Advertisements
Advertisements
प्रश्न
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:
\[\ce{[FeF6]^{3-}, [Fe(H2O)6]^{2+}, [Fe(CN)6]^{4-}}\]
Advertisements
उत्तर
(1) \[\ce{FeF^{3-}6}\]:
\[\ce{Fe^{3+} = 3d^5}\]
Number of unpaired electrons = 5
Magnetic moment = `sqrt(5(5 + 2))` = 5.92 BM
(2) \[\ce{[Fe(H2O)6]^{2+}}\]:
\[\ce{Fe^{2+} = 3d^6}\]
Number of unpaired electrons = 4
Magnetic moment = `sqrt(4(4 + 2))` = 4.9 BM
(3) \[\ce{[Fe(CN)6]^{4-}}\]:
\[\ce{Fe^{2+} = 3d^6}\]
Since CN– is a strong field ligand all the electrons get paired.
No unpaired electrons so diamagnetic.
APPEARS IN
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 Δo decide the actual configuration of d orbitals in a coordination entity?
Why are low spin tetrahedral complexes rarely observed?
Write the electronic configuration of Fe(III) on the basis of crystal field theory when it forms an octahedral complex in the presence of (i) strong field, and (ii) weak field ligand. (Atomic no.of Fe=26)
Complete and balance the following reactions:
\[\ce{P4 + H2SO4 ->}\] ______ + ______ + ______
The CFSE for octahedral \[\ce{[CoCl6]^{4-}}\] is 18,000 cm–1. The CFSE for tetrahedral \[\ce{[CoCl4]^{2-}}\] will be ______.
Arrange following complex ions in increasing order of crystal field splitting energy (∆O):
\[\ce{[Cr(Cl)6]^{3-}, [Cr(CN)6]^{3-}, [Cr(NH3)6]^{3+}}\].
Match the complex ions given in Column I with the hybridisation and number of unpaired electrons given in Column II and assign the correct code:
| Column I (Complex ion) | Column II (Hybridisation, number of unpaired electrons) |
| A. \[\ce{[Cr(H2O)6]^{3+}}\] | 1. dsp2, 1 |
| B. \[\ce{[Co(CN)4]^{2-}}\] | 2. sp3d2, 5 |
| C. \[\ce{[Ni(NH3)6]^{2+}}\] | 3. d2sp3, 3 |
| D. \[\ce{[MnF6]^{4-}}\] | 4. sp3, 4 |
| 5. sp3d2, 2 |
Why are different colours observed in octahedral and tetrahedral complexes for the same metal and same ligands?
The CFSE for octahedral [CoCl6]−4 is 18,000 cm−1. What will be the CFSE for tetrahedral [CoCl3]−2?
Crystal field stabilising energy for high spind4 octahedral complex is:-
What is the difference between a weak field ligand and a strong field ligand?
What is crystal field splitting energy?
Consider that d6 metal ion (M2+) forms a complex with aqua ligands and the spin only magnetic moment of the complex is 4.90 BM. The geometry and the crystal field stabilization energy of the complex are ______.
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:
The correct order of the wavelength of light absorbed by the following complexes is:
- [Co(NH3)6]3+
- [Co(CN)6]3−
- [Cu(H2O)4]2+
- [Ti(H2O)6]3+
Choose the correct answer from the options given below:
