SOUTHERN CALIFORNIA UNIVERSITY OF HEALTH SCIENCES COLLEGE OF SCIENCE AND INTEGRATIVE HEALTH DIVISION OF PROFESSIONAL STUDIES INSTITUTE OF SCIENCE

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1 COURSE INFORMATION SOUTHERN CALIFORNIA UNIVERSITY OF HEALTH SCIENCES COLLEGE OF SCIENCE AND INTEGRATIVE HEALTH DIVISION OF PROFESSIONAL STUDIES INSTITUTE OF SCIENCE Course Title: Course Number(s): Term: General Chemistry II - LECTURE CHEM216 FA2018 Time Requirement: (hours/week) Lecture Hours: 45 Total Units: 3 Prerequisites: High School Diploma or equivalent. Successful completion of General Chemistry I or its equivalent Faculty: Lead Faculty: Okezie Aruoma Contact Information: okeziearuoma@scuhs.edu Office Hours: TBD Faculty Assisting in the Course: TBD COURSE PURPOSE Course Description: The General Chemistry 2 course further develops the concepts of chemical bonding in order to appreciate the size, shape, polarity and macroscopic behavior of molecules. The processes of oxidation-reduction will be explained, particularly as they apply to biological systems. Solution chemistry will be introduced, stressing the concepts of equilibriums and colligative properties. Acid/base chemistry, including titrimetry, buffers, and ph will be studied. Nuclear chemistry in the evolution of matter will be considered. Organic chemistry will be introduced as a corollary to concepts presented in the college chemistry course. University Learning Outcomes: 1. Evidence-Based Knowledge: The student will utilize foundational health science knowledge; and critically appraise and apply relevant scientific literature in professional healthcare practice. 2. Communication: The student will effectively engage patients/clients, colleagues, and the public using appropriate verbal, non-verbal, and written communication. 3. Professionalism: The student will demonstrate leadership, integrity, respect, and self-reflection while employing ethical and legal standards in professional and community interactions. 4. Integrative Healthcare: The student will serve as an effective member of a healthcare team, collaborating with other professionals to improve community health and patient outcomes for the health of individuals and the community. GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 1 P a g e

2 General Chemistry II Program Learning Outcomes: 1. Basic Science Knowledge: The course will begin with a review of some of the major concepts in general chemistry. Students will become proficient in problem solving through calculations, interpreting data and applying efficient methods of analysis. The analytical and quantitative skills will be applicable in future courses. Students will complete activities in lab and submit pre-lab and post-lab assignments summarizing key points of laboratory activities. 2. Scientific Reasoning: This class introduces students to more physiological knowledge through laboratory assessments as well as theoretical knowledge that can be utilized in future testing of claims and assessing accuracy of other people s assertions. 3. Information Literacy: Textbook reading is assigned and students are required to do many hours of independent learning. By asking questions on readings and outside learning, to professors and peers, students will gain more knowledge on how to find and assimilate important information from sources. 4. Communication Effectiveness: Through the utilization of in class discussions, lab reports, online discussion board posts and responses, and the portfolio project, students will learn how to share ideas and give constructive criticisms. Peer and professor critiques will help students grow to become more effective collaborators and communicators. Course : The general objective of this course is to prepare students for future courses involving chemical concepts whether in chemistry, physics, biology, earth science or engineering. To do so, students will be introduced to the content of inorganic chemistry, laboratory practices and equipped with an understanding of the language (write/verbal, mathematical, graphic) of chemistry. At the end of this course, students will be able to: 1. Describe the nature of chemical bonding and describe the types of chemical bonds using Lewis structures, electro-negativity, bond order, bond energies, molecular dipoles and the shape of simple inorganic molecules. 2. Explain how temperature affects intermolecular forces in both liquid and solid states. 3. Understand colligative properties and the fundamentals of osmotic pressure. 4. Classify acids and bases, explain the concept of ph, as well as acid/base equilibria, buffer solutions, and titration curves. 5. Interpret reaction rates, laws, simple reaction mechanisms and chemical equilibrium. 6. Evaluate solubility and complex ion equilibria. 7. Analyze thermodynamics and equilibria. 8. Comprehend oxidation-reduction reactions, electrochemistry and nuclear chemistry. INSTRUCTIONAL MATERIALS Required Text(s): Chemistry: A Molecular approach plus Mastering Chemistry with etext, 3rd Ed., by Tro, Vincent & Libingston (ISBN: ) Classroom Expectations: Please be professional, prompt, prepared, and polite at all times. The professor will adhere to all polices as found in the Student Handbook Cellular phones must be kept on silent during class and lab times. GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 2 P a g e

