AP Chemistry. Overview of AP Chemistry

Transcription

1 AP Chemistry Overview of AP Chemistry Course Times: The AP Chemistry course meets 5 days a week. Four days are 42 minute periods for lecture, problem solving, homework review, questions, and testing. The fifth day is a double period of 88 minutes for laboratory work. This sets about one third of the scheduled time for laboratories. Course Summary: This course is designed to give students a knowledge equivalent to that received by a first yearlong Chemistry course for a science major at an accredited college. In general, we follow the textbook order and detail. The incumbent teacher includes many relationships between the textbook topics and real world chemical industry practices based on his 30 years in the chemical industry. Homework is assessed by each section completed in the test and includes problems based on the text material. Students are expected to spend approximately one hour per school night on studying and homework plus time for lab reports. The laboratory portion is designed to meet the knowledge and experiential requirements of a college level course and to develop hands on laboratory skills including safety. Laboratory: All laboratory experiments are hands on. All students must complete all laboratory experiments and complete a full lab report for grading. Lab reports should include title, objective, partners (some labs are individual), equipment and chemicals used, a detailed procedure, data and observations, any necessary calculations and graphs, results and discussion, error analysis, and conclusions. Laboratory grades should count a minimum of one-third of the student s grade in keeping with the time allocation. Textbooks: Main Textbook Chemistry Seventh Edition Zumdahl & Zumdahl Houghton Mifflin Company Test Prep Book Fast Track to a 5 Preparing for the AP Chemistry Exam To accompany Chemistry 6 th and 7 th Editions by Zumdahl & Zumdahl McDougal Littell (A Houghton Mifflin Company) Laboratory Manuals: Main Laboratory Book

2 Laboratory Experiments for Advanced Placement Chemistry Sally Ann Vonderbrink, Ph.D. Published by Flinn Scientific, Inc. P.O. Box 219 Batavia, IL Additional Laboratory Book Experimental Chemistry James F. Hall Houghton Mifflin Company Additional Laboratory Book Flinn Scientific Spectrophotometer Laboratory Manual Published by Flinn Scientific, Inc. P.O. Box 219 Batavia, IL Additional Laboratory Experiments A few experiments have been written by the incumbent teacher or from a variety of unreferenced sources. These include the following labs Progressive Precipitation which includes a series of precipitation reactions including K sp calculation Gravimetric Determination of Percent Sulfate (or Barium ion) in Solution based on a previous AP free response test question Electroplating which includes electroplating copper with zinc and appropriate calculations Course Outline: Students will be able to Chapters 1-3 (Summer Assignment) Identify and describe all the steps of the scientific method Use and calculate with significant figures Describe Dalton s atomic theory Describe atoms, ions, molecules and the periodic table Name simple compounds Understand atomic masses, the mole, and molar mass Calculate percent composition, empirical and molecular formulas Read, write, and balance chemical equations Perform stoichiometric calculations involving mass Perform stoichiometric calculations with a limiting reactant Calculate percent yield Done in Chem I a prerequisite course Formation and Determination of the percent composition of Magnesium Oxide Detemination of Percent Water in a Hydrate Done in AP Chemistry during first weeks

3 Gravimetric Determination of Ba 2+ Ion in Solution (reference: see above) Gravimetric Determination of Percent Sulfate in an Unknown Salt (reference: see above) Finding the Mole Ratio of Reactants in a Chemical Reaction (Vonderbrink Lab #2) Chapter 4 Solutions and Chemical Reactions (2 weeks) Explain the electronic interactions involved in polar bonds and solvation of ions in water Define solute and solvent Distinguish between materials that are strong and weak electrolytes, acids and bases Read, write, and balance net ionic equations Define and calculate molarity Perform dilution calculations Define three classes of reactions Determine the solubility of materials Determine products of reactions based on principles of solubility (precipitation) (Solubility rules) Describe reaction in solutions Perform stoichiometric calculation for precipitation reactions Define neutralization reactions Define and describe titration Perform stoichiometric calculation for neutralization reactions and titrations Define redox reactions (oxidation-reduction reactions) Determine oxidation states (numbers) for individual reactants Determine reactant oxidized, reduced, reducing agent, and oxidizing agent Balance redox reactions by the half reaction method Explain electron transfer during oxidation-reduction reactions Oxidation-Reduction Titration of Sodium Hypochlorite with Sodium Thiosulfate (Vonderbrink Lab #10) Chapter 5 Gases (1 week) State Boyle s Law, Charles Law, Avogadro s Law, Gay-Lussac and the ideal gas law Perform stoichiometric calculation with gases involving volume Understand the relationship between gas density and molar mass Understand and perform calculations using Dalton s Law of Partial Pressures Describe the Kinetic Molecular Theory of Gases Understand the relationship between temperature and kinetic energy Understand the difference between diffusion and effusion Graham s Law Describe the differences between ideal and real gases Determination of the Molar Volume of a Gas Determination of Molar Mass by Vapor Density (Vonderbrink Lab #7) Chapter 6 Thermochemistry (2 weeks) Define a state function Define potential and kinetic energy, heat, work, endothermic and exothermic Use the First Law of thermodynamics in calculations Define enthalpy, calorimetry, heat capacity, and specific heat Calculate heats of reaction Calculate changes in enthalpy at constant pressure or volume Calculate changes in enthalpy using Hess s Law Calculate heats of formation Calculate heats of reaction from heats of formation

