AP Chemistry Syllabus and Essential Outcomes Overview: The AP Chemistry course is designed to prepare students for the AP Chemistry Exam. It is the equivalent of the general chemistry course usually taken during the first college year. As a result, the AP Chemistry student can expect the course to differ from a high school chemistry course in the kind of textbook used, the topics covered, the emphasis on chemical calculations and mathematical formulations of principles, and the laboratory work completed. AP Chemistry students can expect to cover a greater number of topics, and therefore expect to spend at least five hours a week in unsupervised individual study. Resources: Textbook: The College Board who oversees AP courses nationwide has approved the textbook currently used for the AP Chemistry course. It is: Chemistry: The Central Science. 9 th ed. By Brown, T.L., H.E. LeMay, Jr. and B.E. Bursten. Prentice Hall. Upper Saddle River, N.J. In addition to the textbook, supplementary materials will be included as necessary to reinforce chemical concepts. Laboratory Experiments: Laboratory Experiments are an integral component of the course. They allow for hands-on reinforcement of the concepts covered in class as well as practice and instruction of proper laboratory technique, and use of laboratory equipment. Information and instructions for laboratory experiments will be distributed the class period prior to each scheduled lab. These guides are to be included in each student s Laboratory Portfolio. Study Guides: Study guides will be provided for each chapter. These guides are to be completed as homework before each lecture period. Study guides will focus on the important concepts covered in each chapter as well as provide problems practice. Study guides allow the students the chance to become familiar with the material before it is presented in class. Completed study guides are an excellent resource for each chapter test and semester exams. Additional Problem Sets: Sets of additional practice problems will available for extra reinforcement of material. Student Solution Manual: Student solution manuals for homework problems and additional problem sets are available for student use. These manuals are to be used as a resource when completing homework problems. Student Generated Resources: AP Chemistry Binder: Each student will keep a three ring binder for the course. This binder will include the completed study guides for each chapter, completed homework problems, and any supplemental materials used in class. Laboratory Portfolio: Each student will create a Laboratory Portfolio. This portfolio will contain a sample laboratory report, grading rubrics and peer edit forms for each lab, as well as the the graded, original laboratory report for each of the experiments performed, as well as completed data sheets for laboratory activities.
Class Procedures: Test Corrections: Students may choose to increase their test grades by making test corrections. To be allowed this priviledge the student must complete extra practice (aka Test Insurance) before the test. Students earning a grade of 70% or lower must complete test corrections. If test insurance was not completed before the test it must be completed before corrections will be allowed, and the maximul allowable score will be 70%. These corrections will allow the student a final chance to master the material. A solution guide will be available to help students correct the errors on their tests. Students may collaborate while correcting mistakes. Homework: Homework is designed to introduce and reinforce material as well as allow practice for quizzes and tests. It is imperative that homework be completed before the fact. Therefore only one late assignment will allowed per semester. Chapter study guides will be given well in advance of due dates to allow ample time for completion by due date. We are all busy people, plan your time wisely! Class Meetings: The class is operated on a block schedule with classes meeting every other day for ninety minutes. Topics Covered and Timing: Unit Topic Chapter #Days I. Matter and Measurement: (1.4-6) 2 SI Units, Significant Figures, and Dimensional Analysis II. Atoms, Molecules, and Ions: (2.1-7) 2 Atomic Theory, Naming of Inorganic Compounds III. Stoichiometry: (3.1-7) 3 Chemical Equations, The Mole, Limiting Reactants, Atomic and Molecular Masses IV. Aqueous Reactions and Solution Stoichiometry: (4.1-6) 3 Types of Aqueous Solutions, Solution Stoichiometry and Chemical Analysis V. Thermochemistry: (5.1-7) 4 1 st Law of Thermodynamics, Types of Energy, Enthalpy, and Calorimetry VI. Electronic Structure of Atoms: (6.1-9) 2 Wave Nature of Light, Atomic Orbitals, and Electron Configurations VII. Periodic Properties of the Elements: (7.1-7) 2 Periodicity and Trends in the Periodic Table VIII. Basic Concepts in Chemical Bonding: (8.1-9) 2 Covalent and Ionic Bonding, Octet Rule and Exceptions, Lewis Structures, and Resonance Structures IX. Molecular Geometry and Bonding Theories: (9:1-8) 3 Molecular Shapes, VSPER Model, Molecular and Hybrid Orbitals
