Chemistry 3 Syllabus Spring 2017

Transcription

1 Chemistry 3 Syllabus Spring 2017 Course Title: Chemistry Fundamental (Chemistry 3) Course Schedule: Lecture: Friday 9:00-1:05 pm Location: Lecture: MTSC 438 Required Textbooks: Introductory Chemistry; Charles Corwin, 7th Ed. Instructor: Edward Wen Edward.Wen@rcc.edu Office hour/location: By appointment Website: Supplemental resources: LEARNING OBJECTIVES Upon successful completion of the course, the student should be able to: 1. Solve basic and intermediate level problem (using formulae and unit analysis) relating to unit conversions, stoichiometry, gas law equations, concentrations of solutions. 2. Describe and apply a chemical vocabulary of approximately 200 words. 3. Apply the systematic IUPAC naming system to name inorganic compounds. 4. Relate chemical concepts to physical phenomena studied in the sciences. 5. Collect data using accurate qualitative observations and quantitative measurements of length, mass, temperature, and volume. 6. Analyze experimental results and relate them to the relevant concept. Course Goals: Chemistry is the study of matter and its transformations. A basic knowledge of chemical principles is important to understanding the physical world around us and to making informed decisions on important daily activities and public policy issues facing our society including those dealing with agriculture, medicine, energy use, food supply, water supply and the environment. A major goal of this course is to help the student improve their understanding of general chemical principles and increase their competence in the laboratory. Additional skills emphasized in this course include problem solving and data analysis. GRADING: 3 Exams (cumulative) 45% A % Quizzes (weekly) 10% B 80-89% Laboratory 25% C 70-79% Final Exam 20% D 60-69% Total 100% F 0-59% 1

2 COURSEWORK INFORMATION: EXAMS: There will be three midterm exams (150 pts each). They may cover any material previously discussed in the lecture or the laboratory, containing both standardized and Problem-solving questions. No exams may be made up without a doctor s note. The lowest exam score may be replaced with the final exam score if the final exam gives higher percentage score. QUIZZES: There will be eight quizzes (15 pts each) at the beginning of lecture (a total of 100 points + 5 extra credits) throughout the courses. No quiz may be made up and one lowest quiz score will be dropped. FINAL EXAM: The final exam is cumulative. WORKSHEET & HOMEWORK (not graded) There will be worksheets for each chapter. Make sure go over the worksheet before each quiz and exam. Most worksheet problems will be practiced, reviewed, and discussed after the chapter ends. Homework is your responsibility as it will not be collected nor graded. Homework provides extra practice so the effort you put into working homework problems will be reflected in your exam grades. ATTENTION TO EFFORT: Remember this is a 4-unit chemistry course meeting ONCE per week. It is your responsibility to review and continuously learn. Plan to join a study group during the week and spend an average of 3 to 5 hours per week in addition to the lecture and lab doing homework and studying chemistry. The last 20 minutes of lecture will be for individual discussion and you are welcome to ask for more help. REQUIRED SUPPLEMENTAL MATERIALS: A scientific calculator with log and exponential (scientific) notation is required. An example will be TI- 30X IIS as it is easy to use, inexpensive, and suffice the calculations required in this course. Language Translators and cell phones will not be allowed during exams. Please bring your textbook, calculator, and notebook to each lecture meeting. Buy a stapler if you don t already have one! ATTENDANCE: Attendance in lecture and laboratory is mandatory. Missing too many hours of lecture (and/or laboratory) may result in being dropped from the class by the instructor. TARDYS: Arriving late disrupts the class. Students are expected to arrive on time and ready to work. If you are unavoidably detained, respect your fellow students and instructor by entering the classroom quietly. If you are late to a quiz or exam, no extra time will be granted. CELL PHONES AND OTHER ELECTRONIC DEVICES: Cell phones and other electronic devices MUST be turned off during lecture. They are extremely disruptive to the class, so please respect your fellow students by turning them off. If you need to make a phone call, please feel free to excuse yourself from the classroom. Text messaging is NEVER appropriate in class. Please excuse yourself from the class if you feel the need to do so. ACADEMIC INTEGRITY: Cheating will not be tolerated. Copying another student s lab report, plagiarism, sharing exams etc. etc. etc. may result in a zero for the assignment, a grade of F in the course, or suspension from RCC. All cheating will be reported to the Dean of Student Services and will become part of your permanent record. 2

