AP Chemistry Syllabus Mrs. Paul (301) (school phone) ( )

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1 AP Chemistry Syllabus Mrs. Paul (301) (school phone) ( ) 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 fra m e w ork provided by the College B o a r d. A special emphasis will be placed on the seven science practices, which capture important a s p e c t s of the work that scientists engage in, with learning objectives that combine content with inquiry and reasoning skills. 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. 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 Textbook Brown, LeMay, Bursten, Chemistry, The Central Science, tenth edition. Require d Materials Notebook to hold all handouts, labs, and returned papers Section in notebook or spiral for note taking Black and White composition book for lab reports Scientific Calculator (a graphing calculator is recommended) Black or blue pens (for the lab notebook) Labs The labs completed require following or developing processes and procedures, taking observations, and data manipulation. You will communicate and collaborate in lab groups; however, each of you will write a laboratory report in a lab notebook for every lab they perform. The 10 Parts of a Laboratory Report A specific format will be followed for each lab. You will label all sections very clearly. 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 you 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 at lunch or before/ after school by appointment. Pre-Lab Work Pre-lab work is to be completed and turned in on the day the lab is performed. 1. Title The title should be descriptive. For example, ph Titration Lab" is a descriptive title and "Experiment 5"is not a

2 descriptive title. 2. Date This is the date you performed the experiment. 3. Purpose A purpose is a statement summarizing the "point" of the lab. 4. Procedure Outline You need to write an outline of the procedure. You should use bulleted statements or outline format to make it easy to read. If you are doing a guided inquiry lab, you will be required to write a full procedure that you develop. 5. Pre-Lab Questions You will be given some questions to answer before the lab is done. You 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 your lab notebook, they should be able to tell what the question was by merely looking at your lab report. It is important to produce a good record of lab work. 6. Data Tables You will need to create any data tables or charts necessary for data collection in the lab. During the Lab 7. Data You need to record all you r data directly in your lab notebook. You are not to be recording data on a separate lab sheet. You need to label all data clearly and always include proper units of measurement you should underline, use capital letters, or use any device you choose to help organize this section well. You should space things out neatly and clearly. Post-Lab Work 8. Calculations and Graphs You 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, you must be at least half page in size. 9. Conclusions This will vary from lab to lab. It is expected that all conclusions will be well thought out and well written. 10. Post Lab Error Analysis Questions Follow the same procedure as for Pre-Lab Questions. Advanced Placement Chemistry-The Laboratory Notebook A record of lab work is an important document, which will show the quality of the lab work that you have performed. AP Chemistry Unit Overview Unit 1: Chemistry Fundamentals Homework Sets Assigned: 3 Weeks 1-3 Number of Quizzes: 3 1. Scientific Method 2. Classification of Matter a. pure substances vs. mixtures b. law of definite proportions c. law of multiple proportions d. chemical and physical changes 3. Nomenclature and formula of binary compounds

3 4. Polyatomic ions and other compounds 5. Determination of atomic masses 6. Mole concept 7. Percent composition 8. Empirical and molecular formula 9. Writing chemical equations and drawn representations 10. Balancing chemical equations 11. Applying mole concept to chemical 12. Determine limiting reagent, theoretical and %yield *Guided Inquiry: Relationship between the Concentration of a Solution and the Amount of Transmitted Light through the Solution Determination of the Percent Water in a Compound and its Empirical Formula N e t I o n ic Eq ua tion s Addition/ Decomposition Equations Unit 2: Electrochemistry Homework Sets Assigned: 3 Weeks 3-7 Number of Quizzes: 3 1. Balancing redox equations 2. Electrochemical cells and voltage 3. The Nernst equation 4. Spontaneous and non-spontaneous equations 5. Chemical applications Determination of an Electrochemical Series Measurements Using Electrochemical Cells and Electroplating N e t I o ni c Eq u ati ons Redox Unit 3: Thermochemistry & Thermodynamics Homework Sets Assigned: 3 Weeks 7-10 Number of Quizzes: 3 1. Law of conservation of energy, work, and internal energy 2. Endothermic and exothermic reactions 3. Potential energy diagrams 4. Calorimetry, heat capacity, and specific heat 5. Hess's law 6. Heat of formation/combustion 7. Bond energies *Guided Inquiry: The Hand Warmer Design Challenge: Where Does the Heat Come From? Determination of Enthalpy Change Associated with a Rxn. 8. Laws of thermodynamics 9. Spontaneous process and entropy 10. Spontaneity, enthalpy, and free energy 11. Free energy 12. Free energy and equilibrium 13. Rate and Spontaneity N e t I o ni c Eq u ati ons Double Replacement

