a) Give the electronic configuration of the d-orbitals of Ti in [Ti(H2O)6] 3+ ion in an octahedral crystal field. b) Explain why this complex is coloured based on the distribution of electrons in the dorbitals. c) How does the colour change on heating [Ti(H2O)6] 3+ ion?

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Solution

(a) [Ti(H₂O)₆]³⁺ has d¹ electronic configuration.
(b) The complex is coloured as it has one d-electron-. So d-d transition is possible in it which makes the complex coloured. In [Ti(H₂O)₆]³⁺ complex, d-d transition takes place between t_2g and e_g of d-subshell. The electron get excited to higher energy level when exposed to high energy. When electron returns to its ground state, it emits energy of particular wavelength, due which element shows colour.
(c) On heating the complex will be colourless as the water will be removed on heating and there will be no crystal field splitting. It means there will be no t_2g and e_g. It will have degenerate d-orbitals. Thus no d-d transition can be possible. Hence the complex will appear colourless.

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