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Question : 7
Total: 13
(a) Although both [ NiCl 4 ] 2 − and [ Ni ( CO ) 4 ] have s p 3 hybridisation yet [ NiCl 4 ] 2 − is paramagnetic and [ Ni ( CO ) 4 ] is diamagnetic. Give reason. (Atomic no. of Ni = 28 )
(b) Write the electronic configuration ofd 5 on the basis of crystal field theory when.
(i)∆ o < P and
(ii)∆ o > P
(b) Write the electronic configuration of
(i)
(ii)
Solution:
(a) In [ NiCl 4 ] 2 − , Ni is in +2 oxidation state and each Cl − donates a pair of electron. So, Cl − acts as a weak ligand and does, not cause any forced pairing. Thus, electrons remain unpaired making it paramagnetic.
In[ Ni ( CO ) 4 ] , Ni is in zero oxidation state and CO acts as a strong ligand causing forced pairing. Thus, no electron remains unpaired making it diamagnetic.
(b) (i)t 2 g 3 e g 2
(ii)t 2 g 5 e g 0
In
(b) (i)
(ii)
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