UNIT VII: KINETIC THEORY AND LIQUIDS
(Chapters 15 and 17)

The student will:
1) explain kinetic theory in relation to temperature, energy, and molecular motion.
2) will apply these principles as well as intermolecular forces to liquids and changes of state.
3) will analyze systems in equilibrium in relation to Le Chatliers principle.

Curricular Objectives:

· List and explain the basic assumptions of kinetic theory
· Relate pressure to molecular motion
· Use models to illustrate the effects of changes in temperature and volume upon pressure
· Differentiate among an open-arm manometer, a closed-arm manometer, and a barometer
· Calculate the pressure of gases in both open-arm and closed-arm manometers using appropriate units
· Relate temperature and energy transfer to molecular motion
· Make conversions between temperature scales
· Define plasma (level I)
· Explain the properties of liquids and changes of state in terms of the kinetic theory
· Explain vapor equilibrium and dynamic equilibrium in a closed system
· Use Le Chatliers principle to explain reversible changes of state in a closed system
· Give examples of closed systems in equilibrium as illustrations of Le Chatliers principle
· Determine the relationship between energy and change of state
· Apply intermolecular forces to volatility of liquids
· Define and calculate enthalpy of fusion and enthalpy of vaporization
· Use polarity to explain hydrogen bonding
· Explain the unique properties of water in terms of its molecular structure
· Analyze amino acids in terms of hydrogen bonding (level I)
· Explain surface tension and capillary rise on the basis of unbalanced surface forces
Suggested Laboratory Investigations:

· Too Much in an Elevator Minute Lab
· Changes of State in a Vacuum Chamber
· Changing of Equilibrium - Le Chatliers Principle
· How many drops fit on the head of a penny?
· Lab on freezing point (water or other)
· Heat of fusion (water, wax, etc)

UNIT VIII: GAS LAWS AND STOICHIOMETRY
(Chapters 18 and 19)

At the conclusion of this unit, the student will be able to explain and use the gas laws. The student will be able to perform more types of stoichiometry calculations and identify a limiting reactant.
Curricular Objectives: At the completion of this unit, the student will be able to:

· Explain the concept of an ideal gas, defining it in terms of mass, volume, and molecular attraction
· Describe the conditions of STP
· Explain Boyles law in conceptual and mathematical terms and apply the law in performing calculations
· Explain Daltons law of partial pressures in conceptual and mathematical terms and apply the law in performing calculations
· Explain Charles law in conceptual and mathematical terms and apply the law in performing calculations
· Solve problems involving Daltons law of partial pressures (gases collected over water) in combination with Boyles law (level I)
· Explain the combined gas law in conceptual and mathematical terms and apply the law in performing calculations
· Explain Grahams law in conceptual and mathematical terms and apply the law in performing calculations (level I should recognize the association with the kinetic energy equation)
· Explain the deviations of a real gas from an ideal gas (level I)
· Define molar volume and explain the relationship to Avogadros principle
· Explain the ideal gas equation in conceptual and mathematical terms and apply the equation in performing calculations
· From the ideal gas equation, derive other equations to find mass or molecular mass and apply this equation in performing calculations (level I)
· Solve gas volume-mass, mass-gas volume, and volume-volume stoichiometry problems (level I should be able to solve starting with a word problem)
· Identify the limiting reactant and solve problems based upon it

Suggested Laboratory Investigations:

· Grahams Law of Diffusion of Gases
· Molar Volume in a Bag
· Determine molar volume of a gas