This episode defines electron configuration as the arrangement of electrons in an atom's orbitals. It explain two notation methods: standard notation (e.g., 1s2) and orbital box notation, and outlines the three fundamental filling rules: the Aufbau principle, Pauli exclusion principle, and Hund's rule. It introduce noble gas shorthand for larger atoms and discuss notable exceptions like chromium and copper, which achieve extra stability with half-filled or completely filled orbitals. The episode also covers how electron configurations change for ions and highlights that the shape of the periodic table directly reflects the filling of s, p, d, and f orbitals.

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