As compared to pure atomic orbitals, hybrid orbitals have
A) Low energy
B) Same energy
C) High energy
D) None of these

Hint: We know that, in the process of hybridisation, atomic orbitals composed of similar or close to similar energy undergo the intermixing of orbitals to produce a group of orbitals. Here, we have to determine the energy of the hybrid orbitals.

Formula used: \[H = \dfrac{{V + X + A - C}}{2}\]; Here, H means hybridisation, X is the count of monovalent atoms, A stand for anionic charge, and C stands for cationic charge

Complete Step by Step Answer:
 Let's understand some characteristics of hybridization.
1) The orbitals belonging to the same atom possessing similar energies undergo hybridization.
2) The count of hybrid orbitals produced equates with the count of orbitals undergo hybridization.
3) There is a comparable shape and energy of the hybrid orbitals.
4) In hybrid orbitals, more stable bonds are generated than in the pure atomic orbitals.
5) The aim of hybridization is to form equivalent symmetrical orbitals.
Let's understand the energy of the formed hybrid orbitals. The energy of the hybrid orbitals is less as compared to the pure atomic orbitals. The reason is because of the change in the energy level of the orbitals because of hybridization. The energy possessed by 2s orbital of a Carbon atom is lower than the 2p orbitals as it is of more penetrating nature. After the process of hybridization, the energy content of all the hybrid orbitals has the same energy, lower than orbitals of p but higher than s- orbital.
Hence, option A is right.

Note: It is to be noted that, there are many types of hybridization namely, sp, \[s{p^2}\] , \[s{p^3}\] , \[s{p^3}{d^2}\] etc. Hybridisation determines the molecular shape of a molecule. If no lone pair is present, the \[s{p^3}\]hybridization indicates a tetrahedral-shaped molecule.