
The Pauli exclusion principle asserts that no two identical fermions can occupy the same quantum state simultaneously.The Pauli exclusion principle is a rule of the quantum world that forbids two particles from being in the same state at the same time. Imagine a theater where each seat has a unique row and seat number. Fermion spectators (such as electrons) cannot sit in the same seat together: each needs its own. Thanks to this, atoms do not collapse, and chemical elements differ from each other.
The principle was proposed by Wolfgang Pauli in 1925 based on the analysis of atomic spectra. He noticed that the distribution of electrons among shells could be explained by assuming that electrons are forbidden to occupy already occupied states, characterized by the fourth quantum number — spin. Later, in 1940, Pauli proved the connection of the principle with spin and statistics — the spin-statistics theorem. The principle was further developed in the works of Erwin Schrödinger and Paul Dirac, who linked it to the antisymmetry of the wave function.
The Pauli exclusion principle applies to all fermions, including electrons, protons, neutrons, and quarks. It determines the filling of electron shells, explains the chemical properties of elements, the electrical conductivity of metals, superconductivity, and the behavior of degenerate gas in astrophysical objects. Limits of applicability: the principle is strict for fundamental fermions; in composite systems, effective bosons may arise that do not obey the prohibition, such as Cooper pairs in superconductors.
If it weren't for the Pauli principle, all electrons in an atom would gather in the lowest orbital, and then there would be no chemistry, no life — all atoms would be like inert gases.
