3 Students may not use a phone as a calculator. As a safety precaution, no food or drinks are allowed inside the lab, but there will be a designated break for eating and drinking outside of the lab. TEACHING METHODS AND ACTIVITIES There are 12 hours of lecture each week for 4 weeks. The lectures will be held on Thursdays and Fridays from 4:00pm to 9:30pm of the first week and on Thursdays and Fridays at 4:50pm to 9:30pm of the 2 nd to the 4 th week. Final exam (Exam 4) will take place on Wednesday afternoon at 3:30pm following the fourth week of courses. Best Practices for studying General Chemistry II: Read before and read after each class. Skim the chapter before it is covered in lecture in order to become comfortable with some of the terms associated with each topic. Review each chapter after it is covered in class to enhance your understanding of what was covered in class. Participate during class by taking notes during class and looking over them afterwards. Don't skip class, arrive late, or leave early. Ask questions for clarification when you don t understand the material. Stay on top of the homework and assignments. Do the assigned problems as close to the time as when the topic is covered in the class to increase the depth of your understanding of specific concepts and will help you learn the material more efficiently and effectively. Do not wait until the night before the homework is due to start the assignment. You will get more out of it if you take the time to really learn the concepts and review the material without being rushed. Find a group of students to study with. Seek out students dedicated to doing well in the course. This makes studying more fun and also helps you learn the material better by teaching what you know and learning from your peers what you don t know. Explaining these concepts to others will help you learn the material even better. Stay focused by finding an environment where you can study with few distractions. EVALUATION OF STUDENT LEARNING Grading procedures: Student assessments may include self-assessments, peer assessments, and instructor assessments. The format of these assessments may include multiple choice, essay, short answer, or fill-in examinations; special individual or group projects; or practical examinations, etc. Assessment Weight/%/Points Homework and Class 10% Participation Exam 1 20% Exam 2 20% Exam 3 20% Final Exam (Exam 4) 30% GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 3 P a g e

4 Grading scale: Letter grades will be assigned only at the end of the trimester. A = 90% to 100% B = 80% - less than 90% C = 70% - less than 80% D = 60% - less than 70% F = less than 60% I = Incomplete W = Withdrawal University Policies Students are expected to spend at least two hours for each lecture or practicum hour and one hour for every two laboratory hours of course time per week in activities and assessments outside the classroom. Examples of activities include, but are not limited to: writing papers; reading articles or text; small group work; presentations; completing assignments; preparation for assessments; online activities and other activities that do not include direct instructor interaction and involvement. All university policies apply to this course and all others. For full policy information please consult the university SCU Policy Manual. For a quick reference guide to the following policies: make-up examination, grade posting, results of failing grades, student support information, syllabus amendments, special needs, student conduct, and attendance, please consult the academic policies document housed on the Online Student Services [the preceding is a hyperlink]. However for this course, there will be no make exams. Withdrawal: Students can withdraw from any IoS course by submitting a formal withdrawal online. The student withdrawing from a course must log in to the MySCU portal and click on the "Drop Course" link and complete the course drop request. An confirming the drop request will be sent to the student, acknowledging the withdrawal. Disability: In keeping with the Americans Disabilities Act of 1990, SCU will accommodate a student s known physical or mental limitations in order to enable him or her to perform the essential functions of the curriculum, to the extent the necessary accommodations are reasonable and do not impose undue hardship to the University. Interested students should request information regarding the services offered by the University. The Learning Resource Specialists are located in the library and can assist with the documentation required to access special services due to disabilities. Academic dishonesty: Students are expected to adhere to the highest standards of academic honesty. In this class, cheating will not be tolerated. Plagiarism includes passing someone else s ideas off as your own without citing proper credit. Cheating includes looking at another student's test during an exam, allowing other students to copy your work, use of unauthorized materials during an exam, presenting lab reports that are not your original work, and recording laboratory data that was not actually observed. These are all prohibited in this program. Collaboration and discussion are encouraged, but it is important for each GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 4 P a g e

