AP CHEMISTRY - LEDDY COURSE DESCRIPTION: This AP Chemistry course is designed to be the equivalent of a two semester college introductory chemistry course usually taken by chemistry majors during their first year. Students taking this course will be substantially better prepared for any college science course due to the intensive nature of study required by the content covered, the math involved, the use of higher-level thinking skills, and the more involved laboratory experience. This is a science course that focuses on advanced, key concepts and topics, not typical of general high school chemistry. These concepts are placed in the broader context of six conceptual themes, or Big Ideas as outlined by The College Board: BIG IDEA OVERVIEW: Big Idea 1: Structure of matter Big Idea 2: Properties of matter-characteristics, states, and forces of attraction Big Idea 3: Chemical reactions Big Idea 4: Rates of chemical reactions Big Idea 5: Thermodynamics Big Idea 6: Equilibrium BIG IDEA DETAILS: Big Idea 1: Structure of matter o 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. 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. Big Idea 2: Properties of matter characteristics, states and forces of attraction o 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. Big Idea 3: Chemical Reactions o Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons. Big Idea 4: Rates of chemical reactions o Rates of chemical reactions are determined by details of the molecular collisions. Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Big Idea 5: Thermodynamics o The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter. Big Idea 6: Equilibrium o 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. Each Big Idea is broken down into Key Science Practices detailing the learning targets for the course. This syllabus describes the Big Ideas and Science Practices associated with each chapter and section. Within the schedule grid, these connections will be referenced by the following notation, (BI: Big Idea, SP: Science Practice). In addition, within the course schedule each topic and unit refers back to the Learning Objective as outlined by Collegeboard. SCIENCE PRACTICES: 1. The Student can use representations and models to communicate scientific phenomena and solve scientific problems. 2. The student can use mathematics appropriately. 3. The student can engage in scientific questioning to extend thinking or to guide investigations within the context of the AP course. 4. The student can plan and implement data collection strategies in relation to a particular scientific question. 5. The student can perform data analysis and evaluation of evidence. 6. The student can work with scientific explanations and theories. 7. The student is able to connect and relate knowledge across various scales, concepts, and representations in and across domains.
AP Chemistry places a strong emphasis on students making connections across the Science Practices and Big Ideas. Students also make connections through advanced laboratory experiences designed to further develop important science process and application skills, including experimental design, manipulation of variables, data interpretation, statistical analysis, and operation of technical equipment. The goal is to provide students with the conceptual framework, factual knowledge, and analytical skills necessary to deal critically with the science of chemistry. This is a demanding but rewarding course, covering a large amount of material at a fast pace. TEXTBOOK: Chemistry: A Molecular Approach, AP* Edition, Fourth Edition. Nivaldo J. Tro. Boston, MA: Pearson MATERIAL REQUIRED: Pens (blue/black/red) / Pencils / Highlighter Graphing Calculator / Graph Paper Lab Notebook: Marble Bound Binder / 8 Dividers / Loose Leaf EXPECTATIONS: Students must follow all policies and procedures in the Franklin Towne Student Handbook. Students should be in their assigned seats when the bell rings. For the first 5 minutes of class, students should copy any homework into their planners and complete the COMPOUND OF THE DAY found on the board. Students who are not in their seat working when the bell rings will be marked late and receive a detention. Go to the bathroom and the nurse before class or during lunch. Students will only be allowed to leave the classroom in case of an emergency. COURSE OUTLINE: This course is designed to provide a thorough, first-year university chemistry experience. Students will be required to demonstrate problem-solving skills in both written work and laboratory work. Labs will serve as supplements to concepts covered in lecture with a heavy emphasis on data analysis and interpretation. Because this is a second-year chemistry course, students entering should have a solid understanding of the following concepts: Course Overview and Grading: Mass-mole relationships Atomic structure Stoichiometry Intra- and intermolecular forces Physical Behavior of Gases Atomic Theory Solution Chemistry Although these topics will be covered in detail, students should anticipate a quicker pace for review topics, so that newer concepts can be taught at a greater depth. Concepts covered include all of the above and: Reaction kinetics Chemical equilibrium Thermodynamics Oxidation-Reduction and Electrochemistry ph and Acid-Base Equilibrium Materials Chemistry Organic Chemistry Each chapter in the AP Chemistry textbook will be covered at a rate of one chapter every five to seven days. Students will be assigned various homework problems from the textbook and online and practice worksheets that must be completed on time. Each Friday, students will be quizzed on the week s essential learnings. Students should expect an exam at the end of every unit (every two to three weeks). 2
Students will be graded using the following weighted percentages: Formative (20%) o Notes: It is expected that all students will do the assigned reading before the class section in which the material is covered. o Homework: Each chapter includes a variety of both in-class, online, and at-home practice problems. Homework is a necessary portion of this class. You can expect to be assigned homework several times each week to reinforce the concepts we are learning. You should check the class website and Infinite Campus regularly to stay current with assignments and class information. Late projects will be accepted but will have a 10% deduction for every additional day late (excluding homework.) You will receive an appointment every day until your assignment is complete. Homework passes will not be permitted to be used in this class o Activities o Quizzes Summative (60%) o Exams Exams are given as a culmination at the end of a unit of study. It is expected that students continually study and prepare themselves for assessments. Tests will be objective based and will be assessed based on mastery of those objectives. SEE PROOF OF STUDY AND RETESTING POLICY IN HANDBOOK Retesting will be available for any objectives not mastered at the discretion of the teacher, but only after we have readdressed any material necessary and the Proof of Study was completed adequately. If you fail an objective, you must come in for tutoring until you have mastered the objective regardless of whether or not retesting will be offered. Retesting is up to the teacher s discretion, Grade Cap at 75% for work redone o Labs Throughout AP Chemistry, students will be conducting laboratory investigations as a way to explore and explain various concepts being studied. Students will be engaged in some form of laboratory work no less than 25% of the time. Each lab activity is intended to both challenge and extend the students knowledge of chemical concepts. A prelab assignment (including flow chart) is due prior to the start of ALL labs. Analysis (including calculations) and post-lab discussions will usually be completed in class following the activity. Lab quizzes will be open (lab) notebook, and will test your ability to analyze lab data and apply lab principals to other situations. In addition, a formal lab report will be due as outlined below. Quarterly/Mid-Term/Final Exam: 20% o Cumulative Exams as outline by the Educational Framework of the District Make-Up Work: You will need to follow all Franklin Towne policies regarding