Which of the following is paramagnetic?

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(D) In $[Ni(CO)_4]$,the oxidation state of $Ni$ is $0$ and it has a $d^{10}$ configuration. Since $CO$ is a strong field ligand,all electrons are pair

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$[NiCl_4]^{2-}$

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(D) In $[Ni(CO)_4]$,the oxidation state of $Ni$ is $0$ and it has a $d^{10}$ configuration. Since $CO$ is a strong field ligand,all electrons are paired,making it diamagnetic.In $[Co(NH_3)_6]^{3+}$,$Co$ is in $+3$ oxidation state $(d^6)$. $NH_3$ is a strong field ligand,causing pairing of electrons,making it diamagnetic.In $[Ni(CN)_4]^{2-}$,$Ni$ is in $+2$ oxidation state $(d^8)$. $CN^-$ is a strong field ligand,causing pairing of electrons,making it diamagnetic.In $[NiCl_4]^{2-}$,$Ni$ is in $+2$ oxidation state $(d^8)$. $Cl^-$ is a weak field ligand and cannot cause pairing of electrons. Therefore,it has $2$ unpaired electrons,making it paramagnetic.

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