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MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms .
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1 _______________________________________________________________________________ ________________________________________________________________________________ 5.111 Lecture Summary #14 Readings for today: Section 3.8 (3.9 in 3 rd ed ) – The Limitations of Lewis’s Theory, Section 3.9 (3.10 in 3 rd ed ) – Molecular Orbitals, Section 3.10 (3.11 in 3 rd ed ) – The Electron Configuration of Diatomic Molecules, Section 3.11 (3.12 in 3 rd ed ) – Bonding in Heteronuclear Diatomic Molecules. Read for Lecture #15: Sections 3.4, 3.5, 3.6 and 3.7 (Sections 3.4, 3.5, 3.6, 3.7, and 3.8 in 3 rd ed ) – Valence Bond Theory. Topics: Molecular orbital theory I. Bonding and antibonding orbitals II. Homonuclear diatomic molecules A. Molecules with MO’s originating from s orbitals B. Molecules with MO’s originating from s and p orbitals III. Heteronuclear diatomic molecules MOLECULAR ORBITAL (MO) THEORY In MO theory, valence electrons are _________________ over the entire molecule, not confined to individual atoms or bonds, as in Lewis and valence-bond models. I. BONDING AND ANTIBONDING ORBITALS Molecular orbitals (____________________) of diatomic molecules arise from adding together ( superimposing ) atomic orbitals: linear combination of atomic orbitals (LCAO) to create a molecular orbital. Bonding orbitals
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This note was uploaded on 11/27/2011 for the course CHEMICAL E 20.410j taught by Professor Rogerd.kamm during the Spring '03 term at MIT.

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lecnotes14 - MIT OpenCourseWare http:/ocw.mit.edu 5.111...

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