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Liquids, Solids, and Intermolecular Forces

Outline States of Matter van der Waals Forces Properties of Liquids Phase Changes Phase Diagrams Clausius-Clapeyron Equation Properties of Solids. Liquids, Solids, and Intermolecular Forces. Chapter 11. How do the properties of the three phases of matter compare?.

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Liquids, Solids, and Intermolecular Forces

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  1. Outline States of Matter van der Waals Forces Properties of Liquids Phase Changes Phase Diagrams Clausius-Clapeyron Equation Properties of Solids Liquids, Solids, and Intermolecular Forces Chapter 11

  2. How do the properties of the three phases of matter compare? • Fixed = keeps shape when placed in a container • Indefinite = takes the shape of the container Tro: Chemistry: A Molecular Approach, 2/e

  3. What are degrees of freedom?

  4. How do the densities and molar volumes of the three states of matter compare?

  5. How do the degrees of freedom between the three phases of matter compare?

  6. What is the distance between bonds versus intermolecular forces?

  7. What are dipole – dipole forces or polar - polar interactions?

  8. What are London forces Induced dipole – induced dipole or Nonpolar - Nonpolar interactions?

  9. How can electrons in a molecule move?

  10. How do neighboring molecules interact?

  11. Does molecular shape matter?

  12. Effect of Dispersion Force on Boiling Point of AlkanesBoiling point (°C) vs. Molar Mass (g/mol)

  13. Effect of Intermolecular Forces on Boiling PointBoiling Point (K) vs. Dipole Moment (D)

  14. What is a hydrogen bond?

  15. When will two liquids mix?

  16. Dichloromethane (methylene chloride) Water Ethanol (ethyl alcohol) What are the characteristics of polar solvents? Tro: Chemistry: A Molecular Approach, 2/e

  17. What are the characteristics of nonpolar solvents? Tro: Chemistry: A Molecular Approach, 2/e

  18. What is viscosity?

  19. What is surface tension? • tendency to minimize surface area

  20. Why are water droplets in orbit (Space Shuttle) spherical?

  21. How does capillary action draw a liquid up a tube?

  22. What causes the curve of the meniscus?

  23. How does the amount of vapor and liquid change?

  24. What is vapor pressure?

  25. Chapter 11: Examples – Clausius-Clapeyron Equation Dry ice sublimates at -78 ˚C and has a ΔHsub of 25.2 kJ/mol. Calculate the vapor pressure of carbon dioxide at -100 ˚C.

  26. Chapter 11: Examples – Clausius-Clapeyron Equation Calculate the boiling point of water at the summit of Pikes Peak, Colorado, if the atmospheric pressure is 447 torr and ΔHvap for water is 40.6 kJ/mol.

  27. What are phase transitions? Vaporization Liquid to gas transition Condensation Gas to liquid transition Melting Solid to liquid transition Freezing liquid to solid transition Sublimation Solid to gas transition Deposition Gas to solid transition

  28. Heats of Fusion and Vaporization Tro: Chemistry: A Molecular Approach, 2/e

  29. Heating Curve of Water Tro: Chemistry: A Molecular Approach, 2/e

  30. Chapter 11: Examples – Heating Curves A quantity of ice at 0 ˚C is added to 90.0 g of water at 80 ˚C. After the ice is melted the temperature of the water is 25 ˚C. How many grams of ice was added? Given that cice is 2.06 J/g · ˚C, cwater is 4.184 J/g · ˚C , the enthalpy of fusion of ice is 333 J/g.

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