In [NiCl_4]^{2-},the number of unpaired elect | vedclass

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(B) The oxidation state of $Ni$ in $[NiCl_4]^{2-}$ is calculated as $x + 4(-1) = -2$,which gives $x = +2$.$Ni$ has an atomic number of $28$,so its ele

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$2$

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(B) The oxidation state of $Ni$ in $[NiCl_4]^{2-}$ is calculated as $x + 4(-1) = -2$,which gives $x = +2$.$Ni$ has an atomic number of $28$,so its electronic configuration is $[Ar] 3d^8 4s^2$.For $Ni^{2+}$,the configuration is $[Ar] 3d^8$.Since $Cl^-$ is a weak field ligand,it does not cause pairing of electrons in the $3d$ orbitals.The $3d^8$ configuration has two unpaired electrons in the $d$-orbitals.Therefore,the number of unpaired electrons in $[NiCl_4]^{2-}$ is $2$.

In $[NiCl_4]^{2-}$,the number of unpaired electrons is

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