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Theories of Catalysis

15.why Fe[(NH...

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15.why Fe[(NH3)6] +2 does not have d 2sp 3 hybridization and have sp 3d 2 hybridization

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s p^{3} d^{2}

hybridization the same as

d^{2} s p^{3}

Q. Which one the following does not have

s p^{2}

hybridized carbon?

Q. Based on VBT,

[F e C l_{6}]^{3 -}

C l^{-}

as weak ligands.

F e

s p^{3} d^{2}

hybridized (outer orbital complex) having five unpaired electrons.

[F e (C N)_{6}]^{3 -}

C N^{-}

as strong ligand.

F e

d^{2} s p^{3}

hybridized (inner orbital complex) having only one unpaired electron. Hence,

[F e C l_{6}]^{3 -}

is more paramagnetic than

[F e (C N)_{8}]^{3 -}

.
If true enter 1, else enter 0.

Q. Match list-I (Complexes) with list - II (Hybridization of Central Atom) and select the correct answer using the codes given below the lists :

	List - I		List - II
A.	$[N i (C O)_{4}]$	1.	$s p^{3}$
B.	$[N i (C N)_{4}]^{2 -}$	2.	$d s p^{2}$
C.	$[F e (C N)_{6}]^{4 -}$	3.	$s p^{3} d^{2}$
D.	$[M n F_{6}]^{4 -}$	4.	$d^{2} s p^{3}$
		5.	$s p^{2} d$

In the valence bond theory, hybridization of orbitals is an integral part of the bond formation. Hybridisation consists of mixing or a linear combination of the "pure" atomic orbitals in such a way as to form new hybrid orbitals such as

s p, s p^{2}, s p^{3}, s p^{3} d, s p^{3} d^{3}

Which of the following atomic orbitals does not participate in trigonal bipyramidal hybridization i.e.

s p^{3} d

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