Question
$\left[ NI ( CN )_4\right]^{2-}$ is paramagnetic while $\left[ Ni ( CO )_4\right]^{3-}$ is diamagnetic though both are tetrahedral. Why?
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Answer
In $\left[ NI ( CN )_4\right]^{2-}, Ni$ is in +2 oxidation state with electronic configuration $=3 d^8 4 s^{\circ}$.
$Cl ^{-}$is a weak ligand. It cannot pair up the electrons in 3 d orbitals. Hence, it is paramagnetic. In $\left[ Ni ( CO )_4\right], Ni$ is in zero oxidation state and its configuration is $-3 d^8 4 S^2$. In the presence of CO ligand the 4 s electrons shift to 3 d orbital to pair up the 3 d electrons. Thus, there is no unpaired electron present. Hence it is diamagnetic.
$Cl ^{-}$is a weak ligand. It cannot pair up the electrons in 3 d orbitals. Hence, it is paramagnetic. In $\left[ Ni ( CO )_4\right], Ni$ is in zero oxidation state and its configuration is $-3 d^8 4 S^2$. In the presence of CO ligand the 4 s electrons shift to 3 d orbital to pair up the 3 d electrons. Thus, there is no unpaired electron present. Hence it is diamagnetic.
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