CHEM 107 Lecture Notes - Lecture 45: Electron Configuration, Valence Electron, Noble Gas

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11 Aug 2017
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Two electrons can occupy an s orbital p subshell and p orbitals. P subshell contains 3 orbitals (px, py, and pz) 3 orbitals, 2 e- each = max of 6 e- d subshell and d orbitals. D subshell contains 5 orbitals (dxy, dyz, dxz, dx2y2, dz2) 1s2 n = 1 orbital = s number of electrons in orbital = 2. For degenerate orbitals (same energy), the lowest-energy electron configuration is obtained by maximizing spin. Noble gas core can be used to generate a condensed electron configuration: Ti = 1s22s22p63s23p64s23d2 = [ar]4s23d2 (for the regular elements, go to the previous noble gas, and use that one) Fill the lower energy levels of an atom. Electrons that an atom has in common with the previous noble gas: outer electrons--look up in notes, valence electrons. For main-group elements: highest energy-level electrons are valence (s and p) electrons.

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