Chapter 10 PPt. 2

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Author:
DesLee26
ID:
196959
Filename:
Chapter 10 PPt. 2
Updated:
2013-01-31 17:55:44
Tags:
CHM 112
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Description:
Liquids, Gases, and Phase Changes
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  1. Characteristics and strength of:
    ion-dipole
    • moderate
    • occurs between ions and polar solvents
  2. Characteristics and strength of:
    dipole-dipole
    • weak
    • occurs between polar molecules
  3. Characteristics and strength of:
    london dispersion
    • weak
    • occurs between all molecules; strenght depends on size, polarizability
  4. Characteristics and strength of:
    hydrogen bond
    • moderate
    • occurs between molecules with O-H, N-H, and F-H
  5. Why don't the boiling points of NH3, H2O, and HF not follow the trend of increasing boiling points with increasing molecular mass down a gorup of hte periodic table
    due to Hydrogen bonds the boiling point has to be higher to break the bonds
  6. What us surface tension and why does it occur?
    • resistance of a liquid to spread out and increase its surface area
    • due to tighter attraction at the surface
  7. Viscosity
    Relationship with temperature
    • measure of a liquid's resistance to flow
    • Increase temperature, decrease viscosity
  8. What's one common way of getting from ne phase to another?
    temperature change: breaking weak interactiosn; adding kinetic energy to additional molecules
  9. What is enthalpy?
    Temp adn entropy relationship
    • heat content of materials
    • increase temp, increase entropy
  10. Solid to a liquid
    fusion (melting)
  11. What does frost resemble?
    a crystalline appearance
  12. Phase changes
    a change in physical form but not the chemical identity of a substance
  13. liquid to gas
    vaporization
  14. gas to liquid
    condensation
  15. liquid to solid
    freezing
  16. solid to gas
    sublimation
  17. Molar Heat of Fusion
    energy required to melt one mole of a solid in kJ
  18. Molar Heat of Vaporization
    the energy required to vaporize one mole of liquid

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