3 Tentative Lecture Schedule* (Feb 22, 2017) Week Start Date Chapter** Title 1 2/24 1,2 1. Introduction; PSS: Significant figures, Scientific notation 2. Metric System, Density. Heat calculations 2 3/3 3,4 Practice on your calculator Quiz 1 (PSS,Ch.2) 3. Matter and Energy: Atom, compound, mixtures; states of matter; Physical vs. chemical changes 4A. Atoms: subatomic particles; Isotopes 3 3/10 4,5 Quiz 2 (Ch. 2B,3) 4B: Atomic orbitals 5. Periodic trends 6. Ionic bonding and ionic compounds 4 3/17 5 Exam 1 (Ch. PSS, 2,3,4,5) 6. Naming of ionic compounds 5 3/24 6 Quiz 3 (common ions: name, formula, charge) 7. Chemical Reactions: balancing, double displacement 6 3/31 Holiday no class 4/7 6,7 Quiz 4 (Naming of ionic compound; balancing equation) 8. Mole, molar mass, mass% composition, empirical formula 7 4/14 Spring break 4/21 7,8 Quiz 5 (Ch. 8) 9. Stoichiometry: mole-mole; mass-mass, Limiting reactant 8 4/28 8 Exam 2 (Ch. 6,7,8) Review chapter 9 9 5/5 9 Quiz 6 (Ch. 9) 10. Gas laws; partial pressure 12A: Lewis Dot structures 10 5/12 10 Quiz 7 (Ch. 9B, 10) 12B: VSEPR 13A. Solutions: concentrations 11 5/19 12 Exam 3 (Ch. 8B, 9, 10, 12) 13B: dilutions, solution stoichiometry 12 5/26 12 Quiz 8 (Ch. 13) 14. Acids and Bases: ph scale; Titration; electrolytes; Buffers 13 6/2 13 Final exam 10:00 am 12:30 pm *Please Note: The schedule may change per instructor s discretion without written announcement. Please be on time to class or check course website to check any updates ( **The organization of chapters is based on the 7 th edition. 3

4 NOMENCLATURE For these elements, ions, and acids, you must know their names (spelling counts), symbols/formulas, and charge(s). In addition, you should be able to name any ionic or molecular compound consisting of these species. For the elements, you also need to know their classification (metal, nonmetal, metalloid). Common ionic charges are shown in parentheses. Alkali Metals Metalloids Noble Gases (Nonmetals) Halogens (Nonmetals) (form +1 cations) B He (form 1 anions) Li Si Ge Ne F* Na As Sb Ar Cl* K Te Po Kr Br* Rb Xe I* Cs Rn At Fr Polyatomic Ions + NH 4 ammonium Other Nonmetals Alkaline Earth Metals H 3 O + hydronium (form +2 cations) H (+1)* Be CH 3 COO acetate O (2)* Mg (or C 2 H 3 O 2 ) S (2) Ca CN cyanide Se (2) Sr OH hydroxide N (3)* Ba MnO 4 permanganate P (3) Ra NO 2 nitrite Acids Hydro---ic acid Transition Metals NO 3 nitrate HCl Ag (+1) HBr Cd (+2) HCO 3 hydrogen carbonate (bicarbonate) HI Zn (+2) HSO 4 hydrogen sulfate (bisulfate) HF Ni (+2) HCN Cu (+1, +2) Hg (+1, +2): Hg 2+ 2 ; Hg 2+ -ic acid (oxyacid): ClO 3 chlorate HNO 3 Fe (+2, +3) HClO 3 H 2 SO 4 H 2 CO 3 2 CO 3 carbonate H 3 PO 4 HC 2 H 3 O 2 (CH 3 COOH) 2 CrO 4 chromate HClO 4 2 Cr 2 O 7 dichromate 2 SO 4 sulfate -ous acid: 2 SO 3 sulfite H 2 SO 3 3 PO 4 phosphate HNO 2 HClO 2 4

5 Online resource, your best friend in Chem3: Significant Figures: Density: Naming: Naming: Naming: Mole: Balance equation: Lewis structure: Stoichiometry: Stoichiometry: Le Chatelier's: Gas law practice: Intermolecular force: Solution: ph calculations: 5