Georgia Perimeter College - Dunwoody SYLLABUS 1/05/2011 CRN # 34027 CHEM 1212-200 PRINCIPLES OF CHEMISTRY II Spring 2011 Class Time: M W 8:30-9:45 AM Lecture Room: NE-0300 Instructor: Prof. Myung-Hoon Kim Office: NE-2222, (770) 274-5059, Myung.Kim@gpc.edu Office Hrs: M T* R*1:30-3:30pm (*at LTC); W 10:30-12:30pm; F 12:00-2:00pm Website: facstaff.gpc.edu/~mkim Objective: To acquaint students with fundamental principles and topics of chemistry. Description: This is the second course in college chemistry for those whose majors or areas of interest are in science/engineering. This course is also the appropriate course for pre-medicine, pre-dentistry, prepharmacy, and physical therapy. It is not the normal choice for those going into nursing, dental hygiene, and several other allied health sciences. Areas of emphasis include solutions, reaction rates, chemical equilibrium, acid/base reactions, thermodynamics, and electrochemistry. Requirements: CHEM 1211 with a C or better is a pre-requisite. The student must have evidence in the form of a grade report or a transcript that this prerequisite has been met. CHEM 1212L lab is a co-requisite. Textbook & Materials: Chemistry (8th ed., Zumdahl/Zumdahl, Brooks/Cole, Cengage Learning, 2010) and OWL (an onli ne homework system, www.cengage.com are required (Course ID: Kim CHEM 1212 Spring 2011). A scientific calculator is recommended. Attendance: Students are expected to attend all class meetings. In the event of absence it is the students' responsibility to obtain assignments and information covered during the absence. A grade of W will be assigned if the student officially withdraws by mid-point. After mid-point withdrawal will result in a F grade unless a hardship waiver is granted by the department head. It is the student's responsibility to complete withdrawal through the registrar's office in the event that becomes necessary. Withdrawal from lecture automatically requires withdrawal from the lab and vice versa. A roll sheet will be circulated at the beginning of class. A student who arrives late should stop by at the end of class and sign it. Topics of a missed class, due to school closing from inclement weather (tune to WSB, AM 750 khz, or Channel 2), will be automatically assigned as a take-home project. Tests: There will be four class tests and a final exam. The final exam is required. There are no make-up tests. The final course grade is obtained by averaging the three highest class exams, MasteringChemistry and the final which weighs twice of the hour exams. If one of the class exams is missed, that exam becomes the dropped exam. The grading scale is the standard scale with 90-100 = A (Excellent), 80-89 = B(Good), 70-79 = C(Fair), etc. Three Best Hour Exams: 3 Exam x 100 pts/exam = 300 pts OWL (Online Homework): 10 Chap x 10 pts/chap = 100 pts Final Exam: = 200 pts Total 600 pts. A. Each Hour Exam consists of about 30 Multiple Choice Questions and 1-2 big Write-Out Questions. Sources: (1) Textbook (the Sample, Practice, & EOC Exercises) and Lecture Notes ( ~70%), (2) Applied questions (~30%) B. Bring #2 pencils and the Scantron Forms (882). (Note: An old mark must be completely erased). C. Extra points: 15 pts for a good attendance; Catching mistakes, 1~3pts/catch (max.: 15pts). 1
Time requirements The amount of time outside of class needed to be successful in this class varies with background, interest, motivation, intellect, and study skills. To be successful, expect 6 or more hours per week outside of class to study and do homework. Students must develop skill in solving problems and this can only be obtained by practicing and doing homework. The lab grade is separate and requires additional time. Expect 3 to 6 hours to prepare for lab sessions, calculate results, and prepare reports. Careful attention and good time management can reduce the time required outside of class. Disruptive actions: Students are expected to act with respect for a professor and other class mates. Arriving late for class can be disruptive. In the event of a late arrival you enter and take a seat quietly. Talking to others during lecture/discussion prevents others from hearing the proceedings. Leaving class during session is very disruptive and should occur only in an emergency. Food and drink are not allowed in the classroom.