CHEMISTRY is the study of matter and the changes it undergoes. Chemists are concerned with the composition, behavior, structure and properties of matter, as well as the processes that explain why and how chemical reactions work. Chemistry is often called "the central science" because the study of atoms connects all other disciplines of science.
Chemistry (Major Code 1905.00)
The Associate Degree in Chemistry will provide most lower-division requirements for the student planning to transfer to a four-year institution with a Chemistry major, while at the same time establishing a strong basic foundation in this science.
Students who wish to obtain an associate degree in Chemistry may do so by completing the course requirements listed below plus all other WLAC requirements for an associate degree. Transfer students should consult the Counseling Office for major preparation and general education requirements of the particular transfer institution of their choice. Transfer students who wish to also obtain an Associate Degree may do so by completing all WLAC general education requirements plus at least 18 units in the major as required by the transfer institution (a total of 60 units for an associate degree).
Associate in Arts Degree (45 units, Plan B)
CHEM 101 General Chemistry I (5 units)
CHEM 102 General Chemistry II (5 units)
CHEM 211 Organic Chemistry for Science Majors I (5 units)
CHEM 212 Organic Chemistry for Science Majors II (5 units)
MATH 261 Calculus 1 (5 units) -MATH 262 Calculus II (5 units)
MATH 263 Calculus III (5 units)
PHYSICS 37 Physics for Engineers and Scientists I (5 units)
PHYSICS 38 Physics for Engineers and Scientists II (5 units)
The following courses are offered in the current semester:
Introductory Chemistry (CHEM 51)
This is an introductory one-semester course in college chemistry. Topics covered include general, organic, and biological chemistry. Physical and chemical discoveries that provide some insight into the chemical sciences are presented. Basic atomic theory, nomenclature, molecular structure, chemical reactions and the behavior of gases are also some of the topics covered. The laboratory exercises for this course emphasize basic laboratory skills, fundamental chemical principles, and elementary qualitative and quantitative relationships in chemical analyses.
TEXTBOOK: K. C. Timberlake, An Introductory to General, Organic, and Biological Chemistry, 11th Edition, Prentice Hall, 2012.
STUDENT LEARNING OUTCOMES:
Upon successful completion of this course you will be able to demonstrate a firm understanding of:
measurements in both the English and Metric Systems
general, inorganic and introductory organic chemistry, including nomenclature and writing formulas and chemical equations
basic atomic theory and apply its principles to chemical reactions
reactions of acids/bases, redox, as well as reactions of gases, liquids, and solids in conjunction with one another
functional group categories that differentiate the various organic chemicals and the physical, chemical and physiological properties of each
General Chemistry (CHEM 102)
This course is the second course of a two-semester sequence and the topics covered for this course include: chemical kinetics, chemical equilibrium, the nature of acids and bases, applications of aqueous equilibria, chemical thermodynamics, electrochemistry, and nuclear chemistry. Other topics to be covered include: fundamentals of organic chemistry, coordination chemistry and the chemistry of Representative Elements --- Groups IA through IVA and Groups VA through VIIIA ---, as well as the chemistry of Transition metals.
PREREQUISITE: Successful completion of Chem. 101 with a grade of C or better within the last two years.
TEXTBOOK: Steven S. Zumdahl, and Susan A. Zumdahl, CHEMISTRY, Eighth Edition, Brooks Cole Cengage Learning, 2010.
Lab. Manual: J. A. Beran, Laboratory Manual for Principles of General Chemistry, Eighth Edition, John Wiley & Sons, Inc., 2009.
STUDENT LEARNING OUTCOMES:
Upon the successful completion of this course you will be able to demonstrate a firm understanding of:
(i) Le Systeme International d’Unites (SI Units) as well as the English System for scientific measurements;
(ii) exponential notations and significant digits in calculations involving both linear and nonlinear functions;
(iii) quadratic equations;
(iv) natural and common logarithmic functions, and
(v) graphing techniques for data analysis
the existence of an infinite set of concentrations of products and reactants that satisfy an equilibrium expression, irrespective of the type of equilibrium system studied:
(i) homogeneous equilibria,
(ii) heterogeneous equilibria,
(iii) acid-base equilibria,
(iv) solubility equilibria, or
(v) complex ion equilibria
the Henderson-Hasselbalch equation and its application in the determination and preparation of buffered solutions of desired pHs
the thermodynamic properties of chemical reactions in terms of change in Gibbs free energy and relate the signs (+/-) of delta H, delta S and delta G to the spontaneity of a process at different temperatures
the potential of an electrochemical cell dependence on the differences in energies of reactants and products; and that a cell may be constructed from two solutions of the same type of electrolyte at different concentrations
the process of electrolysis and its commercial uses
nuclear stability and the kinetics of radioactive decay
the chemistry of the representative elements
the fundamentals of coordination chemistry
the chemistry of hydrocarbons and hydrocarbon derivatives