AP Chemistry Syllabus

Transcription

1 Instructor Information: AP Chemistry Syllabus Teacher: James Poindexter Room: Belle Vernon Area High School, Room 412 Contact: Phone: ; ext Website: Required Text: Additional Resources: Tro; Chemistry: A Molecular Approach AP Edition 3e 2014 with MasteringChemistry (etext on ipad) itunes U course (see teacher for enrollment code) Mastering Chemistry program (see teacher for code) Course Description: This AP Chemistry course is designed to be the equivalent of the general chemistry course usually taken during the first year of college. For most students, the course enables them to undertake, as a freshman, second year work in the chemistry sequence at their institution or to register in courses in other fields where general chemistry is a prerequisite. This course is structured around the six big ideas articulated in the AP Chemistry curriculum framework provided by the College Board. [CR2] A special emphasis will be placed on the seven science practices, which capture important aspects of the work that scientists engage in, with learning objectives that combine content with inquiry and reasoning skills. During the year students will use demonstrations and other simulations that work with course content in ways that cannot easily be duplicated in the lab [CR3]. AP Chemistry is open to all students that have completed a year of chemistry who wish to take part in a rigorous and academically challenging course. This course can be taken either after or along with a full year Organic Chemistry course for additional work with the concepts, reactions, and processes from organic chemistry. To keep the students in the cumulative mindset needed to prepare for the AP exam, as well as exams in a university setting, there will be a weekly quiz in non-test weeks on the last student day of the week and each unit exam administered will have questions from previous units included. Students will also take part in discussions that will relate topics covered to real world applications of the concepts [CR4].

2 Course Objectives (see AP Chemistry Curriculum Framework from College Board) e_fall_2013_lkd.pdf By the end of this course, students should be prepared to take the AP chemistry exam offered by the College Board. Course Outline: 1.0 Lab Safety, lab equipment, reading a grad cylinder correctly 1.2 Scientific Method 1.3 Classification of matter (heterogeneous, homogeneous, element, compound, substance vs. mixture) 1.4 Chemical vs. physical Changes 1.5 Energy 1.6 SI Units, Density, Unit conversions, metric system 1.7 Significant Figures 1.8 Unit conversions, dimensional analysis Atomic Theory 2.5 Structure of the Atom 2.6 P, N, E, Isotopes, Ions 2.7 Families on the Periodic Table 2.8 Average atomic mass 2.9 Molar Mass and Mole Conversions *Mass Spectrometry 3.2 Ionic vs. Covalent Bonding 3.3 Chemical formulas and molecular models 3.4 Atomic-level View of Elements and Compounds 3.5 Ionic Nomenclature, Writing Formulas 3.6 Covalent Nomenclature, Acid Nomenclature 3.7 Summary of Nomenclature 3.8 Molar Mass and Mole Conversions 3.9 % by mass 3.10 Empirical and Molecular Formulas 3.11 Balancing Equations

3 3.12 Organic Compounds 4.2 Stoichiometry 4.3 Limiting reactant, theoretical yield, percent yield 4.4 Solution Concentration (Molarity, Dilution), solution stoichiometry 4.5 Electrolytes vs. non-electrolytes (solubility) 4.6 Precipitation reactions 4.7 Molecular, Ionic, Net ionic equations 4.8 Acid-Base/Gas-evolution reactions 4.9 Redox Reactions Pressure 5.3 Gas Laws 5.4 Ideal Gas Law 5.5 Molar Volume, Density, Molar Mass 5.6 Partial Pressure 5.7 Gas Stoichiometry and Molar Volume 5.8 KMT 5.9 Diffusion/Effusion 5.10 Real Gases, IMF s Nature of Energy/Definitions st Law of Thermodynamics 6.4 Heat and Work 6.5 Measuring Energy 6.6 Enthalpy 6.7 Measuring delta H 6.8 Relationships involving delta H 6.9 Enthalpies of Reaction from enthalpies of formation The Nature of Light 7.3 Atomic Spectroscopy and the Bohr Model 7.4 Wave Nature of Matter 7.5 Quantum mechanics and the atom 7.6 Shapes of Atomic Orbitals *Beer s Law Development of the Periodic Table 8.3 Electron Configurations 8.4 Electron Configurations, Valence Electrons 8.5 Quantum-Mechanical Model 8.6 Periodic Trends

4 8.7 Ions-Trends 8.8 Electron Affinities 8.9 Examples of Periodic Behavior *PES, Coulomb s Law Types of Chemical Bonds 9.3 Valence Electrons as dots 9.4 Ionic Bonding-Lewis symbols and Lattice energies 9.5 Covalent bonding-lewis Structures 9.6 Electronegativity and Bond Polarity 9.7 Lewis Structures of Molecular Compounds and Polyatomic Atoms 9.8 Resonance and Formal Charge 9.9 Exceptions to the octet rule 9.10 Bond Energies and Bond Length 9.11 Bonding in Metals-Electron Sea Model 23.4-Alloys 10.2-VSEPR-Shapes 10.3 VSEPR-Lone Pairs 10.4 VSEPR-Molecular Geometries 10.5-Molecular Shape and Polarity 10.6-Valence bond theory-orbital overlap 10.7-Hybridization 10.8-Molecular orbital theory 11.2-Solids, liquids, gases 11.3-IMF s 11.4-Surface tension, viscosity, capillary action 11.5-Vaporization and vapor pressure Sublimation and fusion 11.7-Heating Curve for Water 11.8-Phase Diagrams 11.9-Water X-ray crystallography Crystalline solids-unit cells Types of Crystalline Solids Band Theory (Semiconductors) *Chromatography (in relation to IMF s) Types of Solutions and Solubility 12.3-Energetics of Solution Formation 12.4-Solution Equilibrium and Factors affecting solubility 12.5-Expression Solution concentration

5 12.8-Colloids Colligative Properties *Beer s Law 13.2-Rate of a chemical reaction 13.3-Rate Law 13.4-Integrated Rate Law 13.5-Effect of Temperature on Reaction Rate 13.6-Reaction Mechanisms 13.7-Catalysis Dynamic Equilibrium 14.3-Equilibrium Constant 14.4-Expressing the equilibrium constant in terms of pressure 14.5-Heterogeneous equilibria: reactions involving solids and liquids 14.6-Calculating Equilibrium constant from measured equilibrium concentrations 14.7-Reaction Quotient 14.8-Finding Equilibrium Concentrations 14.9-Le Chatelier s Principle Nature of Acids and Bases 15.3-Definitions of Acids and Bases 15.4-Acid Strength and Ka 15.5-Autoionization of water and ph 15.6-Finding [H3O+] for strong and weak acid solutions 15.7-Base Solutions 15.8-Acid-base properties of Ions and Salts 15.9-Polyprotic Acids Acid Strength and Molecular Structure Lewis Acids and Bases Acid Rain 16.2-Buffers (Henderson-Hasselbach) 16.3-Buffer Capacity 16.4-Titrations and ph Curves 16.5-Solubility Equilibria (Ksp) 16.6-Precipitation (selective precipitation) 16.7-Qualitative Chemical Analysis 17.2-Spontaneous (Favorable) vs. Non-spontaneous Entropy and 2 nd law of thermodynamics 17.4-Heat Transfer and Changes in the Entropy of the Surroundings

