it only applies to Fermions, e.g., electrons. No two electrons can occupy the same orbital state. More generally the many-body wavefunction of a system of electrons must be anti-symmetric with respect to interchange of any two electrons.Strang3r said:Does the exclusion principle mean that no atom and sub atomic particles can exist at the same place?
there can be a degeneracy pressure, e.g., in neutron stars (neutrons are fermions), that opposes gravitational collapse.Can I safely say that in stars the gravity is opposed by this aspect or implication of the principle?
Pauli's Exclusion Principle is a fundamental principle of quantum mechanics that states that no two particles with the same spin quantum value can occupy the same quantum state within a quantum system simultaneously.
Pauli's Exclusion Principle was first proposed by Austrian physicist Wolfgang Pauli in 1925.
Pauli's Exclusion Principle plays a crucial role in understanding the behavior of electrons and other fermions in atoms, molecules, and solids. It explains why electrons occupy different energy levels and why matter is stable.
Pauli's Exclusion Principle is responsible for the organization of the periodic table. The principle dictates that each orbital can hold a maximum of two electrons, and these electrons must have opposite spin values. This results in the periodic filling of electron shells in atoms, creating the pattern of the periodic table.
While Pauli's Exclusion Principle applies to most particles in nature, there are a few known exceptions. For example, in certain extreme conditions, such as in neutron stars, neutron-rich nuclei can violate the principle. However, these exceptions are rare and do not affect the validity of the principle in most cases.