Chapter 11 notes

Chapter 11 notes - Chapter 11: Valence Bond Theory Lecture...

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Slide No. 1 Chapter 11: Valence Bond Theory ± What's The Point ? ² To learn the role of atomic orbitals in molecular structure ² To gain insight into the character of multiple bonds ± Orbital Hybridization ± Sigma and Pi Bonding ± Reading: 11.1 and 11.2 ± Homework Problems: 5(6), 9(10), 13(14), 21(22), 42(40), 58(57) Lecture Outline Slide No. 2 11.0 Review: Lewis Dot Structures and VSEPR ± Lewis Dot Structures ² Number of electrons ² Atom connectivity ² The Lewis Octet Rule ² “Expanded” Octets ² Bond order (bond strength, bond length) ± VSEPR ² Regions of electron density (bonds, lone pairs) ² Electron group arrangements ² Molecular structure ± Questions ² How does VSEPR combine with atomic orbital theory? ² How do double bonds and triple bonds really work?
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Slide No. 3 11.1 Valence Bond Theory and Hybrid Orbitals ± Valence atomic orbitals are different in molecules than in isolated atoms ² Hybridization: Atomic orbitals recombine to form new orbitals • New orbitals are a degenerate set ² Why do orbitals hybridize? • So they can point directly toward the terminal atoms • For example: p-orbitals (90° angles) are not pointing toward the hydrogen atoms in the tetrahedral CH 4 molecule. ± Hybridization is determined by the # of regions of electron density ² Determined for each “central” atom individually ² No. of regions of electron density = No. of orbitals that hybridize Regions Electron group arrangements
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This note was uploaded on 03/31/2008 for the course CHEM 1035 taught by Professor Jgdillard during the Fall '07 term at Virginia Tech.

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Chapter 11 notes - Chapter 11: Valence Bond Theory Lecture...

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