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Each orbital can hold up to 2 electrons. Electron configuration dictates how to distribute an atom's electrons according to the Aufbau principle, which states lowest energy subshells are filled with electrons first before moving on to higher-energy orbitals. Aufbau Principle for filling subshells...
Each shell contains one or more subshells, which are made up of atomic orbitals. Subshells are characterized by Azimuthal quantum numbers (l). The value of 'l' depends on the shell (n) it is associated with. Subshells are labeled as s (l = 0), p (l =1), d (l = 2), and ...
p2 Electron configurations with filled subshells OR HALF-FILLED SUBSHELLS are more stable than other configurations. p3 (can explain some transition metal chemistry) Electrons begin to pair only AFTER all equivalent p4 "p" orbitals are full. Experimental evidence for Hund's rule: "Paramagnetism" ...