Course Syllabus

Karey Marshall [email protected]

I. GENERAL COURSE

INFORMATION

Course Number: CHEM 1808 Course Title: College Chemistry II Credit Hours: 5 credit hours Prerequisite: 1806 College Chemistry I with a grade of C or better Division/Discipline: Academic Division-Liberal Arts and Sciences/ Chemistry Course Description: This course stresses the conceptual and mathematical approach to understanding general chemistry and prepares the student to follow a science oriented four- year program. It provides students with the necessary tools to handle problems of both a theoretical and practical nature. The students taking this course are usually declared Chemistry, Physics, Engineering, Pre-Med, etc., majors. This course is a continuation of College Chemistry I.

II. CLASSROOM POLICY

Students and faculty of Barton County Community College constitute a special community engaged in the process of education. The college assumes that its students and faculty will demonstrate a code of personal honor that is based upon courtesy, integrity, common sense, and respect for others both within and outside the classroom. The College reserves the right to suspend a student for conduct that is detrimental to the College’s educational endeavors as outlined in the College Catalog. Plagiarism on any academic endeavors at Barton County Community College will not be tolerated. Learn the rules of, and avoid instances of, intentional or unintentional plagiarism. Anyone seeking an accommodation under provisions of the Americans with Disabilities Act should notify Student Support Services.

III. COURSE AS VIEWED IN THE

TOTAL CURRICULUM

College Chemistry II is an approved general education course at BCCC, which can be used to fulfill degree requirements as a depth laboratory science course in the natural/physical science. In addition, it is required (or recommended) to be taken by students enrolled in chemistry, life science, physical sciences, Medical Lab Technician, and certain pre-professional programs (e.g. Pre Dentistry, Pre-Medicine, Pre-Pharmacy, Pre-Engineer and others.) This course transfers well and may be used to help fulfill credit and course requirements for general education at all Kansas Regents institutions. However, general educations requirements vary among institutions, and perhaps even among departments, colleges, and programs within an institution. Also, these requirements may change from time to time and without notification. Therefore it shall be the student’s responsibility to obtain relevant information from intended transfer institution during his/her tenure at BCCC to insure that he/she enrolls in the most appropriate set of courses for the transfer program.

IV. ASSESSMENT OF STUDENT

LEARNING/COURSE OUTCOMES

Barton County Community College assesses student learning at several levels: institutional, program, degree and classroom. The goal of these assessment activities is to improve student learning. As a student in this course, you will participate in various assessment activities. Results of these activities will be used to improve the content and delivery of Barton’s instructional program.

This course is intended to: 1. Establish a strong background in general chemistry. 2. Develop an ability to apply the concepts of chemistry in problem solving. 3. Develop general background of thermo-, electro-, and organic chemistry. 4. Provide the general understanding of chemical reactions in solution and to relate the activity and adaptation of everyday life to variation in environmental conditions and constraints. 5. Relate chemical concepts and process to the students’ individual life and to other fields of knowledge, so that the student may live a healthier, happier and more meaningful and productive life.

V. COURSE COMPETENCIES

The learning outcomes and competencies detailed in this syllabus meet, or exceed, the learning outcomes and competencies specified by the Kansas Core Outcomes Project for this course, as sanctioned by the Kansas Board of Regents. The topics listed below are not in any specific order. Upon completion of College Chemistry II, the student will be able to: 1. Electrochemistry A. Describe galvanic and electrolytic cells and their operation. B. Calculate cell potentials and determine spontaneity of oxidation/reduction reactions. C. Understand and use Faraday’s Law. D. Understand and apply the relationship of thermodynamics to electrochemistry. E. Understand and use the Nernst Equation. F. Give examples of natural and/or commercial applications of electrochemical processes. G. Use the activity series of metals.

2. Kinetics A. Discuss the meaning of the rate of a reaction. B. Explain the factors that affect reaction rates. C. Use the initial rate method to determine reaction order from experimental data D. Describe the relationship between order of reaction and molecularity. E. Use experimental data to determine the rate law for a reaction. F. Compare first and second order rate reactions, G. Discuss the collision theory of a reaction rate. H. Use the Arrhenius equation to illustrate the relationship between energy of activation and rate law constant. I. Describe the relationships among the mechanism, the overall reaction, and elementary steps. J. Draw and interpret energy diagrams and illustrate the effect of a catalyst on the energy diagram. 3. Colligative Properties A. Define the following solution terms: a. Saturated solution b. Unsaturated solution c. Supersaturated solution d. Solubility e. Solute

f. Solvent B. Calculate concentration in molality and mole fraction. C. Explain the factors that affect solubility D. Explain and calculate vapor pressure using Raoult’s Law. E. Explain and calculate freezing point depression, boiling point elevation, and osmotic pressure. 4. Thermodynamics A. Explain the similarities and differences between such terms as enthalpy, entropy, and free energy. B. Explain how the First, Second, and Third Laws of Thermodynamics apply to chemical and physical processes. i. Predict whether the entropy change in a given process is positive, negative, or near zero. ii. Use data tables to determine enthalpy, entropy, and free energy changes.

iii. Explain how H°, S°, and G° are related to reaction spontaneity.

iv. Explain how a knowledge of H°, S°, and G° allows one to predict the conditions under which a reaction will occur. C. Describe the relationship between the standard free energy of reaction and the equilibrium constant. D. Calculate G for a chemical reaction that occurs under nonstandard conditions. 5. Equilibrium of Aqueous Solutions A. Name and list the common strong acids and strong bases, i.e., any hydroxide base. B. Describe and recognize Bronsted-Lowry, Lewis, and Arrhenius Acids and Bases. C. Use the definition of acids and bases to distinguish between strong and weak acids and bases, equilibrium relationships among them, and the aqueous properties of their salts. D. Use the concepts of pH, pOH, Ka, and Kb to calculate the pH of aqueous solutions of acids, bases, and their salts. E. Determine the specific species present in an aqueous solution and the concentrations of those species. F. Describe the effect of common ions and calculate concentrations of all species present in solutions of weak acids and bases. G. Describe the ionization of polyprotic acid in aqueous solution. H. Explain the buffer effect, predict the influence of added acids and bases on buffers, and use the Henderson-Hasselbach equation to calculate the concentration of species in solution. I. Identify titration curves for strong, weak, and polyfunctional acids and bases. J. Understand the use of volumetric methods to determine the concentrations of species in solution. K. Write an equation to express the relationship between a solid solute and its constituent ions in a saturated solution. L. Calculate the Ksp from molar solubility and molar solubility from Ksp. M. Calculate the effect of a common ion on the molar solubility of a salt. N. Predict whether precipitation will occur when salt solutions are mixed and determine the concentration of ions remaining in solution after precipitation. 6. Equilibrium Principles A. Explain how the terms reversible reaction and dynamic equilibrium are related. B. Write the general equilibrium constant expression and explain its significance. C. Explain why the concentrations of pure liquids and solids are never used in equilibrium constant expressions. D. Show how the numerical value of the equilibrium constant changes when the stoichiometric coefficients are changed or the reaction is reversed.

E. Explain the differences between the terms Kc and Kp and the relation of either to Qc. F. Explain the difference between an equilibrium position and an equilibrium constant. G. Given Keq and initial concentration of reactants and/or products, calculate the final concentrations of reactants and/or products. H. List and explain the external factors that can affect equilibria. I. Using LeChateleir’s Principle, explain how changes in temperature, pressure, volume, or concentration affect the equilibrium position for a chemical reaction. 7. Optional Topics – in alphabetical order Biochemistry Coordination Chemistry Descriptive Chemistry Nuclear Chemistry Organic Chemistry

LABORATORY - COLLEGE CHEMISTRY II Upon successful completion of this course the student will be able to: A. Work in the laboratory in accordance with good laboratory practices. a. Dress in an appropriate manner as to promote safety in the laboratory, wearing a lab coat and goggles when anyone is working with chemicals in the laboratory. b. Follow written directions accurately. c. Work safely and effectively, using equipment and chemicals carefully d. Demonstrate use of required safety and common laboratory techniques. e. Dispose of waste products in a proper manner. B. Gather and record qualitative and quantitative data accurately. a. Acquire data using balances and volumetric glassware. b. Make and record visual observations. c. Use computers, when appropriate, as data acquisition tools. d. List or describe experimental assumptions made and any deviations from the written experimental procedures. C. Handle and evaluate data in logical, productive, and meaningful ways. a. Create notebooks and laboratory reports that are clear, understandable, and accurately represent the data collected. b. Display computer data in a spreadsheet or graphically, as appropriate. c. Correlate observations with chemical or physical processes. d. Carry out suitable calculations with quantitative data, recognizing when data and calculations are within a reasonable range. e. Use observations of experimental data to present relevant conclusions pertaining to the experimental procedure. D. Correlate laboratory work with principal topics in College Chemistry II lecture.

