Course Outline

First Term

1. Energy level diagrams
2. Atomic structure and the Periodic Table
3. Simple ions - anions and cations
4. Energy level diagrams for ions, and isoelectronic species
5. "Chemical Families" video
6. Alkali metals, Alkaline Earth metals, Halogens, Noble gases
7. Compounds
8. Covalent bonding
9. Binary molecular compounds
10. Molecular formulas
11. Ionic bonding
12. Binary ionic compounds
13. Empirical formulas and formula units
14. Stock and Classical systems
15. Complex (polyatomic ) ions
16. Ternary ionic compounds
17. Structure of ionic vs. molecular compounds
18. Hydrates
19. Acids (binary and oxo)
20. The mole (Avogadro's number)
21. Sig. figs.
22. Atomic molar mass, molar mass of a compound
23. Calculations using Avogadro's number
24. Mass to mole conversions
25. Mole to mass conversions
26. Percent composition
27. Percent composition lab
28. Calculating empirical formulas
29. Lab - The formula of a hydrate
30. Balancing chemical equations
31. Reaction types
32. Predicting products based on the reaction type
33. Using the solubility table to identify a precipitate
34. Lab - Chemical Reactions (predicting products, writing a complete balanced equation, using a solubility table to identify the precipitate)

Second Term

1. Mole Stoichiometry
2. Mass Stoichiometry
3. Mixed Stoichiometry
4. Percent Yields
5. Stoichiometry using limiting reagents
6. Aufbau Principle, Hund's Rule., Pauli Exclusion Principle
7. Electron configurations
8. Orbital diagrams
9. Valence electron configurations
10. Electron configurations and orbital diagrams for ions
11. Isoelectronic species
12. Covalent bonding
13. Lone pairs and bonding electrons
14. Single, double, and triple bonds
15. Lewis diagrams for atoms and ions
16. Lewis diagrams for molecules
17. Structural formulas
18. VSEPR theory and shape diagrams
19. Electronegativity
20. Polar and nonpolar covalent bonds
21. Polar and nonpolar molecules
22. Van der Waals forces
23. London Dispersion forces
24. Dipole-dipole forces
25. Hydrogen bonding
26. Boiling points as an expression of the strength of intermolecular forces
27. Metallic bonding
28. Ionic bonding
29. Network covalent bonding
30. The relative magnitude of intermolecular forces
31. Ranking compounds by their melting/boiling points

You are responsible for all ideas covered in class during this term. This includes all notes, text questions, labs, assignments, etc.