page 1 Brooklyn College - Department of Chemistry Chemistry 1 Fall 2001 Required Texts: Chemistry, The Central Science Brown, LeMay and Bursten Prentice Hall Publishers, 2000, 8 th Edition. Basic Laboratory Principles in General Chemistry Bramwell, Dillard, Shahani, and Wieder Kendall/Hunt Publishers, Dubuque, 1990. Required Items: Scientific calculator; lock for lab drawer; safety glasses; matches; detergent; roll of paper towels. Recommended Items: Lab coat or apron. Study Guide to Brown & LeMay, James C. Hill Prentice Hall Publishers, 8 th Edition Solutions to Exercises in Brown, LeMay and Bursten, R. Wilson, Prentice Hall Publishers. Fundamentals of Chemistry, D. E. Goldberg, Brown Publishers, 3 rd Edition, 2000. Schaum's Outline: Beginning Chemistry, D. E. Goldberg, 2 nd Edition, McGraw Hill Publishers, New York, 1999. General Chemistry Test Bank, D. E. Goldberg, New York, 1981. Schaum's 3000 Solved Problems in Chemistry, McGraw- Hill, 1988. Counseling: Office Hours: General Chemistry Coordinator: Prof. Aronson, 3315N General Chemistry Counseling: Prof. Goldberg, 359NE Health Profession Counseling: Prof. McEntee, 1305J Office hours for all faculty are posted on the bulletin board in the hallway by the Chemistry Department Office, 359NE. Lecture Tests: FIRST EXAM: Wed., Oct. 24 th, 2001, 6:15pm - 7:45pm Covers Recitations 1-5 SECOND EXAM: Wed., Nov. 21 st, 2001, 6:15pm - 7:45pm Covers Recitations 6-10 NOTE: Lab Exemptions: Drop Dates: NO Makeup exams are given for Lecture Tests. We mean it. Students who are repeating the course may be able to obtain laboratory exemptions. See Prof. Goldberg or Prof. Aronson. Students who receive exemptions must take the recitation quizzes and, possibly the laboratory quizzes. Mon., Sept. 17 is the last day to drop a course without a grade. Tues., Nov. 13 is the last day to apply for non penalty withdrawal (W grade). See your lab instructor or the course coordinator for advice.
page 2 Note: You may transfer (possibly with a W) to Chem 1.1, a slower paced course, if Chem 1 is too difficult for you. The LAST day to switch to Chem. 1.1 is Fri., Oct.12 and may be done only if seats are available in Chem 1.1. Grading: See page 5 Chemistrv 1 Lecture Schedule Unless specific sections are indicated, you are responsible for the whole chapter. For best results, read the assigned material before lecture. Lecture No. Topics Assigned Reading 1,2 Math Review, Dimensional Appendix A.1 Analysis, Basic Concepts (pp. 1012-1014) Chapter 1 (memorize Table 1.2) 3,4 Elements, Compounds Chapter 2 (memorize Ions, Periodic Table Table 2.4 and 2.5) 5,6 Chemical Equations, Moles, Chapter 3.1-3.5 Empirical Formulas 7,8 Stoichiometry, Limiting Chapter 3.6-3.7 Reagents 9,10 Chemical Reactions, Molarity, Chapter 4 Solution Stoichiometry (Omit Oxidation Numbers, pp. 121-123) 11-13 Thermochemistry Chapter 5 14,15 Gases Chapter 10.1-10.8 16-18 Atomic Structure, Chapter 6 Periodic Properties Chapter 7.1-7.5 19,20 Ionic and Covalent Chapter 8.1-8.9 Bonding, Polarity 21,22 Molecular Shape, Chapter 9.1-9.3 Dipoles 23,24 Intermolecular Forces, Chapter 11.1,11.2, Phase Changes 11.4,11.5 25,26 Concentration, Solubility, Chapter 13.1-13.5 Colligative Properties 27,28 Phase Diagrams, Solids, Chapter 11.6-11.8 Homework Assignments. Many Students who "did well" in high school chemistry do not get good grades in college chemistry. The reason: they fail to develop the earning skills and problem-solving skills necessary for the advanced level of chemistry at Brooklyn College. The big difference between high school and college is the large amount
page 3 of work you must do on your own and the emphasis we place on THINKING (instead of memorizing). Your key to success? Learning how to study properly and doing LOTS of homework! Falling behind in reading and homework is a SERIOUS MISTAKE. Organize your life around your course-work and keep up with the assignments. As you read Brown, LeMay and Bursten (BLB), do the exercises and example problems in the chapter. In other words, read and work your way through the chapter. After working through each chapter work out the assigned homework problems. Note well that there will not be enough time in class for your instructor to go over every assigned problem. A good indicator of the kinds of problems found in tests is the homework problems. See your teacher during office hours for extra help. NOTE: Your instructor has the option of completing a recitation assignment one week after the scheduled meeting. Reading and Homework Assignments. Meeting 1 Math Review, Dimensional Analysis, Basic Concepts Read: Chapter 1 (Memorize Table 1.2) Homework: Most of the problems below are a review of high school math and will not be covered in class. The problems on dimensional analysis, significant figures and basic chemical concepts (BLB Ch. 1) will be covered. If you have difficulty with the math problems, consider transferring to Chemistry 1.1. Practice Exercises: a-d, p.1014 Chapter 1, Problems 1, 3, 7, 9, 11,13, 15, 19, 23, 29, 31, 33, 35, 38, 41, 63 Meeting 2 Elements, Compounds, Ions, Periodic Table Read: Chapter 2 (Memorize Table 2.4 and 2.5) Homework: Chapter 2, Problems 1, 3, 5, 6, 7, 13, 15, 21, 23, 25, 29, 32, 35, 37, 39, 41, 43, 47, 61, 66. Meeting 3 Chemical Equations, Moles, Empirical Formulas Read: Chapter 3.1-3.5 Homework: Chapter 3, Problems 1, 3, S, 7, 11, 13, 15, 17, 19, 21, 29, 30, 35, 37, 43, 46, 49, 51, 53 Meeting 4 Stoichiometry, Chemical reactions Read: Chapter 3.6, 3.7 Chapter 4.1-4.2 Homework: Chapter 3, Problems 59, 60, 69, 74, 75, 79 Chapter 4, Problems 1, 3, 5, 9, 11, 13 Meeting 5 Acid-Base Reactions, Oxidation of Metals Read: Chapter 4.3, 4.4. Homework: Chapter 4, Problems 17, 18, 25, 27, 33, 35,39, 41, 43 Meeting 6 Molarity, Solution Stoichiometry Read: Chapter 4.5, 4.6 Homework: Chapter 4, Problems 47, 48, 49, 51, 53, 61, 62, 67, 69, 71 Meeting 7 Thermochemistry Read: Chapter 5 Homework: Chapter 5, Problems 1, 2, 3, 12, 14, 15, 23, 27,
page 4 30, 35, 37, 39, 41, 43, 49, 50, 53, 55, 57, 61, 64, 71 Meeting 8 Gases Read: Chapter 10.1-10.8 Homework: Chapter 10, Problems 6, 7, 13, 17, 19, 21, 22, 23, 25, 27, 31, 35, 37, 38, 42, 44, 47, 49, 51, 55, 57, 59, 61, 66, 75 Meeting 9 Atomic Structure Read: Chapter 6 Homework: Chapter 6, Problems 1, 2, 3, 5, 7, 9, 11, 13, 15, 17, 19, 25, 27, 29, 41, 42, 43, 45, 47, 49, 51, 53, 59, 60, 62, 63, 65, 67, 69, 71 Meeting 10 Periodic Properties, Ionic Bonding Read: Chapter 7.1-7.5, 8.1-8.3 Homework: Chapter 7, Problems 5, 9, 11, 13, 14, 15, 17, 19, 21, 23, 25, 28, 29, 32, 33, 35, 41, 43 Chapter 8, Problems 1, 3, 5, 9, 12, 13, 15, 21, 22, 23, 25, 27 Meeting 11 Covalent Bonding, Bond Energy, Polarity Read: Chapter 8.4-8.9 Homework: Chapter 8, Problems 29, 31, 33, 35, 38, 39, 41, 47, 49, 51, 54, 57, 58, 59, 63, 65 Meeting 12 Molecular Shape, Dipoles Read: Chapter 9.1-9.3 Homework: Chapter 9, Problems 5, 7, 9, 11, 13, 15, 16, 19, 21, 23, 25, 26 Meeting 13 Intermolecular Forces, Phase Changes, Solubility, Concentrations Read: Chapter 11.1, 11.2, 11.4, 11.5, 13.1-13.4 Homework: Chapter 11, Problems 1, 2, 3, 4, 5, 7, 9, 10,13, 15, 17, 29, 33, 37, 40, 41, 43 Chapter 13, Problems 3, 4, 11, 15, 19, 20, 23, 25,27, 30, 31, 33 Meeting 14 Colligative Properties, Phase Diagrams, Solids Read: Chapter 13.5, 11.6-11.8 Homework: Chapter 13, Problems 45, 50, 51, 52, 55, 56 Chapter 11, Problems 49, 52, 73, 75, 76 NOTE: Your instructor has the option of scheduling a two hour recitation section for the 14th meeting. Chemistry 2 First Assignment It is necessary to do some preparatory work before your first recitation in Chemistry 2. Read: Chapter 14.1-14.4 in BLB on Chemical Kinetics. In Section 14.3, omit second-order Half-life. In Section 14.4, omit the discussion of the Arrhenius Equation. Homework: Chapter 14, Problems 3, 5, 9, 11, 15, 17, 21, 23
page 5 GRADING: Your final grade will be determined as follows: 30% Two lecture tests 20% Minimum of five quizzes 15% Laboratory reports and performance 10% Two laboratory quizzes 25% Final Exam Chemistry 1 and 1.2 Laboratory Schedule Before coming to laboratory, read the scheduled experiment and any other material assigned. Unless otherwise noted, page numbers refer to your laboratory manual. You must bring the lab manual to each lab class. All students must wear safety or prescription glasses in the laboratory. Your experimental data must be recorded directly on the laboratory report sheet. Lab reports are due in lab the week after the experiment was concluded unless you obtain permission from your instructor. All lab reports not handed in will receive a grade of zero. From meeting four (Expt. 3) on, you are required to hand in an outline described at the end of the lab schedule. Meeting Laboratory Assignment 1 Introduction to laboratory Check in, Lab safety, Bunsen burner and glass working, prepare stirring rods and prepare glass tubing for expt. 7 (see Fig. 7.2, page 64), Measurement, significant figures. Read pp. 1-13 and 23-25 (top) 2 Experiment 2A; Density This experiment handed out at meeting 1; safety quiz. Read pp. 14-18 (top) and 25-29. 3 Experiment 2; Introduction to Gravimetric Analysis Gravimetric determination of water of crystallization. Read pp. 35-38 and Transferring Solid Samples, p. 21 4 Experiment 3; Chemical Reactions Read pp. 39-46 and Read also handling and transfer of reagents, pp. 18-21 5 Experiment 5; Gravimetric Analysis Analysis of carbonate bicarbonate mixture Read pp. 53-56. 6 Experiment 8; Volumetric Analysis Equivalent weight of unknown acid Read pp. 69-74 7 Conclude Experiment 8 Start Experiment 9; Specific Heat Read pp. 75-78. 8 Conclude Experiment 9 (if needed) Experiment 10; Thermochemistry
page 6 Read pp. 79-86. 9 Experiment 7; Molar Gas Constant You must hand in a copy of your data before leaving lab Read pp. 63-68. 10 Special Experiment: Synthesis and analysis of Inorganic Compound The material for this 3-week experiment will be handed out at meeting 9. Read Buchner Filtration, p. 21 in manual. 11 Special Experiment (continued) Begin analysis of compound 12 Special Experiment (continued) Conclude analysis of compound Read Using Pipets on p. 18 in manual and pp. 254-256. 13 Experiment 28; Molecular Weight by Freezing-Point Depression, Procedure B. Read pp. 207-209 and 211-212. 14 Check out and Review No experiments are permitted in the last week. Laboratory Breakage In some schools, a laboratory fee is charged everyone. Our practice is to charge you only for the replacement cost of any items you lose or break. After check out, a bill will be prepared which you may pay at the bursar's office the following semester. NOTE: If you have checked in for any lab course you must check out even if you only attend class for one or two weeks before dropping the course. Students who fail to check out will be charged a fee of $50 plus the cost missing or broken equipment. Students who drop a course must go to the stockroom to check out as soon as possible. PREPARATION FOR LABORATORY Preparation ahead of time for your laboratory experiment will help you to better understand the experiment, to do a better job, and to learn more. In order to encourage you to do advance preparation, we are requiring you to make an outline of the experiment before lab. This outline is to be handed in to your lab instructor at the start of the period and will count toward your laboratory grade. The outline should state the goal of the experiment and briefly outline the procedure. The outline must be neatly done (preferably typed) and on one page. An example of an acceptable outline for experiment 2B is given below. Sample Outline Experiment 2. Goal: Determination of Water of Crystallization of Hydrate. To measure the mass of water in a sample of an ionic salt in order to determine the formula of the hydrated salt. Procedure: 1. Clean a crucible and cover and heat strongly. 2. Cool and weigh empty crucible. 3. A sample of hydrated salt is weighed accurately in the crucible.
page 7 4. The water is driven off by gentle heating of the crucible. 5. The sample is weighed again after cooling the crucible with the cover in place. The Principle of the Experiment: 1. The weight loss gives the mass of water in the sample and allows us to calculate the number of moles of water which was in the hydrated salt. 2. The moles of salt are calculated from the mass of anhydrous salt. 3. The ratio of moles of water to moles of salt gives the formula of the hydrate. Relevance of this Experiment: 1. This experiment gives experience in gravimetric analysis. 2. This experiment is an example of how chemists determine empirical formulas of compounds.