After successful completion of this course, a student will be able to:
1. Use dimensional analysis and stoichiometry to solve quantitative chemical problems.
2. Apply atomic theory in describing matter, including chemical nomenclature and physical and chemical processes.
3. Summarize the quantum mechanical structure of the hydrogen atom in light of its emission spectrum, and apply it to many-electron systems.
4. Calculate energy changes in calorimetry and chemical reactions.
5. Use the periodic table of elements to recognize trends and patterns, and to perform calculations.
6. Describe the bonding and shapes of simple compounds with a range of models.
7. Apply kinetic-molecular theory to the behavior of ideal and real gases.
8. Relate intermolecular forces to the physical properties of matter.
9. Calculate the effects of solute concentration on the physical properties of solutions.
10. Use appropriate techniques to obtain accurate and precise measurements in the laboratory.
11. Identify the uncertainty and analyze experimental error associated with measurements.
12. Graph (as appropriate), interpret, and communicate the results of laboratory experiments in writing.
13. Apply chemical principles to real world situations.
I. Basic Tools and Problem Solving
A. Metric system and units
B. Dimensional analysis and conversions
C. Significant figures
A. Moles and molar mass
B. Mass calculations
C. Limiting reactants and yields
D. Molarity and solution stoichiometry
E. Gas stoichiometry
F. Energy calculations
III. Atomic theory
A. States of matter
B. Nomenclature of simple compounds
C. Chemical composition
1. Mass percent
2. Empirical formulas
3. Molecular formulas
D. Chemical reactions
IV. Structure of the atom
A. Light and the electromagnetic spectrum
B. Emission spectra
C. Bohr model of hydrogen
D. Quantum mechanical model of the atom
E. Quantum numbers
F. Writing electron configurations
B. Pressure-Volume (PV) work
C. Energy vs. enthalpy
D. Hess's law
E. Enthalpies of formation
F. Reaction enthalpies
G. Bond energies and reaction enthalpies
VI. Periodic trends
A. Atomic size
B. Ionization energy
D. Ionic radius
VII. Bonding and Molecular Structure
A. Ionic bonding
B. Born-Haber cycle
C. Lewis structures
D. Valence Shell Electron Pair Repulsion (VSEPR) Theory
E. Covalent bond order, polarity, energy and length
F. Hybridization of atomic orbitals
G. Valence Bond (VB) theory
H. Molecular Orbital (MO) theory
VIII. Kinetic Molecular Theory of Gases
A. Molecular scale understanding of gas pressure and temperature
B. Development and applications of the ideal gas law
C. Dalton's law of partial pressures
D. Graham's law of effusion and diffusion
E. Approximating real gases with the van Der Waals equation
IX. Intermolecular Forces (IMF)
A. Molecular polarity
B. Types of intermolecular forces
C. Physical properties and IMF
D. Phases and phase diagrams
X. Liquids and Solids
XI. Colligative Properties
A. Vapor pressure lowering
B. Freezing point depression
C. Boiling point elevation
Laboratory material may include:
1. Lab safety and maintaining a lab notebook
3. Synthesis and limiting reactants
4. Formula of a compound
5. Gas laws
7. Hydrogen emission spectrum
8. Lewis structures and molecular geometry
9. Determination of an unknown
10. Techniques and skills
a. Determining mass using a balance
c. Using volumetric glassware to prepare solutions
d. Using spreadsheet software to graph data and do calculations
e. Writing laboratory reports
f. Visible light spectroscopy
Chemistry: The Molecular Nature of Matter and Change, 6th Ed., Silberberg, M. (McGraw-Hill, 2011)
Chemistry, 11th Ed., Chang, R. and Goldsby, K. (McGraw-Hill, 2012)
General Chemistry 4th Ed., McQuarrie, D., Rock, P. and Gallogly, E. (University Science Books, 2010)
Chemistry: The Science in Context, 3rd Ed., Gilbert, T., Kirss, R., Foster, N., Davies, G. (Norton, 2011)
Chemistry: A Molecular Approach, 2nd Ed., Tro, N. (Prentice Hall, 2010)