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

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Solution

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.

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On the basis of crystal field theory explain why Co(III) forms paramagnetic octahedral complex with weak field ligands whereas it forms diamagnetic octahedral complex with strong field ligands.

Give the electronic configuration of the following complexes on the basis of crystal field splitting theory. $[C o F_{6}]^{3 -}, [F e (C N)_{6}]^{4 -}$ and $[C u (N H_{3})_{6}]^{2 +} .$

Q. Electronic configuration of

[C u (N H_{3})_{6}]^{2 +}

on the basis of crystal field splitting theory is :

Q. Give the electronic configuration of the following on the basis of crystal field splitting theory.

{[C o F_{6}]}^{3 -}

and

{[C u {({N H}_{3})}_{6}]}^{2 +}

[T i (H_{2} O)_{6}]^{3 -}

absorbs energy equal to wavelength 498 nm. On this basis crystal field splitting energy comes out to be

a \times 10^{- 3} J

. What is the value of a?___

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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?