Which of the following are paramagnetic?A. [N | vedclass

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(C) To determine paramagnetism,we check for the presence of unpaired electrons in the $Ni$ center:$A$. $[NiCl_4]^{2-}$: $Ni^{2+}$ $(3d^8)$. $Cl^-$ is

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$A$ and $D$ only

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(C) To determine paramagnetism,we check for the presence of unpaired electrons in the $Ni$ center:$A$. $[NiCl_4]^{2-}$: $Ni^{2+}$ $(3d^8)$. $Cl^-$ is a weak field ligand,so no pairing occurs. It has $2$ unpaired electrons (Paramagnetic).$B$. $Ni(CO)_4$: $Ni^0$ $(3d^8 4s^2)$. $CO$ is a strong field ligand,causing pairing. It is diamagnetic.$C$. $[Ni(CN)_4]^{2-}$: $Ni^{2+}$ $(3d^8)$. $CN^-$ is a strong field ligand,causing pairing. It is diamagnetic.$D$. $[Ni(H_2O)_6]^{2+}$: $Ni^{2+}$ $(3d^8)$. $H_2O$ is a weak field ligand,so no pairing occurs. It has $2$ unpaired electrons (Paramagnetic).$E$. $Ni(PPh_3)_4$: $Ni^0$ $(3d^8 4s^2)$. $PPh_3$ is a strong field ligand,causing pairing. It is diamagnetic.Thus,only $A$ and $D$ are paramagnetic.

Which of the following are paramagnetic?
$A$. $[NiCl_4]^{2-}$
$B$. $Ni(CO)_4$
$C$. $[Ni(CN)_4]^{2-}$
$D$. $[Ni(H_2O)_6]^{2+}$
$E$. $Ni(PPh_3)_4$
Choose the correct answer from the options given below:

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Which of the following are paramagnetic?$A$. $[NiCl_4]^{2-}$$B$. $Ni(CO)_4$$C$. $[Ni(CN)_4]^{2-}$$D$. $[Ni(H_2O)_6]^{2+}$$E$. $Ni(PPh_3)_4$Choose the correct answer from the options given below: