Central Michigan University
College of Science and Technology
Master Course Syllabus
CHM 161H
I.
Principles of Chemistry
5(4-4)
Bulletin Description
Intensive introduction to chemical principles for the well-prepared, motivated student.
Satisfies University Program Group II laboratory requirements. Prerequisites: Algebra (1
unit), Chemistry (1 unit), or CHM 120; satisfactory Chemistry Placement Test score. (Group
II-B)
II.
Prerequisites
Algebra (1 unit), Chemistry (1 unit), or CHM 120; satisfactory Chemistry Placement Test
score.
III.
Rationale for Course Level
This is an introductory honors-level course in chemistry intended primarily for freshmen or
other beginning chemistry students. The prerequisites are high school algebra and chemistry,
or a lower-level college chemistry course. It is appropriate that this course be at the 100level.
IV.
Textbooks and Other Materials to be Furnished by the Student
1. Oxtoby, Gillis, and Nachtrieb "Principles of Modern Chemistry", 4th Ed., Saunders
College Publishing (1999)
2. Chemistry 161H Laboratory Manual, CMU Press, Current Edition
3. Pfeiffer, "Pocket Guide to Technical Writing", 2nd Ed., Prentice Hall (2001)
4. Approved safety goggles
5. Laboratory notebook (must have alternating carbonless sheets with detachable original)
6. Calculator (should do standard arithmetic and logarithmic calculations including
exponentials, ln, etc.) Non-programmable, non-graphing calculators only will be permitted at
quizzes and exams.
V.
Special Requirements of the Course
None
VI.
General Methodology Used in Conducting the Course
Classroom instruction (four periods per week) involves traditional lectures, problem solving, in-class
quizzes. Laboratory (one four-hour period per week) involves experimentation and data analysis.
VII.
Course Objectives
Upon completion of this course, the student will be able to:
1. Employ basic mathematics (algebra, logarithms, etc.) to solve chemical problems in each
of the areas covered.
2. Perform statistical analyses of experimental data, and distinguish between random and
systematic errors in experimental results.
3. Employ the Scientific Method to trace the development of ideas from hypothesis through
theory to scientific law.
4. Balance chemical equations and demonstrate a practical understanding of their
descriptive and quantitative usage.
5. Write proper Lewis dot diagrams for simple covalent molecules and predict their
geometries as well as polarities.
6. Use the gas laws to calculate and/or predict the behavior of ideal gases.
7. Explain the essential features of the kinetic-molecular theory and describe the different
properties of gases, liquids and solids at the molecular level.
8. Analyze the colligative properties of solutions (vapor pressure lowering, boiling point
elevation, freezing point depression, and osmotic pressure) both qualitatively and
quantitatively, especially as they are concerned with molecular weight determination.
9. Calculate the thermodynamic properties H, S, and G given adequate experimental
data; determine from knowledge of G whether a given reaction is possible; relate Go to
the equilibrium constant of a given reaction.
10. Derive mathematical expressions for the equilibrium constant for any chemical reaction;
use experimental data to calculate yields; and predict the effects of temperature, pressure,
and concentration on the position of equilibrium and the value of the equilibrium
constant.
11. Write expressions for the rate of a chemical reaction in terms of its concentrations of
reactants and products; determine the kinetic order of a chemical reaction from
experimental data; predict the effects of temperature, pressure, concentrations, catalysts,
and the energy of activation on reaction rates.
12. Predict the conditions of temperature, pressure and concentrations necessary to produce
the maximum yield of a chemical reaction in the minimum amount of time.
13. Describe the structure of the atom and specify the ground state electron configuration for
a given atom; use the laws of periodicity to predict the chemical reactivity of the
elements based on their position in the Periodic Table.
VIII.
Course Outline (Fifteen weeks of lecture and one week for final exam)
1. Introduction: matter: substances and mixtures; elements; laws of chemical combination;
atoms; periodic table; molecules; energy (One week)
2. Stoichiometry: empirical and molecular formulas; balanced equations; mass relationships
in chemical reactions; limiting reactant and percentage yield (One week)
3. Chemical bonding: electronegativity; ionic bonding; covalent bonds; Lewis diagrams;
polar covalent bonding; Shapes of molecules: VSEPR (One week)
4. Gases: chemistry of gases; pressure: Boyle's law; Charles' law; ideal gas law; chemical
calculations for gases; mixtures of gases; kinetic theory of gases; Graham's law of
effusion; real gases (One week)
5. Liquids and solids: bulk properties of liquid & solids; intermolecular forces; phase
equilibria, transitions, diagrams (One week)
6. Solutions: composition of solutions; nature of dissolved species; colligative properties;
colloids (One week)
7. Thermochemistry: systems, states and processes; energy, work and heat; heat capacity,
enthalpy and calorimetry (One week)
8. Thermodynamics: nature of spontaneous processes; entropy; Gibbs free energy changes
and chemical reactions (One week)
9. Equilibrium: nature of chemical equilibrium; thermodynamic description; equilibrium
calculations for gas phase reactions; magnitude of K and direction of change; Le
Chatelier's principle (One week)
10. Acids and bases: classification of acids and bases; Bronsted-Lowry scheme; acid and
base strength; equilibria; buffer solutions; acid-base titration curves (One week)
11. Solubility equilibria (One week)
12. Chemical kinetics: rates of chemical reactions; rate laws; integrated rate laws; reaction
mechanisms; reaction mechanisms and rate; effect of temperature on reaction rates;
catalysis (Two weeks)
13. Electronic structure: wave motion and light; energy quantization; Bohr model; waves,
particles, Schrodinger equation; hydrogen atom; many electron atoms and the periodic
table; experimental measures of orbital energies (Two weeks)
IX.
Evaluation
Exams count 60% and labs 40% toward overall grade. A passing grade (D-) requires that passing
scores be earned in both parts of the course. Exam average is based on three in-semester exams, the
average of all in-semester quizzes, and the final exam, all equally weighted. Lab average is based on
the percentage of the total available points earned on lab reports.
Overall (Exams & Laboratory)*
>87 = A; 77-87 = B; 67-77 = C; 57-67 = D; <57 = E
Exams
>86 = A; 76-86 = B; 66-76 = C; 56-66 = D; <56 = E
Laboratory
>90 = A; 80-90 = B; 70-80 = C; 60-70 = D; <60 = E
* Overall = (0.60 x Exams) + (0.40 x Laboratory). Pluses and minuses will be added to course
grades at the upper and lower ends of each range at the discretion of the instructor.
Note: Due to the small size of this course (~20 students) all in-semester quizzes and exams are in
objective format with questions requiring calculations and written answers. The quizzes and three insemester exams account for 4/5 of the exam score, or 48% of the overall grade. In addition, all
laboratory reports require calculations as well as discussion and interpretation of results. The writing
expected on lab reports is beyond the single-sentence (“short answer”) format typically associated
with exams. Given the 40% weighting of the lab portion of the course, combined with the amount of
calculation required on the examinations, it can be concluded that in excess of 50% of a student’s
grade in this course will result from a combination of meaningful writing and calculation.
X.
Bibliography
1. Atkins, Peter W. and Loretta Jones. Chemical Principles. New York: W. H. Freeman and
Company, 1999.
2. Munowitz, Michael. Principles of Chemistry. New York: W. W. Norton & Company,
2000.
3. Oxtoby, David W., H. P. Gillis and Norman H. Nachtrieb. Principles of Modern
Chemistry. Fort Worth: Saunders College Publishing, 1999.
4. Zumdahl, Steven S. Chemical Principles. Boston: Houghton Mifflin Company, 1998.
Syllabus prepared by:
Philip J. Squattrito _______________________
Name
_______________________________________
Signature
May 7, 2002_________________________
Date