AP Chemistry. AP Chemistry Lab and Course Overview. AP Practice Exam Schedule

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1 AP Chemistry AP Chemistry Lab and Course Overview Depending upon the year, 3 to 5 sections of AP Chemistry are offered. The school operates on a 7 period day with 52 minute classes on regular schedule. On average, 2 class periods are allotted per lab and then the lab work is completed whenever the student can arrange to come in for lab work before or after school, during lunch or during a study hall. Since students are expected to repeat trials until the desired results are obtained, the time spent outside of class varies from lab to lab and from student to student. This results in a student spending a minimum of three to four hours a week in lab outside of class time. All 26 labs are hands-on, college level chemistry laboratory experiments. Pre-lab and safety issues are always addressed for each lab. The lab is routinely open daily from 7:00-7:45 am and 3:00-5:00 pm to allow students to do lab work around their sports, band, orchestra, and other extra-curricular schedules. Upon occasion, night labs are scheduled to make it easier to do a lab that is significantly better done in one 3 4 hour block. Students have lab partners and most of the labs are done as partners; however, some of the labs involving unknowns are done individually. Students are expected to follow lab protocols and brainstorm amongst themselves to solve lab dilemmas. A complete lab report is written for each laboratory experiment in a quadrille-lined bound book. AP Chemistry averages are composed of 50% quiz and lab report grades and 50% test grades. There are usually 2 rather comprehensive quizzes per unit dealing with the more difficult aspects of the unit. Homework is assigned for each unit in the form of worksheets with review problems and challenging problems and problem sets from the book; but, neither are formally graded. The more difficult problems are addressed in class. Students have access to solutions to all homework problems from the textbook. All assessments contain questions demanding the critical thinking, reasoning skills and higher level problem solving necessary for success on the AP exam. In the weeks preceding the actual Chemistry AP exam, 3 practice AP chemistry exams are given in their entirety, the last of which counts as the second semester final exam grade. AP Practice Exam Schedule (1) The first of three practice AP Chemistry exams is typically given on a Wednesday or Thursday afternoon four weeks before the actual exam. The students take their exams and a rubric home in order that they might score the exam themselves. This is their first taste of timing and the nature of the exam. This is the first opportunity for the students to see how they must operate and to see what they still need to work on to be successful on the actual exam. (2) Two Saturdays before the actual AP Chemistry exam, a 2 nd practice exam is given. I grade the exam and on Monday the students receive the exam and a copy of the rubric to take home so they can review and evaluate their work. In the days after, the students have the opportunity to figure out their mistakes in small groups before and after school. 1

2 (3) The Saturday before the actual AP Chemistry exam, a 3 rd practice exam is given. I grade the exam and it counts as their second semester final exam grade. The students meet Monday during class and in the afternoon and evening to use a copy of the grading rubric to go over their exam. They work either individually or in groups for this process. I am available to answer questions and help if they need it. Textbook: Zumdahl, Steven S. and Susan S. Zumdahl, Chemistry. 5 th Edition, Houghton Mifflin Company, 2000 Supplemental Resources: Brown, Theodore L., H. Eugene LeMay, Jr. and Bruce E. Bursten, Chemistry: The Central Science, 9 th Edition, Prentice Hall, 2000 Hill, John W. and Ralph H. Petrucci, General Chemistry, 2 nd Edition, Prentice Hall, 1999 Holmquist, Dan D., Jack Randall and Don Volz, Chemistry with Calculators, 2 nd Edition, Vernier Software and Technology, 2000 Kotz, John C. and Keith F. Purcell, Chemistry and Chemical Reactivity, 2 nd Edition, Saunders College Publishing, 1991 Nelson, John H. and Kenneth C. Kemp, Laboratory Experiments, 8 th Edition, Prentice Hall, 2000 [to accompany the 8 th Edition of Chemistry: The Central Science, by Theodore L. Brown, H. Eugene Le May, Jr. and Bruce E. Bursten] Whitten, Kenneth, Raymond E. Davis and M. Larry Peck, General Chemistry, 6 th Edition, Saunders College Publishing,

3 AP Chemistry Course Topics Unit I: Chapters 1-3 Chemistry Basics Review [C1, C4, C5, C6, C7] 5 Lecture days including assessments Safety and Safety Test-Score of 100 is required on Safety Test before any lab is done. Writing Formulas & Naming Compounds Acid Strength History: Becquerel, Thomson, Goldstein, Chadwick, Rutherford and their experiments. Dalton's Atomic Theory and Modern Atomic Theory Conversions Significant figures Dimensional Analysis Density Basic atomic structure Basic periodic law Mole concept Isotopic abundance and percent calculations Mass Percent Basic Empirical & Molecular formula determination Basic Stoichiometric calculations Percent Yield Unit II: Stoichiometry (mass-mass) [C3, C5, C6, C7] 4 Lecture days including assessments Straight-forward mass-mass stoichiometry problems Complex mass-mass stoichiometry Empirical & Molecular formula determination involving data obtained from Nitrogen determination in a second experiment Formula determination based on several stoichiometric relationships and steps The determination of the formula of a hydrate. Calculations of yields in multi-step mechanisms. Limiting Reagent Problems Unit III: Solution Stoichiometry (Including Redox) [C3, C5, C6, C7] 10 Lecture Days including assessments Stoichiometric Calculations with various solution concentrations Volumetric Analysis Problems-Acidic, Basic, Redox 3

4 Balancing Redox reactions in acidic and basic solutions Redox titration calculations Net Ionic Equations Review Solubility Rules Unit IV: Prediction of Products of a Reaction [C3, C4, C5, C7] 9 Lecture days including assessments Application of Solubility Rules Predicting of products of reactions and writing net ionic equations (metathesis, synthesis, decomposition, redox, organic, complex ion) Rudimentary coordination chemistry Unit V: Organic Chemistry [C1, C4, C5, C7] 7 Lecture days including assessments Writing Formulas for and naming: Alkanes, Alkenes, Alkynes, Cyclos Functional Groups: alcohols, aldehydes, acids, ketones, ethers, esters, amines, amides Organic Reactions Isomerism Hybridization Unit VI: Thermodynamics [C3, C5, C6, C7] 8 Lecture days including assessments E, q, w Balloon problems Heating and Cooling Curves H and H problems Bomb Calorimetry Coffee Cup Calorimetry Bond Energy Hess's Law S, S = q/t Gibbs' Free Energy Calculations for G, G, K, Q 4

5 Unit VII: Gases [C1, C2, C5, C6, C7] 7 Lecture days including assessments Gas Theory and KMT PV=nRT and all variations KE Root Mean Square Velocity Van der Waals Equation Gas Stoichiometry Empirical & Molecular Formulas Unit VIII: Atomic Structure/Theory [C1, C4, C5, C6,C7] 6 Lecture days including assessments Electromagnetic Radiation E=hν λ= h/mv Bohr & Quantum Mechanical Models λ= R(1/n 2 f 1/n 2 i) E= -Rhc (1/n 2 f 1/n 2 i) Heisenberg's Uncertainty Principle Quantum Numbers Orbital Notation Aufbau Principle, Hund's Rule, Pauli Exclusion Principle Periodic Trends in detail Lab demos: (1) Flame Tests (2) Spectral Tubes [Neither of these is written up as a lab report, nor counted as a lab.] Unit IX: Chemical Bonding [C1, C2, C4, C5, C7] 7 Lecture days including assessments Covalent and Ionic Bonding Coulomb's Law Bond Polarity and Dipole Moments Ion sizes Lattice Energy Bond Energy- H calculations (as done in Unit VI) Lewis Dot Structures Hybridization Resonance 5

6 Formal Charges Molecular Geometry Molecular Orbital Theory Bond Order Unit X: Solids and Liquids [C1, C2, C5, C6, C7] 5 Lecture days including assessments Solids Liquids IMF's Clausius-Clapeyron Equation Heating and Cooling Curves Phase Diagrams Allotropy Unit XI: Solutions [C1, C2, C5, C6, C7] 7 Lecture days including assessments Concentrations Solubility Henry's Law Raoult's Law Freezing Pt Depression Boiling Pt Elevation Osmotic Pressure Solution Stoichiometry Unit XII: Nuclear Chemistry [C1, C6] 4 Lecture days Each student gives a presentation over some aspect of this unit. Double Quiz Grade [length of test] given over the unit. Radioactive Decay Predicting Type of Decay Nuclear Equations and Decay Series Half-Life Problems- 1 st order reactions Radiocarbon Dating Calculations Binding Energy Calculations Fission & Fusion Nuclear Reactions Applications of Nuclear Chemistry 6

7 Unit XIII: Kinetics [C3, C5, C6, C7] 10 Lecture days including assessments Concentration and Rate Problems Integrated Rate Law Problems, zero, 1 st, 2 nd, 3 rd Mechanisms Temperature Dependence Graphs KE graphs for mechanisms Arrhenius Equation K from E a calculations Order reactions Unit XIV: General Equilibrium [C3, C5, C6] 5 Lecture days including assessments K c and K p calculations and introconversions Determination of Q Le Chatelier's Principle Unit XV: Acids, Bases & Salts [C3, C5, C6, C7] 8 Lecture days including assessments Acid Theory Arrhenius Bronsted-Lowry Lewis Prediction of Direction of Reactions Dissociation Constants Acid Strength- Binary Acids and Oxyacids Acids ph of strong and weak solutions ICE chart calculations for [H + ] and ph [5% Rule] % Dissociation K a from ph and % Dissociation pk a Polyprotic Acids- Concentration Calculations for all Dissociations Bases Base strength ph and poh calculations Salts Hydrolysis Calculations of ph of Salt Solutions 7

8 Unit XVI: Aqueous Equilibrium [C3, C5, C6, C7] 12 Lecture days including assessments Common Ion Problems Buffer Problems Acid-Base ph problems- Titrations Preparation of Buffers Calculations Indicators K sp Problems Unit XVII: Electrochemistry [C3, C5, C6, C7] 4 Lecture days including assessments (Often times we have an extra night class for this unit) Voltaic Cells Electrolytic Cells Nernst Equation Problems Voltaic Cells at non-standard conditions; G and G log K = ne /

9 AP Chemistry Lab Experiments (1) Identification of Substances by Chemical and Physical Properties (Nelson & Kemp) (2) Separation of the Components of a Mixture (Nelson & Kemp) (3) Recycling in the Chemistry Classroom- the conversion of aluminum to alum. (4) Formula & Composition of a Hydrate (Petrucci Weiss, Wismer & Greco) (5) Gravimetric Analysis of a Chloride Salt (Nelson & Kemp) (6) Chemical Reactions (Nelson & Kemp) (7) Reactions in Aqueous Solutions; Metathesis Reactions and Net Ionic Equations (Nelson & Kemp) (8) Heat of Fusion of Ice (Holmquist, Randall & Volz) (9) Hess's Law (CBL-Vernier) (10) Preparation of Aspirin and Oil of Wintergreen (Nelson & Kemp) (11) Evaluation of the Gas Law Constant (Petrucci Weiss, Wismer & Greco) (12) Molecular Weight of a Vapor (Nelson & Kemp) (13) Molecular Geometry construction of models (14) Using Freezing Point Depression to Find Molecular Weight (Holmquist, Randall & Volz) (15) Paper Chromotography : Separation of Cations and Dyes (Nelson & Kemp) (16) Preparation and Standardization of 0.10M NaOH (Nelson & Kemp) (17) Preparation and Standardization of M KMnO 4 (Redox titration) (Hope College) (18) Rate Law Determination for Crystal Violet (Holmquist, Randall & Volz) (19) Synthesis of an Iron Oxalato Salt (Hope College) (20) Percent Water in an Iron Oxalato Salt (Hope College) (21) Percent Oxalate in an Iron Oxalato Salt (Hope College) (22) Percent Potassium and Percent Iron in an Iron Oxalato Salt (Hope College) and Empirical Formula Determination of an Iron Oxalato Salt (Hope College) (23) Titration Curves of Strong and Weak Acids (Holmquist, Randall & Volz) (24) Calculation of K a for a Weak Acid (Holmquist, Randall & Volz) (25) The Buffer in Lemonade (Holmquist, Randall & Volz) (26) Construction of Voltaic Cells (Modification of Holmquist, Randall & Volz without CBL) 9