A.P. Chemistry. Welcome to AP Chemistry!

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1 A.P. Chemistry Mrs. Sarah Beery Room Prep Period: 6 th hour (M, W, F :4 :0, T, TH : :0) Welcome to AP Chemistry! Course Description : The purpose of AP Chemistry is to provide a college level course in chemistry and to prepare the student to undertake a second year of chemistry as a college freshman or to register in courses in other fields where general chemistry is a prerequisite. This course is structured around the six big ideas and seven science practices given in the AP Chemistry Curriculum Framework provided by the College Board ( chemistry course and exam description.pdf ). Hands on laboratory work will be an integral part of the course and account for more than % of class time. AP Chemistry emphasizes depth of understanding and application of science skills. Course Specifics : Students taking AP Chemistry should have successfully completed Chemistry and Algebra II. At the end of each unit/topic, assessments and study guides utilizing questions from old AP exams will be given. Students should be preparing to take the College Board AP exam, which is administered in May of each year. The AP exam involves numerous mathematical calculations and an understanding of how to answer multiple choice and free response questions; therefore, these skills will be both emphasized and developed throughout the year. Grading Policy : The grade you get on your report card is a measurement of what you have learned. Grades are calculated by formative assessments given in class, summative assessments given at the end of each unit, and successful completion of laboratory work. Semester exams, per school policy, will be 0% of your final grade. Text : Brown, Theodore L., et al. Chemistry: The Central Science. th ed. New Jersey: Prentice Hall, 0. Laboratory : All of the laboratory experiments in this course are hands on. Students work in groups of one, two, or three, depending on the lab. Inquiry is emphasized in many of the experiments that students complete. Each lab requires following and/or developing processes and procedures, taking observations, manipulating data, collaborating with peers, and reporting results. For all labs, students are required to report the purpose, procedure, all data, data analysis, error analysis, results, and conclusions in a lab notebook that is submitted for grading. Formal and informal communication and comparison of results will also be required. Laboratory experiments are taken from a variety of sources, including but not limited to,. Nelson, John H., et al. Chemistry: The Central Science, Laboratory Experiments. th ed.. Wagner, Maxine. Chemistry: The study of matter, Laboratory Manual. 4 th ed. 3. Flinn Scientific: ChemTopic Labs. Experiments & Demonstrations in Chemistry. 4. Vonderbrink, Sally Ann. Laboratory Experiments for Advanced Placement Chemistry. nd ed.. The College Board. AP Chemistry Guided Inquiry Experiments: Applying the Science Practices. 03. Demonstration Resources :. Flinn Scientific: ChemTopic Labs. Experiments & Demonstrations in Chemistry.. Koob, John K., et al. A Demo A Day: A Year of Chemical Demonstrations. Vol. and. Classroom Procedures: At this level, you are expected to stay organized and on task at all times. Any assignment given will be due at the beginning of the hour the next day (unless specified differently). Any late assignment is deducted 0%. Once the test is given for the unit, you need to have the assignment completed to retake the test (see requirements below).

2 Absence Policy: Makeup Work It is your responsibility to pick these assignments up upon return. Please label absent work as ABSENT and place in the homework tray! o If you miss class due to an excused absence, you are responsible for any notes and assignments. If it is a school function, get your assignment(s) ahead of time! o If you miss a laboratory exercise, quiz or test, you will need to contact me to make arrangements to come in before or after school or at lunch and complete it. o For lengthier absences, I will make arrangements with you on an individual basis. Test Retake Policy: You may retake any test at any time during the marking period or until the date given to you in class. In order to retake a test, you must o Have no missing assignments for the unit (even if it is for zero credit). o Complete a retake review sheet and a retake test form. o Set up a time outside of the normal class time to come in and take the test. o In addition, the retake score will replace your first test score, and the retake test will be a different test than the original one given. o If you fail your first attempt of a unit test (not the semester final), you will be assigned a retake test. Until this test is retaken, your score in the gradebook will show that you have not mastered the material. If it is not, your parents will be notified and arrangements will need to be made. The above requirements still apply. Phones/Personal Devices: NOT ALLOWED. An SLHS Chromebook and an in class calculator will be the only devices needed for Chemistry. Please see SLHS School Board approved handbook policy. Course Outline : Unit One: Introduction & Basics Review,, 3. Scientific Method Guided Inquiry: Density Lab (SP, 3, 4).7. Separation Science Students demonstrate safe lab practices,.0 3. Temperature and Density 4. The Periodic Table (brief) read chemical labels, and determine the identity of an unknown compound by measuring density. Math Review / Dim. Analysis 6. Units of Measurement Lab: Measuring Skills (SP, 4) 7. Uncertainty in Measurement Students demonstrate knowledge of proper equipment choice and significant figures/unit conversions Activity: Introducing the Periodic Table! (SP 6) Students will present a short report on a chosen aspect of the periodic table, including properties and trends Lab: Paper Chromatography (SP 3, ) Students are introduced to separation science and different procedures while completing a simple chromatography experiment Unit Two: Atomic Structure, 6,. Subatomic Particles Activity: Bean Bag Isotopes (SP,, 4, ).. The Nucleus Students study atomic mass and atomic.6 3. Mass Spectroscopy and Isotopes 4. Stability of the Nucleus. Atomic Structure structure using beans as an isotopic model Lab: Flame Tests of Salt Solutions (SP, 3) Rutherford Experiment Students demonstrate knowledge of.3 7. Cathode Ray Experiments 8. Electromagnetic Radiation electron energy transitions while trying to identify an unknown element.4.

3 9. Quantization of Energy 0. Photoelectric Effect. PES Data. Bohr Atom 3. Spectroscopy 4. Orbital Model of the Atom. Paramagnetism 6. Quantum Model 7. Nuclear Equations Lab: Atomic Spectra and Atomic Structure (SP, 4, ) Students determine the emission spectrum and energies of various known gases from discharge tubes Unit Three: Periodicity and Introduction to Bonding 7, 8,, 3. Atomic Properties. Periodic Law 3. Elemental Properties 4. Types of Bonds. Metallic Bonding 6. Properties of Group One 7. Properties of Period Two 8. Metals vs. Nonmetals 9. Transition Metals 0. Ionic Bonding. Ionic Bonding and Potential Energy Diagrams. Energy of Formation of Ionic Compounds 3. Lattice Energy Guided Inquiry: What s In That Bottle? (SP, 4,, 6, 7) Students determine the type of bonding in unlabeled chemicals using their physical and chemical properties Activity: Graphing of Periodic Trends (SP ) Students are given data sets to analyze and graph in order to predict and identify periodic trends Unit Four: Covalent Bonding and Molecules 8, 9,. Types of Covalent Bonds. Nonpolar Covalent Bonds Lab: Molecular Geometries of Covalent Molecules; Lewis Structures and VSEPR Theory (SP, 6).. 3. Polar Covalent Bonds Students draw Lewis structures of common.3 4. Coordinate Covalent Bonds Lewis Acids and Lewis Bases. Lewis Structures 6. Resonance molecules and then use model kits to predict shapes using VSEPR theory Activity: State, Temperature, and Bonding (SP, 6) Hybridization Given the structure of common molecules,. 8. Molecular Geometry 9. Energy Effects on Molecules 0. Isomerism. Functional Groups. Interactions of Functional Groups 3. Classification of Molecules students must predict the bonding present, the state at room temperature, and explain the differences and/or discrepancies in their reasoning Intermolecular Interactions. Dipole Moments 6. Dielectric Constants 7. Types of Compounds 8. Properties of Metallic, Molecular, Macromolecular and Ionic Compounds Unit Five: Organic Chemistry, 4. Hydrocarbons. Functional Groups 3. Structural Formulas Lab: Synthesis, Isolation, and Purification of an Ester (SP, 4,, 6)