6 17.5-Gibbs Free Energy 17.6-Entropy Changes, Calculating delta S *Maxwell-Boltzman distribution 17.7-Free Energy, Calculating delta G 17.8-Free Energy Changes in non-standard states 17.9-Free Energy and Equilibrium Chapter 20 Organic chemistry-nomenclature Organic chemistry-functional groups Polymers Biomolecules/Polymers with IMF s 18.2-Balancing Redox Equations 18.3-Voltaic Cells 18.4-Standard Electrode Potentials 18.5-Cell Potential, Free Energy, and the Equilibrium Constant 18.6-Cell Potential and Concentration 18.7-Batteries 18.8-Electrolysis 18.9-Corrosion AP chemistry exam review!!! May 4-AP chemistry exam Possible Lab Experiments: The laboratory component of this course may include the following experiments (but is not limited to) [CR5b and CR6]: Traditional Labs: [Science Practices in brackets] 1. Safety in the lab (proper use of equipment) 2. Accuracy and precision in measurements [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 3. Water of crystallization and formula of a hydrate [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 4. Evidence of a chemical change and energy changes in chemical reactions [4.3, 4.4, 5.1, 5.2, 5.3] 5. Percent oxygen in potassium chlorate [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 6. Flame tests and spectroscopy [1.2, 4.3, 5.1, 5.2, 5.3] 7. Molecular modeling to show molecular geometries [1.1, 1.3] 8. Analysis of a sodium bicarbonate-sodium chloride mixture [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 9. Finding the ratio of reactants in a chemical reaction (Stoichiometry of a reaction) [1.4, 2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3]

7 10. Reacting ionic species in aqueous solution [4.3, 5.1, 5.2, 5.3] 11. Molecular mass of a volatile liquid [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 12. Graham s law [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 13. Titration experiment [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 14. Standardization of a base and then an acid [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 15. Analysis of a commercial bleach [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 16. Determination of an equilibrium constant [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 17. K sp of an ionic compound [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 18. Determination of the dissociation constants of weak acids [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 19. Kinetics of a reaction [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 20. Redox titration with potassium permanganate [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] 21. Electrochemical cells [1.2, 1.3, 1.4, 4.3, 5.1, 5.2, 5.3] 22. Thermochemistry and Hess s law [2.1, 2.2, 2.3, 4.3, 5.1, 5.2, 5.3] Guided-inquiry labs: [3.1, 3.2, 3.3, 4.1, 4.2, 4.4, 6, 7.2] 1. How Can Color Be Used to Determine the Mass Percent of Copper in Brass? 2. How Much Acid Is in Fruit Juices and Soft Drinks? 3. How Can We Determine the Actual Percentage of H 2O 2 in a Drugstore Bottle of Hydrogen Peroxide? 4. The Hand Warmer Design Challenge: Where Does the Heat Come From? 5. Can We Make the Colors of the Rainbow? An Application of Le Châtelier s Principle 6. To What Extent Do Common Household Products Have Buffering Activity? 7. Photoelectric spectroscopy AP 1-to-1 Initiative As an AP student, you have been issued an ipad mini for class use, which is a privilege and a responsibility. Bring your device fully charged daily. Loss of class points and possible disciplinary referral will result from failure to bring your device to class or inappropriate use of it (games, social media, etc). Remember, your ipad is your responsibility; however, it is the property of the BVA School District, and its content may be viewed by administration at any time. Also, be advised that you are financially responsible for loss or damage to the device. Academic Honesty: Any work submitted by the student shall be his/her own. Work taken from others shall be deemed as unacceptable. Any doubts will initiate the completion of an alternative assignment or a zero on the required effort, depending on the severity of the infraction.

