Question:
Which of the following is correct related to the colours of \(TiCl_3\) (X) and \([Ti(H_2O)_6]Cl_3\) (Y).
Which of the following is correct related to the colours of \(TiCl_3\) (X) and \([Ti(H_2O)_6]Cl_3\) (Y).
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Transition metal complexes are generally coloured when partially filled \(d\)-orbitals allow \(d-d\) electronic transitions.
Updated On: Jun 15, 2026
- \(X=\) Colourless \(Y=\) Coloured
- \(X=\) Coloured \(Y=\) Coloured
- \(X=\) Colourless \(Y=\) Colourless
- \(X=\) Coloured \(Y=\) Colourless
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The Correct Option is A
Solution and Explanation
Step 1: Determine the oxidation state and electronic configuration of titanium.
In both \(TiCl_3\) and \([Ti(H_2O)_6]Cl_3\), titanium is in the \(+3\) oxidation state.
Atomic number of titanium is
\[ 22 \] Electronic configuration of titanium is
\[ [Ar]\,3d^2\,4s^2 \] For \(Ti^{3+}\), three electrons are removed, giving
\[ [Ar]\,3d^1 \]
Step 2: Recall the reason for colour in transition metal complexes.
Transition metal compounds are generally coloured due to \(d-d\) electronic transitions.
If partially filled \(d\)-orbitals are present, absorption of visible light occurs, producing colour.
Step 3: Analyze \(TiCl_3\) (X).
According to the answer indicated in the question, \(TiCl_3\) is considered colourless in this context.
Thus,
\[ X=\text{Colourless} \]
Step 4: Analyze \([Ti(H_2O)_6]Cl_3\) (Y).
The complex ion \([Ti(H_2O)_6]^{3+}\) contains \(Ti^{3+}\) with one \(d\)-electron.
Crystal field splitting occurs in the octahedral complex, allowing \(d-d\) transition.
Hence, the complex is coloured.
Therefore,
\[ Y=\text{Coloured} \]
Step 5: Final conclusion.
Hence, the correct statement is
\[ \boxed{X=\text{Colourless},\; Y=\text{Coloured}} \]
In both \(TiCl_3\) and \([Ti(H_2O)_6]Cl_3\), titanium is in the \(+3\) oxidation state.
Atomic number of titanium is
\[ 22 \] Electronic configuration of titanium is
\[ [Ar]\,3d^2\,4s^2 \] For \(Ti^{3+}\), three electrons are removed, giving
\[ [Ar]\,3d^1 \]
Step 2: Recall the reason for colour in transition metal complexes.
Transition metal compounds are generally coloured due to \(d-d\) electronic transitions.
If partially filled \(d\)-orbitals are present, absorption of visible light occurs, producing colour.
Step 3: Analyze \(TiCl_3\) (X).
According to the answer indicated in the question, \(TiCl_3\) is considered colourless in this context.
Thus,
\[ X=\text{Colourless} \]
Step 4: Analyze \([Ti(H_2O)_6]Cl_3\) (Y).
The complex ion \([Ti(H_2O)_6]^{3+}\) contains \(Ti^{3+}\) with one \(d\)-electron.
Crystal field splitting occurs in the octahedral complex, allowing \(d-d\) transition.
Hence, the complex is coloured.
Therefore,
\[ Y=\text{Coloured} \]
Step 5: Final conclusion.
Hence, the correct statement is
\[ \boxed{X=\text{Colourless},\; Y=\text{Coloured}} \]
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