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[Fe(CN)6]^(4-) and [Fe(H2O)6]^(2+), are ...

`[Fe(CN)_6]^(4-)` and `[Fe(H_2O)_6]^(2+)`, are of different colours in dilate solution, although in both the cases iron is in +2 oxidation state explain.

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In both the complex compounds, Fe is in +2 oxidation state with configuration `3d^(6)`, i.e. it has four unpaired eelctrons. In the presence of weak `H_(2)O` ligands, the unpaired electrons do not pair up but in the presence of strong ligand `CN^(-)` , they get paired up. Then no unpaired electron is left. Due to this difference in the number of unpaired electrons, both complex ions have different colours.
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