AP CHEMISTRY COURSE SYLLABUS 2012-2013 Periods 3,4 Brendan Haynie brendan.haynie@boyd.kyschools.us Text Chemistry: The Central Science by Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten, and Catherine J. Murphy, Pearson Prentice Hall, 12th edition, 2012. Schedule Listed below is the unit schedule for AP Chemistry. The first semester covers the first six units while the second semester covers the remaining four units. Tests will typically cover multiple units. SUPPLIES: notebook, lab notebook (hard bound), graph paper, calculator GRADING SCALE: 90-100 80-89 70-79 60-69 0-59 A B C D F GRADING PROCEDURE: 1. TESTS - 50% 2. PROBLEM SETS - 15% 3. LAB REPORTS, consisting of purpose, procedure, data, data analysis, and conclusion 25% 4. TERM FINALS - 10% TOPICS TO BE COVERED Unit 1 Reading: Chapters 1-2 of Brown, LeMay, Bursten, and Murphy. Topics: Welcome back to Chemistry (Atoms, Molecules, and Ions) 1. Atoms and the Periodic Table 2. Molecules and molecular compounds 3. Ions Unit 2 Reading: Chapters 3-4 of Brown, LeMay, Bursten, and Murphy. Topics: Stoichiometry and Predicting Reactions Products 1. Chemical equations 2. Patterns of chemical reactivity 3. Formula weights 4. Avogadro's number and the mole 5. Empirical formulas from analysis 6. Quantitative information from balanced equations 7. Limiting reactants 8. Properties of aqueous solutions 9. Precipitations reactions 10. Acid-base reactions 11. Oxidation-reduction reactions, 12. Concentrations of solutions, 13. Solution stoichiometry and chemical analysis Labs: 1. Determination of the Empirical Formula of Silver Oxide The determination of the percent composition and empirical formula of silver oxide 2. Finding the Ratio of Moles of Reactants in a Chemical Reaction The method of continuous variations is used to determine the mole ratio of two reactants in an oxidation-reduction reaction 3. Liquid Chromatography Liquid chromatography is used to separate the components of unsweetened grape Kool-Aid 4. Gravimetric Analysis of a Metal Carbonate The identity of a Group 1 metal carbonate is determined gravimetrically using a double replacement precipitation reaction Unit 3 Reading: Chapter 5 of Brown, LeMay, Bursten, and Murphy. Topic: Themochemistry 1. 2. 3. 4. 5. 6. What is energy? First law of thermodynamics Enthalpy and enthalpies of reactions Calorimetry Hess's Law Enthalpies of formation Labs: 1. Enthalpy of Reaction and Hess's Law Hess’s Law is verified through application to three acid-base reactions and the measurement of heats of reaction using a calorimeter Unit 4 Reading: Chapters 6-7 of Brown, LeMay, Bursten, and Murphy. Topics: The Electronic Structure of Atoms and Periodic Properties of the Elements 1. Wave nature of light 2. Quantized energy and photons 3. Bohr Model 4. Wave behavior of matter 5. Quantum mechanics and atomic orbitals 6. Many electron atoms 7. Electron configurations and the periodic table 8. History of the periodic table 9. Effective nuclear charge 10. Size of atoms and ions 11. Ionization Energy 12. Electron Affinities 13. Properties of metals, nonmetals, and metalloids 14. Trends for Groups 1A, 2A, 6A, 7A, and 8A Labs: 1. Atomic Spectra and Atomic Structure Examine the emission spectra for a series of Group 1A and Group 2A elements 2. An Activity Series Determine the activity series for five metals and three halogens Unit 5 Reading: Chapters 8-9 of Brown, LeMay, Bursten, and Murphy. Topics: Chemical bonding and Predicting and Understanding Molecular Shapes 1. Chemical bonds 2. Lewis structures, and the octet rule 3. Ionic bonding 4. Covalent bonding 5. Bond polarity and electronegativity 6. Resonance structures 7. Exceptions to the octet rule 8. Strengths of covalent bonds 9. Molecular shapes 10. VSEPR model 11. Hybrid orbitals 12. Multiple bonds 13. Molecular orbitals and their application to diatomics and simple systems Labs: 1. Molecular Geometries of Covalent Molecules Examine the Lewis structures, VSEPR models, and three dimensional structures of a series of simple covalently bonded molecules 2. Computational Models for Diatomics and Simple Systems Use ab initio computational methods to compute molecular orbitals for a selection of diatomics and simple polyatomic molecules Unit 6 Reading: Chapters 10-11 of Brown, LeMay, Bursten, and Murphy. Topics: Gasses, Liquids, and Solids 1. Pressure 2. Gas Laws (Boyle's Law; Charles's Law; Avogadro's Law) 3. Ideal Gas Equation 4. Molar Mass 5. Partial