Question

Both \[[Ni{(CO)_4}]\] and ${[Ni{(CN)_4}]^{2 - }}$ are diamagnetic. The hybridizations of nickel in these complexes, respectively, are:
A) $s{p^3},\,\,s{p^3}$
B) $s{p^3},\,\,ds{p^2}$
C) $ds{p^2},\,\,s{p^3}$
D) $ds{p^2},\,\,ds{p^2}$

Answer 1

Hint:To solve this question, we must first understand some basic concepts about Hybridization and Coordinate Compounds. Then we need to assess the important points and try to conclude the Hybridization and then only we can conclude the correct answer.

Complete step by step answer:
Before we move forward with the solution of this given question, let us first understand some basic concepts:
Hybridization: is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory. Hybrid orbitals are useful in the explanation of molecular geometry and atomic bonding properties and are symmetrically disposed in space.
Coordination Compounds: are molecules that poses one or multiple metal centers that is bound to ligands (atoms, ions, or molecules that donate electrons to the metal). These complexes can be neutral or charged. When the complex is charged, it is stabilized by neighboring counter-ions.
Step 1: For \[[Ni{(CO)_4}]\] :
In \[[Ni{(CO)_4}]\] , $Ni$ is in \[0\] oxidation state so there are \[8\] electrons in \[3d\] subshell and $2$ electrons in $4s$ . $CO$ is the strong ligand, so it does pairing with the d subshell atom leaving one d subshell with unpaired electrons. Now, the electron from $s$ shell shifts to d creating vacant space in s subshell and thus the hybridization is $s{p^3}$ .
Step 2: For ${[Ni{(CN)_4}]^{2 - }}$ :
In ${[Ni{(CN)_4}]^{2 - }}$ , $Ni$is in $ + 2$oxidation state so it has \[8\] electrons in d subshell and \[CN\] is also a strong ligand which pairs with $d$ subshell atom and leaves one d orbital empty and thus its hybridization is \[ds{p^2}\] .
So, clearly we can conclude that the correct answer is Option B.

Note:A coordination complex consists of a central atom or ion, which is usually metallic and is called the coordination centre, and a surrounding array of bound molecules or ions, that are in turn known as ligands or complexing agents. Many metal-containing compounds, especially those of transition metals, are coordination complexes. A coordination complex whose centre is a metal atom is called a metal complex of d block element.