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Home »     are of different colours in dilute solutions. Why?

    \[{{[\mathbf{Fe}{{\left( \mathbf{CN} \right)}_{\mathbf{6}}}]}^{\mathbf{4}}}~\mathbf{and}\text{ }{{[\mathbf{Fe}{{({{\mathbf{H}}_{\mathbf{2}}}\mathbf{O})}_{\mathbf{6}}}]}^{\mathbf{2}+}}~\]

are of different colours in dilute solutions. Why?
CBSE | Chemistry | Class 12 | Coordination Compounds | NCERT

    \[{{[\mathbf{Fe}{{\left( \mathbf{CN} \right)}_{\mathbf{6}}}]}^{\mathbf{4}}}~\mathbf{and}\text{ }{{[\mathbf{Fe}{{({{\mathbf{H}}_{\mathbf{2}}}\mathbf{O})}_{\mathbf{6}}}]}^{\mathbf{2}+}}~\]

are of different colours in dilute solutions. Why?

[Fe( H2O)6 ]2+ and [ Fe( CN)6 ]2+ have H2O and CN–  ligands respectively. CN– has a higher CFSE (crystal field splitting energy) than water because it is a strong field ligand. As a result, different wavelengths of light are absorbed and returned by the d-d transitions. As a result, they have various colours in a solution.

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