Explain the violet colour of -Ti-H-2O-6-3- complex on basis of the crystal field theory-

Question

Toppr Admin · Accepted Answer

In the complex -Ti-H2O-6-3- the Ti atom has oxidation state of -3- Its outer electronic configuration is 3d1- It has one unpaired electron- This unpaired electron is excited from t2g level to eg level by absorbing yellow light and hence appears violet coloured-

Explain the violet colour of $[T i (H_{2} O)_{6}]^{3 +}$ complex on basis of the crystal field theory?

In the complex $[T i (H_{2} O)_{6}]^{3 +}$ , the Ti atom has oxidation state of $+ 3$ . Its outer electronic configuration is $3 d^{1}$ . It has one unpaired electron. This unpaired electron is excited from $t_{2 g}$ level to $e_{g}$ level by absorbing yellow light and hence appears violet coloured.

Explain the violet colour of [Ti(H2O)6]3+ complex on basis of the crystal field theory?

In the complex [Ti(H2O)6]3+, the Ti atom has oxidation state of +3. Its outer electronic configuration is 3d1. It has one unpaired electron. This unpaired electron is excited from t2g level to eg level by absorbing yellow light and hence appears violet coloured.

Explain the violet colour of $[T i (H_{2} O)_{6}]^{3 +}$ complex on basis of the crystal field theory?