Answer the following questions:
What is crystal field splitting energy?
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Solution and Explanation
Step 1: Understanding Crystal Field Splitting Energy When ligands approach a transition metal ion, the degeneracy of the d-orbitals is lifted due to electrostatic interactions, causing them to split into two sets of orbitals: \[ t_{2g} \quad \text{(lower energy)} \quad \text{and} \quad e_g \quad \text{(higher energy)} \] The energy difference between these orbitals is called Crystal Field Splitting Energy (\(\Delta\)).
Give reason for the violet colour of the complex [Ti(H2O)6]3+
on the basis of crystal field theory.
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Solution and Explanation
The violet colour arises due to the d-d electronic transition within the split d-orbitals.
Step 1: Electronic Configuration of [Ti(H2O)6]3+ For \( \text{Ti}^{3+} \), the electronic configuration is: \[ \text{Ti}^{3+} = 3d^1 \] Step 2: Crystal Field Splitting and d-d Transition In an octahedral field, the d-orbitals split into: \[ t_{2g} \quad \text{(lower energy)} \quad \text{and} \quad e_g \quad \text{(higher energy)} \] Since Ti\(^{3+}\) has one electron, it occupies the \( t_{2g} \) orbital as: \[ t_{2g}^1 e_g^0 \] Step 3: Cause of Violet Colour When visible light is absorbed, the electron gets excited from the \( t_{2g} \) to the \( e_g \) orbital, causing a d-d transition. The observed colour (violet) is due to the complementary colour of the absorbed wavelength.
\( [\text{Cr(NH}_3)_6]^{3+} \) is paramagnetic while \( [\text{Ni(CN)}_4]^{2-} \) is diamagnetic. Explain why.
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Solution and Explanation
Step 1: Electronic Configuration of Cr\(^{3+}\) and Ni\(^{2+}\) \[ \text{Cr}^{3+} = 3d^3, \quad \text{Ni}^{2+} = 3d^8 \] Step 2: Effect of Ligands on Magnetic Properties - \( NH_3 \) is a weak field ligand, so it does not cause electron pairing in \( [\text{Cr(NH}_3)_6]^{3+} \), leaving unpaired electrons in the \( t_{2g} \) orbitals. - \( CN^- \) is a strong field ligand, so it pairs electrons in \( [\text{Ni(CN)}_4]^{2-} \), making it diamagnetic.
Explain why \( [\text{Fe(CN)}_6]^{3-} \) is an inner orbital complex, whereas \( [\text{Fe(H}_2\text{O)}_6]^{3+} \) is an outer orbital complex.
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Solution and Explanation
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