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The electronic spectrum of [Ti(H2O)6]3+ shows a single broad peak with a maximum at 20,300 cm-1. The crystal field stabilisation energy (CFSE) of the complex ion, in kJ mol-1, is (1 kJ mol-1 = 83.7 cm-1)
  • a)
    145.5
  • b)
    97
  • c)
    242.5
  • d)
    83.7
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
The electronic spectrum of [Ti(H2O)6]3+shows a single broad peak with ...

CFSE = -0.4Δ0 = -0.4 × 20,300 = -8120 cm-1 
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The electronic spectrum of [Ti(H2O)6]3+shows a single broad peak with ...
Understanding Crystal Field Stabilization Energy (CFSE)
The crystal field stabilization energy (CFSE) quantifies the energy gained by a metal ion in a complex due to its interaction with surrounding ligands. In the case of [Ti(H2O)6]3+, we need to calculate the CFSE based on its electronic configuration and the given absorption data.
Electronic Configuration
- Titanium in the +3 oxidation state has the electron configuration of [Ar] 3d1.
- This means there is one electron in the d-orbitals, which will be influenced by the crystal field created by the surrounding water ligands.
Determining CFSE
- The ligand field theory tells us that in an octahedral complex, the d-orbitals split into two sets: t2g (lower energy) and eg (higher energy).
- For [Ti(H2O)6]3+, the d1 electron will occupy one of the t2g orbitals.
Energy Calculation
- The energy difference (Δo) between the t2g and eg levels can be derived from the provided absorption maximum of 20,300 cm-1.
- This energy corresponds to the transition energy required for moving an electron from the t2g to the eg level.
CFSE Formula
- The CFSE can be calculated using the formula:
CFSE = (Number of electrons in t2g) * (-0.4Δo) + (Number of electrons in eg) * (0.6Δo)
- In our case:
CFSE = 1 * (-0.4 * 20,300 cm-1)
= -8,1200 cm-1
Converting to kJ mol-1
- To convert from cm-1 to kJ mol-1, use the conversion factor (1 kJ mol-1 = 83.7 cm-1):
CFSE = -8,1200 cm-1 / 83.7 cm-1/kJ mol-1
= -97 kJ mol-1
This confirms that the correct answer is option 'B' - 97 kJ mol-1.
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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 dorbitals is called the crystal field splitting D.In general, the crystal field splitting energy D corresponds to wavelength 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 the we see is complementry to the colour absorbed.Different metal ion have different values of D, 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 H2O to NH3 to ethylenediamine, D for complexes increases. Accordingly, the electronic transition shifts to higher energy (shorter wavelength) as the ligand varies from H2O to NH3 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 and the spin pairing energy P. Small values favour high spin complexes, and large Dvalues favour low spin complexes.The [Ti(NCS)6]3- ion exhibits a single absorption band at 544 nm. W hat will be the crystal field splitting energy (KJ mol-1) of the complex ? (h = 6.626 x 10-34 J.s ; C = 3.0 x 108 m/s; NA = 6.02 x 1023 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 dorbitals is called the crystal field splitting D.In general, the crystal field splitting energy D corresponds to wavelength 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 the we see is complementry to the colour absorbed.Different metal ion have different values of D, 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 H2O to NH3 to ethylenediamine, D for complexes increases. Accordingly, the electronic transition shifts to higher energy (shorter wavelength) as the ligand varies from H2O to NH3 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 and the spin pairing energy P. Small values favour high spin complexes, and large Dvalues favour low spin complexes.Which of the following statements is incorrect?

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 dorbitals is called the crystal field splitting D.In general, the crystal field splitting energy D corresponds to wavelength 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 the we see is complementry to the colour absorbed.Different metal ion have different values of D, 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 H2O to NH3 to ethylenediamine, D for complexes increases. Accordingly, the electronic transition shifts to higher energy (shorter wavelength) as the ligand varies from H2O to NH3 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 and the spin pairing energy P. Small values favour high spin complexes, and large Dvalues favour low spin complexes.Which of the following complexes are diamagnetic ? [Pt(NH3)4]2+ [Co(SCN)4]2- [Cu(en)2]2+ [HgI4]2-square planar tetrahedral square planar tetrahedral (i) (ii) (iii) (iv)

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The electronic spectrum of [Ti(H2O)6]3+shows a single broad peak with a maximum at 20,300 cm-1. The crystal field stabilisation energy (CFSE) of the complex ion, in kJ mol-1, is (1 kJ mol-1= 83.7 cm-1)a)145.5b)97c)242.5d)83.7Correct answer is option 'B'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The electronic spectrum of [Ti(H2O)6]3+shows a single broad peak with a maximum at 20,300 cm-1. The crystal field stabilisation energy (CFSE) of the complex ion, in kJ mol-1, is (1 kJ mol-1= 83.7 cm-1)a)145.5b)97c)242.5d)83.7Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The electronic spectrum of [Ti(H2O)6]3+shows a single broad peak with a maximum at 20,300 cm-1. The crystal field stabilisation energy (CFSE) of the complex ion, in kJ mol-1, is (1 kJ mol-1= 83.7 cm-1)a)145.5b)97c)242.5d)83.7Correct answer is option 'B'. Can you explain this answer?.
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