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Hybridization shape and magnetic moment ...

Hybridization shape and magnetic moment of `K_(3)[Co(CO)_(6)]` is

A

`d^2sp^3` ,octahedral, 4.9 BM

B

`sp^3d^2` octahedral, 4.9 BM

C

`dsp^2` , square planar, 4.9 BM

D

`sp^3` , tetrahedral, 4.9 BM

Text Solution

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The correct Answer is:
B
4.9 BM in all the choices is excellent clue. It shows the complex has 4 unpaired electrons. Cobalt is in +3 oxidation state ( `d^6` ion). A `d^6` ion having 4 unpaired electrons and co–ordination no. 6 means it is in `sp^3d^2` hybridised state.

If it were `d^2 sp^3` the complex would have been diamagnetic. Note that `CO_3^(2-)` that is a bidentate ligand here. Though it can acts as monodentate ligand in some cases.
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ERRORLESS-COORDINATION COMPOUNDS-NCERT BASED QUESTION (VALENCE BOND THEORY AND GEOMETRY AND MAGNETIC NATURE OF COORDINATION COMPOUNDS)
  1. Which of the following shell form an outer octahedral complex

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  2. Which has square planar geometry

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  3. Hybridization shape and magnetic moment of K(3)[Co(CO)(6)] is

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  4. The correct statement with respect to the complexes Ni(CO)4 and [Ni(CN...

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  5. Which of the following molecules is not tetrahedral ?

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  6. Geometrical shapes of the complex formed by the reaction of Ni^(2+) wi...

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  7. In Fe(CO)(5), the Fe larr CO sigma bond results by the overlap between...

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  8. The number of unpaired electrons in Ni (CO)(4) is

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  9. Which complex compound obeys 18-electron rule

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  10. Both [Ni(CO)4] and [Ni (CN)4]^(2-) are diamagnetic The hybridisation...

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  11. Which of the following complex is an outer orbital complex?

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  12. Which one of the following is an outer orbital complex and exhibits pa...

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  13. The diamagnetic species is

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  14. The bonds in K4[Fe(CN)6] are

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  15. Amongst Ni(CO)(4),[Ni(CN)(4)]^(2-) and NiCl(4)^(2-):

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  16. The geometry of Ni(CO)4 and Ni(PPH3)2Cl2 are

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  17. The species having tetrahedral shape is

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  18. The hybridized state of Al^(3+) in the complex ion formed when AlCl3 ...

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  19. Consider the following two complex ions : [CoF(6)]^(3-) and [Co(C(2)O(...

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  20. Choose the correct statement

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