- Cheating and Plagiarism: Refer to the Green Handout for Academic Honesty Policy and others. Incomplete: An incomplete (I) grade is for special situations. If a student misses the final exam due to illness, or other special circumstance, request an I grade can be petitioned. Documentation is required confirming the difficulty. The I grade must be made up within one semester. CHEMISTRY 1212 SCHEDULE - Dates may be subject to change. - Wk M W Chapter Test Topics & Reading Assignment of the Week Date 1 Jan. 10 12 10 Introduction, Review, Intermolecular Force 2 (17) 19 10 Liquids and Solids 3 24 26 10, 11 Liquids and Solids, Properties of Solutions 4 Feb. 31 2 11 Properties of Solutions, 5 7 9 12 I Properties of Solutions, 6 14 16 12 Chemical Kinetics 7 21 23 13 Chemical Kinetics,Chemical Equilibrium 8 Mar. 28 2 13 II Chemical Equilibrium 9 ( 7 9) - - Spring Break - 10 14 16 14 Acid-Base (*Mid-Point: Mar. 16) 11 21 23 14, 15 Acid-Base Equilibria 12 28 30 16 III Solubility & Complex Ion Equilibria 13 Apr. 4 6 17 Chemical Thermodynamics 14 11 13 17 - Spontaneity, Entropy, & Free Energy 15 18 20 18 Electrochemistry, 16 25 27 18 IV Electrochemistry 17 May 2 4 19 The Nucleus (9) 11 Final Standard Test(Comprehensive), OWL Homework Due Notes: (1) After reading each chapters, you should work out the sample exercises and practice exercises. Many problems at the end of each Chapters will be addressed in the Online Homework. (2) It is necessary to use a scientific calculator during a class and a test. Graphic calculators (such as TI-80's, HP-48G, etc.) are allowed in a test, but HP-48GX is allowed without the plug-in chemistry card. (3) Extra points will be added to your total score for catching any mistakes in lecture materials. Submit an error and a correction with your name and date on a piece of paper. (1~3pt/catch). (4) It is recommended that you form study groups with classmates that meets regularly. (5) The course home page provide other useful information, links, & sample exams from the past, etc. 2
CHEMISTRY 1212 COURSE CONTENTS Chapter 10 Liquids and solids 1. Intermolecular Forces, 2. The Liquid State, 3. Structures and Types of Solids, 4. Structure and Bonding in Metals, 5. Carbon & Silicon: Network Atomic Solids, 6. Molecular Solids, 7. Ionic Solids, 8. Vapor Pressure and Changes of State, 9. Phase Diagrams Chapter 11 Properties of Solutions 1. Solution Composition, 2. The Energies of Solution Formation 3. Factors Affecting Solubility, 4. The Vapor Pressures of Solutions 5. Boiling Pt. Elevation & Freezing Pt. Depression, 6. Osmotic Pressure 7. Colligative Properties of Electrolyte Solutions, 8. Colloids - FIRST CLASS EXAM - covers Chap. 10 & 11 Chapter 12 Chemical Kinetics 1. Reaction Rates, 2. Rate Laws, 3. Determining the Forms of Rate Law, 4. The Integrated Rate Law, 5. Reaction Mechanisms, 6. A Model for Chemical Kinetics 7. Temperature and Rate: Activation Energy, 8. Catalysis Chapter 13 Chemical Equilibrium 1. The Equilibrium Condition, 2. The Equilibrium Constant(K), 3. Equilibrium Expressions involving Pressure, 4. Heterogeneous Equilibrium, 5. Applications of Equilibrium Constant, 6. Solving Equilibrium Problems 7. Le Chatelier's Principle: Factors That Affects Chemical Equilibrium - SECOND CLASS EXAM - covers Chap. 12 & 13 Chapter 14 Acids and Bases 1. The Nature of Acids and Bases, 2. The Acid Strength, 3. The ph Scale, 4. ph of the Strong Acid Solutions, 5. ph of the Weak Acid Solutions, 6. Bases, 7. Polyprotic Acids, 8. Acid-Base Properties of Salts, 9. The Effect of Structure on Acid-Base Properties 10. Acid-Base Properties of Oxides, 11. Lewis Acid-Base Model 12. Solving Acid base Problems Chapter 15 Acid-Base Equilibria 1. Solutions Containing Common Ions, 2. Buffer Solutions, 3. Buffering Capacities, 4. Titrations and ph Curves 5. Acid-Base Indicators - THIRD CLASS EXAM - covers Chap. 14 & 15 3
Chapter 16. Solubility and Complex Ion Equilibria 1. Solubility Equilibria & the Solubility Product, 2. Precipitation & Qualitative Analysis 3. Equilibria Involving Complex Ion Chapter 17. Spontaneity, Entropy (S) and Free Energy (G) 1. Spontaneous Processes and Entropy, 2. Entropy (S) & the Second Law of Thermodynamics 3. Effect of Temperature on Spontaneity, 4. Free Energy, 5. Entropy Change, 6. Free Energy and Chemical Reactions, 7. Dependence of Free Energy on Pressure, 8. Free Energy and Equilibrium, 9. Free Energy and Work Chapter 18. Electrochemistry 1..Balancing Oxidation-Reduction Equations, 2. Galvanic Cells, 3. Standard Reduction Potentials, 4. Cell Potential, Electrical Work, and Free Energy 5. Dependence of Cell Potential on Concentration, 6. Batteries, 7. Corrosion 8. Electrolysis, 9. Commercial Electrolytic Processes - FOURTH CLASS EXAM - covers Chap. 16, 17 & 18 Chapter 19. The Nucleus: A Chemist s View 1. Nuclear Stability and Radioactive Decay, 2. The Kinetics of Radioactive Decay, 3. Nuclear Transformations, 4. Detection and Uses of Radioactivity, 5. Thermodynamic Stability of the Nucleus, 6. Nuclear Fission and Nuclear Fusion 7. Effect of Radiation - FINAL EXAM - COMPREHENSIVE CHEM 1212 EXPECTED EDUCATIONAL RESULTS At the completion of this course students should be able to: 1. calculate the heat required for a phase change of a given mass of substance. 