AP Chemistry Syllabus

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1 AP Chemistry Syllabus Course Description The Advanced Placement (AP) Chemistry program is designed to prepare students for the AP Chemistry exam and for their first year of college chemistry. In some cases, passing the AP Chemistry test will allow students to take a second year chemistry course their first year of college. This course will cover material equivalent to one full year of chemistry at a college or university and to cover all the material, it will move fast. The rigorous course will challenge you as a student and is intended for students who have demonstrated a willingness to commit considerable time to studies and assignments outside of class. The goal of this course is to develop the student s ability to incorporate mathematical skills to the solution of chemistry problems from examples, textbooks and laboratory activities. This course prepares students for the AP Chemistry exam and it is strongly recommended that students purchase an AP Chemistry Study guide and, instead of waiting 2 weeks before the test, begin studying now. As mentioned above, passing the AP Chemistry exam can earn you college credit so this class should not be viewed as college prep but a college class with expectations for college level effort, participation and work. During the duration of this course, you will be assessed in a number of ways including quizzes, tests, homework assignments, labs and a portfolio. The test and quiz portion of this course will be similar to that of any college level test covering material from assigned readings and discussed in class. Homework will be assigned at the beginning of a unit and will be due the date of the test, no late work accepted. As Chemistry is a lab intensive topic, there will be several labs performed during the course of the year. It is imperative that you read the lab procedures before the day of the lab and that you and your lab partner work together to complete the lab with good results in a timely manner. Your lab performance will be based on writing formal lab reports and building / maintaining a Lab Report Portfolio. Instructions and format on writing lab reports are attached Notebooks and Lab Report Portfolios should be kept current and in chronological order as they will be checked periodically and reflect in your grade. Again, the aim of this course is to act as a college level Chemistry course and prepare you for the accompanying AP Chemistry exam. Your dedication and efforts to this class will reflect in your grade as well as the score you earn if you choose to take the AP exam. Text Book and other resources * Chang, Raymond. Chemistry 9 th Edition New York: McGraw Hill. Zumdahl, Steven S., Chemistry 5 th Edition Boston: Houghton Mifflin Harcourt. AP Released Free Response Questions AP Released Multiple Choice Questions AP Course Description Randall, Jack, et al. Advanced Chemistry with Vernier: Experiments for AP *, IB ** and College General Chemistry, 2 nd Edition Beaverton, OR: Vernier Software & Technology Each lab noted with a number in parentheses (XX) indicates lab from Vernier text * Each students has a copy of Chang text Needs / Requirements Graphing / Scientific Calculator 3 ring binder with 5 tabs labeled as: o Notes o Homework o Test o Quizzes o Labs / Lab Reports

2 Course Outline Unit I: Review of General Material: Measurement, Matter, Atoms, Molecules, Ions and Nuclear Chemistry Chapter 1 (3 days) Measurements and conversions Handling numbers and significant figures Dimensional analysis in problem solving Classification and states of matter Physical vs. chemical properties of matter Chapter 2 (1 week) Atomic theory Structure of atom Atomic number, mass number and isotopes Periodic table Molecules and ions Chemical formulas Naming compounds Chapter 24 (one week) Classes of organic compounds Aliphatic and aromatic hydrocarbons Functional groups of carbon compounds Chapter 23 (3 days) Nuclear reactions Nuclear stability Natural radioactivity Nuclear transmutation Nuclear fission Nuclear fusion Biological effects of radiation Unit 1 Labs: Significant digit measurement activity Half-life of m&m s activity Preparation of esters (time permitting) Determining the mole ratios is a chemical reaction using bleach and sodium thiosulfate (9) Unit II: Mass relationships in chemical reactions Chapter 3 (3 weeks) Atomic Mass Avogadro s number and molar mass of elements Molecular mass Percent composition of compounds Empirical formula and experimental determination Chemical reactions and equations Limiting reactants Percent yield Unit II Labs: Determination of the formula of a compound (CuSO 4. 5H 2 O) Determination of the percent of water in a hydrated salt (CuSO 4. 5H 2 O) Synthesis, purification and analysis of aspirin (21)

3 Unit III: Reactions in aqueous solutions Chapter 4 sections 1, 2, 5, 6 (2 week) General properties of aqueous solutions Precipitation reactions Concentrations of solutions Gravimetric analysis Unit IV: Equilibrium Chapter 14 (3 weeks) Chemical Equilibrium and K c constant Equilibrium expressions Relationship between chemical kinetics and chemical equilibrium Factors affecting chemical equilibrium Chapter 16 sections 6 8, 10, 11 (2 weeks) Solubility equilibria Fractional precipitation of ions Common ion effect and solubility Complex ion equilibira and solubility Applications of the solubility product Chapter 4 section 3 (2 days) Acid Base Reactions Chapter 15 (2 weeks) Acid base theory (Brønsted, Lewis) Acid base property of water ph measurements and scale Strength of acids and bases Weak acids and acid ionization constants (K a ) Weak bases and base ionization constants (K b ) Relationship of ionization constants of acids and their conjugate bases Polyprotic acids Molecular structure and strength of acids Acid base properties of salts Acid base properties of Oxides and hydroxides Chapter 16 sections 1 5 (2 weeks) Acid base titrations Homogeneous vs. heterogeneous solution equlibria Buffer solutions Acid base indications MIDTERMS Unit IV Labs: Determination of equilibrium constant (Beer s law in FeSCN 2+ equilibrium) (10) (17) Standardizing a solution of sodium hydroxide Acid base titration of vinegar with sodium hydroxide Investigating indicators (11) Separation and qualitative analysis of anions and cations (14) Conductimetric titration and gravimetric determination of a precipitate (16) Buffers (19)

