CHEM 1040 Chapter 7.3
CHEM 1040 Chapter 7.3 CHEM 1040
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This 2 page Class Notes was uploaded by Hannah B. on Saturday January 30, 2016. The Class Notes belongs to CHEM 1040 at Auburn University taught by Ria Astrid Yngard in Winter 2016. Since its upload, it has received 62 views. For similar materials see Fundamental Chemistry II in Chemistry at Auburn University.
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Date Created: 01/30/16
Chapter 7.3 Intermolecular Forces: attractive forces between neighboring molecules -> London Dispersion, Dipole-Dipole, Hydrogen Bonding, and Ion-Dipole Van der Waals: attractive forces that act between atoms of molecules in a pure substance -> London Dispersion, Dipole-Dipole, Hydrogen Bonding London Dispersion Forces: coulombic attractions between instantaneous dipoles of molecules that is present in all molecules. larger molecule -> more polarizable -> stronger london dispersion force stronger force -> more attached -> higher boiling point Dipole-Dipole interactions: attraction between the partially positive end of one molecule and the partially negative end of another molecule larger dipole -> larger attractive force Hydrogen Bonding: a type of dipole-dipole interaction with attraction between a hydrogen atom attached to a highly electronegative atom (F, O, or N) and a nonbonding electron pair Ion-Dipole interactions: coulombic attractions between ions (positive or negative) and polar molecules mostly in equal solutions of high electrolytes IMF's in Order of Increasing Strength: london dispersion -> dipole-dipole -> hydrogen -> ion- dipole Practice Problem: Arrange BaCl2, H2, CO, HF, and Ne in order of increasing boiling point. Answer: H2, Ne, CO, HF, BaCl2
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