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प्रश्न
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, \[\ce{[Co(NH3)6]^{3+}}\], \[\ce{[Co(CN)6]^{3-}}\], \[\ce{[Co(H2O)6]^{3+}}\]
विकल्प
\[\ce{[Co(CN)_6]^{3-} > [Co(NH3)6]^{3+} > [Co(H2O)6]^{3+}}\]
\[\ce{[Co(NH3)_6]^{3+} > [Co(H2O)6]^{3+} > [Co(CN)6]^{3-}}\]
\[\ce{[Co(H2O)_6]^{3+} > [Co(NH3)6]^{3+} > [Co(CN)6]^{3-}}\]
\[\ce{[Co(CN)6]^{3-} > [Co(H2O)6]^{3+} > [Co(NH3)6]^{3+}}\]
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उत्तर
\[\ce{[Co(H2O)_6]^{3+} > [Co(NH3)6]^{3+} > [Co(CN)6]^{3-}}\]
Explanation:
The CFSE of the ligands is in the order:
H2O < NH3 < CN−
Hence, excitation energies are in the order:
\[\ce{[Co(H2O)6]^{3+} < [Co(NH3)6]^{3+} < [Co(CN)6]^{3-}}\]
From the relation E = `"hc"/λ` ⇒ `"E" ∝ 1/λ`
The order of absorption of the wavelength of light in the visible region is:
\[\ce{[Co(H2O)_6]^{3+} > [Co(NH3)6]^{3+} > [Co(CN)6]^{3-}}\]
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संबंधित प्रश्न
On the basis of crystal field theory, write the electronic configuration for d4 ion if Δ0 > P.
How does the magnitude of Δo decide the actual configuration of d orbitals in a coordination entity?
State the superiority of crystal field theory over valence bond theory.
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Atomic number of \[\ce{Mn}\], \[\ce{Fe}\] and \[\ce{Co}\] are 25, 26 and 27 respectively. Which of the following inner orbital octahedral complex ions are diamagnetic?
(i) \[\ce{[Co(NH3)6]^{3+}}\]
(ii) \[\ce{[Mn(CN)6]^{3-}}\]
(iii) \[\ce{[Fe(CN)6]^{4-}}\]
(iv) \[\ce{[Fe(CN)6]^{3-}}\]
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.
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 ______.
What is the spectrochemical series?
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:
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 ______.
The complex that has highest crystal field splitting energy (Δ) 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.
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:
