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- https://phys.libretexts.org/Bookshelves/University_Physics/University_Physics_(OpenStax)/University_Physics_III_-_Optics_and_Modern_Physics_(OpenStax)/08%3A_Atomic_Structure/8.05%3A_The_Exclusion_Principle_and_the_Periodic_TableThe structure and chemical properties of atoms are explained in part by Pauli’s exclusion principle: No two electrons in an atom can have the same values for all four quantum numbers (n,l,m,ms). This ...The structure and chemical properties of atoms are explained in part by Pauli’s exclusion principle: No two electrons in an atom can have the same values for all four quantum numbers (n,l,m,ms). This principle is related to two properties of electrons: All electrons are identical and they have half-integral spin (s=1/2).
- https://phys.libretexts.org/Bookshelves/University_Physics/University_Physics_(OpenStax)/University_Physics_III_-_Optics_and_Modern_Physics_(OpenStax)/09%3A_Condensed_Matter_Physics/9.02%3A_Types_of_Molecular_BondsMolecules form by two main types of bonds: the ionic bond and the covalent bond. An ionic bond transfers an electron from one atom to another, and a covalent bond shares the electrons. The energy chan...Molecules form by two main types of bonds: the ionic bond and the covalent bond. An ionic bond transfers an electron from one atom to another, and a covalent bond shares the electrons. The energy change associated with ionic bonding depends on three main processes: the ionization of an electron from one atom, the acceptance of the electron by the second atom, and the Coulomb attraction of the resulting ions. Covalent bonds involve space-symmetric wave functions.
- https://phys.libretexts.org/Courses/Georgia_State_University/GSU-TM-Physics_II_(2212)/12%3A_Atomic_Structure/12.04%3A_The_Exclusion_Principle_and_the_Periodic_TableSubshells are determined by the value of l; thus, we first determine which values of l are allowed, and then we apply the equation “maximum number of electrons that can be in a \(subshell = 2(2l + 1\)...Subshells are determined by the value of l; thus, we first determine which values of l are allowed, and then we apply the equation “maximum number of electrons that can be in a \(subshell = 2(2l + 1\))” to find the number of electrons in each subshell. The structure of the periodic table (Figure \(\PageIndex{1}\)) can be understood in terms of shells and subshells, and, ultimately, the total energy, orbital angular momentum, and spin of the electrons in the atom.
