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[Ti(H(2)O)(6)]^(3+) is coloured while [...

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

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To understand why the complex `[Ti(H₂O)₆]³⁺` is colored while `[Sc(H₂O)₆]³⁺` is colorless, we can analyze the electronic configurations and the presence of unpaired electrons in these complexes. ### Step-by-Step Solution: 1. **Identify the Oxidation States:** - For both complexes, titanium (Ti) and scandium (Sc) are in the +3 oxidation state when forming the complexes with water. - The oxidation state of Ti in `[Ti(H₂O)₆]³⁺` is +3, and for Sc in `[Sc(H₂O)₆]³⁺`, it is also +3. ...
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[Sc(H_(2)O)_(6)]^(3+) ion is

[Sc(H_(2)O)_(6)]^(3+) ion is

(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?

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+) .

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