Advanced Placement Chemistry Course Syllabus



AP CHEMISTRY - Milton High SCHOOL 2010--11

Instructor: Dale Snyder

TEXTBOOK: CHEMISTRY :7th ed., Zumdahl, Houghton Mifflin, 2007

COURSE GOALS

This is an advanced placement course designed to prepare the student for the AP Chemistry exam. The course covers the equivalent of one full year of college level general chemistry. The course is a rigorous math-based course, with a strong laboratory component. These laboratory investigations are a critical component that will enhance the student’s appreciation for the practical aspects of chemistry. It is intended for students who have demonstrated a willingness to commit considerable time to studying and completing assignments outside of class, and those who have successfully completed a prior high school chemistry course.

COURSE TOPICS AND TIME FRAME

The course will be taught in this chapter sequence ( read left to right) –see below on page 3 for a detailed AP chemistry curricular requirement analysis regarding the content of the various chapters that will be presented. Students are responsible for the content of chapters 1-3 during the summer prior to taking this course. Students will receive specific assignments, i.e. problem sets, from chapters 1-3 prior to leaving school in June. Students must submit the completed assignments on the first class in late August and will be tested on chapters 1-3 two week later after a brief review. Topics from chapters 1-3 are continually used, thus reviewed, throughout the course of the year. We will spend approximately 1.5 to 2 week per chapter, allowing us to finish the requirements in April and leave time for concentrated AP exam review.

|Chapter 1 |Chapter 2 |Chapter 3 Stoichiometry: |

|Chemical Foundations |Atoms, Molecules, and Ions | |

|Chapter 4 Types of Chemical Reactions and |Chapter 5 Gases |Chapter 6 Thermochemistry |

|Solution Stoichiometry (1.5 weeks) |(2 weeks) |(2 weeks) |

|Chapter 7 Atomic Structure and Periodicity |Chapters 8 Bonding: General Concepts |Chapter 9 Covalent Bonding: Orbitals |

|(2 weeks) |(1.5 weeks) |(1 week) |

|Chapter 10 Liquids and Solids |Chapter 11 Properties of Solutions (2 |Chapter 12 |

|(2 weeks) |weeks) |Chemical Kinetics (2 weeks) |

|Chapter 13 Chemical Equilibrium (1.5|Chapter 14 Acids and Bases |Chapter 15 Applications of Aqueous |

|weeks) |(2 weeks) |Equilibria (1.5 wee |

|Chapter 16 Spontaneity, Entropy, and Free |Chapters 17 Electrochemistry |Chapters 21 Nuclear Chemistry (1.5 weeks, |

|Energy |(2 weeks) |some after the AP exam) |

|(1.5 weeks) | | |

|Chapters 22 Organic Chemistry (0.5 weeks and| | |

|blended into other chapters) | | |

We will cover some of these chapters, such as chapters 21 and 22 in conjunction with other chapters, thus we will not spend 1-2 weeks on these chapters. The workload for this course is quite heavy. By the end of December I expect we will be at chapter 11. Furthermore, some of the topics in the later chapters will be introduced in earlier chapters. For example, chemical equilibrium can be introduced in earlier chapters where equilibria is operative in chemical reactions. The same is true for chemical kinetics. As the course proceeds throughout the school year, I seek to integrate the various chemical topics. This approach will give the student a more thorough understanding of the principles of general chemistry and how different topics are related..

TESTS, QUIZZES, AND LABORATORY REPORTS

1. 7-10 quizzes in addition to short lab quizzes.

2. 3 tests announced at least one week before the test date

3. Students will perform approximately 20 laboratory investigations for the school year. The teacher will supplement these experiments with numerous topic-related demonstrations. Chemistry is a laboratory science. Lab reports are a critical component of the grading rubric. Total points for lab reports will be about 25% of the grade. Because colleges may require proof of a laboratory component to this course, students are required to keep an organized laboratory notebook (see course guidelines for details). All lab reports are to be placed in the laboratory notebook. Students will type the discussion component to the lab report and place it into the notebook with a signature.

HOMEWORK

4. Lots of assigned problems at the end of each chapter or handouts to be completed. Homework will be checked but not collected. Quality and effort on these assignments are critical features in the learning process.

5. Laboratory reports

GRADING

6. Tests and quizes (50 % of grade); ; Lab Reports (25 % each). Late lab reports are penalized 10 points per day.

7. Homework, class participation, effort, progress, etc. - see course guidelines. Generally, about 15% of the term grade. Projects(10% of grade)

8. Grades are calculated on a total points basis. Total points earned divided by total possible points times 100%. Letter grades are assigned according to school grading guidelines.

A 90- 100

B 80-90

C 70-80

D 60-70

F less than 60

AP CHEMISTRY EXAM PREPARATION

In addition to the battery of problems at the end of each chapter, students will be routinely assigned the challenge and integrative problems at end of the chapters in Zumdahl. These problems are designed to hone your chemistry thinking skills and to integrate the various chemistry topics. All tests and quizzes will have AP style questions. Beginning in January AP Chemistry Exam Free Response questions will be part of all tests. In April students will begin taking practice AP tests.

Advanced Placement Chemistry Course Syllabus

(ORGANIZED BY AP CHEMISTRY CURRICULAR REQUIREMENTS)

Curricular Chapter in Chemistry, 7th ed., by Zumdahl

Requirement

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2. Atoms, Molecules, and Ions

Dalton’s atomic theory, history and atomic structure, chemical laws, periodic table, isotopes

7. Atomic Structure and Periodicity

Electromagnetic radiation and nature of matter, models of the atom, periodic table and electron configuration, quantum numbers, trends in the periodic table and periodic nature of chemical reactivity.

I. Structure

of Matter 8. Bonding: General Concepts

Types of bonding and bond energies, electronegativity and bond polarity , ionic radius, lattice energy, valence electrons, covalent bonding and bond energies and lengths, Lewis structures and octet rule and exceptions, resonance, formal charge, molecular geometry and VSEPR theory.

9. Covalent Bonding

Covalent bonding and orbital hybridization, bond order, pi and sigma bonds.

18. The Nucleus: A Chemist’s View

Nuclear transmutation, half-life and kinetics of radioactive decay, radioactivity, radioisotopes, types of nuclear decay, nuclear fission and fusion and application to E=mc2 with mass defect, biological effects of radiation and body dosage.

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5. Gases

Kinetic molecular theory, gas variables and units, gas laws and gas stoichiometry, ideal gases and real gases and deviations from the ideal gas law, properties of gases.

II. States of 10. Liquids and Solids

Matter Intermolecular Forces, properties of liquids and solids, influence of intermolecular forces on liquid boiling points, types and structures of solids, vapor pressure and phase changes, heat curves and phase diagrams.

11. Properties of Solutions

Solution composition, energetics of the dissolving process, factors affecting solubility of gases and solids in liquids, Henry’s law and Raoult’s law, vapor pressure of solutions, molality and colligative properties.

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3. Stoichiometry

Mole concept, compound composition and quantities, balancing chemical equations and stoichiometric calculations, limiting reactants and percent yield, empirical and molecular formulas.

4. Types of Chemical Reactions and Solution Stoichiometry

Aqueous solutions and electrolytes, making solution dilutions, types of chemical reactions, molarity, solubility rules, complete and net ionic equations, stoichiometry of precipitation reactions, acid-base reactions and titrations, oxidation numbers, oxidation-reduction reactions and balancing redox reactions, periodicity of chemical reactions of elements and compounds.

III. Reactions

6. Thermochemistry

Nature of energy, state functions, 1st and 2nd laws of thermodynamics, enthalpy and calorimetry, Hess’s law, enthalpies of reaction and enthalpies of formation (and calculations using thermochemical equations).

12. Chemical Kinetics

Reaction rates, differential and integrated reaction rate laws, reaction mechanisms, molecularity, elementary step/rate-determining step, collision model, catalyst effects and energy of activation.

13. Chemical Equilibrium

Principles of equilibrium, equilibrium constants and reaction quotients and equilibrium position, calculating Kc and Kp, LeChatelier’s Principle.

14. Acids and Bases

Nature of acids and bases and their properties, acid and base definitions, pH scale and calculating pH, pH calc of weak acids and bases, strong acids and bases, how structure and periodicity affect acid-base properties, acid and base anhydrides, solving acid-base problems using Ka and Kb, acid-base properties of salts.

15. Applications of Aqueous Equilibria

Equilibrium calculations of acid-base solutions, buffers, titrations and titration curves, solubility equilibria, common ion effect, complex ions.

16. Spontaneity, Entropy, and Free Energy

Spontaneous reactions, 2nd law of thermodynamics, entropy, free energy and reaction spontaneity, free energy and equilibrium, sign conventions for entropy and free energy, thermodynamic equations, temperature dependence of the equilibrium constant.

17. Electrochemistry

Voltaic and electrolytic cells, redox half-cells, cell potential, free energy and cell potential, cell potential and concentrations, Nernst equation, balancing redox reactions, calculating equilibrium constants, batteries (voltaic and electrolytic).

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1. Chemical Foundations

Classification of matter.

3. Stoichiometry

Nomenclature, introduction to the periodic table.

4. Types of Chemical Reactions and Solution Stoichiometry

IV. Descriptive Types of chemical reactions.

Chemistry Periodicity of element and compound chemical reactivities and predict chemical products (this topic is initially introduced as a separate topic, but in large part is continuously taught, reviewed, and integrated into other topics throughout the academic year as it is integral to many topics related to chemical behavior).

7. Atomic Structure and Periodicity

Electromagnetic spectrum, history of the periodic table, general concepts of the periodic table, trends in the periodic table (periodicity of chemical reactivity of elements and compounds addressed here as well, eg, alkali metal chemical reactivity trend).

22. Organic Chemistry

Saturated and unsaturated hydrocarbons, nomenclature, isomerism, carboxylic acids, alcohols, aldehydes, ketones, esters, ethers, and amines, physical and chemical properties of organic compounds (included in prior defined topics).

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V. Laboratory & Chemical Calculations

AP CHEMISTRY LABORATORY ACTIVITIES

AP chemistry students have had significant laboratory experience prior to taking AP chemistry (see part III). Students in AP chemistry record their experimental data and write laboratory reports in a laboratory notebook which is to serve as an official indication of the laboratories that were performed and also supplement the classroom topics.

Each of the AP Chemistry labs is performed in a 96 minute lab period which occurs once per week (sometimes, single periods are also used to perform short labs, or students finish labs after school). Our high school has a Monday to Friday schedule where each day has the same schedule every week. Some labs are finished after school or in the next AP chemistry class period. AP chemistry students perform one lab exercise per week. Some lab exercises require more than one double period; these labs are finished after school or in the next lab period when possible. Additionally, students have performed numerous lab exercises in their first year of high school chemistry – these labs are also listed below. All labs are hands-on (wet labs). Lab reports are required for these activities. The following laboratory exercises list the labs that AP students have performed during all chemistry courses in high school.

Students must abide by significant figure rules, record observations and raw data in their laboratory notebooks, as well as show their calculations when dealing with quantitative data. Students are to write thoughtful and in-depth discussions of their data, with an emphasis on possible sources of error in the experiment and how they could improve the experiment.

I. Labs for AP Chemistry

From “Laboratory Experiments for Advanced Placement Chemistry” by Sally Ann Vonderbrink, PhD.

Flinn Scientific, Inc.

Batavia, IL

1. Finding the Mole Ratios in a Chemical Reaction - The goal is to determine mole ratios in a chemical reaction using experimental data and stoichiometric calculations. Students also make the solutions for the experiments, thus improving their skills in making molar solutions.

2. Synthesis of Alum – Students perform a synthesis reaction, coupled with filtration techniques and crystallization of the alum. They will calculate limiting reactants and percent yield of alum based on starting quantities.

3. Idenitification of Alum, KAl(SO4)2 12 H2O - Students will construct a capillary tube to determine the melting point of Alum; they will analyze the alum for percent composition of water (by heating) and sulfate ( by a precipitation reaction) , in addition to practicing filtration techniques.

4. An Activity Series- Students construct a metal and halogen activity series , and write oxidation-reduction half reactions for the various reactions performed in this lab activity. Based on the lab data they will construct an activity series and compare their series with the published list.

5. Thermochemistry and Hess’s Law - Students will perform an acid-base neutralization reaction and determine the change in enthalpy of the reaction by monitoring temperature changes. They will use Hess’s Law, write molecular, complete, and net ionic equations for these reactions. In addition, students will perform a calorimetry lab to calculate the heat content of some foods.

6. Molecular Mass of a Volatile Liquid – Students vaporize a volatile liquid to determine its molar mass using gas law variables (and the ideal gas law). Accurate use of an analytical balance is another learned skill in this lab activity.

7. Molecular Mass by Freezing Point Depression - Students apply colligative properties (in this case, freezing point depression) to calculate the molar mass of a compound. They will use molecular substances as solutes and record the freezing point of the solution, thus , facilitating the calculation of molality and molar mass. Students will observe how the phase diagram of a pure solvent is shifted when a solute is dissolved in the solvent.

