An aqueous solution of [Ti(H2O)6]3+ ion has a mild violet colour of low intensity. Which of the following statements is incorrect?
Correct answer: D. The transition is the result of metal-ligand back bonding
- A. The ion absorbs visible light in the region of ~ 5000 Å
- B. The colour results from an electronic transition of one electron from the t2g to an eg orbital
- C. The low colour-intensity is because of a low probability of transition
- D. The transition is the result of metal-ligand back bonding
Explanation
[Ti(H2O)6]3+ has one unpaired electron in its d-subshell which gives rise to the d-d transition to impart colour. Whenever light falls on the transition element compounds electrons excite and electrons absorb energy and excite. When these electrons de-excite they release visible light wavelength. That's why transition element compounds exhibit colour.
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About Electronic Structure of d-Block Elements
The electronic structure of d-block elements covers the filling of the (n-1)d and ns orbitals, general electronic configurations, and the exceptions shown by chromium and copper. It explains how partially filled d orbitals produce variable oxidation states, coloured ions, magnetic behaviour and complex formation, while distinguishing transition elements from elements with completely filled d subshells.
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