Explanation:

Orbitals:
- Orbitals are regions of space around an atomic nucleus where an electron is likely to be found.
- They are characterized by their shape, size, and orientation in space.
- Different types of orbitals have different energy levels.

Hybridization:
- Hybridization is the process of combining atomic orbitals to form new hybrid orbitals that are suitable for bonding.
- It occurs when an atom is involved in bonding and needs to create orbitals with specific characteristics to accommodate the bonding electrons.

Equal Energy:
- When atomic orbitals hybridize, they combine to form new hybrid orbitals.
- These hybrid orbitals have equal energy and are known as degenerate orbitals.
- Degenerate orbitals have the same energy level and are indistinguishable from each other.

Example:
- For example, in the case of sp3 hybridization, one s orbital and three p orbitals combine to form four sp3 hybrid orbitals.
- These four sp3 hybrid orbitals have equal energy and are degenerate.
- They are arranged in a tetrahedral orientation around the central atom.

Other Types of Hybridization:
- Other types of hybridization, such as sp, sp2, and sp3d, also result in the formation of degenerate orbitals with equal energy.
- The number and types of atomic orbitals that combine depend on the hybridization scheme.

Conclusion:
- In summary, the orbitals formed after hybridization have equal energy.
- This is because the atomic orbitals combine to form degenerate orbitals with the same energy level.
- This equal energy allows for effective bonding and the formation of stable molecules.