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CHEM122 Chemistry II

Department of Science, Technology, Engineering & Mathematics: Chemistry

I. Course Number and Title

II. Number of Credits

4 credits

III. Number of Instructional Minutes

4500

IV. Prerequisites

CHEM121 (C or better)

Corequisites

None

V. Other Pertinent Information

Four-hour lecture and two-hour laboratory per week. Safety glasses or goggles required. Non-programmable, non-graphing scientific calculator required.

VI. Catalog Course Description

This lecture and laboratory course is a continuation of CHEM121. Topics include molecular shape, chemical reactions, properties of liquids and solids and changes of state, solutions, reaction kinetics, chemical equilibrium, thermodynamics, and electrochemistry. Equilibrium topics include gaseous reactions, the ionization of weak acids and bases, hydrolysis of salts, and buffers.

VII. Required Course Content and Direction

Chemistry II is a continuation of Chemistry I (CHEM121). Principles developed in Chemistry I are applied to specialized areas in Chemistry II. The concepts of stoichiometry, gases, and concentrations of solutions must be firmly grasped before advancing to Chemistry II. These topics are the foundation upon which the principles of acid-base behavior, equilibrium, kinetics, thermodynamics, and electrochemistry are developed. There is a direct relationship between the type of bonding in a compound and its behavior as an acid or base. A student, therefore, cannot succeed in Chemistry II unless he/she has mastered the generalized principles presented in Chemistry I.

As one of the Natural Sciences, chemistry has evolved out of careful observation and experimentation; as technology evolves, so does the body of chemical knowledge. This course will integrate important technological advances and their impact in the formulation of chemical principles and their applications. Furthermore, the laboratory component of the course will help to illustrate and apply some of these technological advances.

Chemistry II is a quantitative course. The topics covered are treated mathematically. Calculations involving the quadratic formula and logarithms are routine. Students must, therefore, be competent in the fundamental algebraic manipulations and have a working knowledge of the applications of logarithms. Laboratory work in Chemistry II is directly related to the lecture. Rather than merely demonstrating or proving the principles covered in class, the laboratory experiments are designed to show the students how the proper collection and treatment of data leads to an understanding of the detailed chemical behavior of specific systems. Students are, therefore, introduced to the investigative methods employed by working chemists.

Chemistry II is intended to prepare science majors for additional course work in organic, analytical, physical, and inorganic chemistry. Principles presented initially in Chemistry II, as well as in Chemistry I, will be expanded and treated in more precise mathematical terms in future courses. Thus, Chemistry II and Chemistry I serve as the fundamental courses in chemistry for science majors.

Course Learning Goals

Students will:
1. apply the basic laws and principles pertaining to stoichiometry, gases, and solution chemistry to electrochemical, kinetic, thermodynamic, and equilibrium calculations;
2. recognize the relationship between atomic and molecular structure and the behavior of compounds as acids and bases as described by the various acid-base theories, as well as the dependence of properties of liquids and solids on structure;
3. apply mathematical concepts and methods to chemical phenomena and to the solution of chemical problems;
4. define the basic vocabulary and notation of chemistry; and
5. demonstrate acquisition of basic laboratory skills as they pertain to: safety, management of both qualitative and quantitative work, ability to draw conclusions from experiments, and understand the importance of technological advances for the development of scientific knowledge.
Planned Sequence of Topics and/or Learning Activities

Course Outline:
1. BONDING
2. STATES OF MATTER: LIQUIDS AND SOLIDS
3. SOLUTIONS
4. CHEMICAL REACTIONS
5. KINETICS
6. CHEMICAL EQUILIBRIUM
7. ACID-BASE EQUILIBRIA
8. THERMODYNAMICS AND EQUILIBRIUM
9. ELECTROCHEMISTRY
Laboratory Experiments:
While specific laboratory experiments vary depending on the instructor and the semester, the following list is representative of the experiments that are used:
1. Safety Practices in the Chemistry Laboratory
2. Acid-Neutralizing Power of Antacids
3. Oxidation-Reduction Titration
4. Determination of Molecular Weight from Colligative Properties
5. Kinetics: Determination of a Rate Law and of the Activation Energy
6. Determination of an Equilibrium Constant
7. Determination of a Distribution Coefficient
8. Determination of the Dissociation Constant of a Weak Acid
9. Thermochemistry: The Heat of Reaction
10. Electrochemical Cells
Learning Activities:
Instruction aims to enable the student to:
1. discuss ionic and covalent bonds as related to periodicity and atomic structure;
2. understand molecular structure as a consequence of internal bond type, and the resultant properties of various types of liquids and solids and their relationship to changes of state;
3. use the bonding theory as it applies to concepts, such as nomenclature, formula writing, and acid and base properties;
4. describe the properties of solutions and the application of the mole concept to substances in solution;
5. write and balance oxidation-reduction equations;
6. predict the chemical changes occurring at the anode and cathode in electrolytic and voltaic cells;
7. perform calculations involving cell voltages at standard temperature and concentration conditions and at non-standard concentration conditions;
8. use cell voltages to predict the direction of spontaneous chemical change;
9. use calorimetric data to calculate the values of ΔH, ΔE, ΔS, and ΔG;
10. use standard thermodynamic variables to describe a chemical process as spontaneous or non-spontaneous;
11. use data collected in the laboratory to determine the equilibrium constant for a chemical system, and to derive the rate equation and energy of activation of a chemical reaction;
12. apply the principles of chemical equilibrium and acid-base concepts in the laboratory;
13. use equilibrium constants to calculate concentrations of reactants and products at equilibrium;
14. use appropriate reference books in the library related to the field of chemistry, such as the Handbook of Chemistry and the Handbook of Chemistry and Physics;
15. work as a member of a team in solving classroom problems and in the laboratory; and
16. use appropriate current technology in the laboratory to obtain data and understand the impact that this latest technology has on the field.
Assessment Methods for Course Learning Goals
Course learning goals are continuously assessed by: periodic written examinations, class exercises, laboratory preparation, laboratory results, laboratory reports, and assigned work.
Reference, Resource, or Learning Materials to be used by Student:
Students will use course approved text, laboratory modules and handouts, laboratory and demonstration equipment, library, science learning center, and computer programs. Please refer to the course syllabus for specific information.

Review/Approval Date - 2/99; Revised 6/08; New Core 8/2015

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