chm115_lecture17 - Chemistry 115 Lecture 17 Outline Chapter...

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Chemistry 115 Lecture 17 Outline Chapter 8 VSEPR – molecular shapes EXAM: THURS MARCH 10, 8:00 Elliot Hall of Music Recitation: Electronegativity VSEPR, molecular shapes Molecular polarity
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Valence Shell Electron Pair Repulsion Theory VSEPR Decide shape by choosing forms that minimize energies of repulsion These forms depend on the number of bonds and lone pairs attached to a central atom in a molecule: These are defined as the “Number of Electron Groups” Lewis Dots and bonds between atoms define the Chemical connectivity Lewis Dots also help define the Chemical shape In order to do that we will develop the Valence-Shell Electron Pair Repulsion (VSEPR) theory
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Valence Shell Electron-Pair Repulsion Theory VSEPR –explains why molecules take the shapes they do Why is shape important? Medicines, odors, tastes, depend on one (large) molecule recognizing the shape of another. Basic idea of VSEPR – electron groups try to get as far away from one another as possible. These groups are single, double triple bonds, lone pairs, and even lone electrons. VSEPR predicted shapes have been verified using infrared spectroscopy, x-ray scattering and other methods.
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VSEPR theory
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This note was uploaded on 04/09/2011 for the course CHM 115 taught by Professor Towns during the Spring '08 term at Purdue University-West Lafayette.

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chm115_lecture17 - Chemistry 115 Lecture 17 Outline Chapter...

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