ࡱ> tws ETbjbj 4rrL&nnnnn8t.D+"*******$ .0~*n*nn*nn**(|)PZO˷(*+0D+(P1P1$))P1n)**D+P1 4: AP CHEMISTRY COURSE SYLLABUS & CLASS REQUIREMENTS SOUTHWEST HIGH SCHOOL Instructor: Mrs. Turner Room: I-50 Email:  HYPERLINK "mailto:cturner@cuhsd.net" cturner@cuhsd.net Office Hours: 7:00AM 8:00AM M-F Website: http://turnersclassofscience.weebly.com 3:00PM 4:00 PM M-W Text Chemistry, The Central Science 13e by Brown, LeMay, Bursten, Murphy, Woodward, Stoltzfus. Pearson Publishing. AP Program AP Chemistry enables students to pursue college-level chemistry studies while still in high school. This course provides willing and academically prepared high school students with the opportunity to earn college chemistry credits. AP Chemistry also demonstrates to college admission officers that the student has sought out the most rigorous course work available to them. AP Chemistry concludes with a college-level assessment developed and scored by college and university faculty, as well as experienced AP chemistry teachers. Research consistently shows that students who score a 3 or higher on AP exams typically experience greater academic success in college and have higher graduation rates than their non-AP peers. To develop the requisite academic and laboratory skills, students have a minimum of 275 minutes per week classroom and laboratory time. A minimum of 25% of instructional time is dedicated to the lab activities. In addition, students are required to spend at least 5 hours per week studying outside of class. We will be required to complete between 10 - 16 labs prior to the AP exam. Laboratory work is important in fulfilling the requirements of a college level course and in preparing a student for sophomore level college chemistry. Some college professors ask to see a record of the laboratory work done by an AP student before making a decision about granting credit, placement, or both. Since labs are an integral part of the AP program, lab activities will be done 1 2 class periods per week with an additional minimum of 1 hour per week outside of class. Course Goals This course is designed to satisfy a solid first year college chemistry requirement and follows the College Boards AP Chemistry Curricular Requirements. College Board AP curricular requirements can be viewed on http://turnersclassofscience.weebly.com. Key concepts and related content that defines the AP Chemistry course and exam are organized around principles call the big ideas. These encompass the core scientific principles, theories, and processes that govern chemical systems and that all students are required to understand. Big Idea 1: The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions. All matter is made of atoms. Atoms of each element have unique structures arising from interactions between electrons and nuclei. Elements display periodicity in their properties when the elements are organized by increasing atomic number. Atoms are so small they are difficult to study directly, so we use atomic models. Atoms are conserved in physical and chemical processes. Big Idea 2: Chemical and physical properties of materials can be explained by the structure and the arrangement of atoms, ions, or molecules and the forces between them. Matter is described by its physical properties. Forces of attraction between particles are important in determining many macroscopic properties of a substance. Strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds. The type of bonding in the solid state can be deduced from the properties of the solid state. Big Idea 3: Changes in matter involve the rearrangement and/or reorganization of atoms and/or transfer of electrons. Chemical changes are represented by a balanced chemical equation that identifies the ratio with which reactants react and products form. Chemical reactions can be classified by considering what the reactants are, what the products are, or how they change from one into the other. Chemical and physical transformations may be observed in several ways and typically involve a change in energy. Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions. Reaction rates that depend on temperature and other factors are determined by measuring changes in concentrations or reactants or products over time. Elementary reactions are mediated by collisions between molecules. Many reactions proceed via a series of elementary reactions. Reaction rates may be increased by the presence of a catalyst. Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Two systems with different temperatures will exchange energy. Energy is neither created nor destroyed, but only transformed from one form to another. Breaking bonds requires energy and making bonds releases energy. Electrostatic forces exist between molecules as well as between atoms or ions. Breaking these interactions requires energy. Chemical or physical processes are driven by a decrease in enthalpy or an increase in entropy. Big Idea 6: Any bond or intermolecular attraction that can be formed can be broken. These two processes are in a dynamic competition, sensitive to initial conditions and external perturbations. Chemical equilibrium is a dynamic, reversible state. Systems at equilibrium are responsive to external stimuli, with the response leading to a change. Chemical equilibrium plays an important role in acid-base chemistry. The equilibrium constant is related to temperature and the difference in Gibbs free energy. College chemistry departments spend three hours per week on laboratory work. It is mandated by the College Board that laboratory work be an important part of an AP Chemistry course so the course is comparable to a college general chemistry course. A minimum of two hours a week is needed. At the end of the course, the student will have participated in a minimum of 10 Advanced Inquiry labs. Curriculum Content Map First Semester Big Idea # 1: All matter is composed of atoms. Timing Topic Textbook Section Weeks 1 4 Matter & Measurement Classification of matter 1.2 Properties of matter 1.3 Units of measurement 1.4 Significant Figures 1.5 Dimensional analysis 1.6 Atoms, Molecules, & Ions Atomic Theory of Matter 2.1 Modern View of Atomic Structure 2.3 Molecules & molecular compounds 2.6 Ionic, & ionic compounds 2.7 Stoichiometry Chemical Equations - 3.1 Simple patterns of chemical reactivity - 3.2 Formula weights 3.3 Avogadros number & moles 3.4 Empirical formulas 3.5 Quantitative information from balanced eqns. - 3.6 Limiting reagents - 3.7 Weeks 5 7: Electron Structure of Atoms Quantized energy and photons 6.2 Quantum mechanics and atomic orbitals 6.5 Representation of orbitals 6.6 Electron configurations 6.8 Electron configurations & Periodic Table 6.9 Periodic Properties of the Elements Effective nuclear charge 7.2 Sizes of ions 7.3 Ionization energy 7.4 Electron affinities 7.5 Metals, non-metals, & metalloids 7.6 Labs Big Idea #1: Gravimetric Analysis of Calcium & Hard Water Advanced Inquiry Lab Acidity of Beverages Advanced Inquiry Lab Big Idea #2: Bonding & intermolecular forces explain the physical and