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[Ti(H2O)6]^(3+) is coloured while [Sc(H2...

`[Ti(H_2O)_6]^(3+)` is coloured while `[Sc(H_2O)_6]^(3+)` is colourless . Explain.

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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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These questions consist of two statements each, printed as Assertion and Reason. While answering these questions you are required to choose any one of the following four responses: Assertion: [Ti(H_2O)_6]^(3+) is coloured while [Sc(H_2O)_6]^(3+) is colourless. Reason: d-d transition is not possible in [Sc(H_2O)_6]^(3+) .

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+) .

(a). Why Mn^(2+) compounds are more stable than Fe^(2+) towards oxidation to their +3 state? (b). Calculate the magnetic moment of V^(3+) ion. (c). [Ti(H_2O)_6_^(3+) gives violet coloured aqueous solution but [Mg(H_2O)_6]^(2+) solution is colourless. (d). [Ti(H_2O)_6]^(3+) is coloured whereas [Sc(H_2O)_6]^(3+) is colourless. Why?

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

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