Select the option with correct property -
- $[Ni(CO)_4]$ and $[NiCl_4]^{2-}$ both diamagnetic
- $[Ni(CO)_4]$ and $[NiCl_4]^{2-}$ both paramagnetic
- $[NiCl_4]^{2-}$ diamagnetic, $[Ni(CO)_4]$ paramagnetic
- $[Ni(CO)_4]$ diamagnetic, $[NiCl_4]^{2-}$ paramagnetic
The Correct Option is D
Solution and Explanation
In \([\text{Ni}(\text{CO})_4]\), nickel is in the zero oxidation state and has a \(3d^{10}\) electron configuration, leading to a fully paired electron configuration, making it diamagnetic.
In contrast, in \([\text{NiCl}_4]^{2-}\), nickel is in the \(+2\) oxidation state with a \(3d^8\) electron configuration. The chloride ligands are weak-field ligands and do not pair up the electrons, resulting in unpaired electrons and a paramagnetic nature.
Thus, the correct answer is:
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