chemical properties of matter. Weeks 8 11: Basic Concepts of Chemical Bonding Lewis symbols and the octet rule 8.1 Ionic bonding 8.2 Covalent bonding 8.3 Bond polarity and electronegativity 8.4 Drawing Lewis structures 8.5 Resonance structures 8.6 Exceptions to the octet rule 8.7 Strengths of covalent bonds 8.8 Molecular Geometry & Bonding Theory Molecular shapes 9.1 The VSEPR Model 9.2 Molecular shape and polarity 9.3 Hybrid orbitals 9.5 Weeks 12 16: Gases Pressure 10.2 The Gas Laws 10.3 Ideal-Gas equation 10.4 Further applications of the Ideal-Gas equation 10.5 Gas mixtures and partial pressures 10.6 Kinetic-Molecular Theory of Gases 10.7 Real gases: deviations from Ideal Behavior 10.9 Liquids & Intermolecular Forces Comparison of gases, liquids, & solids 11.1 Intermolecular forces 11.2 Select properties of liquids 11.3 Phase changes 11.4 Vapor pressure 11.5 Solids and Modern Materials Classification of solids 12.1 Structure of solids 12.2 Metallic solids 12.3 Metallic bonding 12.4 Ionic solids 12.5 Molecular solids 12.6 Covalent-network solids 12.7 Weeks 17-18: First Semester Finals Second Semester Week 19: Properties of Solutions The solution process - 13.1 Satd. solutions and solubility - 13.2 Factors affecting solubility - 13.3 Expressing solution concentration - 13.4 Labs Big Idea #2: Separation of a Dye Mixture Using Chromatography Adv. Inquiry Lab Qualitative Analysis & Chemical Bonding Advanced Inquiry Lab Big Idea #3: Chemical Reactions Involve the Rearrangement of Atoms and Describe How Matter Changes. Weeks 20 22: Stoichiometry: Calculations with Chemical Formulas & Equations Sections 3.1, 3.2, 3.6, & 3.7 covered in weeks 1-4. Reactions in Aqueous Solution General properties of aqueous solutions - 4.1 Precipitation reactions - 4.2 Acids, bases, & neutralization reactions - 4.3 Concentration of solutions - 4.5 Solution stoichiometry & chemical analysis - 4.6 Thermochemistry The First Law of Thermodynamics (covered in weeks 25 28) Electrochemistry Oxidation-reduction reactions - 4.4 Oxidation states & oxidation reduction rxn. - 20.1 Balancing redox equations - 20.2 Voltaic cells - 20.3 Cell potentials under standard conditions - 20.4 Free energy & redox reactions - 20.5 Batteries & fuel cells - 20.7 Electrolysis - 20.9 Labs Big Idea #3: Green Chemistry Analysis of a Mixture Advanced Inquiry Lab Analysis of Hydrogen Peroxide Advanced Inquiry Lab Separating a Synthetic Pain Relief Mixture Advanced Inquiry Lab Big Idea #4: Molecular Collisions Determine the Rates of Chemical Reactions. Weeks 23 24: Chemical Kinetics Factors that affect reaction rates - 14.1 Reactions rates - 14.2 Concentration & rate laws - 14.3 Change of concentration with time - 14.4 Temperature & rate - 14.5 Reaction mechanisms - 14.6 Catalysis - 14.7 Labs Big Idea #4: Rate of Decomposition of Calcium Carbonate Advanced Inquiry Lab Big Idea #5: Thermodynamics Describes the Role Energy Plays in Chemical and Physical Changes. Weeks 25 27: Thermochemistry The nature of energy - 5.1 The First Law of Thermodynamics - 5.2 Enthalpy - 5.3 Enthalpies of Reaction - 5.4 Calorimetry - 5.5 Hesss law - 5.6 Enthalpies of formation - 5.7 Foods and fuels - 5.8 Chemical Thermodynamics Spontaneous processes - 19.1 Entropy & Second Law of Thermodynamics - 19.2 Molecular interpretation of entropy - 19.3 Entropy change in chemical reactions - 19.4 Gibbs Free Energy - 19.5 Free energy and temperature - 19.6 Free energy and the equilibrium constant - 19.7 Labs Big Idea #5: Designing a Hand Warmer Advanced Inquiry Lab Big Idea #6: Equilibrium Represents a Balance Between Enthalpy and Entropy for Reversible Physical and Chemical Changes. Weeks 28 32: Chemical Equilibrium Concept of equilibrium - 15.1 Equilibrium constant - 15.2 Working with equilibrium constants - 15.3 Heterogeneous equilibria - 15.4 Calculating equilibrium constants - 15.5 Applications of equilibrium constants - 15.6 LeChateliers Principle - 15.7 Acid-Base Equilibria Bronstad-Lowry acids and bases - 16.2 Auto-ionization of water - 16.3 pH scale - 16.4 Strong acids and bases - 16.5 Weak acids - 16.6 Weak bases - 16.7 Relationship between Ka & Kb - 16.8 Acid-base properties of salt solutions - 16.9 Acid-base behavior and chemical structures - 16.10 Additional Aspects of Aqueous Equilibria Common-ion effect - 17.1 Buffered solutions - 17.2 Acid-base titrations - 17.3 Solubility equilibria - 17.4 Factors that affect solubility - 17.5 Labs Big Idea #6: Acid-Base Titrations Advanced Inquiry Lab Buffers in Household Products Advanced Inquiry Lab Weeks 33 35: Study for AP Chemistry Exam There will be six review sessions between 4:00 7:00 PM and two Saturday sessions during these three weeks of review. During the Saturday sessions, you will take two actual AP exams from previous years. You are required to attend one of the two Saturday sessions and three of the six review sessions. AP Chemistry Exam in 2015 will be administered on May 4 at 8:00 AM. Supplemental Instructional Materials AP Chemistry Free Response Questions: Selection of AP Chemistry Free Response Questions from 1961-2014 made available for classroom instruction by the College Board. AP Chemistry Multiple Choice Questions: Selection of AP Chemistry Multiple Choice Questions from 1961 2014 made available for classroom instruction by the College Board. Flinn Scientific Advanced Inquiry Labs for AP Chemistry Lab Manual. AP Chemistry Guided Inquiry Experiments Manual by the College Board. Chemical Demonstrations: Handbook for Teachers of Chemistry Volume 4 by Shakhashiri, Bassam. Pearson Education Test Prep Series for AP Chemistry by Edward Waterman. Kits: Molecular Modeling Kits Laboratory Equipment & Chemicals: supplies necessary for successful completion of required labs. Recommended Instructional Materials to be Purchased by Student Kaplan AP Chemistry Review Study Guide 2013/14 by David Wilson Barrons How to Prepare for the AP Chemistry Examination 8th edition by Neil D. Jespersen 5 Steps to a 5: AP Chemistry, 2015 edition by John Moore & Richard Langley Required Supplies to be Purchased by Student Calculator: scientific or graphing. Basic calculators are not accepted. Calculators on cell phones, PDAs and other electronic devices are not accepted. You must bring your calculator to class every day. Student Lab Notebook with spiral binding 50 carbonless duplicate sets by Hayden McNeil. These can be ordered through the instructor and will cost approximately $15.00. 3 Ring Binder: Dividers will be determined. Required daily. Writing Utensils: pen or pencil. Required daily. Assessments Students will receive assessments in the form of formative quizzes, tests, projects, labs, and homework. Tests Unit tests will be given after the completion of 1 3 chapters in the textbook. These tests will model AP testing conditions. Half of your test will be multiple choice questions similar in difficulty to those questions that would be found on the AP Test. The other half of your test will resemble the free-response questions. At least one question on the free response section will be calculator-based. At