EASTERN ARIZONA COLLEGE General Chemistry II
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1 EASTERN ARIZONA COLLEGE General Chemistry II Course Design Course Information Division Science Course Number CHM 152 (SUN# CHM 1152) Title General Chemistry II Credits 4 Developed by Phil McBride, Ph.D. Lecture/Lab Ratio 3 Lecture/3 Lab Transfer Status ASU NAU UA CHM 116, Natural Science - Quantitative (SQ) CHM 152L also satisfies: Lab Science [LAB] --and- - CHM 152 also satisfies: Science & Applied Science [SAS] CHEM 152 Activity Course No CIP Code Assessment Mode Post Test/ACS Standardized Second Term Form 2002 Exam (80 Questions/80 Points) Semester Taught Spring GE Category Lab Science Separate Lab Yes Awareness Course No Intensive Writing Course No Prerequisites CHM 151 Educational Value This course is a continuation of General Chemistry I and is designed for adults in associate degree programs and/or transfer programs that leads to a degree in any of the Physical or Biological Sciences, or leads to a degree in a Health-related field such as Medical Doctor, Chiropractor, Optometrist, Dental Hygienist, Dentist, etc. Students will gain an understanding of chemistry and how it affects their lives. The laboratory experiments use many household chemicals which the students will learn to deal with in a safe and effective manner. Students will work cooperatively with others in a laboratory and group setting. The students will learn how to identify problems and then work successfully at solving those problems. Students will learn to communicate with others through written reports and oral presentations. EASTERN ARIZONA COLLEGE General Chemistry II
2 Description Provides the student with knowledge of the fundamental principles of chemistry with an emphasis on the control of chemical reactions and the chemistry of the elements. Chemical kinetics, equilibria, acids-base chemistry, entropy of reactions, electron transfer reactions, nuclear chemistry, and an introduction to organic chemistry will be explored. The student will also apply critical thinking strategies in scenario and inquiry-based laboratory activities. Supplies Laboratory Notebook: Comp Book 5x5 QUAD ruled (required) Scientific Calculator (required) Competencies and 1. Evaluate solutions and their colligative properties in detail. a. Define the terms solution, solvent, solute, and colligative properties. b. Use the following concentration units: molality, weight percent, and parts per million. c. Describe the process of dissolving a solute in a solvent, including the energy changes that may occur. d. Understand the distinctions between saturated, unsaturated, and supersaturated solutions. e. Define and illustrate the terms miscible and immiscible. f. Use Henry s law to calculate the solubility of a gas in a solvent. g. Calculate the mole fraction of a solute or solvent and the effect of a solute on solvent vapor pressure using Raoult s law. h. Use colligative properties to determine the molar mass of a solute. i. Use the van t Hoff factor, i, in calculations involving colligative properties. o By successfully completing periodic written examinations o Through completion of a weekly laboratory report Criteria Performance will be satisfactory when: 2. Attain an understanding of the principles involved in rate of reactions (kinetics). a. Explain the concept of reaction rate. b. Derive the average and instantaneous rate of a reaction from experimental information. c. Describe the various conditions that affect reaction rate (i.e., reactant concentrations, temperature, presence of a catalyst, and the state of the reactants). d. Describe and use the relationships between reactant concentration and time zero-order, EASTERN ARIZONA COLLEGE General Chemistry II
3 first-order, and second-order reactions. e. Apply graphical methods for determining reaction order and the rate constant from experimental data. f. Use the concept of half-life, especially for first-order reactions. g. Use collision theory to describe the effect of reactant concentration on reaction rate. h. Describe the functioning of a catalyst and its effect on the activation energy and mechanism of a reaction. i. Acknowledge the effect of molecular orientation and temperature on reaction rate. j. Define the rate-determining step in a mechanism and identify any reaction intermediates. o by achieving greater that 70% on a written exam Criteria Performance will be satisfactory when: 3. Explore Chemical Equilibrium. a. Acknowledge the nature and characteristics of the state of equilibrium: (a) chemical reactions are reversible: (b) equilibria are dynamic, and (c) the nature of the equilibrium state is the same, no matter what the direction of approach. b. Write an equilibrium constant expression for any chemical reaction. c. Recognize that the concentrations of solids and solvents are not included in equilibrium constant expressions. d. Calculate an equilibrium constant given the reactant and product concentrations at equilibrium. e. Use equilibrium constants to calculate the concentration of a reactant or product at equilibrium. f. Apply Le Chatelier s principle to predict the effect of a disturbance on a chemical equilibrium: a change in temperature, a change in concentrations, or a change in volume or pressure for a reaction involving gases. o by achieving greater that 70% on a written exam Criteria Performance will be satisfactory when: EASTERN ARIZONA COLLEGE General Chemistry II