4 4. Saturated and Unsaturated Compounds. Nomenclature 6. Isomers 7. Alcohols 8. Aldehydes 9. Ketones 0. Acids. Esters. Ethers 3. Amines 4. Polymers Unit Six: Reactions Students conduct a synthesis reaction, isolate the product by solvent extraction, and purify the product by distillation Activity: Comparison of Functional Groups (SP, 6, 7) Students create a visual representation of each functional group, the basic properties of the group, and some known compounds in that group, as well as identifying key differences between groups 4, 6, 0. Naming Compounds. Balancing Chemical Equations Guided Inquiry: Redox Titration (Determination of % H O ) (SP, 4, 6) Types of Chemical Equations Students will create procedures to Types of Chemical Reactions. Predicting Based on Stability 6. Predicting Based on Type 7. Chemical Reactivity and Products of Chemical Reactions 8. Hydrates 9. Net Ionic Equations standardize a potassium permanganate solution and then use that to evaluate the concentration of commercial H O bottles Lab: Percent Water in a Hydrate (SP,, ) Students determine the percent water in a hydrate in order to identify an unknown hydrate from a list of possibilities Activity: The Synthesis of a Common Drink (Research Project) (SP, 3,, 6, 7) Students research a household drink in order to determine if it is created by chemical reaction or a mixture of multiple substances Unit Seven: Stoichiometry, 3, 4. Law of Constant Composition and Guided Inquiry: Stoichiometry (Green Chemistry). Calculations Based on Law (SP, 4,, 6) 3.. Using Moles to Find a Quantity Students design a procedure to separate two.3 3. Stoichiometry substances using green chemistry principles and.4 4. Limiting Reagents then analyze the reports.7. Using Density.8 6. Solution Terms Lab: Finding the Ratio of Moles of Reactants in a.9 7. Solution Stoichiometry Chemical Reaction (SP, 4, ) Using the method of continuous variations, 3.4 students will determine the mole ratio of two 3. reactants 3.6 Unit Eight: Thermochemistry, 3, 9. Intro to Thermodynamics. Conservation of Energy 3. State Functions 4. Potential Energy. Kinetic Energy 6. Calorimetry 7. Heat of Fusion 8. Heat of Vaporization 9. Specific Heat Guided Inquiry: The Hand Warmer Design Challenge (SP,, 4,, 6, 7) Students will determine which substances, in what amounts, to use in order to make a hand warmer that is economical and both safe and environmentally friendly Lab: Enthalpy of Reaction and Hess s Law (SP, 4, )

5 0. Heat of Dilution. Heat of Solution. Hess s Law 3. Bond Dissociation Energies 4. Gibbs Free Energy Equation Students verify Hess s Law using calorimetry Activity: Entropy and Human Society (SP, 3, 6, 7) Students will use the growth of the human population to model entropy and discuss the consequent effects Unit Nine: States of Matter 0,,. Real Gases vs. Ideal Gases. Ideal Gas Equation 3. Derivations Based on the Ideal Gas Equation 4. Gases Collected Over Water. Kinetic Molecular Theory 6. Van Der Waals Equation 7. Molecular Speeds 8. Diffusion and Effusion 9. Phase Changes 0. Entropy. Heating and Cooling Curves. Interfaces 3. Pressure 4. Vapor Pressure. Boiling Points and Freezing Points 6. Vapor Pressure Curves 7. Phase Diagrams/Energy Changes 8. Viscosity 9. Surface Tension 0. Types of Solids and Crystal Structure Lab: Determining the Molar Volume of a Gas (SP, 4, ) Students perform a chemical reaction in order to determine the volume of one mole of hydrogen gas at STP Lab: Determination of the Molar Mass of Volatile Liquids (SP, 4, ) Students volatize and condense liquids in a fixed volume in order to determine the liquids molar mass Activity: Rate of Effusion (SP, 3, 4, ) Students predict which gas will effuse better and then watch a simple demonstration of gases effusing Activity: Life on Planet V (SP Students are given a list of items and asked to decide and defend which would work on a planet with no atmosphere Unit Ten: Solutions 3. Types of Solutions. Electrolytes 3. Miscibility and Immiscibility Guided Inquiry: Spectroscopy: The Relationship Between the Concentration of a Solution and the Transmitted Light (SP, 4,, 6) Dissolution vs. Ionization Students will use spectroscopy to design an. Solubility Terms 6. Solubility Curves experiment that determines how the concentration of a solution is related to transmitted light 7. Henry s Law 8. Molarity, Molality, %, Mole Fraction, ppm, ppb Lab: Molar Mass by Freezing Point Depression (SP,, 4,, 6) 9. Dilution Problems Students identify an unknown substance by 0. Raoult s Law. Colligative Properties determining its molar mass through freezing point depression. van t Hoff Factor 3. Osmosis 4. Colloids

