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  1. Intermolecular forces
    Between molecules/ atoms /ions
  2. Intramolcular forces
    between atoms themselves
  3. Intermolcular focres (types)
    • Dispersion
    • Dipole-dipole
    • hydrogen bonding
  4. Dispersion increases with..
    molar mass
  5. Dipoledipole occurs in
    polar molecules
  6. Hydrogen bonding (super dipole) occurs when
    hydrogen atoms bonded directly (intra-molecularly) to fluorine, oxygen, or nitrogen
  7. Most electronegative element is
  8. List forces from strongest to weakest
    (intra) 1 Ionic 2 covalent (inter) 3 hydrogen 4 dipole-dipole 5 dispersion
  9. intermolecular forces are directly related to
    surface tension and viscosity
  10. The ability to mix without separating into two phases is called
  11. Miscibility-what mixes with what?
    • Polar with polar, nonpolar with nonpolar
    • like dissolves like
  12. Viscosity
    is the resistance of a liquid to flow.

    Liquids that are viscous flow more slowly than liquids that are not viscous.
  13. Strongest intermolecular forces to weakest:
    solids > liquids > gases
  14. Vapor pressure
    pressure existing from transition from liquid to gas
  15. Dynamic equilbrium
    reached over time with stoped solution of fluxuating between gas and liquid constantly
  16. solid - gas
  17. gas to solid
  18. Liquids that evaporate easily are termed
  19. Liquids that do not vaporize easily
    are termed
  20. The rate of vaporization increases with
    • •Increasing surface area
    • • Increasing temperature;
    • •Decreasing strength of intermolecular forces
  21. Heat of fusion
    The amount of heat required to melt 1 mol of a solid
  22. The heat of fusion for water is
    6.02 kJ/mol
  23. During boiling, the temperature remains
    at 100°C until
    all the liquid is evaporated.
  24. The amount of heat required to vaporize one mole of liquid is
    the heat of vaporization (ΔHvap).
  25. The heat of vaporization of water at its normal boiling point (100 °C) is
    40.7 kJ/mol
  26. Melting and boiling points will be higher for substances that
    have stronger inter/intra forces
  27. Electrolyte solutions contain
    • dissolved ions (charged
    • particles) and therefore conduct electricity.
  28. Nonelectrolyte solutions contain
    dissolved molecules (neutral particles) and so do not conduct electricity.
  29. Henry’s law:
    The higher the pressure of a gas above a liquid, the more soluble the gas is in the liquid.
  30. Pressure
    The solubility of gases in water
    • increases with increasing pressure above the
    • liquid
  31. Molarity
    • moles solute / liter
    • of solution
    M1V1 = M2V2
  33. The Arrhenius Definition of Acids
    An acid produces H+ ions in aqueous solution
  34. The Arrhenius Definition of Bases
    • A base produces OH− ions
    • in aqueous solution.
  35. The brønsted-Lowery Definition of Acids and Bases
    acid is H donor, base is H acceptor
  36. amphoteric substances
    can act as either an acid or a base
  37. Do i need to know leuis base?
  38. Strong acids
    • hydrochloric acid (HCl)
    • hydrobromic acid (HBr)
    • Hydroiodic acid (HI)
    • Nitric acid (HNO3)
    • Perchloric acid (HCLO4)
    • Sulfuric acid (H2SO4)
  39. Strong Bases
    • lithium hydroxide (LiOH)
    • sodium hydroxide (NaOH)
    • potassium hydroxide (KOH)
    • strontium hydroxide (SrOH)2)
    • Calcium hydroxide (CA(OH)2)
    • barium hydroxide (Ba(OH)2)
  40. Titration is a technique that uses reaction stoichiometry to determine the concentration of an unknown solution.
    is a technique that uses reaction stoichiometry to determine the concentration of an unknown solution.
  41. pF formulas
    • pH= -log[x]
    • H3O= 1x10^-14
  42. Hydronium Ion Concentration

Card Set Information

2011-12-07 15:47:55
Chem 1050

Last test for chem 1050
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