Advanced Placement Chemistry Course Syllabus, Page 4
Advanced Placement Chemistry Course Syllabus
2011-12 School Year
Instructor: Dr. Gene Wicks, Sault Area High School and Career Center, 904 Marquette Ave., Sault Ste. Marie, MI 49783, Room 233, (906) 635-3839 ext. 5884,
Course Materials: (1) Chang, R. (2010). Chemistry (10th ed). Boston: McGraw-Hill. (2) Laptop computer. (3) Scientific calculator.
Lab Materials: The primary sources for lab activities are: (1) Beran, J. A. (2004). Laboratory Manual for Principles of General Chemistry (7th ed). New York: John Wiley and Sons, Inc. (2) Randall, J. (2004). Advanced Chemistry with Vernier, Experiments for AP, IB, and College General Chemistry. Beaverton: Vernier Software and Technology.
Course Objectives: Advanced Placement Chemistry is a one-year, algebra-based chemistry course for 11th and 12th grade students. It includes topics in atomic theory, atomic structure, chemical bonding, periodic table relationships, states of matter, solution chemistry, reaction types, stoichiometry, chemical equilibrium, kinetics, thermodynamics, and electrochemistry. This rapidly paced course will emphasize lab experimentation and technology, and it will help students interested in science and engineering careers to develop better conceptual and numerical problem-solving skills. It will also help them to develop better critical thinking skills. At the completion of the course, students may take an advanced placement test with the possibility of receiving college credit for the course.
Learning Objectives: Click on http://www.collegeboard.com/student/testing/ap/sub_chem.html?chem for the complete AP Chemistry Course Description
Prerequisites: (1) Approval from the first-year chemistry teacher. (2) Minimum grade point average of 3.0. (3) Successful completion of Algebra I and Chemistry. (4) Successful completion or concurrent enrollment in Algebra II and Physics.
Grading: 25 % Short Assignments. These assignments will include in-class work, homework, quizzes, computer-based learning, writing assignments, and discussion activities. Tests will emphasize the knowledge and problem-solving skills acquired from completing these assignments. A list of upcoming assignments is available at sault.eup.k12.mi.us/67007041193445/
25 % Laboratory. Hands-on lab activities will take place nearly every week. There will be a strong emphasis on using modern technology to collect data, perform statistical analyses, and represent data graphically. Your graded labs will become part of a lab portfolio which you will turn in for additional credit in May. You will receive lab safety training throughout the school year, and you will be expected to work safely while participating in all lab activities.
50 % Tests. There will be several tests per marking period. Remember to bring a scientific calculator on test days. A table of A.P. Chemistry equations and a table of physical constants and conversion factors, both obtained from the College Board, will be available during tests.
Final Exam: There will be a comprehensive final exam given at the end of each semester. The final exam will be worth 20 % of the overall semester grade. Students who take the College Board’s AP Chemistry Exam in May will be exempt from taking the second semester final exam.
Grading Scale: 90-100 A (Grades for all assignments are available on Skyward.)
80-89 B
70-79 C
60-69 D
0-59 E
Teaching Methods: A variety of teaching methods will be used in this course including guided inquiry, cooperative learning groups, demonstrations, discussions, computer-based learning, and direct instruction. Our discussions, demonstrations, and lab activities will often begin with a question or problem, which will encourage students to form hypotheses. Whenever possible, these hypotheses will be tested and the results discussed. During lab activities, the hypotheses will naturally lead to experimentation, data gathering and organization, explanations, and conclusions leading to further hypotheses.
Help Sessions: Help sessions will be available before or after school for students who desire extra assistance.
Extra Credit: Extra credit is rarely available in college-level coursework. However, when particularly challenging concepts are covered, Mr. Wicks will announce when test corrections may be turned in for one-third of the original credit.
Cheating: Any student suspected of cheating on a test will receive a zero and will not be allowed to retake the test. With the exception of a scientific calculator, no electronic devices (laptops, netbooks, cell phones, iPods, or similar devices) may be used during tests.
Absences: For every day they are absent, students will be given two days to complete make-up assignments. Students will have a maximum of one week from an absence to complete a missed test or lab. Otherwise the score will be zero. Make arrangements with Mr. Wicks to complete missed tests or labs before or after school.
Late Assignments: Late assignments will be penalized by approximately 15 % of the overall score if they are turned in before graded assignments have been returned to the class. Late assignments will receive half credit if they are turned in after graded assignments have been returned to the class.
Lab Portfolio: Students are required to prepare a portfolio of lab reports so that they can show evidence of their lab work if a college requests it. Presenting evidence of adequate college-level laboratory experience is quite helpful to students who desire credit for (or exemption from) an introductory science course that includes a lab component.
Special Needs: Mr. Wicks requests that students with special needs privately inform him of their needs during the first two weeks of school. This will ensure that appropriate accommodations are made in collaboration with a special education teacher.
Teacher Availability: Mr. Wicks will be available before and after school to assist students most days during the week. Students may also schedule times before and after school to make up tests or labs. Parents are encouraged to phone before 7:30 AM, between 9:00-9:45 AM, or after 3 PM to discuss concerns with the teacher.
Classroom
Expectations: Students are expected to read, understand, and follow the rules given in the student handbook. They are also expected to know and follow the instructor’s posted classroom expectations for student conduct.
