN+Fe(CN)_(2)darr to K_(4)[Fe(CN)_(6)]

Fe(CN)_(2)darr+4KCN to K_(4)[Fe(CN)_(6)]

Fe(CN)_(2)darr+4KCN to K_(4)[Fe(CN)_(6)]

Hydrogen peroxide oxidises [Fe(CN)_(6)]^(4-) to [Fe(CN)_(6)]^(3-) in acidic medium but reduces [Fe(CN)_(6)]^(3-) to [Fe(CN)_(6)]^(4-) in alkaline medium. The other products formed are, respectively