Question:
Which of the following species represent the example of $dsp^2$ -hybridization ?
Which of the following species represent the example of $dsp^2$ -hybridization ?
Updated On: Jul 12, 2022
- $[Fe(CN)_6]^{3-}$
- $[Ni(CN)_4]^{2-}$
- $[Zn(NH_3)_4]^{2+} $
- $ [FeF_6]^{3-}$
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The Correct Option is B
Solution and Explanation
In $Fe(CN)_6]^{3-}$, and $[FeF_6]^{3-}$ there are six ligands, as such $dsp^2$-hybridisation is not possible.
For structure of $[Ni(CN)_4]^{2-}$, see hint to 27 above. In it the state of hybridisation of $Ni^{2+}$ is $dsp^2$.
In $[Zn(NH_3)_4]^{2-} \, ,Zn^{2+}$ has configuration of $[Ar]^{18} \,3d^{10}$. Thus $dsp^2$-hybridisation is not possible
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Concepts Used:
Coordination Compounds
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.