4 Unit V: Oxidation reduction reactions Chapter 4 section 4 (1 week) Oxidation reduction reactions Chapter 19 (1 week) Redox and galvanic cells Standard reduction potentials Spontaneity of redox reactions The effect of concentration of cell emf Batteries Corrosion Electrolysis Unit V Labs: Oxidation reduction titration: Reaction of Fe 2+ and Ce 4+ (8) or titration of vitamin C with iodine to determine the percentage of vitamin C in a tablet Electrochemistry: Voltaic Cells (20) Electroplating (21) Unit VI: Entropy, Free Energy and Equilibrium Chapter 18 (1 week) Thermodynamic laws Spontaneous processes Entropy Gibbs free energy Free energy and equilibrium Unit VII: Thermochemistry Chapter 6 (1 week) Nature and types of energy Energy changes in chemical reactions Introduction to thermodynamics Enthalpy Calorimetry Standard enthalpy of formation and reactions Heat of solution and dilutions Unit VIII: Chemical Kinetics Chapter 13 (1 week) Reaction Rate Rate Law Relationship between concentrations and time Activation energy and temperature dependence of rate law Reaction mechanisms Catalysis Unit VIII labs: Rate of reaction: The decomposition of hydrogen peroxide (12) Determining the enthalpy of a chemical reaction using Hess law (13)

5 Unit IX: Gases Chapter 5 (1 week) Pressure Gas laws and the ideal gas equation Gas stoichiometry Dalton s law of partial pressures Kinetic molecular theory of gases Deviation from ideal behavior Unit IX Labs: Molar mass of a volatile liquid (3) Molar volume of a gas (5) Unit X: Electron configurations, relationships and bonding Chapter 7 (1 week) Photo electric effect Bohr s theory of the hydrogen atom Dual nature of the electron Quantum mechanics and quantum numbers Atomic orbital Electron configurations Pauli exclusion principle, Aufbau principle and Hund s Rule Chapter 8 (1 week) Organization of periodic table Classification of elements Variations of physical properties Periodic trends Chapter 9 (1 week) Lewis dot symbols and structures Ionic bonding and lattice energy Covalent bonds Electronegativity Resonance Exceptions to the octet rule Bond enthalpy Chapter 10 (1 week) Molecular geometry Dipole Hybridization of atomic orbitals Molecular orbital theory and configuration Unit XI: Intermolecular forces of solids and liquids and physical properties of solutions Chapter 11 (1 week) Kinetic molecular theory of liquids and solids Intermolecular forces Properties of liquids Amorphous solids Phase changes and diagrams

6 Chapter 12 (1 week) Types of solutions Molecular view of solutions Colligative properties of electrolyte and non-electrolyte solutions Unit XI labs: Using freezing-point depression to find molecular weight (4) The synthesis and analysis of Alum (15) Liquid chromatography (18) Independent reading of chapters 20, 21 and 22

7 Lab Report Requirements The following is information that needs to be included in each lab report. All sections must be included in reports unless otherwise specified by instructor. Each student must write a lab report for each experiment performed. In the case where lab partners are involved, you are required to write separate and different reports, copied or plagiarized reports may result in earning no points and disciplinary action. Lab reports should be written in your own word avoiding the use of names, pronouns or other information relating to people performing the lab. Lab reports should be written as you would write and English report, correct grammar, punctuation and spelling are expected. The report should be neat and on full sheets of paper. The only abbreviations that you should use are standard scientific measurements (mm, ml, g, etc.). All statements and descriptions should be specific and clearly worded. Refer to particular parts of the experiment when describing observations and discussing results. The top of each report should include the name of the experiment, your name and the name of your lab partner (if applicable). The body of the report should be written using the following format. Label each part and separate it from the other parts of the report. 1. INTRODUCTION / PURPOSE Describe, in your own words, the purpose of the experiment. Include a brief description of the method used in the experiment. This section should be no more than a few sentences long. 2. MATERIALS This section should list the materials and quantities of each item used in the lab experiment. 3. PROCEEDURES You will be required to complete a detailed procedure of the lab in your own words before the day of the lab. This means you should read the lab procedures before the day of the lab and use the lab sheets as a guide. 4. DATA This section should include all experimental data recorded and any observations. Present all data in a form that will allow it to be readily understood by the reader. Numerical data should not be presented in sentences or paragraph form, but in clearly labeled and well-designed data tables. Attach correct units where appropriate. 5. DATA ANALYSIS / CALCULATIONS show the set-up used to perform each calculation. Units and significant figures should be carried through the calculations. If the same calculation must be performed multiple times, you only need to show the complete calculation once. The results of the calculations are sufficient for the remaining pieces of data. Graphs should be included with this section as well. They should have a brief title at the top describing the nature of the graph. Axes should be clearly labeled with appropriate scales, titles and units used. Graphs must be drawn on graph paper or printed using graphing programs. 6. DISCUSSION / ERROR ANAYLSIS Briefly summarize the results of the experiment. Discuss your results both qualitatively and quantitatively. While the form of the discussion may vary depending on the experiment, you should answer the following questions. a. What do the results of the experiment show or what conclusion can be drawn from the experiment? b. Do the results agree with theory or established values of experimental quantities? c. What errors, both actual and possible, are present in the experiment? d. How large is each of the errors in the experiment and what effect would the error have on the experimental results? e. If your results do not agree with theory or established values of experimental quantities, why do they disagree and are the errors in the experiment large enough to account for the disagreement? 7. QUESTIONS Some experiments will contain questions for you to answer. Questions that are included as part of the procedure should be answered in your discussion. Otherwise, answer questions in this section. Complete sentences should be used to answer questions 8. CONCLUSION Only a brief one or two sentence statement summarizing the experiment and the results obtained is required.

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