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[Ti(H(2)O)(6)]^(2+) is coloured whereas ...

`[Ti(H_(2)O)_(6)]^(2+)` is coloured whereas `[Sc(H_(2)O)_(6)]^(3+)` s colourless, though it is a transition metal complex. Explain the observation.

Text Solution

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Tit has one electron in the d-orbital `(3d^(1))` which can absorb energy corresponding to yellow wavelength and jump from lower energy level to higher energy level. But `Sc^(3+)`has no electron in d-orbital
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[Ti(H_(2)O)_(6)]^(3+) is coloured while [Sc(H_(2)O)_(6)]^(3+) is colourless. Why?

[Ti(H_(2)O)_(6)]^(3+) is coloured while [Sc(H_(2)O)_(6)]^(3+) is colourless. Why ?

Knowledge Check

  • [Sc(H_(2)O)_(6)]^(3+) ion is

    A
    Colourless and diamagnetic
    B
    Coloured and octahedral
    C
    Colourless and paramagnetic
    D
    Coloured and paramagnetic

  • [Sc(H_(2)O)_(6)]^(3+) ion is

    A
    Colourless and diamagnetic
    B
    Coloured and octahedral
    C
    Colourless and paramahnetic
    D
    coloured and paramagnetic

  • [Sc (H_(2)O)_(6)]^(3+) ion is :-

    A
    Coloured and paramagnetic
    B
    Colourless and paramagnetic
    C
    Colourless and diamagnetic
    D
    Coloured & octahedral

    • Similar Questions

    Explore conceptually related problems

    [Ni(CN)_(4)]^(2-) is colourless whereas [Ni(H_(2)O)_(6)]^(2+) is green. Why ?

    [Ni(CN)_(4)]^(2-) is colourless whereas [Ni(H_(2)O)_(6))^(2+) is green. Why?

    [Co(H_(2)O)_(6)]^(3+) complex is

    The colour of [Ti(H_(2)O)_(6)]^(3+) is due to

    Assertion: [Ti(H_(2)O)_(6)]^(4+) is coloured while [Sc(H_(2)O)_(6)]^(3+) is colourless. Reason: d-d transition is not possible in [Sc(H_(2)O)_(6)]^(3+) .

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