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AP CHEMISTRY COURSE SYLLABUS COURSE OVERVIEW This course is a college-level chemistry course for competent and highly motivated high school students and is designed to be the equivalent of a college-level introductory chemistry course. The course is a second year chemistry course where general chemistry is a prerequisite. The overall curriculum follows the guidelines of the Collegeboard for AP Chemistry. AP chemistry differs significantly from your general chemistry course with respect to the kind of textbook used, the range and depth of topics covered, the kind of laboratory work done, and the time and effort required. The aim of this course is to provide you with the conceptual framework, factual knowledge, and analytical skills necessary to deal critically with the theoretical and practical applications of chemistry. MEETING TIMES: This course meets every other day for 90 minutes. This provides adequate time to perform laboratory activities on any given day. THEMES: This course is centered on the 4 major themes, Structure of Matter, States of Matter, Chemical Reactions, and Descriptive Chemistry, listed in the AP Chemistry description. Within each of these themes, there will be topics that are extensions of subject matter learned in general chemistry as well some completely new topics that will be discussed in detail. LAB COMPONENT Students work in small groups to complete the labs. Labs involve setting up the lab, answering a series of pre-lab questions, performing the experiment, analyzing results and formalize their conclusion which we then discuss at the beginning of the next class period. Labs write-ups are completed in a lab notebook and turned in for grading following the discussion. Many of the labs are interfaced with computers and labquest sensors to accurately collect and analyze data using temperature, pressure, pH, and colorimeters. Statistical analysis of data is emphasized. . Text: Chemistry – Zumdahl 5th Edition Chapters 1-17. Theme AP Required Topics Coursework/ Text Resource Laboratory Work Review Topics covered in General Chemistry (summer) Scientific Method, hypotheses, laws, theories, significant figures, Classification of Matter, Writing Ionic and covalent compounds, solve problems involving basic stoichiometry, basic gas laws, basic periodic table relationships Lab: Vernier: “Find the relationship” (transposing graphical data to linear relationships to determine relationships between x and y. Atomic theory and atomic structure 1. Evidence for the atomic theory 2. Atomic masses; determination by chemical and physical means 3. Atomic number and mass number; isotopes Structure of 4. Electron energy levels: atomic Matter spectra, quantum numbers, atomic orbitals Work and solve basic stoichiometry problems using the mole concept and basic gas law problems using the ideal and combination gas law equations. Chapter 2: Atoms, Molecules and Ions. (1 lesson) History of AtomDalton, Thomson, Rutherford, Atomic Mass, Mass Number, Isotopes, Ions, Protons, Neutrons, Electrons Chapter 7: Atomic Structure and Periodicity (2wk) Electromagnetic Radiation, Bohr Model, Quantum Model, Quantum Numbers and orbital shapes Work and solve problems using Atomic Structure Equations. Lab: “Beer’s Law Mechanical Universe: Models of the Atom Video. Lab: Bohr Model Energy Levels of Hydrogen (Spectral Lines) Theme Structure of Matter (cont) AP Required Topics Coursework/ Text Resource 5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states Periodic Trends for Ionization energy, Atomic radii, Ionic radii, electron affinities. Reasons for oxidation numbers based on Quantum model B. Chemical bonding 1. Binding forces a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces) b. Relationships to states, structure, and properties of matter c. Polarity of bonds, electronegativities 2. Molecular models a. Lewis structures b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds c. VSEPR 3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure Chapter 8-9: Bonding: General Concepts And Orbital Bonding. (3 lessons) C. Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical Applications Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces) Polarity of bonds via electronegativity. Polarity of molecules based on Lone-pair electrons and VSPER Lewis structures. Hybridization, Resonance, sigma and pi bonds. Laboratory Work Lab: Bonds, Polarity and Solubility Lab: “Liquid Chromatography” Chapter 20: Sec 1-7 (1 lesson) Isomerism and Coordination Complex Compounds Chapter 21: The Nuclear Atom (2 lessons) Types of Decay: Alpha, Beta, Gamma. Nuclear Reactions, Half-lives. Fission, fusion Lab: Radioactive decay and half life Lab: Shielding (alpha, beta, gamma) Theme States of Matter AP Required Topics Coursework/ Text Resource Laboratory Work A. Gases 1. Laws of ideal gases a. Equation of state for an ideal gas b. Partial pressures 2. Kinetic molecular theory