$ [NiCl_4]^{2-} $ is diamagnetic while $ [Ni(CO)_4] $ is paramagnetic and both the complexes have square planar geometry
$ [NiCl_4]^{2-} $ is paramagnetic while $ [Ni(CO)_4] $ is diamagnetic and both the complexes have tetrahedral geometry
$ [NiCl_4]^{2-} $ is paramagnetic while $ [Ni(CO)_4] $ is diamagnetic and both the complexes have square planar geometry
$ [NiCl_4]^{2-} $ is diamagnetic while $ [Ni(CO)_4] $ is paramagnetic and both the complexes have tetrahedral geometry
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The Correct Option isB
Solution and Explanation
$[NiCl_4]^{2-}$ Configuration:
Oxidation state of metal $= + 2$ Type of hybridisation $= sp^3$ (tetrahedral) Number of unpaired electrons $= 2$ Magnetic nature $=$ Paramagnetic $[Ni(CO)_4]$ Configuration:
Oxidation state of metal $= O$ Type of hybridisation $= sp^3$ (tetrahedral) Number of unpaired electrons $= O$ Magnetic nature $=$ Diamagnetic Hence, $[NiCl_4]^{2-}$ is paramagnetic while $[Ni(CO)_4]$ is diamagnetic and both the complexes have tetrahedral geometry.
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.
