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Lecture1 - • Present between all molecules exclusively...

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Nature of Course Qualitative / Quantitative Macroscopic / Microscopic Concept / Memorize
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Solids, Liquids, Intermolecular Forces Reading: Chapter 10 HW: Page 487 # 25, 33, 38, 39, 93, 101
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Ionic Substance (Salts) Lattice of metal cations, nonmetal anions Held together by ionic bonds Lattice Energy = charge / radius
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Molecular Substance
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Vapor Pressure
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Boiling
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Heating Curve - Water
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Vapor Pressure Curve
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Phase Diagram - Water
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Types of Intermolecular Forces
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Strengths of Attraction Strong 1) Covalent Bond 2) Ionic Bond Weak 1) Hydrogen Bond 2) Dipole-Dipole Force 3) Dispersion Force
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London Dispersion Force Random asymmetries in electron distribution give rise to temporary dipoles Larger molecules, stronger LDFs
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Unformatted text preview: • Present between all molecules, exclusively between nonpolar molecules Dipole-Dipole Force • Present between polar molecules • Typically stronger than dispersion force, if similar size molecules Hydrogen Bond • Uniquely strong dipole-dipole attraction • H-F or H-O or H-N bond must be present for hydrogen bonding to occur Substances 1) CaCl 2 2) HBr 3) CH 3 OH 4) O 2 5) KCl 6) AlCl 3 7) CF 4 8) CH 3 NH 2 A. Label each substance as ionic or molecular. B. Which ionic substance has highest greatest lattice energy? C. Give IM force present in molecular substances. D. Which substance has lowest boiling point?...
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