a. Interpretation of ideal gas laws on the basis of this theory b. Avogadro’s hypothesis and the mole concept c. Dependence of kinetic energy of molecules on temperature d. Deviations from ideal gas laws Chapter 5: Gases (Conceptual and mathematical relationships) (3 lessons) Boyles, Charles, Avagadro’s Laws, Combination Law, Ideal Gas law. Dalton’s Law of partial Pressure Gas Stoichiometry Kinetic Theory of Gases Root mean square velocity Deviations from the ideal gas law Work and solve problems using Gas Law equations: Labs: 1)“Gas laws relationships” 2) Molar Mass of Butane Lab 3) Diffusion Lab Theme States of Matter (cont) AP Required Topics Coursework/ Text Resource B. Liquids and solids 1. Liquids and solids from the kineticmolecular viewpoint 2. Phase diagrams of one-component systems 3. Changes of state, including critical points and triple points 4. Structure of solids; lattice energies Chapter 10: Liquids and Solids: (3 lessons ) Explanation of boiling pts based on molar mass and types of bonding (London, dipole-dipole, hydrogen bonding) Structure of water in all three phases including relative number of hydrogen bonds in each phase. Connection to surface tension in liquid phase. Ionic solids, molecular solids, metallic solids, network solids and their lattice structures. Phase change vs time diagrams for substances. Pressure vs. temp. phase change diagrams for substances and descriptions of critical points and triple points. Laboratory Work Lab: Freezing and Melting pt of water. Theme States of Matter (cont) AP Required Topics Coursework/ Text Resource Laboratory Work C. Solutions 1. Types of solutions and factors affecting solubility 2. Methods of expressing concentration (use of normalities is not tested) 3. Raoult’s law and colligative properties (nonvolatile solutes); osmosis 4. Nonideal behavior (qualitative aspects) Chapter 11: Solutions (2 lessons) Molality and Molarity conceptual and mathematical Mole fraction (math) Lab: Mixing Solutions Structure, pressure, temp effects on solubility Lab: Freezing pt depression Raoult’s Law concepts and mathematical Freezing pt depression, Boiling pt Elevation (math) Osmotic Pressure Non-ideal Solutions (math) Work and solve problems using solutions equations: Theme Reactions AP Required Topics Coursework/ Text Resource Laboratory Work A. Reaction types 1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism Chapter 4: Reactions and Solution Stoichiometry (3 lessons) 1.Predicting and balancing reactions by recognizing, composition, decomposition, single replacement, double replacement reactions (review Gen Chem) 2. Balancing Molecular, Ionic and net ionic reactions Predicting precipitation reactions based on solubility rules. (review Gen Chem) 3. Balancing Redox reactions including halfreaction method. Lab: “Deterinining the Mole ratio in a chemical reaction” Lab: “Conductimetric Titration and Gravimetric determination of a precipitatie 2. Precipitation reactions 3. Oxidation-reduction reactions a. Oxidation number b. The role of the electron in oxidationreduction 4. Acid-Base definitions based on Arrhenius, Bronstead-Lowry and Lewis Concepts. 5. Acid-Base Reactions including Stoichiometry Lab: OxidationReduction Titration: Reaction of Fe2+ and Ce4+ Lab: Acid-Base Titration (Determining concentration of unknown acid) Lab: “Investigating Indicators” Theme AP Required Topics Coursework/ Text Resource Laboratory Work Reactions (cont) c. Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions Chapter 17: Electrochemistry (3 lessons) Galvanic and Electrolytic Cells Faraday’s Law Standard Cell Potential, Calculating Cell potential using Nernst Equation (math) and predicting direction of redox half reactions. Lab:“Electrochemistry: Voltaic Cells” Lab: ”Electroplating” Work and solve problems using Electrochemistry equations: B. Stoichiometry 1. Ionic and molecular species present in chemical systems: net ionic equations 2. Balancing of equations including those for redox reactions 3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants C. Equilibrium 1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s Chapter 3: Stoichiometry (2 lessons) (80% review from Gen Chemistry) 1. Predicting and balancing reactions by recognizing, composition, decomposition, single replacement, double replacement reactions and net ionic reactions. 2. Mole concept with reactions. Determining Mass, moles, volume @STP and non-STP values. 3. Calculate empirical, molecular formulas, and percent yield for reactions and or lab activities. Empirical formula labs Lab: “Tin(II) or Tin (IV)Oxide” Lab: “Formula of a hydrate” Lab: “%Yield of a chem. Reaction” Theme AP Required Topics Coursework/ Text Resource principle; equilibrium constants 2. Quantitative treatment a. Equilibrium constants for gaseous reactions: Kp, Kc Chapter 13: Chemical Equilibrium (3 lessons) 1. Equilibrium Constant and concepts 2. Le Chatelier’s Principle and direction of equilibrium shift based on changes in conditions. 