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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.
संबंधित प्रश्न
On the basis of crystal field theory, write the electronic configuration for d4 ion if Δ0 > 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?
State the superiority of crystal field theory over valence bond theory.
The colour of the coordination compounds depends on the crystal field splitting. What will be the correct order of absorption of wavelength of light in the visible region, for the complexes, \[\ce{[Co(NH3)6]^{3+}}\], \[\ce{[Co(CN)6]^{3-}}\], \[\ce{[Co(H2O)6]^{3+}}\]
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) \[\ce{[Ni(NH3)6]^{2+}}\]
An aqueous pink solution of cobalt (II) chloride changes to deep blue on addition of excess of HCl. This is because:
(i) \[\ce{[Co(H2O)6]^{2+}}\] is transformed into \[\ce{[CoCl6]}^{4-}\]
(ii) \[\ce{[Co(H2O)6]^{2+}}\] is transformed into \[\ce{[CoCl4]}^{2-}\]
(iii) tetrahedral complexes have smaller crystal field splitting than octahedral complexes.
(iv) tetrahedral complexes have larger crystal field splitting than octahedral complex.
Give the electronic configuration of the following complexes on the basis of Crystal Field Splitting theory.
\[\ce{[CoF6]^{3-}, [Fe(CN)6]^{4-} and [Cu(NH3)6]^{2+}}\].
\[\ce{CuSO4 . 5H2O}\] is blue in colour while \[\ce{CuSO4}\] is colourless. Why?
Using crystal field theory, draw energy level diagram, write electronic configuration of the central metal atom/ion and determine the magnetic moment value in the following:
\[\ce{[FeF6]^{3-}, [Fe(H2O)6]^{2+}, [Fe(CN)6]^{4-}}\]
Why are different colours observed in octahedral and tetrahedral complexes for the same metal and same ligands?
Considering crystal field theory, strong-field ligands such as CN–:
The CFSE of [CoCl6]3– is 18000 cm–1 the CFSE for [CoCl4]– will be ______.
What is the difference between a weak field ligand and a strong field ligand?
What is crystal field splitting energy?
The correct order of intensity of colors of the compounds is ______.
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 d4 with a strong field ligand for which Δ0 > P.
On the basis of Crystal Field Theory, write the electronic configuration of d4 ion if Δ0 > P.
