![[ NiCl4] 2– is paramagnetic while [ Ni(CN) 4 ] 2– is diamagnetic](https://blogger.googleusercontent.com/img/b/R29vZ2xl/AVvXsEhwbwYzbTnE9yhRuMJRUzMb5kJIDBF1EuZr6NMga3PUHTOg5eoFtr7Av-1ybb41axuaGCmpmQRfsWt3xlDHkdVPBcNCNdgMXZbuF7jinN7ioyLqXebiN_at60fQr_G4enCvRYumnlKubek/w640-h284/bSE.jpg)
Why is [ NiCl4 ] 2– paramagnetic while [ Ni(CN) 4 ] 2– is diamagnetic ?
The
Ni(II) ion is 3d8 system.
According to Hund’s rule the outer
electronic configuration of Ni(II) ion
is [ Ar ] 3d8. From
electronic configuration of Ni(II) ion , it is shown that it has two unpaired electrons.
Now,
depending upon the hybridization, there are two types of possible structure of Ni(II) complex are formed with co-ordination number 4.
If
the complex involves ‘sp3’ hybridization, it would have
tetrahedral structure . Again, If the complex involves ‘dsp2’ hybridization, it would have square planar structure .
![[ NiCl4] 2– is paramagnetic while [ Ni(CN) 4 ] 2– is diamagnetic](https://blogger.googleusercontent.com/img/b/R29vZ2xl/AVvXsEhwbwYzbTnE9yhRuMJRUzMb5kJIDBF1EuZr6NMga3PUHTOg5eoFtr7Av-1ybb41axuaGCmpmQRfsWt3xlDHkdVPBcNCNdgMXZbuF7jinN7ioyLqXebiN_at60fQr_G4enCvRYumnlKubek/s1600/bSE.jpg "[ NiCl4] 2– is paramagnetic while [ Ni(CN) 4 ] 2– is diamagnetic")