5 student to individually complete each assignment. Any student who is academically dishonest can receive a failing grade. COURSE SCHEDULE Pre-class assignments: Any pre-class assignments are to be completed by each student prior to attending class on Saturday. These assignments must be typed or hand written (must be legible) and physically turned in at the beginning of class. Week One Understand type of chemical bonds and Lewis Structures Understand VSEPR theory and molecular shapes Electronegativity and polarity Investigate molecular orbital theory Evaluate intermolecular forces Examine trends in melting and boiling points Analyze phase diagrams Identify the types of solutions Understand surface tension Express solution concentration numerically Textbook Read Chapters 9 and 11 Homework Introduction: Course Orientation, Polarity and Dipoles, Lewis structures, Molecular shapes, VSEPR Theory, Bond Order, Types of Intermolecular Forces, Phase Diagrams Properties of Solution, Colligative Properties: Freezing Point Depression and Boiling Point Elevation, Molality, Solubility, Saturation, Supersaturation, lattice structures Homework problems will be given in class Exam 1* There will be an exam covering all week 1 lecture material Week 2 Thursday 20% Week Two Define Reaction Kinetics, Categorize colligative properties, Calculate rates of chemical reactions, GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 5 P a g e

6 Define the rate law, Investigate the effect of temperature on reaction rate, Understand catalysis Describe the equilibrium constant K Find equilibrium concentrations Predict the direction of change using the reaction quotient Discover how a system at equilibrium responds to change Apply Le Chatelier's Principle Consider the effects of free energy in chemical reactions Explore the laws of thermodynamics Textbook Read Chapters Rates, Rate Laws, Reaction Order, Equilibrium Constants, Kinetic Calculations, Reaction Quotients, Catalysis, Le Chatelier's Principle Entropy, Gibbs Free Energy, Spontaneity, solubility and energetics of solutions, freezing point depression and boiling point elevation, reaction mechanisms, catalysis, state of matter and the equilibrium constant Homework Homework problems will be assigned in class website Exam 2* There will be an exam covering all week 2 lecture material Week 3 Thursday 20% Week Three Describe the nature of acids and bases Classify acid strength using Ka Investigate the autoionization of water Calculate ph levels Examine buffer solutions Perform titrations Analyze ph curves Explore electrochemistry Balance oxidation-reduction equations Classify the 3 different types of cells Calculate standard electrode potentials Textbook Read chapters Acid/Base Definitions, Relative Strengths, Calculations using Ka, pka, ph, poh, Buffers, Titrations, Electrochemistry, Voltaic and Electrolytic Cells Oxidation-Reduction Half Reactions, Standard Electrode Potential Calculations, autoionization of water and ph, Lewis acids and bases, Determine the overall acidity or basicity of salt solution GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 6 P a g e

7 Homework Homework and worksheet assignment will be given in class Exam 3* There will be an exam covering all week 3 lecture material Week 4 Thursday 20% Week Four Understand spontaneous and non-spontaneous processes Explain entropy and the second law of thermodynamics Understand heat transfer Explain changes in entropy of the surroundings Understand balancing oxidation-reduction equations Understand voltaic cells and electricity generation Explain standard electrode potentials Explain electrolysis and corrosion Assess nuclear chemistry Categorize types of radioactivity Calculate rates of decay Textbook Read Chapters Homework Exam 4* Spontaneous and non-spontaneous processes, entropy and the second law of thermodynamics, heat transfer and changes in entropy of the surroundings, balancing oxidation-reduction equations, voltaic cells and electricity generation, standard electrode potentials, electrolysis and corrosion, nuclear chemistry, radioactivity, rates of decay Homework and worksheet assignment will be given in class A Final exam covering all material from Week 4 and reflecting on the Wee1 through Week 3 take place on the Wednesday immediately following Week 4. Wednesday 30% *The will be NO make exam IoS (SS): General Chemistry 2 CHEM 216 Syllabus prepared by: Okezie Aruoma Revised: 1/30/18 GENERAL CHEMISTRY 2 CHEM 216 Chemistry Lecture ARUOMA 7 P a g e

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