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

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

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`rarr` In the given complexes Fe has + 2 oxidation state with `3d^(6)` outer electronic configuration. It has four unpaired electrons in presence of weak ligand `H_(2)O`. But in presence of strong ligand `CN^(-)` the electrons are paired up. Due to the difference in the no of unpaired electrons both complex have different colours in dilute solutions.
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VIKRAM PUBLICATION ( ANDHRA PUBLICATION)-D AND F- BLOCK ELEMENTS AND CO-ORDINATION COMPOUNDS -VERY SHORT ANSWER QUESTIONS
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  2. What is a ligand ?

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  3. Give one example each for ionic and neutral ligands.

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  10. How many geometrical isomers are possible in the following coordinatio...

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  13. A solution of [Ni(H(2)O)(6)]^(2+) is green but a solution of [Ni(CN)(4...

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  16. What is the oxidation state of cobalt in [Co(NH(3))(6)]^(3+) ?

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