4 Calculate enthalpy changes during phase changes (heats of fusion and vaporization) Perform calorimetric calculations Hess Law (Vonderbrink Lab #6) An Activity Series (Vonderbrink Lab #5) Chapter 7 Atomic Structure and Periodicity (2 weeks) Describe the electromagnetic spectrum Describe the relationship between frequency and wavelength Describe the relationship between energy and wavelength of light Describe the dual nature of light Describe diffraction Describe the atomic spectrum of hydrogen Describe the quantum mechanical model of the atom including the Schrödinger equation and wave functions Describe the orbital shapes and energies of an atom Describe quantum numbers Describe electron spin and the Pauli exclusion Principle Describe the problems of the Schrödinger equation with polyelectronic ions Describe the periodic table and the Aufbau Principle Describe Hund s rule and electron configuration Describe periodic trends such as atomic radii, ionization potential, electron affinity, electronegativity, reactivity, oxidation numbers, and ion radii Describe the properties of the alkali metals Name and describe properties of other main groups (alkaline earth metals, transition metals, halogens, and noble gases) Spectrophotometric Determination of Copper Ion in Aqueous Solution (Flinn Scientific Spectrophotometer Laboratory Manual Experiment #2) Emission Lines of Some Metallic Elements (Flame Tests) (Hall, Experimental Chemistry Lab #18-3) Chapter 8 & 9 Chemical Bonding (3 weeks) Describe and distinguish between ionic, nonploar covalent, and polar covalent bonds Understand electronegativity and use electronegativity to assess the polarity of bonds and bond types Determine the dipole moment of a molecule Relate electron configurations to ion sizes Describe an ionic lattice Describe the chemical bond model of chemical compounds Understand bond energies and calculate enthalpy from bond energies Describe the localized electron bonding model Write Lewis structures for chemical compounds Describe exceptions to the octet rule and the concept of resonance Describe the Valence Shell Electron Pair Repulsion (VSEPR) Model Describe orbital hybridization Describe the molecular orbital model Qualitative Analysis for Anions (Vonderbrink Lab #20) Chapter 10 Liquids and Solids (2 weeks)