3. Equilibrium expressions in terms of Pressure and concentration Kp, Kc (math) 4. Using ICE method to determine concentrations at equilibrium. b. Equilibrium constants for reactions in solution (1) Constants for acids and bases; pK; pH Reactions (cont) (2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds (3) Common ion effect; buffers; hydrolysis Chapter 14: Acids and Bases (2 lessons) Determining equilibrium constants for weak acids and bases. Chapter 15: Solubility Products (2 lessons) Apply equilibrium concepts to Solubility. Determine solubility product for chemical reactions Chapter 15: Applications of Aqueous Equilibrium (3 lessons) 1. Calculating pK for acids and bases (math) 2. Calculating pH of strong, weak and Buffer solutions including math. 3. Acid-Base properties of Salts…neutral pH, acidic pH, basic pH conceptual and mathematical 4. Titration curves for strong-strong, weakstrong, and weak-weak acid base reactions. 5. Hydrolysis applications Laboratory Work Lab: “Determination of the equilibrium constant” Lab: Determining Ksp Lab: pH titration Curves Lab: Buffers Theme AP Required Topics Coursework/ Text Resource Work and solve problems using Equilibrium equations: Reactions (cont) Laboratory Work Theme Reactions (cont) AP Required Topics Coursework/ Text Resource Laboratory Work D. Kinetics 1. Concept of rate of reaction 2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws 3. Effect of temperature change on rates 4. Energy of activation; the role of catalysts 5. The relationship between the ratedetermining step and a mechanism Chapter 12: Chemical Kinetics (3 lessons) 1. Rate law concepts and equation 2. Conceptual understanding of how temp effect the rate of reaction. 3. Determine the order of reactions (0,1,2) based on concentration vs. time graphs and based on tables of initial concentrations and rates or graphs of concentration vs. time 4. Concepts of catalysts 5. Determining half-life based on rate equations 6. Determining activation energy based on concentration data. Work and solve kinetics problems using Kinetics equations: Lab:“Rate and Order of a Chemcial Reaction” Lab: “Rate determination and Activation energy” Theme AP Required Topics Coursework/ Text Resource Laboratory Work E. Thermodynamics 1. State functions 2. First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law; heats of vaporization and fusion; calorimetry Chapter 6: Thermochemistry (2 lessons) 1. Explain each of the 3 laws of thermodynamics and their consequences and connections. 2. Enthalpy concepts and calculations. 3. Hess’s Law (enthalphy calculations) 4. Heats of vaporization and Fusion. 5. Calorimetry within one phase. 6. Multiple phase calorimetry Lab: Determining the Enthalpy of a chemical Reaction Work and solve problems using Thermo equations. Reactions (cont) 3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes 4. Relationship of change in free energy to equilibrium constants and electrode Potentials Chapter 16: Spontaneity, Entropy, and Free Energy (2 lessons) 1. Spontaneity and change in Entropy 2. Entropy change in chemical reactions 3. Free Energy and Chemical reactions 4. Relationship between entropy, Enthalpy and Free energy (math) 5. Free energy and electric potential (math) Lab: Heat of Vaporization of liquid Nitrogen Lab: Melting/Freezing of water. Theme AP Required Topics Coursework/ Text Resource Laboratory Work Work and solve problems using the Thermodynamic equations Reactions (cont) Descriptive Chemistry 1. Chemical Reactivity After students have completed the first nine weeks of coursework which includes the atomic structure and chemical reactions every Monday begins with a series of reactions that they must identify and complete. (similar to net ionic reactions free response from AP Exam). This process requires them to formalize their understanding of solubility rules, redox, Oxide reactions etc. As the course progresses additional reaction types are added such as Acid-Base reactions until they are very comfortable with the reaction and reactivity relationships. Lab: “Seperation and Qualitative Analysis of Cations” Lab: “Seperation and Qualitative Analysis of Anions” Theme AP Required Topics 2. Relationships in periodic table Descriptive Chemistry (cont) 3. Organic Chemistry Coursework/ Text Resource Laboratory Work These topics are built into the atomic structure section and referred to throughout the course to provide the atomic level understanding of each topic covered throughout the course. Students will: 1. Apply periodic law to predit reaction products 2. Discuss activity series 3. Distinguish between metals and nonmetals 4. Use periodic table to predict common oxidation states. 5. Predict single replacement reactions based on activity series. 6. Predict products of aqueous double replacement reactions based on solubility rules. Chapter 22: Organic Chemistry Sec 1-5 (1 lessons) Alkenes, Alkanes, Alkynes Structures Lab: Synthesis and Analysis of Aspirin