Course Schedule: The course text is Chang, R. (2010). Chemistry (10th ed). Boston: McGraw-Hill. The chapter numbers, information included, and presentation/discussion order are given below. The discussion order and chapter contents have been reorganized to better meet the College Board’s set of AP Chemistry learning objectives.
Chapter 1: Chemistry: The Study of Change (First Marking Period Begins)
Course introduction, scientific method, unit systems, physical and chemical properties, dimensional analysis, significant figures.
Chapter 2: Atoms, Molecules, and Ions
Atomic theory, structure of the atom, atomic number, mass number, isotopes, chemical formulas, naming compounds.
Chapter 24: Organic Chemistry
Classes of organic compounds, aliphatic hydrocarbons, aromatic hydrocarbons, functional groups, structure, nomenclature, chemical properties.
Chapter 3: Mass Relationships in Chemical Reactions
Atomic mass, Avogadro’s number, mole concept, molar mass, percent composition, empirical formulas, chemical reactions and chemical equations, stoichiometry, limiting reactant, percent yield.
Chapter 4: Reactions in Aqueous Solution
Electrolytic properties, precipitation reactions, spectator ions, net ionic equations, acid-base reactions, oxidation-reduction reactions, balancing equations for redox reactions, concentration of solutions, gravimetric analysis, acid-base titration, redox titration.
Chapter 6: Thermochemistry
Enthalpy changes, specific heat, heat of fusion, heat of vaporization, calorimetry, heat of formation, heat of reaction, Hess’s law, heat of solution, state functions, work, heat, first law of thermodynamics.
Chapter 7: Quantum Theory and the Electronic Structure of Atoms (Second Marking Period Begins)
Waves, electromagnetic radiation, Bohr’s theory of the hydrogen atom, quantum mechanics, quantum numbers, atomic orbitals, electron configuration.
Chapter 8: Periodic Relationships Among the Elements
Development of the periodic table, classification of the elements, periodic variation in physical and chemical properties (for example, atomic radii, ionization energies, electron affinities, oxidation states).
Chapter 9: Chemical Bonding
Lewis dot symbols, ionic bonds, lattice energy, covalent bonds, electronegativity, Lewis structures, bond polarity, formal charge, resonance, bond energy.
Chapter 10: Molecular Geometry and Hybridization of Atomic Orbitals
Valence-shell electron-pair repulsion theory (VSEPR), electron-pair geometry, molecular geometry, geometry of polyatomic ions, dipole moments, hybridization of atomic orbitals, sigma and pi bonds.
Chapter 5: Gases
Pressure of a gas, ideal gases versus real gases, the gas laws, the ideal gas equation, gas stoichiometry, Dalton’s law of partial pressures, kinetic molecular theory, deviation from ideal behavior.
Chapter 11: Intermolecular Forces and Liquids and Solids
Intermolecular forces (hydrogen bonding, dipole-dipole, and London dispersion forces), properties of liquids and solids, how the kinetic molecular theory relates to liquids and solids, crystal structure, lattice energy, phase changes, phase diagrams, triple point, critical point.
Chapter 12: Physical Properties of Solutions (Third Marking Period Begins)
Types of solutions, concentration units, effect of temperature on solubility, effect of pressure on the solubility of gases, colligative properties (vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure), Raoult’s law.
Chapter 18: Entropy, Free Energy, and Equilibrium
The three laws of thermodynamics, entropy, enthalpy, Gibb’s free energy, free energy of formation, free energy of reaction.
Chapter 13: Chemical Kinetics
Reaction rate, reactant order, rate constant, rate law, half-life, activation energy, temperature dependence of rate constants, Arrhenius equation, reaction mechanisms, rate-determining step, catalysis, use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws.
Chapter 14: Chemical Equilibrium
Concept of a dynamic equilibrium, equilibrium constants for gaseous reactions (Kp, Kc), equilibrium constants for reactions in solution, using an equilibrium constant to predict the direction of a reaction, factors that affect equilibrium, Le Chatelier’s principle, free energy and equilibrium.
Chapter 15: Acids and Bases
Acid and base concepts, pH, Arrhenius acids and bases, Brønsted-Lowry acids and bases, Lewis acids and bases, acid and base strengths, weak acids and Ka, weak bases and Kb, amphoterism, diprotic and polyprotic acids, molecular structure and strength of acids, salts, hydrolysis.
Chapter 16: Acid-Base Equilibria and Solubility Equilibria (Fourth Marking Period Begins)
Common ion effect, buffer solutions, acid-base indicators, solubility product constants (Ksp) and their application to precipitation reactions and the dissolution of slightly soluble compounds.
Chapter 19: Electrochemistry
Redox reactions, electrochemical cells, half-cell reactions, standard reduction potentials, spontaneity of redox reactions (free energy and electrode potentials), effect of concentration on cell emf, Nernst equation, galvanic versus electrolytic cells, electrolysis.
Chapter 23: Nuclear Chemistry
Balancing nuclear equations, nuclear stability, radioactivity, half-life, transmutation, nuclear fission, nuclear fusion.
Selected Topics from Chapters 17,20,21, & 22
Acid rain, photochemical smog, alkali metals, introduction to complex ions, chemical and physical properties of selected nonmetals.
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