least one question on the free response question will resemble the essay questions. In addition to the above described assessments, a comprehensive final exam will be administered at the close of each semester. Formative quizzes will be given after each unit section. These will be student assessed and graded. It is STRONGLY RECOMMENDED that each student commit his/her self to taking and passing the AP examination in May 2015. Labs Advanced inquiry labs provide students with the opportunity to perform multiple trials and use statistical analysis to derive conclusions. You will be required to keep a bound student carbonless duplicate lab notebook of your lab work. You will also be required to keep a portfolio of lab reports. Many colleges require a copy of your lab work to assure that you had an appropriate college chemistry lab experience. You may not be granted college credit without it. Lab reports will be required to have a table of contents, numbered pages, title, purpose, theory, procedures, data reporting, discussion and conclusion, full sentences, and thorough explanation of data and results. A lab format that must be followed will be given to all students at the beginning of the year. Lab safety will be reviewed at the beginning of the year. Students will be required to sign and comply with a safety contract. Violations will result in points lost and a possible zero for a specific number of labs that semester. It is extremely difficult to make up labs. If you are absent during a lab you will need to schedule time with your partner and instructor to make up this lab outside of the class. Homework Homework is a constructive tool in the learning process. Homework enhances student achievement and develops self-discipline and good working habits. Homework assigned will be planned and organized; will be purposeful to the student; and will be evaluated and returned to students in a timely manner. Successful homework completion and study will enable students to master chemical principles and to develop powerful problem-solving skills. Assume you will spend at least five hours a week in unsupervised individual study. Keep a portfolio of all returned assignments until after the semester grade is issued. Policies Absent/Late/Missing Work Late homework will not be accepted unless you have an excused absence or it has been cleared with the teacher. For excused absences all exams and quizzes must be made up during the posted make up times before or after school. Homework must be made up within the same amount of days a student was absent. Labs must be made up during the lab make up times before or after school. Students are responsible for getting all missed work, notes, and activities on the days absent. Class Rules Be on time and prepared. You will not be allowed to leave class to get materials that you have forgotten. If you are tardy you will lose citizenship points and homework points. No electronic devices of any kind. Follow all lab safety rules. No food or drink in the classroom, except water. Do not talk to anyone while the instructor or another student is talking. Grading Policies Grade Scale: Percent Grade Percent Grade 100-93 A 77.9-73 C 92.9-90 A- 72.9-70 C- 89.9-88 B+ 69.9-68 D+ 87.9-83 B 67.9-63 D 82.9-80 B- 62.9-60 D- 79.9-78 C Below 59.9 F Academic Grade Breakdown: Activity Percent of Grade Homework 10% Labs & Projects 25% Exams 65% Citizenship Grade Breakdown: Activity Percent of Grade Attendance 10% Tardy 20% Conduct 30% Work Habits 40%     PAGE  PAGE 10 HI|}$ % ) * + K L Q n ÷yhWFWhFh h{h?