This means that the first electrons target the lowest energy orbital and once the lowest region is occupied, they ascend into higher energy orbitals. This principle states that electrons occupy their respective energy orbitals in accordance with the increasing order of energies. The electrons are filled into the orbitals of atoms in accordance with the following principles: Aufbau Principle For example, for the M orbital, n = 3.Д¬alculating the Energy Level of an Orbital It is denoted by n and can take only positive integer values. The principal quantum number assigned to each electron in an atom describes the electronвЂ™s state. These numbers are called Principal Quantum Numbers. Accordingly, the orbitals were named as K,L,M,N or 1,2,3,4 in ascending order. He established that electron orbitals represent an energy level in terms of their distance from the nucleus of the atom.

It was Bohr who laid down the foundation of orbital chemistry as we know it today. (NOTE: Degenerate orbitals is the name given to orbitals belonging to the same subshell).

The energy of an orbital depends mainly on shell and subshells, or to put in technical terms, on principle quantum numbers and azimuthal quantum numbers respectively. (The term вЂњorbitalвЂќ here refers to the region of space in which electrons populate). Energy of orbitals refers to the energy needed to take an electron present in that orbital to infinity or the energy released when that electron is shifted from infinity to that orbital.

Relative energies of atomic orbitals