6 Unit Eleven: Chemical Kinetics 4. Rate s relationship to collisions. Reaction Mechanisms Guided Inquiry: How Long Will That Marble Statue Last? (SP 3, 4,, 6, 7) Activation Energy Students will change the variables relating Nature of Reactants and Interfacial Surface Area. Temperature and Pressure Effects on Rates to the reactants in a reaction in order to investigate the speed of the reaction Activity: Iodine Clock Reaction (SP, 3) Catalysts Homogeneous and Students discuss the variables that changed 4.8 Heterogeneous 7. Activated Complex and Intermediates 8. Arrhenius Equation 9. Maxwell Boltzmann Diagram during a class demonstration of the iodine clock reaction Guided Inquiry: Temperature and Reaction Rates (SP, 3, 4, ) Average Rate Students design and carry out a procedure. Graphical Determination of Instantaneous Rate that investigates the effects of temperature on a reaction between magnesium and hydrochloric acid. Rate Laws 3. Order of Reactions Activity: Sudsy Kinetics (SP, 3, 7) 4. Calculations Based on Order Students use different concentrations of H O to discuss kinetics concepts as part of a class demonstration/discussion Unit Twelve: Chemical Equilibrium. Reversible Processes and Reactions. Types of Systems 3. Kinetics and Equilibrium 4. Equilibrium Expressions. Equilibrium Constants 6. LeChatelier s Principle 7. Equilibrium Stresses 8. Equilibrium Calculations 9. Molar Solubility 0. Reaction Quotients Lab: Exploring Equilibrium (SP, 3,, 6) Students use two reversible reactions to explore equilibrium and identify conditions that affect the position of equilibrium Lab: The Determination of K eq for FeSCN + (SP, 3, 4,, 6) Students use the reaction of iron(iii) ions with thiocyanate ions under different conditions to calculate the equilibrium constant Activity: The Effect of Le Chatelier (SP, 6, 7) Students will use Le Chatelier s Principle both quantitatively and qualitatively to discuss the effects on a chemical reaction Unit Thirteen: Acid Base Chemistry 6, 7. Preparation of Acids, Bases and Salts Lab: Determination of K a of Weak Acids (SP, 3,, 6, 7) 3.0. Classification of Acids and Bases Students identify unknown weak acids Bronsted Lowry Theory 4. Degree of Ionization. Equilibrium Constants for Acids by determining their pk a values for ionization Activity: Factors Affecting Buffers (SP,, 3, 7) and Bases Students determine ph of various buffer Weak Acids and Bases 7. Ionization of Water 8. ph and poh solutions and describe the mechanism that would occur within the buffer system upon addition of an acid or a base

7 9. Ionization Calculations of Weak Acids and Bases 0. Henderson Hasselbach Equation. Titration Calculations. Common Ion Effect 3. Buffered Solutions 4. Solubility Product Constant Guided Inquiry: To What Extent Do Common Household Products Have Buffering Activity? (SP 4,, 6) Students investigate a variety of household substances to determine which of them exhibit buffering activity Unit Fourteen: Electrochemistry and Thermodynamics 9, 0. Oxidation and Reduction Lab: Electrochemical Cells (SP, 3, ) Substances Gaining Potential Students experimentally construct a Types of Electrochemical Cells 4. Voltaic Cells. Cell Potentials 6. Concentration Dependence of E 7. Nernst Equation 8. Cell Potentials and Equilibrium 9. Metal / Reference / Indicator Electrodes 0. Electrolysis. Faraday s Law. Electrolytic Cells 3. Order of Reduction 4. Gibbs Free Energy Equation. Relationship of Equilibrium, Q and E standard table of reduction potentials, and then use that to experimentally compare a measured voltage with a calculated voltage (using the Nernst equation) Unit Fifteen: Review All All Review AP Chemistry Exams