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Standard XII
Chemistry
Crystal Field Theory
Question

$$[NiCl_4]^{2-}$$ is paramagnetic while $$Ni(CO)_4]$$ diamagnetic though both are tetrahedral. Why? (Atomic no. of $$Ni = 28$$)

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Solution
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In $$Ni{\left( CO \right)}_{4}$$, the oxidation state of $$Ni$$ is zero whereas in $${\left[ Ni{Cl}_{4} \right]}^{2-}$$, the oxidation state of $$Ni$$ is $$+2$$.
The presence of $$CO$$ ligand, which is a strong ligand, can pair all electrons in $$Ni{\left( CO \right)}_{4}$$ and thus it is diamagnetic in nature but $${Cl}^{-}$$ is a weak ligand and is unable to pair up the unpaired electrons and thus $${\left[ Ni{Cl}_{4} \right]}^{2-}$$ is paramagnetic in nature.

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