Give reason for the statement. $??Ni(CN)_{4}]^{2-}$ is diamagnetic while $[NiCl_{4}]^{2-}$ is paramagnetic in nature.?
Updated On: Jul 6, 2022
In $[NiCl_{4}]^{2-}$, no unpaired electrons are present while in $[Ni(CN)_{4}]^{2-}$ two unpaired electrons are present
In $[Ni(CN)_{4}]^{2-}$, no unpaired electrons are present while in $[NiCl_{4}]^{2-}$ two unpaired electrons are present
$[NiCl_{4}]^{2-}$ shows $dsp^{2}$ hybridisation hence it is paramagnetic
$[Ni(CN)_{4}]^{2-}$ shows $sp^{3}$ hybridisation hence it is diamagnetic
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The Correct Option isB
Solution and Explanation
In $[Ni(CN)_{4}]^{2-}$ there is no unpaired electrons because $CN^{-}$ is a strong field ligand. Therefore it is diamagnetic in nature.
In $[NiCl_{4}]^{2-}$, there are two unpaired electrons because $Cl^{-}$ is a weak field ligand. Therefore, it is paramagnetic in nature.
A coordination compound holds a central metal atom or ion surrounded by various oppositely charged ions or neutral molecules. These molecules or ions are re-bonded to the metal atom or ion by a coordinate bond.
Coordination entity:
A coordination entity composes of a central metal atom or ion bonded to a fixed number of ions or molecules.
Ligands:
A molecule, ion, or group which is bonded to the metal atom or ion in a complex or coordination compound by a coordinate bond is commonly called a ligand. It may be either neutral, positively, or negatively charged.
