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Liquids and Solids

Liquids and Solids. Zumdahl, Ch. 10. Try to remember - KMT. Volume of the particle is negligible Particles are in constant random motion Particles exert no forces between each other. Intermolecular Forces (IMF). Also known as Van der Waals forces Dipole-Dipole Force Hydrogen Bonding

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Liquids and Solids

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  1. Liquids and Solids Zumdahl, Ch. 10

  2. Try to remember - KMT • Volume of the particle is negligible • Particles are in constant random motion • Particles exert no forces between each other

  3. Intermolecular Forces (IMF) • Also known as Van der Waals forces • Dipole-Dipole Force • Hydrogen Bonding • London Dispersion

  4. Intramolecular Forces • Also known as bonds • Ionic bond: 400 - 4000 kJ/mol • Covalent bond: 150 – 1000 kJ/mol • Intermolecular forces significantly less • Importance of Intermolecular Forces (IMF) • Freezing point and boiling point • Vapor pressure

  5. Dipole – Dipole Force • Polar molecules attract each other • 5 – 25 kJ/mol (decrease with distance)

  6. Hydrogen “Bonding” • Special case of dipole-dipole: 10-40 kJ/mol • H atom and N, O, F, (Cl) • Role in DNA structure • THE example: H2O

  7. London Dispersion Force • Any molecule with positive nuclei and negative electrons has LDF. • So, EVERYTHING HAS LDF! • 0.05 – 40 kJ/mol Why such a huge range? • As molar mass increases, LDF increases

  8. LDF = Atomic-Sized Dipole

  9. Summary of IMFs • London Dispersion • Typically weakest IMF • Dominates for large molecules • Dipole-Dipole Force • Found in polar molecules • Dominates as EN differences increase • Hydrogen Bonding • H and N, O, F, (Cl) • Typically the strongest IMF

  10. IMFs Impact on Liquids • As IMF increases, boiling point increases • As IMF increases, vapor pressure decreases • As IMF increases, surface tension increases • As IMF increase, viscosity increases • Capillary action

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