5 Understand intermolecular forces such as dipole-dipole interactions, London dispersion forces, surface tension, capillary action, and hydrogen bonding Understand metallic bonds, network solids, molecular solids, ionic solids Understand vapor pressure and changes of state Read and interpret phase diagrams including critical point and triple point Describe crystal structures and lattice energies Qualitative Analysis for Cations (Vonderbrink Lab #19) Chapter 11 Properties of Solutions (2 weeks) List types of solutions Define and calculate mass percent, molality and normality Understand the energy changes associated with dissolution and hydration of materials Understand the effects of temperature and pressure on solubility Define and perform calculations using Henry s Law Define and perform calculations using Raoult s Law Calculate changes in boiling and freezing points of solutions Understand the van t Hoff factor and ion pairing in solution including non-ideal behavior Define and perform calculations of osmotic pressure Understand reverse osmosis Understand the Tyndall effect Freezing Point Depression (Carolina Biological Supply Company) Chapter 12 - Chemical Kinetics (2 weeks) Define chemical kinetics as the change in concentration of a reactant or product over time List factors affecting reaction rates including temperature, concentration, pressure, surface area, and catalysis Understand the concepts of the rate law, half-life, and the order of a rate law Write a rate law and perform calculation using rate laws Describe the concept of reaction mechanisms and rate determining step Understand the chemical kinetics model including energy diagrams, activation energy, and activated state Define catalysis Describe the collision model of reactions Describe how reaction rates can be experimentally measured and perform such calculations including using experimental data and graphical analysis Study of the Kinetics of a Reaction (Vonderbrink Lab #12) Paper Chromatography of Inks (Hall, Experimental Chemistry Lab) #9-1 Chapter 13 Chemical Equilibrium (2 weeks) Explain the equilibrium condition and dynamic equilibrium Define the law of mass action and the equilibrium expression Define and calculate equilibrium constants, K c Calculate concentrations knowing the equilibrium constant Define the equilibrium expression involving pressure, K p Define the equilibrium expression for heterogeneous equilibrium Define and calculate reaction quotients Solve problems involving chemical equilibrium Define and use Le Chatelier s principle

6 Determination of K eq for FeSCN 2+ by Spectrophotometric Method (Vonderbrink Lab #14) Equilibrium and LeChatelier s Principle (Vonderbrink Lab #17) Chapter 14 & 15 Acids and Bases (3 weeks) Explain the concepts of an Arrhenius acid and base, a Bronstead acid and base, a conjugate acid and base Define the terms strong acid, weak acid, organic acid, and amphoteric substance Define and use K w and the ph scale Calculate the ph of a strong acid solution Calculate the ph of a weak acid solution Use the equilibrium expression to calculate and use K a and pk a Define the terms strong base, weak base, and organic base Calculate the ph of strong and weak bases Use the equilibrium expression to calculate and use K b and pk b Calculate the ph of polyprotic acids Explain the acid base properties of salts (hydration of salts) Explain the acid base properties of oxides Explain the Lewis acid base model Define common ion Define buffer solution Calculate the ph of a buffer solution Perform equilibrium and ph calculations for a variety of strong/weak acid/base reactions and titrations Choose the proper indicator for a titration Define and perform calculations using solubility products K sp Predict reaction product based on solubilities Define a complex ion Determination of Equivalent Mass and pka of an Unknown Acid by Titration (including standardization of a base with a primary standard) (Vonderbrink Lab #16) Acids, Bases, and Buffered Systems (Hall, Experimental Chemistry Lab #28) Chapter 16 - Chemical Thermodynamics (2 weeks) Define spontaneity and entropy State the Second Law of Thermodynamics Describe the effect of temperature on spontaneity Describe and understand the concept of free energy and its relationship to spontaneity Understand entropy changes in chemical reactions Calculate standard enthalpy, entropy, and free energy for a variety of materials and reactions Calculate free energy of formation Calculate the free energy at varying temperatures and pressures Mathematically relate free energy and equilibrium constants and the effect of temperature on equilibrium constants and electrode potentials Preparation of a Coordination Complex of Copper (Hall Experimental Chemistry Lab #35-1) Progressive precipitation (reference: see above) Chapter 17 Electrochemistry (2 weeks) Describe a redox reaction Describe the construction of a galvanic cell Describe standard a standard reduction potential Describe how standard half cell potentials relate to activity series

7 Predict reaction products bassed on oxidation-reduction potentials Calculate free energy for a cell reaction Understand and perform calculation with the Nernst equation Define electrolysis Describe the construction of an electrolytic cell Perform molar calculations in electrolytic reactions based on the concept of a Faraday and Faraday s Law Electroplating (reference: see above) Electrochemical Cells (Vonderbrink Lab #18) Chapter 18 Nuclear Chemistry (0.5 weeks) Describe radioactive decay and the changes that accompany that decay Understand half-life Write and balance nuclear equations Differentiate nuclear fission and fusion Describe chemical applications of nuclear chemistry Chapter 22 Organic Chemistry (0.5 weeks) Identify and name straight and branched chain hydrocarbons Define structural isomerism Identify the nine principal hydrocarbon derivatives and their nomenclature and chemical properties Synthesis of Aspirin (Hall Experimental Chemistry Lab #39-1 a & b) Identification of an Unknown White Solid (based on a Science Olympiad problem)