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Advanced Placement Chemistry Advanced Placement Chemistry Text Chemistry, The Central Science by Brown, LeMay, and Bursten, 10th ed., Pearson Prentice Hall, 2006. ISBN: 0-13-193719-7 Test Preparation 5 Steps to a 5: AP Chemistry, by John T. Moore and Richard H. Langley, McGraw Hill, 2012 Laboratory Resources Laboratory Experiments for Advanced Placement Chemistry, by Sally Ann Vonderbrink Advanced Chemistry With Vernier, by Jack Randall Chemistry, The Central Science, by Brown, Lemay, and Bursten Flinn Scientific AP Chemistry Labs Prerequisite Honors Chemistry Requirements AP Chemistry is a second-year chemistry course for the advanced student. The class meets 8 periods per week with two single (45-minute) period classes and three double (90- minute) classes. An additional 4-5 hours per week outside of class is expected. Each week, at least one of the double periods will be devoted to laboratory experimentation. Students will record all experiments in a laboratory notebook and follow the prescribed format. This lab report format includes the purpose, a brief description of the procedure followed, data and observations, calculations and a conclusion. The notebook is mandatory and graded at the completion of each lab. Students will work with a lab partner on all experiments. All students are expected to take the Advanced Placement Chemistry Exam in May. AP practice problems and free-response questions are completed at the end of each chapter. Students are encouraged to work together in order to facilitate learning. Grading Tests 40% Lab Reports 30% Quizzes 20% Homework 10% Course Outline Chapter 1: Matter and Measurement Chapter 2: Atoms, Molecules, and Ions 1.0 Weeks Chapters 1 and 2 are completed during the summer. A brief review will precede the first exam. The student will: Classify and distinguish between pure substances, mixtures, elements, and compounds Identify chemical and physical properties of substances Describe the most appropriate means of separating various types of mixtures Differentiate between quantitative and qualitative properties Demonstrate fluency in the use of the metric system and SI units and unit conversion Demonstrate competency in the necessity and use of significant figures in measurements Describe atomic structure and the experiments leading to its discovery Describe the relationship between isotopes, mass number, and average atomic mass Use the periodic table to predict the charges of ions and the empirical formulas of ionic compounds Apply the rules of chemical nomenclature to organic compounds Laboratory Basic Laboratory Techniques (Chemistry, The Central Science) Chapter 3: Stoichiometry 2.0 Weeks The student will: Interpret and balance chemical equations Differentiate between synthesis, metathesis, decomposition, combustion, and single-displacement reactions Use formula weights to calculate percent composition of a compound Interconvert between masses, moles, and number of particles Calculate empirical and molecular formulae of compounds Determine empirical formula by combustion analysis Calculate limiting and excess reactants , theoretical and percent yield for a reaction Demonstration: Types of Reactions Laboratory Finding the Ratio of Moles of Reactants in a Chemical Reaction (Vonderbrink) Determining the Formula of a Hydrate Finding the Ratio of Moles of Reactants in a Chemical Reaction (Vonderbrink) Chapter 4: Aqueous Reactions and Solution Stoichiometry 2.0 Weeks The student will: Differentiate between non-electrolytes, strong and weak electrolytes Use solubility rules to differentiate between soluble and insoluble compounds Identify precipitates and spectator ions in a chemical reaction Represent a chemical reaction with a net-ionic equation Predict the products of a neutralization reaction Determine oxidation numbers of atoms to differentiate between oxidation and reduction processes Identify Redox reactions using the Activity Series of Metals Use stoichiometry to determine amounts or concentrations of various substances Interconvert molarity, moles, and volume Prepare a dilution from a stock solution Use solution stoichiometry to identify the concentration of a solute by titration Demonstration: Strong, Weak, and Non-Electrolytes Laboratory Acid Base Titration (strong acid-strong base and weak acid-strong base) (Vernier) Determining the Empirical Formula of Copper (II) Oxide An Activity Series (Flinn Scientific) Chapter 5: Thermochemistry 2.0 Weeks The student will: Differentiate between kinetic and potential energy Identify the units used to measure energy and interconvert between units Differentiate between system and surroundings as they apply to energy changes accompanying a chemical reaction Apply the first law of thermodynamics quantitatively Differentiate between endothermic