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AP Chemistry Course Syllabus

1. Evidence for atomic theory
2. Atomic masses and how to determine them experimentally
3. Atomic number and mass number; isotopes
4. Electron energy levels: atomic spectra, quantum numbers, and atomic orbital
5. Periodic trends (atomic radii, ionization energies, electron affinities, oxidation states)

• Types: ionic, covalent metallic, hydrogen bonding, van der Walls (London dispersion forces)
• Relationships to states, structure, and properties of matter
• Polarity, electrons, negativity

• Lewis structures
• Valence electrons, hybridization of orbitals, resonance, sigma and pi bonds
• VSEPR

1. Ideal gas laws

• Equation of state for an ideal gas
• Partial pressures, Dalton’s Law

2. Kinetic molecular theory

• Interpretation of ideal gas laws on the basis of this theory
• Avogadro’s hypothesis and the mole concept
• Dependence of kinetic energy of molecules on temperature, Graham’s law
• Deviation from ideal gas laws

1. Liquids and solids and kinetic molecular theory

2. Phase diagrams

3. Changes of state, including critical points and triple points

4. Structure of solids; lattice energies

1. Types of solutions and factors affecting solubility

2. Molarity, molality, mole fraction and density

3. Raoult’s law, colligate properties, osmosis

4. Non-ideal behavior

Members:

• Usha Bhatnagar
• Don Broderson
• Charles Davenport
• Susann Evans
• Maria Farrell
• Paul Korc
• Angela Montez
• Stephen Nash
• Stacy Strausborger
• Ethell Wilson

Departmental Chairperson:

Don Broderson

Departmental Meetings: Every third Wednesday of the month at 1:15 p.m. or 1:30 p.m. as determined by the departmental members.