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Give the electronic configuration of the following complexes on the basis of Crystal Field Splitting theory. [CoFX6]X3−,[Fe(CN)X6]X4− and [Cu(NHX3)X6]X2+. - Chemistry

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प्रश्न

Give the electronic configuration of the following complexes on the basis of Crystal Field Splitting theory.

\[\ce{[CoF6]^{3-}, [Fe(CN)6]^{4-} and [Cu(NH3)6]^{2+}}\].

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उत्तर

\[\ce{[CoF6]^{3-} : Co^{3+} (d^6)}\]

\[\ce{[Fe(CN)6]^{4-} : Fe^{2+} (d)^6}\]

\[\ce{[Cu(NH3)6]^{2+} : Cu^{2+} (d^9)}\]

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पाठ 9: Coordination Compounds - Exercises [पृष्ठ १२४]

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एनसीईआरटी एक्झांप्लर Chemistry [English] Class 12
पाठ 9 Coordination Compounds
Exercises | Q III. 30. | पृष्ठ १२४

संबंधित प्रश्‍न

How does the magnitude of Δ0 decide the actual configuration of d orbitals in a coordination entity?


How are the following conversions carried out?

Benzoic acid into metanitrobenzoic acid.


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:

\[\ce{P4 + H2SO4 ->}\] ______ + ______ + ______


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) \[\ce{[Fe(CN)6]^{3-}}\]


Why are low spin tetrahedral complexes not formed?


\[\ce{CuSO4 . 5H2O}\] 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:

\[\ce{[CoF6]^{3-}, [Co(H2O)6]^{2+}, [Co(Cn)6]^{3-}}\]


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:

\[\ce{[FeF6]^{3-}, [Fe(H2O)6]^{2+}, [Fe(CN)6]^{4-}}\]


The CFSE for octahedral [CoCl6]−4 is 18,000 cm−1. What will be the CFSE for tetrahedral [CoCl3]−2?


What is the spectrochemical series?


The correct order of intensity of colors of the compounds is ______.


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 for the d5 ion with a weak 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.


Read the passage carefully and answer the questions that follow.

Crystal field splitting by various ligands

Metal complexes show different colours due to d-d transitions. The complex absorbs light of specific wavelength to promote the electron from t2g to eg level. The colour of the complex is due to the transmitted light, which is complementary of the colour absorbed.

The wave number of light absorbed by different complexes of Cr ion are given below:

Complex Wavenumber of light absorbed (cm-1) Energy of light absorbed (kJ/mol)
[CrA6]3- 13,640 163
[CrB6]3+ 17,830 213
[CrC6]3+ 21,680 259
[CrD6]3- 26,280 314

Answer the following questions:

(a) Out of ligands "A", "B", "C" and "D", which ligand causes maximum crystal field splitting? Why?

OR

Which of the two, “A” or “D” will be a weak field ligand? Why?

(b) Which of the complexes will be violet in colour? [CrA6]3- or [CrB6]3+ and why?
(Given: If 560 - 570 nm of light is absorbed, the colour of the complex observed is violet.)

(c) If the ligands attached to Cr3+ ion in the complexes given in the table above are water, cyanide ion, chloride ion, and ammonia (not in this order).

Identify the ligand, write the formula and IUPAC name of the following:

  1. [CrA6]3-
  2. [CrC6]3+

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