X. Gases: (10.1-9) 3 Pressure, Gases Laws, Kinetic-Molecular Theory, Real Gases XI. Intermolecular Forces, Liquids, and Solids: (11.1-8) 2 Molecular Comparison of Liquids and Solids, Phase Changes, and Phase Diagrams XII. Properties of Solutions: (13.1-6) 3 Solubility, Colligative Properties, and ways of expressing concentration. Semester 1 Exam (Chapters 1-13) XIII. Chemical Kinetics: (14.1-6) 4 Reaction Rates and Factors that affect the rates of reactions. XIV. Chemical Equilibrium: (15.1-6) 4 Equilibrium and Calculating Equilibrium Constants XV. Acid-Base Equilibria: (16.1-11) 3 ph Scale, Weak and Strong Acids/Bases, Different Views of Acids and Bases XVI. Additional Aspects of Aqueous Equilibria: (17.1-7) 4 Common-Ion Effect, Buffered Solutions, Acid-Base Titration s XVII. Chemical Thermodynamics: (19.1-7) 4 Entropy and the 2 nd Law of Thermodynamics, Spontaneous Processes XVIII. Electrochemistry: (20.1-9) 4 Oxidation-Reduction Reactions, Voltaic Cells, Cell EMF, Electrolysis XIX. Nuclear Chemistry: (21.1-8) Radioactivity, Rates of Radioactive Decay, Nuclear Fission and Fusion 5 XX. Chemistry of Nonmetals: (22.1-11) 4 Periodic Trends and Chemical Reaction of Non-metals XXI Chemistry of Coordination Complexes (24.1) 2 Coordination Complexes Review for Exam 4
AP Chemistry Laboratory Component: Approximately 20% (1 lab day for every 4 class days) of class time will be spent in the laboratory. The laboratory experience is an integral part of the class. Students will be assigned lab partners or groups (depending on the nature of the experiment) to collaborate in order to solve the problems presented. In the lab, students will become familiar with laboratory techniques and equipment through their use. Students will learn to hypothesize, observe, record, and manipulate data from their lab experience. This data will then be presented in either a formal lab report, or a laboratory investigation form. Both will be kept in a Laboratory Portfolio. All of the labs listed below are hands-on (wet) laboratory investigations to be performed by the students. Laboratory Manual: Many of the labs to be performed are taken from Chemistry: The Central Science. 9 th ed. By Brown, T.L., H.E. LeMay, Jr. and B.E. Bursten, Laboratory Experiments by J.H. Nelson and K. C. Kemp. Prentice Hall. Upper Saddle River, N.J. Some experiments will be designed by the students themselves to solve a problem. Lab Number Name Book Page 1 Diet Coke and Mentos explained: Original Use the scientific method to design an experiment to explain the Diet Coke- Mentos phenomenon. 2 Chemical Formulas: BLB 47 Determine the molecular formula of zinc chloride and copper sulfide using percent composition. 3 Colligative Properties: BLB 203 Relating Freezing Point Depression and Molar Mass. 4 Behavior of Gases: Molar Mass BLB 137 Observe how changes in temperature and pressure affect the volume of a gas. Determine the molar mass of a gas. 5 Determination of the Dissociation BLB 237 Constant of a Weak Acid Calculate the K a of a weak acid using ph. 6 Analysis of Bleach BLB 459 Use a redox reaction to calculate the amount of hypochlorite in three brands of bleach. 7 Chemical Reactions of BLB 59 Copper and Percent Yield Determine the percent yield of copper from a given sample.
8 Titration of Acids and Bases BLB 215 Determine the amount of acid (KHP) in an unknown sample by titration. 9 Rate and Order of H 2 O 2 BLB 325 Decomposition Determine the rate and order of reaction for the decomposition of hydrogen peroxide. 10 Snack food Calorimetry Original Use calorimetry to compare the calories in corn chips and cheese curls. 11 Qualitative Analysis: BLB 386 Analysis of Simple Salt Identify an unknown salt by its ions. 12 Colorimetric Determination of Iron BLB 403 Analyze the concentration of iron in a sample by colorimetric analysis. 13 Gravimetric Determination of BLB 87 Phosphorus in Plant Food Use gravimetric analysis to determine percent composition. 14 Hydrolysis of Salts and ph of BLB 269 Buffer Solutions Become familiar with acid-base indicators and the behavior of buffered solutions. 15 Electrochemical Cell and BLB 175 Thermodynamics Construct an electrochemical cell and measure its potential at various temperatures. 18 Preparation of Aspirin BLB 481 19 Analysis of Aspirin: Original Determine the mass of salicylic acid in two different aspirin tablets through titration. BLB: Brown, LeMay, and Bursten: Laboratory Experiments by J.H. Nelson and K. C. Kemp. Prentice Hall. Upper Saddle River, N.J.