Question

\[s{p^3}{d^2}\] hybrid orbitals are
A) Linear bipyramidal
B) Pentagonal
C) Trigonal bipyramidal
D) Octahedral

Answer 1

Hint: We know that hybridization is the process in which atomic orbitals of similar energies combine to form new orbitals. And the new orbitals that formed have different shapes and energies than the original orbitals.

Complete step by step solution:There are four orbitals namely s, p, d and f in which electrons are filled. The electron distribution in these orbits stabilize the molecule to acquire the lowest state of energy.
Now, we will discuss \[s{p^3}{d^2}\] hybridization. In this hybridization, overlap of s, p and d orbital takes place to achieve the lowest state of energy. Three numbers of p orbital, one s orbital and two d orbital undergo overlapping to give \[s{p^3}{d^2}\]hybridization. In this hybridization, six numbers of identical \[s{p^3}{d^2}\]hybrid orbital forms. The positions of these six orbits are at the corners of an octahedron. And their inclination is at ninety degrees towards each other. Therefore, the octahedral molecular shape is because of the \[s{p^3}{d^2}\]hybridization.

Hence, option D is right.

Additional Information:Also, in case of \[{d^2}s{p^3}\] hybridization, six numbers of hybrid orbital forms. Here also, one s, two d orbital and three numbers of p orbitals undergo hybridization to form six \[{d^2}s{p^3}\]hybrid orbital.

Note: Hybridisation also helps to give an idea of the shapes of the molecules. The \[s{p^3}\] hybridization means the shape is tetrahedral if no lone pair is present. The \[s{p^2}\] hybridization means the molecular shape is trigonal planar. And the sp hybridization means the shape is linear.