and exothermic processes and calculate accompanying changes in enthalpy Determine the specific heat of a substance using calorimetry Determine the change in enthalpy for a chemical reaction using Hess’s Law Determine the change in enthalpy for a chemical reaction using enthalpies of formation Laboratory Determination of the Specific Heat of Lead Determining the Enthalpy of a Chemical Reaction (Vernier) Chapter 6: Electronic Structure of Atoms 1.0 Weeks The student will: Differentiate between the wave and particle nature of electromagnetic radiation Explain the relationship between wavelength, frequency, energy of a photon, and speed of light Describe the arrangement of electrons in atoms, identify a substance by its line spectrum Identify an element by its quantum numbers Using the periodic table, determine the electron configuration and orbital diagram for atoms and ions Demonstration: Observation of Line Spectra of Gases Laboratory Flame Test Lab Chapter 7: Periodic Properties 1.0 Weeks The student will: Examine periodic trends in the atomic size, ionization energy, and electron affinity of atoms Relate ionization energy and electronegative to effective nuclear charge Differentiate between metals, nonmetals, and metalloids, and their physical and chemical properties Laboratory None Chapter 8: Basic Concepts of Chemical Bonding 1.0 Weeks The student will: Differentiate between ionic, polar and nonpolar covalent, and metallic bonds Demonstrate the formation of a bond using Lewis symbols Compare lattice energies of various compounds Represent a molecular compound by drawing its Lewis Structure Differentiate between ionic, polar covalent, and nonpolar covalent bonds using electronegativity values Identify resonance structures and use formal charge to determine the most reasonable structure Calculate the enthalpy of a reaction using bond enthalpies, compare bond enthalpy to bond length Laboratory None Chapter 9: Molecular Geometry and Bonding Theories 1.5 Weeks The student will: Differentiate between electron-domain geometry and molecular geometry using the VSEPR Model Predict bond angles for molecules based on their electron-domain geometry (including large molecules) Use molecular shape to determine the polarity of the molecule Explain molecular geometry using hybrid orbitals Differentiate between sigma and pi bonds, and delocalized bonding Describe molecular properties using electron configurations Laboratory Molecular Modeling Activity (includes chiral molecules) Chapter 10: Gases 2.0 Weeks The student will: Compare and contrast the characteristics of gases to those of solids and liquids Use a manometer to measure gas pressure Interconvert between Torr, atmospheres, and kilopascals Evaluate the effects of changes in pressure, volume, temperature, and number of moles on a gas Calculate density and molar mass of a gas Relate the volume of a gas to the amount of another substance in a reaction using stoichiometry Apply Dalton’s Law of Partial Pressures to gas mixtures Relate mole fraction to partial pressures of gases in a mixture Calculate an amount of gas collected over water Apply the Kinetic-Molecular Theory to the empirical observations of gas properties Calculate root-mean square speed of a gas Apply Graham’s Law of Effusion to the properties of gases Differentiate between effusion and diffusion Differentiate between the behavior of ideal and real gases Laboratory Exploring the Properties of Gases (Vernier) The Molar Volume of a Gas (Vernier) Chapter 11: Intermolecular Forces, Liquids, and Solids 2.0 Weeks The student will: Relate the strengths of intermolecular forces (ion-dipole, dipole-dipole, London Dispersion, hydrogen bonds) to the properties of a substance, including boiling and melting points, viscosity, and surface tension Relate energy changes to phase changes Calculate the enthalpy change of a process using a heating curve Interpret a phase diagram Relate the volatility of a substance to its vapor pressure and temperature Explain the relationship between vapor pressure, atmospheric pressure, and boiling point Relate the structure of molecular, covalent network, ionic , and metallic solids to their respective physical properties and intermolecular forces Laboratory Vapor Pressure and Enthalpy of Vaporization of Water (Vonderbrink) Chapter 13: Properties of Solutions 2.0 Weeks The student will: Relate intermolecular forces to the solution process Differentiate between endothermic and exothermic processes as they relate to energy changes of reactants and products Assess changes in entropy relative to a chemical process and changes in state Differentiate between saturated, unsaturated, and super-saturated solutions Predict the solubility of a substance based on its molecular structure and that of its solvent Explain
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