UNIT 8: SOLIDS, LIQUIDS, AND GASES
THE FOREST: Gas particles move independently of each other and are far apart. The behavior of gas particles can be
modeled by the kinetic molecular theory. In liquids and solids, unlike gases, particles are close to each other.
THE TREES:
6.1 Using the kinetic molecular theory, explain the behavior of gases and the relationship between pressure and
volume (Boyle’s law), volume and temperature (Charles’s law), pressure and temperature (Gay-Lussac’s
law), and the number of particles in a gas sample (Avogadro’s hypothesis). Use the combined gas law to
determine changes in pressure, volume, and temperature.
 List and explain the basic assumptions of the kinetic molecular theory.
 Relate pressure to molecular motion.
 Relate temperature and energy transfer to molecular motion.
 Determine the relative velocities of gas molecules at the same temperature.
 Relate the laws of Boyle, Dalton, and Charles and perform calculations using these laws.
 Solve problems involving the change of more than one condition for gases.
 Explain Graham’s law and solve problems using it.
 State Avogadro’s principle.
6.2 Perform calculations using the ideal gas law. Understand the molar volume at 273 K and 1 atmosphere (STP).
 Explain the concept of an ideal gas.
 Differentiate between an ideal gas and a real gas.
 Describe the conditions of STP.
 Define molar volume.
 Explain and use the ideal gas equation.
 Compute the molar mass of a gas from its mass, temperature, pressure, and volume.
 Solve gas volume-mass, mass-gas volume and volume-volume problems.
 Identify the limiting reactant and be able to solve problems based upon it.
6.3 Using the kinetic molecular theory, describe and contrast the properties of gases, liquids, and solids.
 Describe characteristics of substances in each of the three common states of matter in terms of the kinetic
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molecular theory and intermolecular forces within the substances.
Describe characteristics of all solid substances.
Explain the relationship of melting point to bonding type and crystal type.
Explain the properties of liquids in terms of the kinetic molecular theory.
Explain the unique properties of water in terms of its molecular structure.
Explain surface tension and capillary rise on the basis of unbalanced surface forces.
IMPORTANT VOCABULARY
Absolute zero
adiabatic system
amorphous
anhydrous
Avogadro’s principle
barometer
Body-centered cubic
Face-centered cubic
Graham’s law
Hexagonal closest packing
Hydrated ion
Hydrogen bond
hygroscopic
Ideal gas
pascal
Phase diagram
plasma
Point mass
polymorphous
pressure
Real gas
Boyle’s law
Capillary rise
Charles’s law
Crystal
Cubic closest packing
Dalton’s law
Deliquescent
Diffusion
Dislocation
Doped
Dynamic equilibrium
Enthalpy of fusion
Enthalpy of vaporization
Equilibrium
Excess reactant
Ideal gas equation
isomorphous
Kelvin scale
Kinetic theory
Limiting reactant
Liquefaction
Liquid crystal
Macromolecule
Manometer
Mean free path
Melting point
Metastable
Molar volume
Network crystal
Normal boiling point
Reversible change
saturated
Simple cubic
Space lattice
Standard atmospheric press.
Standard temperature
STP
sublimation
Surface tension
Triple point
Unit cell
Vapor
viscosity
volatile
STUDY GUIDE
CONTENT:
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Assumptions of kinetic molecular theory
Define pressure in terms of particle motion
Define temperature in terms of particle motion
Define kinetic energy in terms of particle motion and temperature
STP
Avogadro’s principle
Direct v. inverse for Boyle, Charles, and Gay-Lussac
Ideal v. real gases
Molar volume
Properties unique to solids, liquids, and gases
Compare and contrast solids, liquids, and gases
Four major types of solids
MATH SKILLS:
 Convert pressures and temperatures to standard units
 Boyle’s law, Charles’s law and Gay-Lussac’s law
 Dalton’s law of partial pressures
 Combined Gas law
 Graham’s law of diffusion and effusion
 Ideal gas law
 Gas stoichiometry at STP and at non-STP