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[Fe(CN)6]^(4-) and Fe(H2 O)6]^(2+) are d...

`[Fe(CN)_6]^(4-)` and `Fe(H_2 O)_6]^(2+)` are different colours in dilute solutions . Why ?

Text Solution

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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. In the presence of weak `H_2 O` ligand, they do not pair up. In the presence of strong CN ligand, they pair up leaving no unpaired electron. Due to the difference in the number of unpaired electrons, they have different colours.
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Knowledge Check

  • [fe(CN)_6]^3- ion is

    A
    hexacyanoferrate (II)ion
    B
    hexacyanoferrate(III)ion
    C
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    D
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  • In the complexes [Fe(H_(2)O)_(6)]^(3+), [Fe(CN)_(6)]^(3-), [Fe(C_(2)O_(4))_(3)]^(3-) and [FeCl_(6)]^(3-) , more stability is shown by

    A
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    B
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    C
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    D
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  • [Ti(H_2O_6)]^(3+) is purple in colour because it is complimentary colour of

    A
    blue
    B
    red
    C
    green
    D
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