______________________________________________________________________________ Fayetteville State University College of Basic and Applied Sciences Department of Natural Sciences CHEM 160 – 01 General Chemistry II Summer Session II 2007 I. Locator Information: Instructor: Dr. Daniel E. Autrey Course # and Name: CHEM 160 – 01, General Chemistry II Semester Credit Hours: 4.0 credits Total Contact Hours: 72 Day and Time Class Meets: (Lecture) MTWRF 10:00 am – 11:50 am LS 304E (Laboratory) TR 1:00 pm – 3:50 pm LS 302 Office Location: LS 325 Office Phone: 910-672-1354 Office Hours: MWF 2:00 pm – 4:00 pm Or By Appointment Email address: [email protected] Faculty Webpage: http://faculty.uncfsu.edu/dautrey/ FSU Policy on Electronic Mail: Fayetteville State University provides to each student, free of charge, an electronic mail account that is easily accessible via the Internet. The university has established email as the primary mode of communicating with enrolled students about impending deadlines, upcoming events, and other information important to student progression at the university. Students are responsible for reading their email on a regular basis to remain aware of important information disseminated by the university. The university maintains open-use computer laboratories throughout the campus that can be used to access electronic mail. Students making inquiries via email to FSU faculty and staff about academic records, grades, bills, financial aid, and other matters of a confidential nature are required to use their FSU email account. Rules and regulations governing the use of FSU email may be found at: http://www.uncfsu.edu/PDFs/EmailPolicyFinal.pdf 1II. Course Description: General Chemistry II (CHEM 160) is the second part of a two-semester (one year) course in college-level chemistry. It is a course investigating kinetics, chemical equilibria, acid-base equilibria, solubility equilibria, thermodynanics, and electrochemistry, with laboratory activities examining reaction rates, acid-base and reduction-oxidation titrations, and qualitative and elementary quantitative analysis. Prerequisites: A grade of "C" in CHEM 140 General Chemistry I or the equivalent at another university/college. Also either MATH 124 (College Trigonometry) or MATH 130 (Precalculus Mathematics II) is either a prerequisite or co-requisite for CHEM 160. It is up to each student to make sure that he/she meets the course prerequisites. Note that your chances of successfully completing this course are poor if you do not meet the prerequisites. III. Textbook:  T. L. Brown, H. E. LeMay, B. E. Bursten, and J. R. Burdge, Chemistry, The Central Science, 10th Ed., Prentice Hall, 2006. (lecture)  J. H. Nelson and K. C. Kemp, Laboratory Experiments, Chemistry, The Central Science, 10th Ed, Prentice Hall, 2006. (laboratory) IV. Student Learning Outcomes: Upon completion of this course, students will be able to: 1. Identify the fundamental laws and principles of chemistry, including: a. The types of intermolecular forces (dispersion, ion-dipole, dipole-dipole, and hydrogen-bonding) and their roles in predicting the physical properties (viscosity, boiling point, density, vapor pressure, surface tension, heats of fusion and vaporization etc.) of matter. b. The types of crystal structure and their relationship to the density of solids. c. The Kinetic Theory and the concepts of chemical kinetics by:  Identifying the factors that affect the rate of chemical reactions.  Understand the difference between rates of reaction, rate laws, and rate constants.  Determining the order of a reaction from experimental chemical data.  Using the concept of half-life and integrated rate laws to determine the variation of concentration with time for first and second order reactions.  Using the Arrhenius Equation to predict the affect of temperature on chemical reaction rates.  Understanding how homogeneous and heterogeneous catalysts increase the rates of chemical reactions.  Understanding the concept of reaction mechanism and be able to identify the rate-determining step. 2d. The concept of dynamic chemical equilibria by:  Performing calculations involving equilibrium constants.  Understanding the principles of heterogeneous equilibria.  Using the reaction quotient to predict the direction of chemical reaction.  Using the Le Châtelier’s Principle to predict the direction of chemical reaction for changes in reactant or product concentrations, volume and pressure changes, temperature changes, and the inclusion of a catalyst. e. The concept of acid-base equilibria by:  Understanding the Brønsted-Lowry Theory and be able to identify conjugate acid-base pairs.  Understanding the autoionization of water.  Determining the pH, pOH, and percent dissociation/ionization for aqueous solutions of both strong and weak acids and bases.  Predicting the relative strengths of acids and bases from their equilibrium constants.  Predicting the acid-base properties of salts and calculating the pH for both acidic and basic salt solutions.  Understanding the Lewis Theory and using it to understand the hydrolysis of metal ions. f. The concepts of aqueous equilibria by:  Understanding the common-ion effect and its role in the properties of buffer solutions.  Identifying what constitutes a buffer solution and how to prepare a buffer a particular pH and buffer capacity.  Determining the pH of a buffer solution using the Henderson-Hasselbach Equation.  Using solution stoichiometry to determine the pH of a buffer after the addition of a small amount of either a strong acid or base.  Understanding the principles of acid-base titrations, such as those involving strong acid–strong base titrations, weak acid–strong base titrations, and the titrations of polyprotic acids.  Using solution stoichiometry to determining the pH of a solution that is prepared by the quantitative mixing of acids and bases. g. The concepts of solubility equilibria by:  Performing calculations involving the solubility product, molar solubility, and solubility.  Understanding the difference between unsaturated, saturated, and supersaturated solutions.  Understanding the factors that affect