Advertisements
Advertisements
प्रश्न
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) \[\ce{[Fe(CN)6]^{3-}}\]
Advertisements
उत्तर
(i) \[\ce{[Co(NH3)6]^{3+}}\]
(iii) \[\ce{[Fe(CN)6]^{4-}}\]
Explanation:
(i) Molecular orbital electronic configuration of \[\ce{Co^{3+}}\] in \[\ce{[Co(NH3)6]^{3+}}\] is
Number of unpaired electron = 0
Magnetic property = Diamagnetic
(ii) Molecular orbital electronic configuration of \[\ce{Mn^{3+}}\] in \[\ce{[Mn(CN)6]^{3-}}\]
Number of unpaired electron = 2
Magnetic property = Paramagnetic
(iii) Molecular orbital electronic configuration of \[\ce{Fe^{3+}}\] in \[\ce{[Fe(CN)6]^{4-}}\] is
Number of unpaired electron = 0
Magnetic property = Diamagnetic
(iv) Molecular orbital electronic configuration of \[\ce{Fe^{3+}}\] in \[\ce{[Fe(CN)6]^{3-}}\]
Number of unpaired electron = 1
Magnetic property = Paramagnetic
APPEARS IN
संबंधित प्रश्न
Draw figure to show the splitting of d orbitals in an octahedral crystal field.
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 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, \[\ce{[Co(NH3)6]^{3+}}\], \[\ce{[Co(CN)6]^{3-}}\], \[\ce{[Co(H2O)6]^{3+}}\]
The CFSE for octahedral \[\ce{[CoCl6]^{4-}}\] is 18,000 cm–1. The CFSE for tetrahedral \[\ce{[CoCl4]^{2-}}\] will be ______.
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.
\[\ce{CuSO4 . 5H2O}\] is blue in colour while \[\ce{CuSO4}\] is colourless. Why?
Why are different colours observed in octahedral and tetrahedral complexes for the same metal and same ligands?
The correct order of increasing crystal field strength in following series:
Using crystal field theory, write the electronic configuration of d5 ion, if Δ0 > P.
What is the spectrochemical series?
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 ______.
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.
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:
