CHE 121 Fundamentals of General, Organic and Biological Chemistry I 2010 SYLLABUS AND COURSE OUTLINE

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1 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) , x5082 Room: N661 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: ISBN-13: 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: ISBN-13: E. Use of Technology Computer with internet service is required to access most of the course materials.

2 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 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: % % 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

3 G. Other Resources Tutoring is available at the Science Learning Center (N734) and Science Resource Center (S500) E-tutoring service is available at Tech support is 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 # ). 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 Measurement and Scientific Notation Measured Numbers and Significant Figures Significant Figures in Calculations Prefixes and Equalities Writing Conversion Factors Problem Solving Density Energy 2.1 Energy Temperature Specific Heat Energy and Nutrition Classification of Matter 72 74

4 States and Properties of Matter Changes of State Atoms and Elements 3.1 Elements and Symbols The Periodic Table The Atom Atomic Number and Mass Number Isotopes and Atomic Mass Electron Energy Levels Electron Configurations Periodic Trends Nuclear Chemistry 4.1 Natural Radioactivity Nuclear Reactions Radiation Measurement Half-Life of a Radioisotope Nuclear Fission and Fusion Compounds and Their Bonds 5.2 Ionic Compounds Naming and Writing Ionic Formulas Polyatomic Ions Covalent Compounds Naming and Writing Covalent Formulas Electronegativity and Bond Polarity Shapes and Polarity of Molecules Attractive Forces in Compounds Alkanes 11.1 Organic Compounds

5 11.2 Alkanes Alkanes with Substituents Properties of Alkanes Functional Groups Chemical Reactions and Quantities 6.1 Chemical Reactions Types of Reactions Oxidation-Reduction Reactions The Mole Molar Mass Mole Relationships in Chemical Reactions Mass Calculations for Reactions Energy Changes in Chemical Reactions Gases 7.1 Properties of Gases Gas Pressure Pressure and Volume (Boyle s Law) Temperature and Volume (Charles s Law) Temperature and Pressure (Gay Lussac s Law) The Combined Gas Law Volume and Moles (Avogadro s Law) The Ideal Gas Law Partial Pressures (Dalton s Law) Solutions 8.1 Solutions Electrolytes and Non Electrolytes Solubility Percent Concentration

6 8.5 Molarity and Dilution Physical Properties of Solutions Biomolecules Carbohydrates Disaccharides Lipids Fatty Acids Waxes, Fats and Oils Proteins and Amino Acids Formation of Peptides Protein Structure: Primary and Secondary Levels Components of Nucleic Acids Primary Structure of Nucleic Acids DNA Double Helix Chemical Equilibrium 9.1 Rates of Reactions Chemical Equilibrium Equilibrium Constants Using Equilibrium Constants Changing Equilibrium Conditions: Le Chatelier s Principle Acids and Bases 10.1 Acids and Bases Strengths of Acids and Bases Ionization of Water The ph Scale Reactions of Acids and Bases Acid-Base Properties of Salt Solutions Buffers

7 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 Energy and States of Matter Nuclear Radiation Compounds and Their Formulas Electron Dot Structures and Molecular Shape Structures of Alkanes Chemical Reactions and Equations Moles and Chemical Formulas Gas Laws Soluble and Insoluble Salts Solutions, Electrolytes and Concentrations Reaction Rates and Equilibrium Acid-Base Titration 193

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