Pressure (Dalton's Law of Partial Pressures) 6. Kinetic-Molecular Theory 7. Effusion & Diffusion (Graham's Law) 8. Real Gases 9. Comparison of gases, liquids, and solids 10. Intermolecular forces & properties of liquids 11. Phase changes 12. Vapor Pressure 13. Phase diagrams 14. Structures and bonding of solids Labs: 1. Determining the Molar Volume of a Gas Determine the volume of one mole of H2 gas at STP 2. Determination of the Molar Mass of Volatile Liquids Determine the molar masses of various volatile liquids 3. Analysis of Alum Determine the melting point and mole ratio of hydrated water to anhydrous aluminum potassium sulfate in AlK(SO4)2.12H2O Unit 7 Reading: Chapters 13-14 of Brown, LeMay, Bursten, and Murphy. Topics: Properties of Solutions and Chemical Kinetics 1. The solution process 2. Saturated solutions and solubility 3. Factors affecting solubility 4. Expressing concentration 5. Colligative properties 6. Colloids 7. Description of reactions rates and factors affecting reaction rates 8. The rate law and impact of concentration 9. Change of concentration with time (1st and 2nd order reactions) 10. Temperature and rate 11. Reaction mechanisms 12. Catalysis Labs: 1. Molar Mass by Freezing Point Depression Determine the molar mass of an unknown by measuring the freezing point depression of a solution of the unknown and BHT 2. Preparation and Analysis of Tetraamminecopper(II) Sulfate Monohydrate Synthesize Tetraamminecopper(II) Sulfate Monohydrate (one class period). 3. Kinetics of a Reaction Determine total rate law for the oxidation of iodide ions by bromate ions in the presences of acid Unit 8 Reading: Chapters 15-16 of Brown, LeMay, Bursten, and Murphy. Topics: Chemical Equilibrium and Acid-Base Equilibria 1. Concept of equilibrium and the equilibrium constant 2. Interpreting and working with equilibrium constants 3. Heterogeneous equilibria 4. Calculating equilibrium constants 5. Applications of equilibrium constants 6. Le Châtelier's Principle 7. Brønsted-Lowry acids and bases 8. Autoionization of water 9. pH scale 10. Strong acids and bases 11. Weak acids and bases 12. Relationship between Ka and Kb 13. Acid-base properties of salt solutions 14. Acid-base behavior and chemical structure 15. Lewis acids and bases 16. Expressing concentration Labs: 1. The Determination of Keq for FeSCN2+ Determine the equilibrium constant for the reaction of Fe3+ and SCN2. The Determination of Ka for a Weak To experimentally determine the pKa values for two weak acids Unit 9 Reading: Chapters 17 and 19 of Brown, LeMay, Bursten, and Murphy. Topics: Aqueous Equilibria and Chemical Thermodynamics 1. The common ion effect 2. Buffered solutions, acid-base titrations 3. Solubility equilibria, Ksp 4. Factors affecting solubility 5. Precipitations and separation of ions 6. Qualitative analysis for metallic elements 7. Spontaneous processes 8. Entropy and the second law of thermodynamics 9. Molecular interpretation of entropy 10. Entropy changes in chemical reactions 11. Gibbs free energy 12. Free energy and the equilibrium constant Labs: 1. Acid Base Titrations Standardize a solution of NaOH and then titrate an unknown acid 2. Preparation and Properties of Buffer Solutions Prepare and investigate the properties of several buffer solutions 3. Separation and Qualitative Determination of Cations and Anions Determine the cations and anions present in a solution by qualitative analysis Unit 10 Reading: Chapters 20, 21, and 25 of Brown, LeMay, Bursten, and Murphy. Topics: Electrochemistry, Nuclear Chemistry, and Organic Chemistry 1. Oxidation states and oxidation-reduction reactions 2. Balancing oxidation-reduction equations 3. Voltaic cells 4. Cell EMF under STP 5. Free Energy and Redox reactions 6. Cell EMF under nonstandard conditions 7. Batteries and fuel cells 8. Corrosion 9. Electrolysis 10. Radioactivity 11. Patterns of Nuclear stability 12. Nuclear transmutation 13. Rates of radioactive decay 14. General characteristics of organic molecules 15. Hydrocarbons 16. Alkanes, alkenes, and alkynes (structures and reactions) 17. Organic functional groups 18. Chirality in organic chemistry Labs: 1. Analysis of Commercial Bleach The amount of NaClO in commercial bleach will be determined 2. Electrolysis Use an electrolysis cell to electrolyze an acidic solution of CuSO4 3. Synthesis of Aspirin and Wintergreen Oil Synthesize acetylsalicylic acid and methyl salicylate using salicylic acid as our starting point