^5B*OJQJph h{hA#5B*OJQJph h{h/VE5B*OJQJph#h{hA#56B*OJQJph#h{h/VE56B*OJQJphhgh/VE5>*OJQJhgh/VE>*OJQJhzbh/VE5OJQJ h{hA#5B*OJQJphhA#0J5OJQJjhA#5OJQJUhA#5OJQJhA#5OJQJ 2HIs$ % * gdA#$a$gdA#$a$gdA# B N nxȹȱȥwfffw饃U h{hf5B*OJQJph h{hZ[5B*OJQJphhzbh?^5OJQJ h{h/VE5B*OJQJph h{h?^5B*OJQJphhzbh/VE5OJQJhZ[OJQJh{hfB*OJQJphh{hZ[B*OJQJphhZ[>*OJQJh/VE>*OJQJhgh/VE>*OJQJhzbh/VEOJQJmxYZjkjk _`$XY[޼tktktktktktbkbhL)5OJQJhc\5OJQJ h{haU>5B*OJQJph h{h0"5B*OJQJphhaU>5OJQJh0"5OJQJh7%56OJQJh7%5OJQJ h{hf5B*OJQJph h{hn5B*OJQJph h{hn5B*OJQJph h{h7%5B*OJQJph"a!YZ6 jkjjk`  & Fgdc\ & Fgdc\ & Fgdc\ & Fgdc\@_`$Y\]    D E k l gd9hgdn & Fgdc\ & Fgdc\[\]      D E K N S Z j k l r òπpg\g\g\N= h{h/VE5B*OJQJphhnhn5>*OJQJhn5>*OJQJhn5OJQJhnh9h5CJ OJQJaJ h9h5OJQJhzbh/VE5OJQJhgh9xE>*OJQJ h{h/VE>*B*OJQJph h{h9xE>*B*OJQJphhzbhn5OJQJh/VE5OJQJhh&/5OJQJhV75OJQJhn5OJQJh7%hL)5OJQJr w x { !!!!;!?!B!e!!!!!!!!!!!!!!!""""i"j"p""""""""ɮɄh5OJQJhzbhg5OJQJhg5OJQJhzbhA5OJQJh/VE5OJQJhn5OJQJhA5OJQJhzbh/VE5OJQJh9h5OJQJ h{h/VE5B*OJQJph h{hg5B*OJQJph4 !C!`!!!!""7"j"""" #-#3#^#### $@$A$i$^gd/VEgd/VE @ ^@ `gd/VE"""""",#-#3#:#>#?#]#^#######$$;$<$$$$$$$$$%%#%$%%%&&&D&E&l&o&&&ằwwwhH5OJQJhnh9h5CJOJQJaJhnh9h5CJ OJQJaJ h{h">5B*OJQJphh">5OJQJh9h5OJQJhzbhg5OJQJhg5OJQJh/VE5OJQJhn5OJQJh5OJQJhzbh/VE5OJQJ.i$$$$$#%$%z%%%&&E&t&&&& '/'Z''''''(9(:(P(k(gd/VE&&&&&''''+'S'V'}''''''''''((0(5(>(?(`(f((((((())B)D){)|)))))))%*(*B*G*b*g*******++1+7+T+Y+|+}++++++++hg5OJQJh5OJQJh9xE5OJQJh6O5OJQJh9h5OJQJhn5OJQJhH5OJQJIk(((()I)))))*-*L*l*m*****+<+^+++++++++gd/VE++++,,,.-/-------$.o//01122D3333 4 456666>7̿ᶭضح~ull_h5L*5CJ OJQJaJ h5L*5OJQJh?5OJQJhEY5OJQJh]W5CJ OJQJaJ h6Oh6O5OJQJh6O5CJ OJQJaJ h]W5OJQJh6O5OJQJhg5CJ OJQJaJ h">h">5OJQJh 85OJQJhg5OJQJh">5OJQJhzbh/VE5OJQJ"++,4,`,,,,*-/---$.%.G.{....5/6/J///// 030R0gd6OgdgR000000I11112292j22223(3D3E333334B4n444gd6O444 5(5)5E5j5556"6L66666?7@7e7777868i88888gd6O>7@7H7L7M79999@::u;w;x;;;;<<<<<<<<===A=B=C=ĻIJIJħq_#h{h/VE5>*B*OJQJph h{h/VE>*B*OJQJphhzbh5OJQJh"h56OJQJh"56OJQJh56OJQJh"5OJQJhr5OJQJhzbh/VE5OJQJhg5OJQJh 85OJQJh.5H*OJQJhEY5OJQJh.5OJQJ899C9_9{999::@:b::::::<;u;y;;==B=C===^gd/VE^gd"gd/VEgd6OC====>>>>? ?$?%???R@@@@@ A AAA-A0ANAPAyAzA|AպveTKhuUs>*OJQJ h{h 5B*OJQJph h{h:5B*OJQJphh h 5H*OJQJh 5OJQJh:5OJQJhgh/VE>*OJQJhzbh/VE5OJQJhzbh5OJQJh5OJQJhr5OJQJhiK5OJQJh 85OJQJ h{h 85B*OJQJph h{h/VE5B*OJQJph=>>>>%?&???????Q@R@@@@@,A-AyAzA{A|AAAyBzB%Cgd/VE|AAAAyBzBBBB$C%CCCCCCC D(DLDSDdDFFFFF9G:GFGeGgGnGGGٷȦٌٌكznȷe\h?5OJQJhi,{5OJQJhzbhfe5OJQJhfe5OJQJh/VE5OJQJhuUs5OJQJ h{h+I5B*OJQJph h{hfe5B*OJQJph h{huUs5B*OJQJph h{h/VE5B*OJQJphhzbh/VE5OJQJhgh/VE5>*OJQJhgh/VE>*OJQJ"%C&CbCcCCCCC DDDDFFFFFFgGhGmGnGGG~JJiKjK!L"Lgd/VEGGGGHHH[HbHzHEIGI}J!L"L,LYMM=NNNNNNN:PPP5QпЮпТТТzqeSe#h{h/VE5>*B*OJQJphhgh/VE5OJQJhfe5OJQJhfeh/VE5>*OJQJ h{h/VE>*B*OJQJphhi,{5OJQJhzbh/VE5OJQJ h{h0m5B*OJQJph h{h+I5B*OJQJph h{h/VE5B*OJQJphhzbh0m5OJQJh/VE5OJQJh0m5OJQJ"L+L,LMM=N>NNNNNNN+O,O9P:PPPPP]Q^QQQQQQQRgd/VE5Q[QQQRR/R0R>RLRNR]ReRfRRRRSSS#S4SBSDSXScSfShSiSSSSSSĶިިޟޟގ}k}k}}}YY#h{hfe5>*B*OJQJph#h{h/VE5>*B*OJQJph h{h/VE5B*OJQJph h{hfe5B*OJQJphhfe5OJQJh>Rh/VE5>*OJQJh lh/VE5CJOJQJhfeh/VE5>*OJQJh lh/VE5OJQJh>Rh/VE5OJQJhgh/VE5OJQJhM5OJQJ!RR/R0R=R>R]RuRvRRRRRRRRRRRSS4SDSZShSiSSSSSgd/VESSSSSSSSTTTTTT!T"T$T%T'T(T*T+T1T2T3T5T6T6666666666666666666666666666666666666666666666666hH6666666666666666666666666666666666666666666666666666666666666666662 0@P`p2( 0@P`p 0@P`p 0@P`p 0@P`p 0@P`p 0@P`p8XV~_HmH nH sH tH @`@ NormalCJ_HaJmH sH tH DA`D Default Paragraph FontRiR  Table Normal4 l4a (k (No List 4 @4 AFooter  !.)@. 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