Question

Orbital \[{{d}_{{{x}^{2}}-{{y}^{2}}}}\] is involved in which of the following hybridizations?
This question has multiple correct options.
A.$s{{p}^{3}}d$ (square pyramidal)
B.$ds{{p}^{2}}$
C.$s{{p}^{3}}{{d}^{2}}$
D.$s{{p}^{3}}{{d}^{3}}$

Answer 1

Hint:In organic chemistry, hybridisation is used to explain the covalent bonds in organic molecules. It is defined as the intermixing of atomic orbital of different shape and has the same energy to give the same number of hybrid orbital of the same energy, orientation and shape so that there will be minimum repulsion between the hybrid orbitals.

Complete step-by-step answer:\[{{d}_{{{x}^{2}}-{{y}^{2}}}}\]orbital lies in the xy plane in which the lobes are directed along x and y axis. The lobes of orbitals ${{p}_{x}}$ and ${{p}_{y}}$ are along the x and y axis.
Let us discuss the above options:
A.The shape for $s{{p}^{3}}d$hybridization is trigonal bipyramidal. It contains one $s$ orbital with three $p$ orbitals that are ${{p}_{x}},{{p}_{y}}$ and ${{p}_{z}}$ and one $d$ orbital that is ${{d}_{{{z}^{2}}}}$ . The example of $s{{p}^{3}}d$hybridization is $PC{{l}_{5}}$ . Therefore, this option is incorrect.
Let us see the structure:

B.As we have discussed that \[{{d}_{{{x}^{2}}-{{y}^{2}}}}\]orbital lies in the xy plane in which the lobes are directed along x and y axis. The lobes of orbitals ${{p}_{x}}$ and ${{p}_{y}}$ are along the x and y axis. In $ds{{p}^{2}}$ , it has square planar geometry that means the four hybridized orbital lies in xy plane. ${{d}_{{{x}^{2}}-{{y}^{2}}}}$ orbital is used in $ds{{p}^{2}}$ geometry having square planar shape. This hybridization involves $s,{{p}_{x}}$ and ${{p}_{y}}$ orbital. The example of $ds{{p}^{2}}$geometry is $Xe{{F}_{4}}$ geometry. Therefore, this option is correct.
Let us see the structure:

C.The shape of $s{{p}^{3}}{{d}^{2}}$ hybridization is octahedral. It contains $s,p$ and $d$ orbitals which undergo mixing to form six identical $s{{p}^{3}}{{d}^{2}}$orbitals. They are inclined at an angle of ${{90}^{{}^\circ }}$ to one another. Here, the $d$ orbital is ${{d}_{{{x}^{2}}-{{y}^{2}}}}$ and ${{d}_{{{z}^{2}}}}$ . Therefore, this option is correct. The example of $s{{p}^{3}}{{d}^{2}}$is $S{{F}_{6}}$ .
Let us see the structure:

D.The shape of $s{{p}^{3}}{{d}^{3}}$ hybridization is pentagonal bipyramidal. It contains one$s$ orbital with $p$ orbitals that are three ${{p}_{x}},{{p}_{y}}$ and ${{p}_{z}}$ and three $d$ orbitals. The $d$ orbitals involved are ${{d}_{{{x}^{2}}-{{y}^{2}}}},{{d}_{{{z}^{2}}}},{{d}_{xy}}$ . Therefore, this option is correct. The example is Iodine heptafluoride.
Let us see the structure:

Note:It is to note that the type of hybridisation tells us the geometry of a molecule. The hybridised orbitals have equal energy and shape. In hybridisation, atomic orbitals are combined to form a new atomic orbital. The number of hybrid orbitals is equal to the number of orbitals in the hybridisation.