The exclusion principle states that no two electrons in an atom can have the same set of quantum numbers i.e. be in the same quantum state. Note, if this principle wasn’t valid, every electron would occupy the 1st atomic state (state of lowest energy), the chemical behaviour of the electrons would be significantly different and nature as we know wouldn’t exist.
The exclusion principle stem from the notion that electrons are identical particles called fermions. Fermions are described by wavefunctions that are antisymmetric in the electron coordinates. Wavefunctions that are symmetric in the particle coordinates describe another class of objects called bosons to which no exclusion principle applies. All known particles are either fermions or bosons. Photon is an example of a boson.
Applying the exclusion principle and the principle of minimum energy, one can establish the electronic configuration of the elements. This serves as the foundation for understanding atomic structure and the physical and chemical properties of elements.
Also Read: Einstein’s Special Theory of Relativity
Also Read: The Unfinished Quest for the Meaning of Quantum Physics
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