Lecture_23 - Today's Lecture Bonding: General Concepts...

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1 1 Bonding: General Concepts Today’s Lecture 13.13 Molecular Structure: The VSEPR Model Covalent Bonding: Orbitals 14.1 Hybridization and the Localized Electron Model 1 VSEPR Model - Complicated Molecules H C H methanol O H H 2
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2 2 ± recall that bonds between nonmetal atoms of different electronegativities are polar covalent bonds VSEPR and Molecular Polarity ± bond polarity is different than molecular polarity! ± to determine if a molecule is polar in the absence of measured dipole moments one must consider the individual bond polarities and molecular geometry ± a molecule with only nonpolar bonds will be a nonpolar 3 molecule ± however, a molecule with polar bonds is not necessarily a polar molecule (i.e. it may be nonpolar) CH 4 (Methane) ± the individual C-H bonds in CH 4 are slightly polar ± but the individual bond dipoles all cancel out and hence CH 4 is a nonpolar molecule ± for a tetrahedral molecule with four 4 identical bonds, the molecule is nonpolar (i.e. no net dipole moment)
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3 3 Determining Molecular Polarity ± to determine whether a molecule is polar or nonpolar: ± determine the Lewis structure ± determine the geometry using VSEPR theory ± take the vector sum of the individual bond dipole moments to determine if there is any net molecular dipole moment e g determine if the SF molecule has a net dipole 5 ± e.g. determine if the SF 4 moment Valence Bond Theory (VBT) ±
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This note was uploaded on 06/27/2009 for the course CHEM CHEM 121 taught by Professor Peggy during the Spring '09 term at Simon Fraser.

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Lecture_23 - Today's Lecture Bonding: General Concepts...

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