Chemistry 002 General Chemistry I Spring 2016

Chemistry 002 General Chemistry I Spring 2016 Mon, Wed, Fri 10:30 11:20am COB 102 Instructor: Gary Abel Email: gabel@ucmerced.edu Office hours: Mon & Fri 3:00 4:00pm, in SE1 room 300 Laboratory: Mon Fri in SE1 rooms 108 & 126 (see class schedule for specific times) Course description: Chem 2 is the first semester of the full year General Chemistry course sequence required for chemistry, physics, engineering and biological science majors. Students will learn the fundamental concepts and quantitative calculations relevant to the following topics: basic quantum theory related to atomic and molecular structure, chemical bonding, periodic properties, chemical reaction types, stoichiometric calculations, properties of gases, liquids, & solids, and thermochemistry. Prerequisites: A passing grade in Chemistry 001, OR passing the chemistry placement exam, OR a score of 3 or higher on the chemistry AP exam. Course Learning Outcomes and Relevant Program Learning Outcomes: Successful completion of each outcome will be assessed by performance on quizzes, exams, and reports. Upon successful completion of this course, students will be able to: Describe the structure of the atom and its relationship to the nuclear properties of isotopes; Apply the concepts of quantum theory for single and multi-electron atoms, valence bond and MO theories of bonding, and make predictions about atomic and molecular structure and properties; Derive the names and formulas of compounds based upon the IUPAC system of inorganic nomenclature for ionic and binary covalent compounds, as well as oxyacids; Determine empirical and molecular formulae from elemental analysis data, balance chemical equations, predict aqueous inorganic reaction products, and use stoichiometric relationships to calculate product and reactant amounts with applications to limiting reagents and percent yield; Analyze the energy change associated with chemical reactions, perform simple chemical thermodynamic calculations, and be able to apply these concepts to the first law of thermodynamics, heat capacity and calorimetry, enthalpy (including stoichiometric relationships) and Hess s law; Relate the physical properties of gases, liquids, and solids to interrelationships between kinetic molecular theory, structure, and intermolecular attractions; Perform basic chemistry laboratory techniques, use common laboratory instruments, record data and observations accurately, and describe sources of error and uncertainty in experimental data. This course is an introduction to all of the program learning outcomes (more detailed information on Chemical Sciences Program Learning Outcomes can be found in the UCM Catalog): PLO 1: Fundamental knowledge and skills PLO 2: Scientific methodology

PLO 3: Communication and teamwork skills PLO 4: Citizenship, ethics, and the role of chemistry in society Attendance: All students are required to attend every lecture and laboratory session. It is mandatory that every student performs at least 9 out of 11 laboratory experiments in order to receive a passing grade in the course. Excused absences may be granted in the case of a medical or family emergency if proper documentation is presented; however, missing more than 2 labs for any reason will result in a failing grade for the course. Laboratory experiments (and quizzes) can only be made up in the case of a valid emergency or University sanctioned event, and only with proper documentation. Required texts: Recommended: Required for lab: (items available at campus bookstore) Chemical Principles, 6 th Edition, by Atkins, Jones & Laverman W. H. Freeman and Co. New York Chem 2 Laboratory Manual, will be posted on the CatCourses site Chemical Principles Student Solutions Manual, 6 th Ed, by Hoeger, Lavelle & Ma W. H. Freeman and Co. New York American Chemical Society (ACS) General Chemistry Study Guide: http://chemexams.chem.iastate.edu/general chemistry Carbonless copy laboratory notebook Scientific calculator non graphing, non programmable (also for exams) Safety goggles with indirect vent splash protection (ANSI Z87.1 compliant) Lab coat Assignments and Examinations: Homework will be assigned weekly, but will not be collected for grading; essentially, the time and effort spent on the homework will translate into how well students perform on the quizzes and exams. There will be 2 in class midterm exams (see calendar, page 2) and a cumulative American Chemical Society (ACS) final exam on May 7 (8:00 11:00 am). Quizzes will be given at the beginning of each lab period, and lab reports will be due the following lab meeting after the experiment is performed. Late lab reports will lose 1 point per day late, and quizzes cannot be made up after the week in which they were given. The overall point breakdown is as follows: Assignment/Exam Points each Number Total pts Lab reports (best 10 of 11) 30 10 300 Quizzes (best 10 of 11) 20 10 200 Midterm Exams 150 2 300 ACS Final Exam 200 1 200 Overall total 1000 Grading Scale: Letter grades will be assigned according to the following scale: 100 80% 79.99 70% 69.99 60% 59.99 50% 49.99% or less A B C D F 100 95% = A+, < 95 85% = A, < 85 80% = A ; < 80 77% = B+, < 77 73% = B, < 73 70% = B ; etc...

Course Calendar: The following schedule is subject to change as the semester progresses (the dates of laboratory experiments will not change). Week Date Chapter(s) Lecture Topic(s) Midterm Lab Experiment Report due (in lab) Quiz (in lab) 1 1/18 Fund. A, B Atomic Theory No lab Mon holiday 2 1/25 Fund. CF Compounds, Moles Intro, safety ACS Diagnostic 3 2/1 1 Quantum Theory E1 Zinc Iodide Quiz 1 Fund. AF 4 2/8 2 Orbitals, Periodicity E2 Atomic emission Report 1 Quiz 2 Ch.1 5 2/15 3 Chemical Bonding No lab Mon holiday 6 2/22 34 Structure & Bonding E3 Atomic orbitals Report 2 Quiz 3 Ch.2 7 2/29 4 Valence & Molec. Orbitals E4 Molec. structure Report 3 Quiz 4 Ch.3 8 3/7 Fund. G, H Reactions MT 1 E5 Molec. orbitals Report 4 9 3/14 Fund. I, J, K Aqueous Reactions E6 Pigments Report 5 Quiz 5 Ch.4 10 3/21 No lecture Spring break No lab Spring break 11 3/28 Fund. L, M Stoichiometry E7 Copper cycle Report 6 Quiz 6 Fund. G, H 12 4/4 5 Properties of Gases E8 Alum Report 7 Quiz 7 Fund. I, J, K 13 4/11 5/8 Gases, Heat & Work E9 Charles' Law Report 8 Quiz 8 Fund. L, M 14 4/18 8 Thermochemistry MT 2 E10 Heat capacity Report 9 Quiz 9 Ch.5 15 4/25 8 Heat Capacity E11 Hess's Law Report 10 Quiz 10 Ch.8 16 5/2 6 IM Forces, Liquids & Report (Turn in report) Solids 11 Quiz 11 Ch.8 CatCourses learning management system: All students enrolled in the course will automatically be given access to the CatCourses site for the class. You can either log in to your MYUCMERCED portal (https://my.ucmerced.edu/) and click on the CatCourses link at the top on the right, or go directly to the CatCourses gateway: https://canvas.ucmerced.edu/. After logging in to CatCourses, click on the Courses tab at the top of the page and then select S16 CHEM 002 20 in the drop down menu to access the course site. You will find the course syllabus, laboratory manuals, quiz keys, TA office hours, lecture announcements, and any other necessary materials on the CatCourses site. All students should download the lab manuals for each experiment and save them to a disk as they become available. You will also want to download the quiz keys to help study for the exams. The CatCourses system, as you may have experienced, does crash from time to time, so you should not expect that it will be available at all times. Technical difficulties such as a website outage will not be accepted as an excuse for being unprepared for laboratory, quizzes or exams. Lecture Expectations: Lectures are meant to clarify and supplement the material in the textbook. Students are expected to have read the assigned textbook sections before coming to lecture. While using a laptop to take notes during lecture may seem like a good idea, research has shown that the

