States of Matter and Phase Changes

Viscosity

Resistance of liquid to flow. Higher the IMF, higher the viscosity

Capillary action

Ability to flow against gravity up a narrow tube. Greater IMF, greater capillary action

Vaporization

Increases with increase in temperature and surface area and decreasing strength of IMF. Volatile: vaporize easily. Nonvolatile: does not vaporize easily.

Heat of vaporizations

Heat required to vaporize one mole of liquid to gas. Energy is required to break IMF, ideally no IMF between gas particles

Vapor pressure

When molecules enter the gas phase they exert pressure. Depends on temperature and on rate of evaporation per unit area of liquid surface. Higher IMF, less vapor pressure

Dynamic equilibrium

In a closed container, rate of vaporization = rate of condensation. If the system is disturbed, it will shift to minimize disturbance and return to equilibrium

Heat fusion

The heat absorbed as one mole of solid liquifies. Energy is required. Melting is endothermic.

Phase diagram

Phase of a substance is a function of pressure and temp

Triple point

The unique set at which the 3 states are equally stable and in equilibrium

Critical point

Critical temp and pressure the liquid and gas states coexist into a supercritical fluid