making up work. It is your responsibility to obtain your missed work by checking the website, Infinite Campus, and the missed work file in class. Any questions you have must be discussed during an appointment. Work that was assigned before the absence will be due on the first day back in class. If you are absent the day an assignment is due, it is your responsibility to turn it in when your return. Tests, quizzes, and labs can be made up after school. In some cases, missed labs will be made up by an alternative assignment. Absences of less than 2 days will not excuse you from taking a test since all tests will be on the previous week s material. LABS: The labs in this course will require following or developing processes and procedures, taking observations, and data manipulation. In addition, through the labs the students will gain experience using new equipment such a volt meter, Buchner funnel, spectrometer, buret, colorimeter, ph Meter and conductivity probes. 3
LAB NOTEBOOK: Students must maintain a proper lab notebook throughout this course. A specific format will be given to the student for each lab. Students must follow that format and label all sections very clearly. The lab notebook will be a Marble Notebook which will include a Table of Contents and all data tables including observations, graphs and reactions. AP Chemistry lab reports are much longer and more in depth than the ones completed in the first year chemistry course. Therefore, it is important that students don t procrastinate when doing pre-lab and post-lab work. Late labs will not be accepted. Labs not completed in class must be done before/ after school by appointment. Pre-lab work is to be completed and turned in on the day the lab is performed. LAB REPORT: The 10 Parts of a Laboratory Report 1. Title: a. The title should be descriptive. For example, ph Titration Lab is a descriptive title and Experiment 5 is not a descriptive title. 2. Date: a. This is the date the student performed the experiment. 3. Purpose: a. A purpose is a statement summarizing the point of the lab. 4. Procedure Outline: a. Students need to write an outline of the procedure. They should use bulleted statements or outline format to make it easy to read. If a student is doing a guided inquiry lab, they may be required to write a full procedure that they develop. 5. Pre-Lab Questions: a. Students will be given some questions to answer before the lab is done. They will need to either rewrite the question or incorporate the question in the answer. The idea here is that when someone (like a college professor) looks at a student s lab notebook, they should be able to tell what the question was by merely looking at their lab report. It is important to produce a good record of lab work. 6. Data Tables a. Students will need to create any data tables or charts necessary for data collection in the lab. During the Lab 7. Data: a. Students need to record all their data directly in their lab notebook. They are NOT to be recording data on their separate lab sheet. They need to label all data clearly and always include proper units of measurement. Students should underline, use capital letters, or use any device they choose to help organize this section well. They should space things out neatly and clearly. 8. Calculations and Graphs: a. Students should show how calculations are carried out. Graphs need to be titled, axes need to be labeled, and units need to be shown on the axis. To receive credit for any graphs, they must be at least ½ page in size. 9. Conclusions a. This will vary from lab to lab. Students will usually be given direction as to what to write, but it is expected that all conclusions will be well thought out and well written. 10. Post Lab Error Analysis Questions: a. Follow the same procedure as for Pre-Lab Questions. 4