VI. COURSE SCHEDULE Unit Reading Assignments Points

Week 1 Admin - Academic Integrity Quiz 5

Week 1 Admin - M.C. Intro Quiz 10

Week 1 Admin - Orientation Quiz 5

Week 1 Admin - PreTest 20

Week 1 Admin Discussion - Introductions 10

1 Ch 14 Unit 1 MC HW Ch 1 4 30

Unit 1 Discussion 10

Unit 1 Labs 30

Unit 1 Quiz 50

2 Ch 15 Unit 2 MC HW Ch 15 30

Unit 2 Discussion 10

Unit 2 Labs 30

Unit 2 Quiz 50

3 Ch 16 Unit 3 MC HW Ch 16 30

Unit 3 Discussion 15

Unit 3 Labs 25

Unit 3 Quiz 50

4 Ch 17 Unit 4 MC HW Ch 17 30

Unit 4 Discussion 10

Unit 4 Labs 30

Unit 4 Quiz 50

5 Ch 19 Unit 5 MC HW Ch 19 30

Unit 5 Discussion 15

Unit 5 Labs 30

Unit 5 Quiz 50

6 Ch 20 Unit 6 MC HW Ch 20 30

Unit 6 Discussion 10

Unit 6 Labs 30

Unit 6 Quiz 50

7 Ch 21 Unit 7 MC HW Ch 21 30

Unit 7 Discussion 10

Unit 7 Labs 25

Unit 7 Quiz 50

8 Ch 24 Unit 8 MC HW Ch 24 30

Unit 8 Discussion 10

Unit 8 Quiz 50

Final - Post Test – Review

Post Test 20

Final Exam 100

1100

VII. TEXTBOOKS AND OTHER

Online Homework Access & eText: You are required to purchase access to the online homework system either through the classroom (on the first day of the course) or through the

REQUIRED MATERIALS

bookstore. This online homework access comes with an eText that is accessible in the classroom. To purchase instant access, open the course as usual then click on the HW and Quizzes section. It will guide you through the purchasing process.

If you want to purchase a hardcopy of the book, the course is based on Brown, LeMay and Bursten, Chemistry: the Central Science, 12th Edition. This book is available through the BartOnline Bookstore or your favorite book retailer. If you are on financial aid, you will need to use the financial aid voucher through the bookstore. Purchase the Required materials listed in the bookstore. Lab Kit You will also need a labkit for your lab assignments. This is a custom kit that you can obtain from the bookstore or by ordering from QualityScienceLabs.com. http://www.qualitysciencelabs.com/barton-community-college/ You need the Barton Community College Chem 2 (1808) Kit.

A scientific calculator is also required. I purchased mine from Target for about $20.

VIII. REFERENCES Any reference that a student finds are helpful in understanding the material may be used to supplement the required materials. The instructor will also have linked supplementary materials that will help provide clarification for material contained in that unit.

IX. METHODS OF INSTRUCTION AND

EVALUATION

Exams are held online and make-ups are not allowed. These due dates are announced in the course schedule stated in the course home page. You are allowed 1 hour and 30 minutes for each exam. The exams are multiple choice and short answer questions. Labs are listed under the Units where they are due. Labs will be assigned with the appropriate section and will be due upon completion of the appropriate unit. Homework assignments are found in the HW and Quizzes section under the course home. Please feel free to email the instructor with any questions regarding your grade, your work, and any other questions you may have regarding your success in the course. I am glad to help and am willing to provide the necessary direction for you to be able to succeed. Please also know that I make every effort to have assignments graded by the Wednesday following the assignment due date. Grades will be available when I complete grading assignments. During semester, students who are getting C, D, or F are especially encouraged to arrange for a tutor and/or seek help from other students or the instructor. Grading Scheme: 90%-100% = A 80% - 89% = B 70% - 79% = C

60% - 69% = D Less than 60% = F