2. calculate vapor pressure and heats of vaporization. 3. identify intermolecular forces(imf) or attraction. 4. determine relative vapor pressure, BP, MP, surface tension, viscosity on the basis of IMF. 5. identify types of solids. 6. determine the # of atoms/unit cell, atomic mass from unit-cell dimension & density, and vise versa. 7. apply Henry's Law to predict solubility of a gas. 8. calculate solution concentration and convert concentration from one unit to another. 9. calculate VP lowering, BP elevation, FP depression and osmotic pressure. 10. determine molecular weight from measurements of change in colligative properties. 4
11. identify acid and base species given a proton transfer reaction. 12. decide whether reactants or products are favored in an acid/base reaction. 13. identify Lewis acid and base species. 14. assign oxidation numbers of atom in a compounds or in an ion. 15. balance oxidation-reduction reaction. 16. handle stoichiometry problems associated with a titration. 17. calculate the average reaction rate. 18. determine the order of a reaction from the rate law. 19. determine the rate law from initial rates. 20. use the concentration-time equations for a first-order and second-order reactions. 21. relate the half-life of a reaction to the rate constant. 22. use the Arrhenius Equation to predict a rate constant at a different temperature knowing E a. 23. write the overall chemical eqn from a mechanism: determine molecularity of an elementary rxn. 24. write the rate equation from an elementary reaction: determine rate law from a mechanism. 25. apply stoichiometry to an equilibrium mixture. 27. write equilibrium-constant expression. 28. obtain equilibrium-constant from reaction composition. 29. use reaction quotient. 30. obtain one equilibrium concentration given the others. 31. solve equilibrium problems. 32. apply Le Chatelier's principle to predict composition of a mixture in an equilibrium. 33. calculate ph from H + concentration, or vice versa. 34. calculate H + and OH - concentration in solutions of a strong acid or base. 35. determine K a (or K b ) from the solution ph. 36. calculate concentrations of species in a weak acid solution using K a. 37. calculate concentrations of species in a weak base solution using K b. 38. predict whether a salt solution is acidic, basic, or neutral. 39. obtain K b from K a or K a from K b of a conjugate base or acid. 40. calculate concentrations of species in a salt solution. 41. apply the common ion effect calculate degree of ionization of a weak acid. 42. calculate ph of a buffer given concentrations and volumes of acid and conjugate base. 43. calculate ph during a titration (the initial, mid-point, equivalence points, limiting ph values). 44. write solubility product expressions. 45. calculate K sp from the solubility or vice versa. 46. calculate solubility of a slightly soluble salt in a solution of common ion. 47. predict whether a precipitation will occur. 48. determine effect of ph on solubility. 49. separate metal ions by fractional precipitation. 50. calculate concentration of a metal ion in equilibrium with a complex ion. 51. predict whether a precipitate will form in the presence of the complex ion. 52. calculate solubility of a slightly soluble salt in a solution of the complex ion. 53. calculate kinetic and other energies. 54. write and manipulate thermochemical equations. 55. calculate the heat of the reaction from the stoichiometry. 56. relate heat and specific heat. 57. calculate ΔH from calorimetric data. 58. apply Hess's Law. 59. calculate the heat of phase change from standard enthalpies of formation. 60. calculate the enthalpy of reaction from standard enthalpies of formation, and vice versa. 61. calculate the entropy change for a phase transition. 62. predict the sign of the entropy change of a reaction, and calculate ΔS o for a reaction. 63. calculate ΔG o from ΔH o and ΔS o. 64. calculate ΔG o from ΔG o f: interpret the sign of ΔG o. 65. calculate K eq from the standard free energy change of the reaction, ΔG o. 66. calculate the quantity of work from given amount of cell reactant. 67. determine the relative strengths of oxidizing and reducing agents. 68. calculate the emf from standard potentials. 69. calculate the free energy change from the electrode potentials and the cell emf from ΔG o. 70. calculate the equilibrium constant from cell emf. 5