The Pauli Exclusion Principle, formulated by Wolfgang Pauli in 1925, states that no two fermions can occupy the same quantum state simultaneously within a quantum system. Fermions are particles like electrons, protons, and neutrons that have half-integer spin values (e.g., 1/2, 3/2). This principle is fundamental in explaining the structure of the periodic table and the behavior of electrons in atoms. As a result, electrons in an atom fill available energy levels in such a way that each energy state can accommodate only one electron with a specific spin orientation, leading to the formation of distinct electron shells. The mathematical representation of this principle can be expressed as:
where is the wavefunction of a two-fermion system, indicating that swapping the particles leads to a change in sign of the wavefunction, thus enforcing the exclusion of identical states.
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