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Pauli proposes that no two equivalent atomic electrons can occupy the same complete four-quantum-number state, using strong-field spectral bookkeeping to account for closed electron groups and restricted atomic terms, without deriving a general spin-statistics theorem. Why do atoms have different electron groups instead of putting every electron into the same available state? Pauli introduced a rule about occupation: once a complete atomic electron state is occupied, another equivalent electron cannot occupy that same state. Electrons can still share some quantum numbers; the entire label, including the principal quantum number, matters. The paper connects this rule to shell capacities and the number of spectral terms. It develops Stoner's earlier classification and uses existing spectral evidence. Pauli openly states that he cannot give a deeper justification for the rule and that complex spectra still need tests. This is an important organizing principle, rather than a calculation of every atom's energies or the later quantum-field proof about spin and statistics.
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Scientific scope
The original rule concerns the stated electron-state quantum numbers and atomic-spectrum framework. It is not the later complete spin-statistics theorem or an experimental proof for every particle. Historical terminology and later spin interpretation must be distinguished. Dirac/Fermi statistical developments retain separate credit.
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- W. Pauli jr., Ueber den Zusammenhang des Abschlusses der Elektronengruppen im Atom mit der Komplexstruktur der Spektren; original1925
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W. Pauli jr.
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English catalogue narrative
Pauli: an occupation rule explains atomic electron groups
Pauli proposes that no two equivalent atomic electrons can occupy the same complete four-quantum-number state, using strong-field spectral bookkeeping to account for closed electron groups and restricted atomic terms, without deriving a general spin-statistics theorem.
Why do atoms have different electron groups instead of putting every electron into the same available state? Pauli introduced a rule about occupation: once a complete atomic electron state is occupied, another equivalent electron cannot occupy that same state. Electrons can still share some quantum numbers; the entire label, including the principal quantum number, matters. The paper connects this rule to shell capacities and the number of spectral terms. It develops Stoner's earlier classification and uses existing spectral evidence. Pauli openly states that he cannot give a deeper justification for the rule and that complex spectra still need tests. This is an important organizing principle, rather than a calculation of every atom's energies or the later quantum-field proof about spin and statistics.
Scientific scope
The original rule concerns the stated electron-state quantum numbers and atomic-spectrum framework. It is not the later complete spin-statistics theorem or an experimental proof for every particle. Historical terminology and later spin interpretation must be distinguished. Dirac/Fermi statistical developments retain separate credit.
People and systems
W. Pauli jr.