Chapter 8: Gases, Liquids, and Solids Flashcards
change of state
the change of a substance from one state to another
melting point
the temperature at which solid and liquid are in equilibrium
boiling point
the temperature at which liquid and gas are in equilibrium
sublimation
straight from solid to gas
deposition
straight from gas to solid
Intermolecular Forces (IMFs)
forces that act between molecules and hold molecules close to one another
dipole-dipole force
the attractive force between positive and negative ends of polar molecules
london dispersion force
the short lived attractive force due to the constant motion of electrons within molecules
hydrogen bond
the attraction between a hydrogen atom bonded to an electronegative O, N, or F atom and another nearby electronegative O, N, or F atom
kinetic-molecular theory of gases
a group of assumptions that explain the behavior of gases:
a gas consists of many particles moving about at random with no attractive forces between them
amount of space occupied by gas particles is less than the amount of space between particles
the average kinetic energy of gas particles is proportional to the temperature
collisions of gas particles are elastic - the total kinetic energy of the particles is constant
ideal gas
a gas that obeys all the assumptions of the kinetic-molecular theory
pressure
the force per unit area pushing against a surface
gas law
a series of laws that predict the influence of pressure, temperature, or volume on any gas (mixture)
Boyle’s Law
PV=PV
Charles’ Law
V/T=V/T
