SYLLABUS AND COURSE OUTLINE Title of Course: Fundamentals of General, Organic and Biological Chemistry I Course Code/Section: CHE 121/985 Lab Hours: 3 Academic Year: 2010 Credits: 4 Instructor Information Name: Ling Chen, Ph.D. Office: (212) 220-8000, x5082 Room: N661 Email: lchen@bmcc.cuny.edu A. Course Description This course is a two-semester course sequence that introduces principles and concepts of general, organic and biological chemistry. The laboratory provides experimental applications of these chemical topics. CHE 121-CHE 122 Two terms required. Liberal Arts Elective. Recommended for students intending to transfer to bachelor degree in nursing and allied health science curricula. CHE 121-CHE 122 cannot be granted credit to fulfill degree requirements for A.S. (Science) and for A.S. (Engineering Science). CHE 121-CHE 122 does not meet science requirement for A.A. (Liberal Arts). B. Prerequisites and/or Co-requisites Basic Skills Prerequisites: RDG 062, ENG 088 or ESL 062, and MAT 051. C. Student Learning Outcomes 1. Students will be able to explain that living cells are made of elements and compounds with different chemical properties. Water is a universal solvent. 2. Students will be able to demonstrate chemistry as prerequisite to how living organisms work. 3. Students will be able to explain that the diverse topics of chemistry are logical when considered in the context of principles. 4. Students will be able to apply chemical principles to the life sciences. 5. Students will be able to solve mathematical problems such as density, moles, gas laws, percent concentrations (mass/mass, mass/volume, and volume/volume), molarity and all types of conversions. D. Required Texts and/or Supplementary Materials 1. TEXTBOOK: General, Organic and Biological Chemistry (3 rd Edition) written by Timberlake, Karen C. and published by Pearson Prentice Hall (2009). ISBN-10: 0136054544 ISBN-13: 9780136054542 2. LAB MANUAL: Laboratory Manual for General, Organic, and Biological Chemistry (2 nd Edition) written by Timberlake, Karen C. and published by Pearson Prentice Hall (2010) ISBN-10: 0321695291 ISBN-13: 9780321695291 E. Use of Technology Computer with internet service is required to access most of the course materials.
Firefox internet browser is required for the course assessments such as Quizzes and Practice Exercises. Acrobat Reader is needed to open the course documents: Lecture Notes, Learning Checks and others. A scientific calculator is required for labs and exams. In addition to read the class materials online, you must participate in Discussion Board discussions from Blackboard by posting one question and response to one of others postings for each chapter. Once a week we have chat hour during Virtual Office Hour so your questions and concerns can be answered synchronously. You may email me for any personal questions. F. Evaluation and Requirements of Students There will be total five exams: four-term examinations (total 40%), and a final examination (20%). You must fulfill all laboratory assignments (total 20%). You must participate in class discussions via the Discussion Board (total 5%) every week, complete one Quiz for each chapter (total 5%), and one Practice Exercise before each exam (total 10%). 1. Time: You must dedicate a great deal of time to the readings and assignments. This course is as timeconsuming as the face-to-face course and you must be comfortable using a computer, the Internet, and are highly motivated and disciplined to allot the appropriate amount of time every week to the course in order to successfully complete the assignments on time. 2. Discussion Board Participation: You must post a question and response other s posting by the due date. After a specified date, you will no longer be available to complete the tasks. 3. Assignments: Due dates for Quizzes and Practice Exercises are listed in Study Schedule, which can be found in Course Information and weekly folders. NO LATE WORK WILL BE ACCEPTED. Missing assignments will negatively impact your final grade. 4. Laboratory: Weekly completion of assigned lab work (see Lab Schedule) is required. GRADES WILL BE LOWERED FOR MISSING LABS. There is no make-up lab. 5. Exams: There will be total of five exams given in the course, i.e., one exam for every two or three chapters. There is no make-up exam. G. Final grade: Your final grade will be based on the following guidelines: Participation in the discussion boards 5% Quizzes 5% Practice Exercises 10% Labs 20% Term examinations 40% Final examination 20% Your final letter grade is given according to BMCC s grading system: % 93-100% 90-92% 87-89% 83-86% 80-82% 77-79% 73-76% 70-72% 67-69% 63-66% 60-62% Grade A A- B+ B B- C+ C C- D+ D D- If you receive a C- or lower, see the F/C-grading policy
G. Other Resources Tutoring is available at the Science Learning Center (N734) and Science Resource Center (S500) E-tutoring service is available at http://www.bmcc.cuny.edu/etutoring/. Tech support is http://www.bmcc.cuny.edu/it/ Students with disabilities who require reasonable accommodations or academic adjustments for this course must contact the Office of Services for Students with Disabilities (Room N-769; Telephone # 220-8180). BMCC is committed to providing equal access to all programs and curricula to all students. Measurements Statement on Plagiarism Plagiarism is the presentation of someone else s ideas, words, or artistic, scientific, or technical work as one s own creation. Using the idea or work of another is permissible only when the original author is identified. Paraphrasing and summarizing, as well as direct quotations require citations to the original source. Plagiarism may be intentional or unintentional. Lack of dishonest intent does not necessarily absolve a student of responsibility for plagiarism. Students who are unsure how and when to provide documentation are advised to consult with their instructors. The library has guides designed to help students to appropriately identify a cited work. The full policy can be found on the BMCC s web site, 1.1 Scientific Method 15 18 1.2 Measurement and Scientific Notation 18 21 1.3 Measured Numbers and Significant Figures 21 24 1.4 Significant Figures in Calculations 24 27 1.5 Prefixes and Equalities 27 32 1.6 Writing Conversion Factors 32 37 1.7 Problem Solving 37 43 1.8 Density 43 49 Energy 2.1 Energy 56 59 2.2 Temperature 59 63 2.3 Specific Heat 63 67 2.4 Energy and Nutrition 68 71 2.5 Classification of Matter 72 74
2.6 2.7 States and Properties of Matter Changes of State 75 79 79 87 Atoms and Elements 3.1 Elements and Symbols 96 98 3.2 The Periodic Table 98 104 3.3 The Atom 105 107 3.4 Atomic Number and Mass Number 108 110 3.5 Isotopes and Atomic Mass 110 113 3.6 Electron Energy Levels 114 119 3.7 Electron Configurations 119 126 3.8 Periodic Trends 126 131 Nuclear Chemistry 4.1 Natural Radioactivity 139 143 4.2 4.3 4.4 Nuclear Reactions Radiation Measurement Half-Life of a Radioisotope 143 149 150 153 153 156 4.6 Nuclear Fission and Fusion 160 161 Compounds and Their Bonds 5.2 Ionic Compounds 174 176 5.3 Naming and Writing Ionic Formulas 176 179 5.4 Polyatomic Ions 180 183 5.5 Covalent Compounds 183 189 5.6 Naming and Writing Covalent Formulas 189 192 5.7 Electronegativity and Bond Polarity 192 195 5.8 5.9 Shapes and Polarity of Molecules Attractive Forces in Compounds 195 200 200 202 Alkanes 11.1 Organic Compounds 416 419
11.2 Alkanes 419 422 11.3 Alkanes with Substituents 423 429 11.4 Properties of Alkanes 429 434 11.5 Functional Groups 434-439 Chemical Reactions and Quantities 6.1 Chemical Reactions 211 216 6.2 Types of Reactions 216 221 6.3 Oxidation-Reduction Reactions 221 225 6.4 The Mole 226 230 6.5 Molar Mass 230 234 6.6 Mole Relationships in Chemical Reactions 235 237 6.7 Mass Calculations for Reactions 237 240 6.8 Energy Changes in Chemical Reactions 246 249 Gases 7.1 Properties of Gases 262 264 7.2 Gas Pressure 264 266 7.3 Pressure and Volume (Boyle s Law) 267 270 7.4 Temperature and Volume (Charles s Law) 270 273 7.5 Temperature and Pressure (Gay Lussac s Law) 273 276 7.6 The Combined Gas Law 276-277 7.7 Volume and Moles (Avogadro s Law) 277 281 7.8 The Ideal Gas Law 281 285 7.9 Partial Pressures (Dalton s Law) 285 289 Solutions 8.1 Solutions 296 300 8.2 Electrolytes and Non Electrolytes 300 304 8.3 Solubility 305 312 8.4 Percent Concentration 312 316
8.5 Molarity and Dilution 316 321 8.6 Physical Properties of Solutions 322 329 Biomolecules 15.1 15.5 Carbohydrates Disaccharides 543 545 557 563 17.1 Lipids 603 604 17.2 Fatty Acids 604 611 17.3 Waxes, Fats and Oils 611 614 19.1 Proteins and Amino Acids 673 677 19.3 19.4 Formation of Peptides Protein Structure: Primary and Secondary Levels 680 682 683-686 21.1 Components of Nucleic Acids 739 743 21.2 21.3 Primary Structure of Nucleic Acids DNA Double Helix 743 745 745-747 Chemical Equilibrium 9.1 Rates of Reactions 337 342 9.2 Chemical Equilibrium 342 344 9.3 Equilibrium Constants 344 348 9.4 Using Equilibrium Constants 349 353 9.5 Changing Equilibrium Conditions: Le Chatelier s Principle 353 362 Acids and Bases 10.1 Acids and Bases 372 377 10.2 Strengths of Acids and Bases 377 383 10.3 Ionization of Water 383 386 10.4 The ph Scale 386 393 10.5 Reactions of Acids and Bases 393 398 10.6 Acid-Base Properties of Salt Solutions 399 401 10.7 Buffers 401 405
Laboratory Syllabus Expt Title Page Laboratory Safety and Procedures 1 Measurement and Significant Figures 1 2 Conversion Factors in Calculations 11 3 Density and Specific Gravity 25 9 6 Energy and States of Matter Nuclear Radiation 85 51 7 Compounds and Their Formulas Electron Dot Structures and Molecular Shape 72 22 10 12 Structures of Alkanes Chemical Reactions and Equations Moles and Chemical Formulas 211 97 119 13 Gas Laws 129 16 Soluble and Insoluble Salts 159 15 Solutions, Electrolytes and Concentrations 147 11 Reaction Rates and Equilibrium 107 20 Acid-Base Titration 193