English
Karnataka Board PUCPUC Science 2nd PUC Class 12

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+.

Advertisements
Advertisements

Question

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

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

Short/Brief Note
Advertisements

Solution

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

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

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

shaalaa.com
  Is there an error in this question or solution?
Chapter 9: Coordination Compounds - Exercises [Page 124]

APPEARS IN

NCERT Exemplar Chemistry Exemplar [English] Class 12
Chapter 9 Coordination Compounds
Exercises | Q III. 30. | Page 124

RELATED QUESTIONS

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 are the following conversions carried out?

Benzoic acid into metanitrobenzoic acid.


State the superiority of crystal field theory over valence bond theory.


Why are low spin tetrahedral complexes rarely observed?


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.


Why are low spin tetrahedral complexes not formed?


Arrange following complex ions in increasing order of crystal field splitting energy (∆O):

\[\ce{[Cr(Cl)6]^{3-}, [Cr(CN)6]^{3-}, [Cr(NH3)6]^{3+}}\].


\[\ce{CuSO4 . 5H2O}\] is blue in colour while \[\ce{CuSO4}\] is colourless. Why?


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?


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 difference between a weak field ligand and a strong field ligand?


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.


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×