Advertisements
Advertisements
प्रश्न
Using crystal field theory, write the electronic configuration of d5 ion, if Δ0 > P.
Write the electronic configuration of d5 ion when Δ0 > P.
Advertisements
उत्तर
When the crystal field splitting energy (Δ0) is greater than the pairing energy (P), electrons prefer to pair up in the lower‑energy t2g orbitals rather than occupy the higher‑energy eg orbitals. This situation corresponds to a strong field ligand and results in a low‑spin complex.
Therefore, for a d5 ion in an octahedral field, the electronic configuration becomes `t_(2g)^5` `e_g^0`, meaning that no electron enters the eg orbitals.
संबंधित प्रश्न
The hexaquo manganese (II) ion contains five unpaired electrons, while the hexacyanoion contains only one unpaired electron. Explain using Crystal Field Theory.
How are the following conversions carried out?
Benzoic acid into metanitrobenzoic acid.
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) \[\ce{[Ni(NH3)6]^{2+}}\]
Why are low spin tetrahedral complexes not formed?
Give the electronic configuration of the following complexes on the basis of Crystal Field Splitting theory.
\[\ce{[CoF6]^{3-}, [Fe(CN)6]^{4-} and [Cu(NH3)6]^{2+}}\].
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:
\[\ce{[CoF6]^{3-}, [Co(H2O)6]^{2+}, [Co(Cn)6]^{3-}}\]
The CFSE for octahedral [CoCl6]−4 is 18,000 cm−1. What will be the CFSE for tetrahedral [CoCl3]−2?
The correct order of increasing crystal field strength in following series:
The correct order of intensity of colors of the compounds is ______.
