Objectives: To meet the requirements of Goal I, you must be able to:

1. describe and compare:
• the volume-shape characteristics and relative densities of solids, liquids and gases;
• amorphous and crystalline solids;
• the relative compressibilities of solids, liquids and gases.

Objectives: To meet the requirements of Goal II, you must be able to:

2. distinguish between intermolecular attractions and intramolecular attractions (chemical bonds).

3. compare the relative strengths of inter- and intra-molecular forces in terms of the energies necessary to overcome these forces.

4. distinguish between ion-ion attractions and dipole-dipole interactions.

5. explain the origin of dipole-dipole forces and recognize, from chemical formulas and a knowledge of molecular geometry,  compounds in which dipole-dipole forces exist between constituent molecules.

6. identify from chemical formula compounds in which dipole-dipole forces called hydrogen bonds exist between constituent molecules.

7. explain the origin of London dispersion forces and recognize from chemical formula those substances (compounds or elements) in which only London forces exist between constituent molecules (compounds) or atoms (elements). Understand "polarizability" and predict trends in "polarizability" across a period and down a group.

8. compare the relative strengths of intermolecular London dispersion attractions between molecules of different compounds based on:
• molecular shape (geometry);
• size (volume occupied);
• mass.

9. compare the relative importance of dipole-dipole and London dispersion attractions.
   
10. describe the properties of viscosity, surface tension and capillary action and relate these properties to intermolecular attractions between molecules and to temperature.

Objectives: To meet the requirements of Goal III, you must be able to:

11. explain the process of evaporation in terms of the kinetic-molecular theory.
    
12. describe the state of dynamic equilibrium established between a liquid and its vapor confined to a closed container.
    
13. explain the effect of temperature changes on an established liquid-vapor equilibrium in terms of:

• the rates of condensation and vaporization;
• the number of particles in the liquid and in the vapor states;
• a shifting of equilibrium.
14. define equilibrium vapor pressure of a liquid and describe its dependence on:
• intermolecular attractions between the liquid's constituent particles;
• temperature of the system; understand and use the Clausius Clapeyron Equation to understand the relationship between temperature, vapor pressure and the heat of vaporization
• amount of liquid present.
15. define normal boiling point and predict relative normal boiling points of different liquids based on a knowledge of the existing intermolecular attractions in the liquids.
    
16. explain the effect of external pressure on the actual boiling point of a liquid.
    
17. define normal melting point and contrast this to the freezing point of a substance.
    
18. describe the roles of energy and entropy in the equilibrium established between a liquid and its melt at the freezing point.
    
19. interpret a heating or cooling curve by:

• defining the terms used to describe the thermal energies involved for each region of the curve;
• explaining the slope of the curve and the phases present within each region;
• calculating energy involved in melting, freezing, boiling, condensing or heating a given mass of substance.
  
20. interpret a phase diagram by:
• defining the terms: supercritical fluid, critical point, triple point, critical temperature, critical pressure, sublimation, deposition;
• relating the slope of the liquid-solid equilibrium line to the relative densities of the liquid and solid phases;
• predicting the stable phase or phases in equilibrium at a given temperature-pressure.

Objectives: To meet the requirements of Goal IV, you must be able to:

21. distinguish among and give example of atomic, molecular, ionic, covalent network and metallic crystals on the basis of:
• constituent particles (units);
• forces between units;
• properties.
  
22. describe the simple cubic, face-centered cubic, and body-centered cubic packing arrangements.
    
23. define conductor, semiconductor, superconductor and insulator (non-conductor). Understand the effect of temperature on the conductivity of conductors, semiconductors, superconductors. Understand the Molecular Orbital Bend Theory, and explain the difference in electrical conductivity of conductors, semiconductors, superconductors, and insulators. Distinguish between n-type and p-type semiconductors.