physical act of writing by hand actually enhances the learning process and retention of key concepts. Also, it can be distracting to students seated behind the screen, so those students that are planning on using computers in class should sit in the back of the room. Taking pictures of the screen with a cellphone or tablet is a poor substitute for taking good notes. All cellphones and other electronic devices must be silenced before coming to lecture. Any student disrupting the lecture will be asked to leave. In general, a majority of the class time will be spent reviewing key concepts and working example problems. Some portion of the class time will be dedicated to solving problems, where students will either work in groups, individually, or a combination of both. Students are responsible for learning all of the material in the assigned sections of the textbook, whether or not it was explicitly covered in lecture. Laboratory Expectations: As mentioned above, all students must complete 9 laboratory experiments at the very least in order to pass Chem. 2. Missing 3 experiments will result in an automatic failing grade in the course. Laboratory experiments cannot be made up after Friday during any given week. Each laboratory experiment will only be set up in the laboratory for one week, so by the next Monday, new equipment will be set up in the lab room and the previous experiment cannot be performed. All pre lab assignments must be completed before arriving to each laboratory meeting. Laboratory notebook data and lab reports must be hand written in pen in the lab notebook, and must be legible. Strict adherence to safety standards and protocols at all times is expected in the chemistry laboratory. Students will sign a contract in the laboratory stating that the safety rules are understood and will be followed while in the laboratory. Unexpected explosions, fires, and other chemical and physical surprises occur in chemistry laboratories all of the time; knowing how to react to a situation automatically is a result of training and experience, both of which your TA and laboratory staff have enough of to keep you safe, if you listen closely and follow their directions. Absence and Make Up Policies: In the event of an emergency or university sanctioned event, such as a conference, it may be possible to make up a missed lab section if supporting documentation is provided. Please note that emergencies do not include transportation issues such as traffic or car trouble; many alternative transportation options are available, and you should leave early with plenty of extra time just in case something comes up. Emergencies include incapacitating injury or illness (of the student), the funeral of a family member, or other unforeseen circumstance, out of the student s control, which makes it impossible to attend the regularly scheduled lab section. In the case of a legitimate emergency, with supporting documentation, a make up lab may be scheduled with another lab TA during the same week while that particular experiment and quiz are being performed. This is at the discretion of the TA and depends upon available space in the lab (24 student capacity). Always CC (carbon copy) the TA of the section you are registered in on all email correspondence when attempting to arrange a make up lab. If the emergency prevents the student from being able to make up the lab, that student will receive the average of their scores on the rest of the labs and quizzes, after the lowest scores are dropped, for the missed lab, at the end of the semester. If an excused absence prevents a student from taking a midterm (midterm exams cannot be made up or rescheduled), that student will receive the score that they earn on the final exam, in place of the missed exam score. Please remember that as a condition of any excused absence, documentation of the reason for the absence must be provided. The final exam cannot be rescheduled or taken at a different time or place than that scheduled by the Registrar s office before the semester begins. If a student misses the final exam for a legitimate reason (e.g. medical or family emergency), that student will receive an incomplete (I) grade for the course and will have to take the final exam with the class at the end of the following semester. Unexcused absences from any exam will result in a 0 score on the exam.

Student Learning Outcomes: Upon successful completion of this course, students will have gained the ability to: describe the different subatomic particles and how they make up the structures of atoms and isotopes; explain the concepts of quantum theory applied to single and multi electron atoms, valence bond and molecular orbital theories of chemical bonding, and how they lead to atomic & molecular structure and properties; derive the names and formulas of chemical compounds using the IUPAC system of nomenclature for ionic compounds, polyatomic ions, and covalent molecules; determine the empirical and molecular formulae of compounds from elemental analysis data, balance chemical reactions, categorize reactions and predict products for redox, acid/base, and precipitation reactions, and use stoichiometry and the limiting reactant concept to calculate percent yield & product/reactant amounts; analyze energy changes associated with chemical reactions, perform simple thermodynamic calculations related to heat capacity, calorimetry, and Hess Law; relate the physical properties of gases, liquids, and solids to their structure and underlying intermolecular interactions; perform basic chemistry laboratory techniques using common laboratory equipment, record data and observations accurately, and describe sources of error and uncertainty in experimental data. Student Learning Outcomes will be assessed by student performance on quizzes, exams, and lab reports. Academic Support Services: Academic Support Services are designed to provide equal access to the instructional learning environment for all qualified students with disabilities deemed eligible to receive academic adjustments according to the implementing regulations of Section 504 of the Rehabilitation Act of 1973 and the Americans with Disabilities Act (ADA) of 1990. To be eligible for academic adjustment services, students must provide appropriate documentation according to UC documentation of disability guidelines. Each service must be approved by Disability Services and is generally tailored to the individual need of each student. Please see the Academic Support Services website for more information: http://disability.ucmerced.edu/node/3 Academic Honesty: All students are expected to follow the student code of conduct regarding academic honesty. Please read the UC Conduct Standards on the Student Judicial Affairs website: http://studentlife.campuscms.ucmerced.edu/content/uc conduct standards From this page, students should also download the document describing Academic Honesty: http://studentlife.ucmerced.edu/sites/studentlife.ucmerced.edu/files/documents/ucm_student_org_p olicies_regs_6_10_14_r.3_.pdf If any instances of cheating or misrepresentation are found to have occurred, Student Judicial Affairs will be notified and discipline will be handled by their office. No first time warnings will be given; cheating is cheating, no matter how slight the infraction. All work handed in for credit must be performed by the individual student, and in their own words this applies to lab reports, pre lab write ups, and quizzes. During all exams, no electronic devices will be allowed other than a nongraphing, non programmable calculator. Students will need to leave their cell phones, laptops, tablets, etc. in their backpacks at the side or back of the room.

