Question

On hybridization of one s-and one p-orbital, we get :

• A. two mutually perpendicular orbitals.
• B. two orbitals at ${180}^{\circ }$.
• C. four orbitals directed tetrahedrally.
• D. three orbitals in a plane.

Answer 1

The correct option is B two orbitals at ${180}^{\circ }$.

On hybridization of one s-and one p-orbital, we get two orbitals at ${180}^0$. The number of hybrid orbitals formed is equal to the number of participating atomic orbitals, which in present case is $2$. The angle between these two is equal to ${360}^0$ divided by the number of orbitals. $\frac{{360}^0}{2}={180}^0$