Which of the following is diamagnetic in natu | vedclass

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(D) To determine the magnetic nature,we look at the number of unpaired electrons in the central metal ion:$1$. In $[CoF_6]^{3-}$,$Co^{3+}$ is $d^6$. $

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$[Ni(CN)_4]^{2-}$

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(D) To determine the magnetic nature,we look at the number of unpaired electrons in the central metal ion:$1$. In $[CoF_6]^{3-}$,$Co^{3+}$ is $d^6$. $F^-$ is a weak field ligand,so it is high spin: $t_{2g}^4 e_g^2$,having $4$ unpaired electrons (Paramagnetic).$2$. In $[NiCl_4]^{2-}$,$Ni^{2+}$ is $d^8$. $Cl^-$ is a weak field ligand,forming a tetrahedral complex: $e^4 t_2^4$,having $2$ unpaired electrons (Paramagnetic).$3$. In $[Ni(NH_3)_6]^{2+}$,$Ni^{2+}$ is $d^8$. $NH_3$ is a strong field ligand,but for octahedral $d^8$,it remains $t_{2g}^6 e_g^2$,having $2$ unpaired electrons (Paramagnetic).$4$. In $[Ni(CN)_4]^{2-}$,$Ni^{2+}$ is $d^8$. $CN^-$ is a strong field ligand,forming a square planar complex. The electrons pair up in $d_{xy}, d_{yz}, d_{zx}$ and $d_{z^2}$ orbitals,leaving the $d_{x^2-y^2}$ empty. There are $0$ unpaired electrons (Diamagnetic).

Which of the following is diamagnetic in nature?

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