GC2 Intermolecular Forces and Properties of Liquids Quiz

Phase Diagram

• The temperature of a boiling liquid remains constant because the added heat is used to convert the liquid into vapor.
• The temperature above which a gas can no longer be liquefied is called the critical point.
• The critical temperature and pressure of water are 374℃ and 218 atm, respectively.

Phase Diagram - CO2

• At a temperature of -56.4℃, CO2 is in its liquid state.
• The critical point of CO2 is 31.1℃ and 73 atm.

Solutions

• A solution can contain a single solvent and one or more solutes.
• Unsaturated solutions are those that can dissolve more solutes.
• Supersaturated solutions contain more dissolved solutes than what is typically possible at a given temperature.
• Saturated solutions are those that cannot dissolve any more solutes.

Intermolecular Forces of Attraction

• The possible IMF of a compound depend on the type of molecules involved:
  • Compounds containing only C and H exhibit London dispersion forces (LDF).
  • Compounds containing H and F, O, or N exhibit hydrogen bonding (H-bond), LDF, and dipole-dipole forces (D-D).
  • Noble gases exhibit LDF.
  • Diatomic elements such as I2, F2, Cl2 exhibit LDF.
  • Polar compounds exhibit D-D and LDF.
  • Nonpolar compounds exhibit LDF.

Properties of Liquids

• The cohesive force of water creates surface tension, causing it to form a spherical droplet shape.
• Vapor pressure is the characteristic of a liquid that is a function of its temperature.
• When a liquid vaporizes in a closed container, the space above the liquid becomes saturated with vapor, and an equilibrium exists between the liquid and the vapor.
• The relationship between vapor pressure and boiling point is inversely proportional.
• Rubbing alcohol feels cold when applied to the skin due to evaporative cooling.
• The temperature of a boiling liquid remains constant even when heat is continuously added because the added heat is used to convert the liquid into vapor.