4 4. Illustrate the basic principles of acid-base reactions. a. Recognize common monoprotic and polyprotic acids and bases and write balanced equations for their ionization in water b. Give Recognize the Bronsted acid and base in a reaction and identify the conjugate partner of each. c. Recognize some common weak bases and understand that they can be neutral molecules. d. Calculate the ph of a solution from a knowledge of the hydronium ion or hydroxide ion concentration. e. Calculate the equilibrium constant for a weak acid or weak base from experimental information. f. Describe the acid-base properties of salts and calculate the ph of a solution of a salt of a weak acid or of a weak base. g. Calculate the ph of a solution of a polyprotic acid. h. Appreciate the connection between the structure of a compound and its acidity or basicity. i. Characterize a compound as a Lewis base (an electron-pair donor) or Lewis acid (an electron-pair acceptor). Criteria Performance will be satisfactory when: 5. Solve problems dealing with acid-base reactions. a. Predict the ph of an acid-base reaction at its equivalence point. b. Calculate the ph at the equivalence point in the reaction of a strong acid with a weak base, or in the reaction of a strong base with a weak acid. c. Predict the effect of the presence of a "common ion" on the ph of the solution of a weak acid or base. d. Describe the composition of a buffer solution and explain how buffers work. e. Calculate the ph of a buffer solution before and after adding excess acid or base. f. Describe how a buffer solution of a given ph can be prepared. g. Calculate the ph at any point in an acid-base titration. h. Acknowledge the differences between the titration curves for a strong acid/ strong base titration versus cases in which one of the substances is weak. i. Describe how an indicator functions in an acid-base titration. EASTERN ARIZONA COLLEGE General Chemistry II
5 6. Explore the conditions under which some compounds precipitate and others do not. a. Recall the solubility guidelines and write balanced equations for precipitation reactions. b. Write the equilibrium constant expression -- the solubility product constant, Ksp--for any insoluble salt. c. Calculate Ksp values from experimental data. d. Use Ksp values to decide the order of precipitation of two or more insoluble salts. e. Calculate the ion concentrations that are required to begin the precipitation of an insoluble salt. f. Calculate the solubility of a salt in the presence of a common ion. g. Use Ksp values to devise a method of separating ions in solution from one another. h. Calculate the equilibrium constant for the net reaction for a situation in which two or more equilibrium processes are occurring in solution. i. Recognize that the solubility of insoluble salts containing basic anions is affected by the ph of the solution. 7. Predict whether a chemical reaction is product-favored or reactant-favored. a. Describe the difference between the information provided by kinetics and thermodynamics. b. Understand that entropy is a measure of matter and energy dispersal. c. Predict the sign of the entropy change for a reaction or change in state. d. Calculate the entropy change for a change of state or for a chemical reaction. e. Use entropy and enthalpy changes to predict whether a reaction is product-or reactant- EASTERN ARIZONA COLLEGE General Chemistry II
6 favored. f. Understand the connection between enthalpy and entropy changes for a reaction and the Gibbs free energy change. g. Calculate the change in free energy for a reaction from the enthalpy and entropy changes or from the standard free energy of formation of reactants and products. h. Describe the relationship between the free energy change for a reaction and its equilibrium constant. i. Show that a reactant-favored reaction can become product-favored if coupled with another reaction that is strongly product-favored. 8. Solve problems dealing with electron-transfer reactions. a. Define and use the terms battery, or electrochemical cell; fuel cell; electrolysis; electrode; electrolyte; salt bridge; anode; and cathode. b. Balance equations for oxidation - reduction reactions in acidic or basic solutions using the half-reaction approach. c. Explain the workings of an electrochemical cell. d. Appreciate the meaning of the standard electrode potential E, and its connection to the free energy change. EASTERN ARIZONA COLLEGE General Chemistry II
7 9. Obtain a basic understanding of organic molecules. a. Classify organic compounds based on structure. b. Draw structures of common organic compounds. c. Identify structural isomers and stereoisomers. d. Draw structures for benzene and substituted benzenes, and describe the bonding in benzene. e. Recognize, draw structures, and name alcohols, amines, aldehydes, ketones, carboxylic acids, esters, and amides, and amino acids. f. Understand the structures of fats and oils and their properties. g. Recognize chemical properties of the classes of organic compounds. h. Write equations for the formation of addition and condensation polymers. i. Know the basic reactions of alkanes, alkenes, alcohols, amines, aldehydes, ketones, and carboxylic acids. o by successfully completing periodic written examinations Types of Instruction Classroom Presentation On Campus Laboratory Field Trips Grading Information Grading Rationale Quizzes are optional for the instructor. Homework will be turned in and graded. There will be at least 5 exams, of which the lowest exam score will be dropped. Laboratory activities will be held each week. Laboratory reports will be turned in and graded each week. The students will participate in the S=CH-A (Student Chemistry Adventure) for visiting high school students as one laboratory activity. A final exam will be given at the end of the semester. Pre-test is 0% of the final grade. Homework is 15% of the final grade. Labs are 25% of the final grade. Exams are 50% of the final grade. Final Exam is 10% of the final grade and is an ACS Standardized General Chemistry Exam (80 Questions/80 Points) EASTERN ARIZONA COLLEGE General Chemistry II
8 Grading Scale A % B 80-89% C 70-79% D 60-69% F 0-59% EASTERN ARIZONA COLLEGE General Chemistry II
CHM 152 GENERAL CHEMISTRY II
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