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Unformatted text preview: b) Consider phase of wavefunctions 4) Valence Bond theory Normal orbitals don’t match with VSEPR. We need new orbitals. How to form? Take combinations of old orbitals! a) One orbital needed for every pair of electrons - σ bond - lone pair b) # orbital in = # orbitals out Use lowest energy orbitals c) σ bonds = 1 lobe overlap; π = 2 lobes overlap Orbitals available for carbon: Example: Compare… Ethane, CH3-CH3 Ethene, CH2=CH2 Ethyne,HCΞCH [Practice: check Exam2; 3.35-40] 5) Molecular orbital theory Also concerned with orbital overlap to form bonds, but we use the normal orbitals. Two questions: Bond order? Paramagnetic? Candace’s method: a) Choose (and USE) the right diagram b) Count total # of electrons c) Fill molecular orbitals according to Aufbau (Ch 1) [Practice: Exam 2 paramagnetism question; 3.49-53]...
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