4 Unit 4: Kinetics Homework Sets Assigned: 3 Weeks Number of Quizzes: 3 1. Rates of reactions 2. Factors that affect rates of reactions collision theory 3. Reaction Pathways 4. Rate equation determination a. rate constants *Guided Inquiry: What Is the Rate Law of the Fading of Crystal Violet Using Beer s Law? b. mechanisms c. method of initial rates d. integrated rate laws 5. Activation energy and Boltzmann distribution Single Replacement Unit 5: General & Solubility Equilibrium Homework Sets Assigned: 3 Weeks Number of Quizzes: 3 1. Characteristics and conditions of chemical 2. Equilibrium expression derived from rates 3. Factors that affect equilibrium 4. Le Chatelier's principle *Guided Inquiry: Can We Make the Colors of the Rainbow? equilibrium 5. The equilibrium constant 6. Solving equilibrium problems Anhydrides Unit 6: Acids and Bases/ Buffers and Titrations Homework Sets Assigned: 3 Weeks Number of Quizzes: 3 1. Definition and nature of acids and bases 2. Kw and the ph scale 3. ph of strong and weak acids and bases 4. Polyprotic acids 5. ph of salts 6. Structure of Acids and Bases Standardization of NaOH & Acid Base Titration Determination of Appropriate Indicators & Buffers *Guided Inquiry: Preparation of a Buffer 7. Characteristics and capacity of buffers 8. Titrations and ph curves 9. Choosing Acid Base Indicators 10. ph and solubility 11. K,P Calculations and Solubility Product Neutralization Unit 7: Atomic Structure/ Periodicity/Nuclear Homework Sets Assigned: 4

5 Weeks Number of Quizzes: 3 1. Electron configuration and the Aufbau principle 2. Valence electrons and Lewis dot structures 3. Periodic trends 4. Table arrangement based on electronic properties 5. Properties of light and study of waves 6. Atomic spectra of hydrogen and energy levels 7. Quantum mechanical model 8. Quantum theory and electron orbitals 9. Orbital shape and energies 10. Spectroscopy Synthesis of Alum Analysis of Alum Combustion Unit 8: Chemical Bonding/Organic Homework Sets Assigned: 2 Weeks Number of Quizzes: 3 1. Lewis Dot structures 2. Resonance structures and formal charge 3. Bond polarity and dipole moments 4. VSEPR models and molecular shape 5. Polarity of molecules 6. Lattice energies 7. Hybridization 8. Molecular orbitals and diagrams *Guided Inquiry: What s in That Bottle *Guided Inquiry: Investigation of Solids Molecular Geometries of Covalent Molecules Dry Lab Complex Ions Unit 9: Gas Laws Homework Sets Assigned: 3 Weeks Number of Quizzes: 3 1. Measurement of gases 2. General gas laws- Boyle, Charles, Combined, and Ideal 3. Dalton's Law of partial pressure 4. Molar volume of gases and Stoichiometry 5. Graham s Law 6. Kinetic Molecular Theory 7. Real Gases and deviation from ideal gas law 8. Graham's Law demonstration Determining the Molar Volume of a Gas Equations

6 Unit 10: Liquids, Solids, and Solutions Weeks Homework Sets Assigned: 4 1. Structure and bonding a. metals, network, and molecular b.ionic, hydrogen, London, van der Waals 2. Vapor pressure and changes in state 3. Heating and cooling curves Number of Quizzes: 2 Number of Exams: 1 4. Composition of solutions 5. Colloids and suspensions 6. Separation techniques 7. Effect on biological systems Determination of Molar Mass by Vapor Density Equations AP Review Class Periods: Approximately 8 Homework Sets Assigned: 8 Number of Quizzes: 8 Review of ALL topics 4 AP Style Review Exams Mock AP The Green Crystal Lab Students examine a demonstration size model of DNA or an alpha helix, and use their fingers to identify which atoms j base pairs are particularly involved in hydrogen bonding within the molecule, causing the helical structure. Students then discuss how the increased UV light because of ozone depletion can cause chemical reactions and thus mutations and disruption of hydrogen bonding.