[CHEM 1110] - Final Exam Guide - Comprehensive Notes fot the exam (47 pages long!)
30 Mar 2017
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Chemical bonds form by pairing valence electrons such that atoms get a ng config (octet rule) 2h+ o = h20: tells us why water is stable. Valence shell electron pair reulsipon: e pairs repel each toher. Electrostatic or quantum mechanical: pauli exclusion: 1 orbital 2 electrons. Hard to generalize to more complex structures. Predicts trig pyramial for ch3 but its planar. 1st qm model: valence bond theory: energy of atomic or hybrid orbitals centered on atoms that make molecule: calculated as atoms get closer together. Nuclei get closer: s orbitals interact: can be energetically favoralb (h) or repulsive. Have to stay at a finite distance so energy rapidly increases as you compress the bond. H2s: h 1s, h 1s, s 3s2 3p4. Half filled orbitals overlap: 1s and 1s: 3p4. C: 2s2, 2p2: hybridization: 4 sp3 orbitals. Methane: correctly predicts chem structure and molecular geo if hybridized orbitals on carbons are used.