8 Class Policies and Expectations: Classroom and Laboratory Expectations 1. Be on time and prepared for class (ipad, notebook, homework, pen, pencil, calculator, etc.) 2. No food or drink. 3. No horseplay. 4. Respect others, their property, and this classroom. Academic Expectations All students are expected to participate in classroom activities and labs and to complete homework assignments. Success in chemistry requires practice. Each assignment is designed to help you succeed in this class. Therefore, you will be held accountable for completing every assignment. Homework may be graded on accuracy, completeness, or both. Homework is due at the beginning of class. Class begins when the bell rings, and the expectation is that all students are in their seats and ready to work. There will be a warm-up each day, which students are to begin as they enter the room. If I see or hear your cell phone or ipod, I will take it off of you and give it to administration. Assignments are due at the beginning of class. Points will be deducted from your score if the assignment is turned in late. Late Work With an excused absence, students have the same number of days to make-up work as the number of days they were absent. For example, if you are absent two days (Monday and Tuesday), you have two days (Wednesday and Thursday) to make up work. Homework or other work that is one day late will be worth half credit. Work will not be accepted more than one day late unless you have spoken to the teacher ahead of time. Chemistry is a cumulative subject which means that each topic builds on top of the previous topic. Therefore, it is crucial that you attend EVERY class period ON TIME. Tests and quizzes will be given approximately once a week. It is very difficult to catch up on classwork or make up labs from several absences. Missing work will result in a zero on that assignment. It is your responsibility to see the teacher after class or after school to make up any missed work. MAKEUP TESTS: You have one week to make up a missed test, quiz, or lab. It is your responsibility to schedule a time before or after school. This is done by scheduling an appointment with me. If you need to make up a lab or a test, you must arrange a time during study hall or before/after school to meet with the teacher. If you are absent the day before a test you must still take the test on test day. If you have an excused absence, you will have an equal number of days to make up the work for full credit. Make up tests will be different than the test given on the assigned date.

9 Plagiarism/Cheating: Plagiarism or cheating will not be tolerated. Plagiarism or cheating in any form will result in a zero on the assignment with notification of the parents and administration. Each and every student is responsible for his/her own work. Supplies All students are expected to keep a notebook. The notebook is designed to help you stay organized and as a studying tool. Please use it to your advantage. You should bring the following supplies to class every day: Three ring binder or folder to keep papers organized Pen or pencil (preferably both) ipad Scientific Calculator Course Grading Criteria: All quizzes, tests, and projects will be graded according to the Belle Vernon Area School District grading policy. Total points will be accumulated for all evaluated efforts in this class rather than having letter grades per each effort. The grading scale is as follows: A B C D F Emphasis will be on formal assessments. Therefore grades will be weighted in this course. Formal Assessments will account for 90% of a student s grade (quizzes, tests, projects, performance-based rubrics, essays, graded homework, etc.) Informal Assessments will account for 10% of a student s grade (homework for completion, class participation, exit tickets, etc.) Assignments per Quarter: Homework/Classwork: 10 points each (approximately 20) = Quizzes: 10 points each (approximately 7 quizzes) = Tests: points each (approximately 3-4 tests) = Labs: 10 points each (approximately 8 per quarter) = approx pts approx.. 70 pts approx pts approx.. 80 pts

10 TOTAL POINTS = 950 Points (approximate) *Assignments or assessments may vary due to pace of class and individualized instruction. Study Island: Students will be expected to take advantage of the Study Island Preparation Software aligned to the Keystone Exam Standards, AP Course Competencies, and SAT/ACT Preparation. The students that invest their time utilizing this program have overwhelming performed better than those that do not. If you are unable to have access to a computer or internet for this requirement, there are ample opportunities during the school day to utilize laptops or the computers in the Library. Academic Standards: Students will be reacquainted with the Pennsylvania Academic Standards that have been adopted by the Department of Education, along with the Common Core Standards that are in the process of being implemented nationwide. Students will be made aware of the importance of the standards and the efforts to meet them. Home Access Center: Grades will be updated every week on the HAC. If you lost or cannot remember log in information, please contact our Child Accounting Department at ext Schoolwires (Website): My website will be updated every Friday. Course Topics, Assignments, and Quizzes and Tests are also posted weekly. In this course, I will also use the itunes U course to assign homework. Contact Information School phone: (724) ext. Chemistry can be a difficult subject for some students. My goal is to help each student succeed, but the responsibility is shared. Each student is expected to participate, work on assignments and ask questions. If you feel your student is struggling, please contact me immediately. I look forward to a new and exciting year of chemistry!

11 Course Policy-AP Chemistry Please sign to indicate that you have read and understand the expectations for the class this year as stated in the course syllabus and return it to the teacher. Student s Name Student s Signature Student s Address: Parent/Guardian s Name Parent/Guardian s Signature Date Comments or any other information you would like to share? Does your child have access to a computer or the internet at home to complete homework assignments?