A metal ion `M^(n+)` having `d^(4)` valence electronic configuration combines with three didentate ligands to form a complex compound. Assuming `Delta_(@)gt P` :
(i) Draw the diagram showing d-orbital splitting during this comples formation.
(ii) What type of hybridisation will `M^(n+)` have?
(iii) Name the type of isomerism exhibited by this complex.
(iv) Write the electronic configuration of metal `M^(n+)`
A metal ion `M^(n+)` having `d^(4)` valence electronic configuration combines with three didentate ligands to form a complex compound. Assuming `Delta_(@)gt P` :
(i) Draw the diagram showing d-orbital splitting during this comples formation.
(ii) What type of hybridisation will `M^(n+)` have?
(iii) Name the type of isomerism exhibited by this complex.
(iv) Write the electronic configuration of metal `M^(n+)`
(i) Draw the diagram showing d-orbital splitting during this comples formation.
(ii) What type of hybridisation will `M^(n+)` have?
(iii) Name the type of isomerism exhibited by this complex.
(iv) Write the electronic configuration of metal `M^(n+)`
Text Solution
AI Generated Solution
To solve the given question step by step, we will address each part of the question systematically.
### Step 1: Draw the diagram showing d-orbital splitting during complex formation.
**Solution:**
In an octahedral complex, the d-orbitals split into two sets due to the presence of ligands. The lower energy set is called T2g (comprising dxy, dyz, and dxz orbitals), and the higher energy set is called Eg (comprising dx2-y2 and dz2 orbitals).
1. Start with the five degenerate d-orbitals: dxy, dyz, dxz, dx2-y2, and dz2.
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A metal ion M^(n+) HAVING D^(4) valence electronic configuration combines with three bidentate ligands to form a complex compound . Assuming Delta_(0) gt P : (i) write the electronic configuration of d^(4) ion . (ii) what type of hybridisation will M^(n+) ion has ? (iii) Nmae the type of isomerism exhibited by this complex .
A metal M^(n+) having d^(4) valence electronic configuration combines with three bidentate ligands to form a complex compound. Assuming Delta_(0)gtP . (i) Write the electronic configuration of d^(4) ion. (ii) What type of hybridisation will M^(n+) ion has ? (iii) Name the type of isomerism exhibited by this complex.
Knowledge Check
Crystal field theory views the bonding in complexes as arising from electrostatic interaction and considers the effect of the ligand charges on the energies of the metal ion d-orbitals In this theory, a ligand lone pair is modelled as a point negative charge that repels electrons in the d-orbitals of the central metal ion.The theory concentrated on the resulting splitting of the d-orbitals in two groups with different energies and used that splitting to rationalize and correlate the optical spectra,thermodynamic stability, and magnetic properties of complexes.This energy splitting between the two sets of d-orbitals is called the crystal field splitting Delta . In general, the crystal field splitting energy Delta corresponds to wavelenght of light in visible region of the spectrum, and colours of the complexes can therefore be attributed to electronic transition between the lower and higher energy sets of d-orbitals. In general, the colour that we see is complementry to the colour absorbed. Different metal ions have different value of Delta , which explains why their complexes with the same ligand have different colour. Similarly the crystal field splitting also depends on the nature of ligands and as the ligand for the same metal varies from H_2O to NH_3 to ethylenediamine, Delta for complexes increase.Accordingly, the electronic transition shifts to higher energy (shorter wavelength) as the ligand varies from H_2O from NH_3 to en, thus accounting for the variation in colour. Crystal field theory accounts for the magnetic properties of complexes in terms of the relative values of Delta and the spin pairing energy P. Small Delta values favour high spin complexes, and large Delta values favour low spin complexes. The [Ti(NCS)_6]^(3-) ion exhibits a single absorption band at 544 nm.What will be the crystal field splitting energy (in kJ mol^(-1) ) of the complex ? (h=6.626xx10^(-34) J.s, C=3.0xx10^5 m//s, N_A=6.02xx10^23 ions/mole.
Crystal field theory views the bonding in complexes as arising from electrostatic interaction and considers the effect of the ligand charges on the energies of the metal ion d-orbitals In this theory, a ligand lone pair is modelled as a point negative charge that repels electrons in the d-orbitals of the central metal ion.The theory concentrated on the resulting splitting of the d-orbitals in two groups with different energies and used that splitting to rationalize and correlate the optical spectra,thermodynamic stability, and magnetic properties of complexes.This energy splitting between the two sets of d-orbitals is called the crystal field splitting Delta . In general, the crystal field splitting energy Delta corresponds to wavelenght of light in visible region of the spectrum, and colours of the complexes can therefore be attributed to electronic transition between the lower and higher energy sets of d-orbitals. In general, the colour that we see is complementry to the colour absorbed. Different metal ions have different value of Delta , which explains why their complexes with the same ligand have different colour. Similarly the crystal field splitting also depends on the nature of ligands and as the ligand for the same metal varies from H_2O to NH_3 to ethylenediamine, Delta for complexes increase.Accordingly, the electronic transition shifts to higher energy (shorter wavelength) as the ligand varies from H_2O from NH_3 to en, thus accounting for the variation in colour. Crystal field theory accounts for the magnetic properties of complexes in terms of the relative values of Delta and the spin pairing energy P. Small Delta values favour high spin complexes, and large Delta values favour low spin complexes. The [Ti(NCS)_6]^(3-) ion exhibits a single absorption band at 544 nm.What will be the crystal field splitting energy (in kJ mol^(-1) ) of the complex ? (h=6.626xx10^(-34) J.s, C=3.0xx10^5 m//s, N_A=6.02xx10^23 ions/mole.
A
240
B
220
C
270
D
250
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