Chem 2 and 2H Learning Outcomes Successful completion of each outcome will be assessed by performance on quizzes, exams, and reports. Upon successful completion of this course, students will be able to: Describe the structure of the atom and its relationship to the nuclear properties of isotopes; Apply the concepts of quantum theory for single and multi-electron atoms, valence bond and MO theories of bonding, and make predictions about atomic and molecular structure and properties; Derive the names and formulas of compounds based upon the IUPAC system of inorganic nomenclature for ionic and binary covalent compounds, as well as oxyacids; Determine empirical and molecular formulae from elemental analysis data, balance chemical equations, predict aqueous inorganic reaction products, and use stoichiometric relationships to calculate product and reactant amounts with applications to limiting reagents and percent yield; Analyze the energy change associated with chemical reactions, perform simple chemical thermodynamic calculations, and be able to apply these concepts to the first law of thermodynamics, heat capacity and calorimetry, enthalpy (including stoichiometric relationships) and Hess s law; Relate the physical properties of gases, liquids, and solids to interrelationships between kinetic molecular theory, structure, and intermolecular attractions; Perform basic chemistry laboratory techniques, use common laboratory instruments, record data and observations accurately, and describe sources of error and uncertainty in experimental data. Mapping to Chemistry Major Program Learning Outcomes: Key: Mastery [M], Developed [D], and Introductory [I] level of understanding; Not Applicable [NA] [I] PLO 1-Fundamental knowledge and skills [I] PLO 2-Scientific methodology [I] PLO 3-Communication and teamwork skills [I] PLO 4-Citizenship, ethics, and the role of chemistry in society General Education Guiding Principles Addressed by Chem 2 and Chem 2H: Scientific Literacy Decision Making Ethics and Responsibility

General Education Guiding Principles Addressed by Chem 2 and Chem 2H: I. Scientific Literacy The atomic and molecular theory of matter taught in Chem 2/2H is the underlying principle for our understanding of all chemistry and biochemistry. A knowledge of how molecular composition and structure lead to different chemical properties and a basic grasp of the laws governing the chemical states and changes, are foundational to understanding how the modern world works. II. III. Decision Making A central theme of Chem 2/2H is the use of theoretical models and empirical data to make predictions about how physical and chemical processes will behave under different conditions. (e.g., Will a reaction occur spontaneously?, Will a chemical process emit or absorb heat?, or How much usable energy can be extracted from a chemical reaction? ) Such quantitative predictions and observations are playing an increasing role in decision making at all levels. For example: How do the fundamental energy capacities of hydrogen vs petroleum fuels affect their feasibility for their use in transportation? or Why are even trace amounts of halogen-containing refrigerants dangerous to the ozone layer? Ethics and Responsibility In the 21 st century, many of the most challenging ethical questions are occurring at the intersection of human values and scientific capabilities, and in many cases at least a basic understanding of chemistry is important to grasp the relevant issues. For example, Why is lead a much more pernicious toxin than organic compounds? Moreover, fulfilling our responsibility for the increasing impact of human activities on global ecosystems and climate, is increasingly dependent society s ability to evaluate scientific (and often chemical) arguments calling for economic or political change. For example, Why does carbon dioxide act as a carbon sink, and how does it affect both the acidity of the oceans and the heating of the planet?