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If [Cu(H2O)4]2+ absorbs a light of wavelength 600 nm for d-d transition, then the value of octahedral crystal field splitting energy for [Cu(H2O)6]2+ will be ________ × 10-21 J. (Nearest Integer)
(Given: h = 6.63 × 10-34 Js and c = 3.08 × 108 ms-1)
Correct answer is '766'. Can you explain this answer?
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If [Cu(H2O)4]2+absorbs a light of wavelength 600 nm for d-d transition...
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If [Cu(H2O)4]2+absorbs a light of wavelength 600 nm for d-d transition...
The value of octahedral crystal field splitting energy for [Cu(H2O)6]2 can be calculated using the formula:

Δ = hc/λ

Where:
Δ = octahedral crystal field splitting energy
h = Planck's constant (6.626 x 10^-34 J·s)
c = speed of light (3.0 x 10^8 m/s)
λ = wavelength of light absorbed (600 nm)

First, convert the wavelength from nanometers to meters:
λ = 600 nm = 600 x 10^-9 m

Now, substitute the values into the formula and calculate Δ:
Δ = (6.626 x 10^-34 J·s x 3.0 x 10^8 m/s) / (600 x 10^-9 m)

Δ ≈ 3.313 x 10^-19 J

Therefore, the value of octahedral crystal field splitting energy for [Cu(H2O)6]2 will be approximately 3.313 x 10^-19 J.
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If [Cu(H2O)4]2+absorbs a light of wavelength 600 nm for d-d transition...
To calculate the octahedral crystal field splitting energy for [Cu(H2O)6]2, we need to use the relationship between wavelength and energy for electromagnetic radiation:

E = hc/λ

Where:
E = energy of the light
h = Planck's constant (6.626 x 10^-34 J.s)
c = speed of light (3.00 x 10^8 m/s)
λ = wavelength of the light

Given that the wavelength of the absorbed light is 600 nm (or 600 x 10^-9 m), we can calculate the energy:

E = (6.626 x 10^-34 J.s)(3.00 x 10^8 m/s) / (600 x 10^-9 m)
= 3.313 x 10^-19 J

Since this energy corresponds to a d-d transition in [Cu(H2O)4]2, we can assume that the same transition occurs in [Cu(H2O)6]2. The difference in energy between the initial and final states in the d-orbitals of the copper ion is equal to the octahedral crystal field splitting energy, denoted as Δ:

Δ = 3.313 x 10^-19 J

Therefore, the value of the octahedral crystal field splitting energy for [Cu(H2O)6]2 is 3.313 x 10^-19 J.
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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 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)

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?

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If [Cu(H2O)4]2+absorbs a light of wavelength 600 nm for d-d transition, then the value of octahedral crystal field splitting energy for [Cu(H2O)6]2+will be ________ × 10-21J. (Nearest Integer)(Given: h = 6.63 × 10-34Js and c = 3.08 × 108ms-1)Correct answer is '766'. Can you explain this answer?
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