Which of the following complex ions will exhi | vedclass

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(B) To determine paramagnetism,we check for unpaired electrons:$1$. In $[Ni(CO)_4]$,$Ni$ is in $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong fie

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$[Ni(H_2O)_6]^{2+}$

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(B) To determine paramagnetism,we check for unpaired electrons:$1$. In $[Ni(CO)_4]$,$Ni$ is in $0$ oxidation state $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing of electrons,resulting in $0$ unpaired electrons (diamagnetic).$2$. In $[Ni(H_2O)_6]^{2+}$,$Ni^{2+}$ is $3d^8$. $H_2O$ is a weak field ligand,so electrons remain unpaired in $t_{2g}$ and $e_g$ orbitals,resulting in $2$ unpaired electrons (paramagnetic).$3$. In $[Co(NH_3)_6]^{3+}$,$Co^{3+}$ is $3d^6$. $NH_3$ is a strong field ligand,causing pairing,resulting in $0$ unpaired electrons (diamagnetic).$4$. In $[Zn(H_2O)_4]^{2+}$,$Zn^{2+}$ is $3d^{10}$,resulting in $0$ unpaired electrons (diamagnetic).Therefore,$[Ni(H_2O)_6]^{2+}$ is paramagnetic.

Which of the following complex ions will exhibit paramagnetic behavior?

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