QUARTER 1 Chapter & Big Ideas [BI] Topics & Learning Objectives [LO] Labs / Assessments Chapter 1: Matter Measurement & Problem Solving [BI: 1, 2, 3] (2 Classes) 1.1 Atoms and molecules 1.2 Scientific approach to knowledge [LO 1.13, 1.16, 1.17] 1.3 Classification of matter [LO 1.17, 3.1] 1.4 Physical and chemical changes and physical and chemical properties [LO 1.17, 3.1, 3.2, 3.10] 1.5 Energy: A fundamental part of physical and chemical change [LO 3.10] 1.6 Units of measurement 1.7 Reliability of measurements 1.8 Solving chemical problems Chapter 2: Atoms & Elements [BI: 1,2,3] (2 Classes) 2.1 Brownian Motion: Atoms Confirmed 2.2 Early ideas about the building blocks of matter 2.3 Modern atomic theory and the laws that led to it [LO 1.12, 1.13, 3.5, 3.6] 2.4 The discovery of the electron [LO 1.12, 1.14] 2.5 The structure of the atom [LO 1.1,1.13] 2.6 Subatomic particles: Protons, neutrons and electrons [LO 1.1] 2.7 Finding patterns: The periodic law and the periodic table [LO 1.1] 2.8 Atomic mass [LO 1.1, 1.4, 1.14, 1.18] 2.9 Molar mass [LO 1.4, 1.18] Chapter 3: Molecules, Compounds and Chemical Equations [BI: 1, 2, 3] (1 Week) 3.1 Hydrogen, oxygen, and water 3.2 Chemical bonds [LO 2.1] 3.3 Representing compounds: Chemical formulas and molecular models [LO 1.18, 2.1] 3.4 An atomic-level view of elements and compounds [LO 1.18, 2.1] 3.5-3.7 IUPAC Nomenclature [LO 1.18, 2.1] 3.8 Formula mass and the mole concept for compounds [LO 1.4, 1.18] 3.9 Composition of compounds [LO 1.1, 1.2, 1.4, 1.18] 3.10 Determining a chemical formula from experimental data [LO 1.1, 1.2, 1.4, 1.18] 3.11 Writing and balancing chemical equations [LO 1.4, 1.18, 3.1, 3.2 3.3 3.4] 5
Chapter 4: Chemical Reactions and Aqueous Reactions [BI: 1,2,3] (2 weeks) Chapter 6: Thermochemistry [BI: 3, 5] (1 weeks) Chapter 18: Free Energy and Thermodynamics [BI: 5] (1.5 weeks) Chapter 5: Gases [BI: 2, 3] (1 week) 4.1 Climate change and the combustion of fossil fuels 4.2 Reaction stoichiometry: How much carbon dioxide? [LO 1.17, 3.3, 3.4, 3.10] 4.3 Limiting reactant, theoretical yield, and percent yield from initial reactant masses [LO 3.3, 3.4, 3.10] 4.4 Solution concentration and solution stoichiometry [LO 2.2, 2.9, 3.10] 4.5 Types of aqueous solutions and solubility [LO 2.1, 2.2, 2.9, 3.10] 4.6 Precipitation reactions [LO 3.1, 3.2, 3.10] 4.7 Representing aqueous reactions: molecular, ionic and complete ionic equations [LO 2.2, 3.1, 3.2, 3.10] 4.8 Acid-base and gas-evolution reactions [LO 1.20, 2.2, 3.1, 3.2, 3.3, 3.4, 3.7, 3.10] 4.9 Oxidation-reduction reactions [LO 3.2, 3.3, 3.4, 3.8, 3.10] 6.1 Chemical hand warmers [LO 3.11, 5.2, 5.3, 5.4, 5.6] 6.2 The nature of energy: Key definitions [LO 3.11, 5.2, 5.3, 5.4, 5.6] 6.3 The first law of thermodynamics [LO 3.11, 5.2, 5.3, 5.4, 5.5, 5.6] 6.4 Quantifying heat and work [LO 3.11, 5.2, 5.3, 5.4, 5.4, 5.5, 5.6] 6.6 Enthalpy: The heat evolved in a chemical reaction at constant pressure [LO 3.11, 5.6, 5.7, 5.8] 6.7 Constant-pressure calorimetry: Measuring ΔHrxn [LO 5.4, 5.6, 5.7, 5.8] 6.8 Relationships involving ΔHrxn [LO 5.4, 5.6, 5.8] 6.9 Determining enthalpies of reaction from standard enthalpies of formation [LO 5.6, 5.8] 6.10 Energy use and the environment 18.1 Nature s heat tax [LO 5.13, 5.18] 18.2 Spontaneous and nonspontaneous processes [LO 5.13, 5.18] 18.3 Entropy and the 2 nd law of thermodynamics [LO 5.13, 5.18] 18.4 Heat transfer and changes in the entropy of the surroundings [LO 5.12, 5.13, 5.18] 18.5 Gibbs free energy [LO 5.12, 5.13, 5.14, 5.18] 18.6 Entropy changes in chemical reactions: Calculating ΔS o rxn [LO 5.12, 5.13, 5.14, 5.18] 18.7 Free energy changes in chemical reactions: Calculating ΔG o rxn [LO 5.12, 5.13, 5.14, 5.15, 5.16, 5.18] 18.8 Free energy ehanges for nonstandard states: The relationship between ΔG o rxn and ΔGrxn[LO 5.12, 5.13, 5.18] 18.9 Free energy and equilibrium: Relating ΔG o rxn to the equilibrium constant (K) [LO 5.12, 5.13, 5.18] 5.1 Breathing: putting pressure to work 5.2 Pressure: the result of molecular collisions 5.3 The simple gas laws [LO 2.4, 2.6, 3.1] 5.4-5.5 The ideal gas law [LO 2.4, 2.5, 2.6, 2.15] 5.6 Mixtures of gases and partial pressures [LO 2.4, 2.5] 5.7 Gas stoichiometry [LO 2.4, 2.5, 3.3, 3.4] 5.8 Kinetic molecular theory: A model for gases [LO 2.4, 2.5] 5.9 Mean free path, effusion and diffusion of gases [LO 2.4, 2.5] 5.10 Real gases: The effects of size and intermolecular forces [LO 2.4, 2.5] 6
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