Here’s a explanation:
Degenerate Orbitals in MOT
- Degenerate orbitals are molecular orbitals that have the same energy.
- In diatomic molecules, certain orbitals (like the two π orbitals in a p-subshell) have exactly the same energy level.
- Electrons can occupy any of these orbitals without changing the total energy of the molecule.
Example
- In the O₂ molecule, the two π(2px) and π(2py) orbitals are degenerate.
- Both orbitals have the same energy, so electrons fill them according to Hund’s rule (one electron in each first, then pairing).
Key Points
- Degenerate orbitals always belong to the same type and energy level.
- Electrons fill separately first before pairing.
- Degeneracy affects the magnetic properties of the molecule (like paramagnetism in O₂).
In short:
Degenerate orbitals are “equal-energy orbitals” where electrons can freely occupy without affecting the molecule’s overall energy.