According to VBT i.e. valence bond theory,
Electronic configuration of Ni = [Ar]3d
84s
2.
(a) NiCl
2 . 6H
2O
NiCl
2 . 6H
2O
→ NiCl
2 + 6H
2O
Oxidation number of Ni(x) = x + 2(
−1) = 0; where x,
−1 and 2 are the oxidation number of Ni, oxidation number of Cl and number of Cl atoms respectively.
NiCl
2 ⇒ x + (
−2) = 0
⇒ x = 2
Electronic configuration of Ni
2+ = [Ar]3d
84s
0Cl
− is a weak field ligand. So, no pairing of electrons occurs.
For C.N. = 6

(b) K
2[Ni(CN)
4]
K
2[Ni(CN)
4]
→ 2K
+ + [Ni(CN)
4]
2−x + 4(
−1)
− (
−2) = 0; where x, 4,
−1 and
−2 are the oxidation number of Ni, number of CN ligands, charge on one CN and charge on complex.
[Ni(CN)
4]
2− ⇒ x
− 4 + 2 = 0
⇒ x = +2
Electronic configuration of Ni
2+ ⇒ [Ar]3d
84s
0CN
− is a strong field ligand. So, pairing of electrons occur. For C.N. = 4

(c) Ni(CO)
4CO is neutral and strong field ligand. So, pairing of electrons occur.
Oxidation number of Ni is zero
Electronic configuration of Ni = [Ar]3d
104s
0For C.N. = 4

(d) Na
2[NiCl
4]
Na
2[NiCl
4]
→ 2Na + [NiCl
4]
2−x + 4(
−1)
− (
−2) = 0; where x, 4,
−1 and
−2 are the oxidation number of Ni, number of CN ligands, charge on one CN and charge on complex.
[NiCl
4]
2− ⇒ x
− 4 + 2 = 0
⇒ x = +2
Electronic configuration of Ni
2+ = [Ar]3d
84s
0For C.N. = 4

Hence, only K
2[Ni(CN)
4] has dsp
2 hybridization.