1. Use dimensional analysis and stoichiometry to solve quantitative chemical problems.
2. Apply atomic theory in describing the physical and chemical properties of matter.
3. Summarize the quantum mechanical structure of the hydrogen atom in light of its emission spectrum, and apply it to many-electron systems.
4. Apply kinetic-molecular theory to the behavior of ideal and real gases.
5. Calculate energy changes in calorimetry and chemical reactions.
6. Relate an understanding of changes in entropy and free energy to the spontaneity of physical and chemical processes.
7. Describe the bonding and shapes of simple compounds and ions with a range of models.
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 analytical measurements in the laboratory.
11. Use advanced instrumentation, such as UV-Visible and infrared (IR) spectroscopy, gas chromatography (GC) and atomic absorption (AA) in analysis of unknowns.
12. Analyze experimental error qualitatively and with statistical methods.
13. Graph (as appropriate), interpret, and communicate the results of laboratory experiments in writing.
14. Apply chemical principles to real world situations.
A. Metric system and units
B. Dimensional analysis and conversions
C. Significant figures
D. Atomic theory
E. Nomenclature of binary ionic and covalent compounds
F. Chemical composition
G. Basic chemical reactions
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. Structure of the atom
A. Light and the electromagnetic spectrum
B. Wave and particle properties of light
C. Emission spectra
D. Bohr model of hydrogen
E. Quantum mechanical model of the atom
F. Quantum numbers
G. Writing electron configurations
A. Calorimetry and the first law of thermodynamics
B. Pressure-Volume (PV) work
C. Energy vs. enthalpy
D. Hess's law
E. Reaction enthalpies
G. Entropy and the second law of thermodynamics
H. Spontaneity and Gibbs free energy
V. Periodic trends
A. Atomic size
B. Ionization energy
D. Ionic radius
VI. 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. Bond energies and reaction enthalpies
G. Hybridization of atomic orbitals
H. Valence Bond (VB) theory
I. Molecular Orbital (MO) theory
VII. Kinetic Molecular Theory of Gases
A. Molecular scale understanding of gas pressure and temperature
B. Heat capacity of gases
C. Development and applications of the ideal gas law
D. Dalton's law of partial pressures
E. Graham's law of effusion and diffusion
F. Approximating real gases with the van Der Waals equation
VIII. Intermolecular Forces (IMF)
A. Molecular polarity
B. Types of intermolecular forces
C. Physical properties and IMF
D. Phases and phase diagrams
IX. Liquids and Solids
X. Colligative Properties
A. Using molality and mole fraction to measure solution concentration
B. Vapor pressure lowering
C. Freezing point depression
D. Boiling point elevation
1. Lab safety and maintaining a lab notebook
3. Gravimetric analysis
4. Determining a stoichiometric ratio
5. Synthesis and limiting reactants
6. Determining the formula of a compound
7. Gas laws
9. Hydrogen emission spectrum
10. Determination of an unknown
12. Instrumental analysis
a. Ultraviolet-Visible spectroscopy
b. Infrared (IR) spectroscopy
c. Atomic absorption (AA)
d. Gas chromatography (GC)
e. Mass spectrometry (MS)
13. Techniques and skills
a. Determining mass using a balance
b. Use of a buret
c. Using volumetric glassware to prepare solutions
d. Using spreadsheet software to graph data and perform calculations
e. Writing laboratory reports
Chemical Principles, 7th Ed., Zumdahl and DeCoste (Cengage, 2013).
Chemical Principles: The Quest for Insight, 6th Ed., Atkins and Jones (Freeman, 2012).
General Chemistry: Principles and Modern Applications, 10th Ed., Petrucci, Herring, Madura, Bissonnette (Pearson, 2010).
Chemistry: The Molecular Nature of Matter and Change, 6th Ed, Silberberg (McGraw-Hill, 2011).
Principles of Modern Chemistry, 7th Ed., Oxtoby, Gillis and Campion, (Cengage, 2011).
Instructor Prepared Materials
Laboratory Experiments for Chemistry: The Central Science, 12th Ed., Brown, Nelson, Kemp and Stoltzfus (Pearson, 2011).
Quantitative Chemical Analysis, 8th Ed., Daniel Harris, (Freeman, 2010).
Fundamentals of Analytical Chemistry, 9th Ed., Skoog, West, Holler and Crouch (Cengage, 2013).