$[NiCl {]_{4}}^{2 -}$ is paramagnetic while $[Ni (CO)_{4}]$ is diamagnetic though both are tetrahedral. Why?

In Ni(CO)₄, Ni is the zero oxidation state whereas in NiCl₄^2–, it is in +2 oxidation state. In the presence of CO ligand, which is strong ligand can paired all electron in Ni(CO), Hence it is a diamagentic in nature. But Cl^– being a weak ligand is unable to pair up the unpaired electrons. Hence NiCl₄^2- is paramagnetic in nature.

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Coordination Compounds

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$[NiCl {]_{4}}^{2 -}$ is paramagnetic while $[Ni (CO)_{4}]$ is diamagnetic though both are tetrahedral. Why?