ti3+ salts are coloured. whereas ti4+ salts are white.why?

Open in App

Solution

Transition metal compounds are coloured as they can undergo d-d transitions. The five d-orbitals are degenerate but in the presence of solvent or ligand these split up into two sets with different energies. The electrons in the lower energy state can easily move from lower to higher energy state by absorption of light. As the energy difference is small, absorbed and emitted light is in the visible range and the compound is coloured. Ti has the valence configuration, 3d¹⁰ 4s², Ti³⁺ ; 3d¹4s⁰ and Ti⁴⁺ ; 3p⁶3d⁰4s⁰. As Ti⁴⁺ has no electrons in d orbital, no d-d transition is possible and thus it forms compounds that are white in colour.

Suggest Corrections

Similar questions

S c^{3 +}

C r^{3 +}

3

T i^{4 +}

C r^{3 +}

Z n^{2 +}

C u^{2 +}

Join BYJU'S Learning Program