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प्रश्न
Draw figure to show the splitting of d orbitals in an octahedral crystal field.
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उत्तर
- Let the six ligands be symmetrically located along the Cartesian axes and the metal atom is at the origin.
- On approaching the ligand, the energy of the d-orbitals increases as expected compared to the free ions. As is the case in a spherical crystal field.
- The orbitals along the axes (`d_(z^2)` and `d_(x^2 - y^2)`) repel more strongly than the dxy, dyz and dzx orbitals and have lobes directed between the axes.
- In the spherical crystal field, the `d_(Z^2)` and `d_(x^2 - y^2)` orbitals increase in energy and the dxy, dyz, dzx orbitals decrease in energy compared to the average energy.
d orbital splitting in an octahedral crystal field - Therefore, the degenerate set of d-orbitals splits into two groups: the low energy orbital group t2g and the high energy orbital group eg separated by energy Δo.
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संबंधित प्रश्न
On the basis of crystal field theory, write the electronic configuration for d4 ion if ∆0 < P.
The hexaquo manganese(II) ion contains five unpaired electrons, while the hexacyanoion contains only one unpaired electron. Explain using Crystal Field Theory.
How does the magnitude of Δ0 decide the actual configuration of d orbitals in a coordination entity?
The CFSE for octahedral \[\ce{[CoCl6]^{4-}}\] is 18,000 cm–1. The CFSE for tetrahedral \[\ce{[CoCl4]^{2-}}\] will be ______.
Atomic number of \[\ce{Mn, Fe, Co}\] and Ni are 25, 26, 27 and 28 respectively. Which of the following outer orbital octahedral complexes have same number of unpaired electrons?
(i) \[\ce{[MnCl6]^{3-}}\]
(ii) \[\ce{[FeF6]^{3-}}\]
(iii) \[\ce{[CoF6]^{3-}}\]
(iv) \[\ce{[Ni(NH3)6]^{2+}}\]
Give the electronic configuration of the following complexes on the basis of Crystal Field Splitting theory.
\[\ce{[CoF6]^{3-}, [Fe(CN)6]^{4-} and [Cu(NH3)6]^{2+}}\].
Arrange following complex ions in increasing order of crystal field splitting energy (∆O):
\[\ce{[Cr(Cl)6]^{3-}, [Cr(CN)6]^{3-}, [Cr(NH3)6]^{3+}}\].
The CFSE for octahedral [CoCl6]−4 is 18,000 cm−1. What will be the CFSE for tetrahedral [CoCl3]−2?
In a coordination entity, the electronic configuration of the central metal ion is t2g3 eg1
Draw the crystal field splitting diagram for the above complex.
Considering crystal field theory, strong-field ligands such as CN–:
The magnitude of CFSE depends upon ______
The CFSE of [CoCl6]3– is 18000 cm–1 the CFSE for [CoCl4]– will be ______.
The correct order of intensity of colors of the compounds is ______.
For octahedral Mn(II) and tetrahedral Ni(II) complexes, consider the following statements:
- Both the complexes can be high spin.
- Ni(II) complex can very rarely below spin.
- With strong field Ligands, Mn(II) complexes can be low spin.
- Aqueous solution of Mn (II) ions is yellow in colour.
The correct statements are:
On the basis of Crystal Field theory, write the electronic configuration for the d5 ion with a strong field ligand for which Δ0 > P.
On the basis of crystal field theory, write the electronic configuration for the d5 ion with a weak ligand for which Δ0 < P.
On the basis of Crystal Field Theory, write the electronic configuration of d4 ion if Δ0 > P.
The value of the spin only magnetic moment for one of the following configurations is 2.84 BM. The correct one is:
