“electrons will not pair in a set of equal energy orbitals if an empty orbital is available” is a statement of
LectureNotes’ statement, “electrons will not pair in a set of equal energy orbitals if an empty orbital is available,” is a reflection of the Pauli exclusion principle in quantum mechanics.
The Pauli exclusion principle states that no two electrons within an atom can have the same set of quantum numbers. One of the consequences of this principle is that when electrons occupy orbitals with the same energy level (referred to as degenerate orbitals), they will not pair up until each orbital has at least one electron.
In other words, if there is an empty orbital available within a set of equal energy orbitals, electrons will occupy separate orbitals rather than pairing up. This behavior is a result of the tendency of electrons to minimize their mutual repulsion by occupying different orbitals within the same energy level.
By following this principle, electrons ensure that the overall energy of the atom is minimized and the stability of the electron configuration is maintained. This principle has significant implications in understanding the electronic structure, chemical bonding, and properties of atoms and molecules.