8. Vapor Pressure and Enthalpy of Vaporization of Water - Students learn how the vapor pressure of water changes as the temperature of the water changes. They learn to read volumes of air in a cylinder and apply the ideal gas law to find pressure. They will make use of the Clausius-Clapeyron equation to calculate the enthalpy of vaporization.

9. Analysis of Commercial Bleach - Students perform a oxidation-reduction titration analysis with indicator to determine the percentage of sodium hypochlorite in commercial bleach. Students will perform pipetting techniques, further practice the use of a buret, write redox half reactions, and solidify their titrations skills. They will use the MV = MV equation to calculate molarity of bleach.

10. Study of Kinetics of a Reaction – Students will supplement their knowledge of reaction kinetics by performing a microscale reaction to determine the rate law for the oxidation of iodide ion by bromate ions. Students will calculate reaction order and the rate constant.

11. Determination of the Solubility of an Ionic Compound – Students will use chemical equilibrium principles and the equilibrium expression to determine the solubility of calcium hydroxide in water.

12. Equilibrium and LeChatelier’s Principle – Students learn how a reaction in equilibrium will shift when it is placed under a stress. Changes in temperature, reactant and product concentration changes will be studied to demonstrate LeChatelier’s Principle.

13. Electrochemical Cells – Students construct minature electrochemical cells in microtiter wells and measure voltages (electrochemical potential ) between different wells. They will identify the anode and cathode, write net ionic equations for the redox reactions, and construct their own standard reduction potential chart based on their data.

14. Preparation of Esters - Students will perform and organic synthesis by reacting a carboxylic acid (acetic acid) with an alcohol (methanol) to make methyl acetate in the presence of acid. This reaction will only be performed on a small scale. Students will identify the product by its odor when compared to a known product.

II. Other Laboratory Activities by AP Chemistry Students

15. Students design a lab, prepare solutions, and perform the procedures to precipitate 1.00 g of Cu(OH)2 - students use all the skills that they have learned, including, but not limited to use of appropriate equipment, accuracy, correct significant figures, error calculations to precipitate 1.00 g of Cu(OH)2 . In the lab report students are to emphasize all possible sources of error in their experiments.

16. Determining the Molar Volume and Molar Mass of Gases - Two labs are performed in one lab period. Students will determine the molar volume of any gas at STP and measure the molar mass of butane, both by water displacement procedures. Students will use gas law equations, subtract for water vapor a given temperature, and perform calculations to determine molar volume and molar mass at STP.

17. Determining the percent composition of acetic acid in vinegar – Students titrate a diluted solution of vinegar with a standared NaOH solution and calculate the percent composition of acetic acid in vinegar. Student graph the titration curve and use computer-based lab probes (Vernier, Inc) to measure pH. They will also determine the Ka of acetic acid from their data.

18. Flame Tests and the use of Spectroscopes – students relate wavelength of light and color using a handheld spectroscope when metals are burned. Gas discharge tubes are also used to demonstrate specific line spectra of elements.

19. Constructing molecules using molecular model kits – students learn and demonstrate the molecular geometries predicted by VSEPR theory.

20. Using a spectrophotometer – students determine the absorption spectrum of a compound and they learn to use a spectrophotometer (Spectronic 20). Additionally, they demonstrate the princples of the Beer-Lambert Law.

21. Radioactivity exposure - students learn the inverse square law as it applies to radiation exposure as a function of distance from the radioisotope source. Students use Vernier equipment for this lab. This lab is in conjunction with the 1989 PBS documentary on Chernobyl.

22. Analysis of ions in tap water (qualitative analysis lab)– students perform qualitative analyses to determine the presence of particular ions in tap water.

23. Chromatography lab – demonstration of paper chromatography as it relates to

intermolecular forces.

III. Laboratory Activities from Textbook Laboratory Manuals that were performed by AP Chemistry students in the prior year chemistry course . These laboratory activities were performed in a 96 minute lab period. Lab reports were required for most of these activities.

1. Purification of Foul Water – demonstrates miscibility, filtration, and adsorption of material.

2. Physical and Chemical Properties and Changes

3. Specific Heat of Liquids and Solids

4. Isotopes and Average Atomic Mass

5. Half-life lab – a model

6. Percent of Water in a Hydrate

7. Law of Definite Composition and Multiple Proportions

8. The Formula of a Compounds

9. Molar Quantities

10. Stoichiometry of a Chemical Reaction – Making Chalk, CaCO3

11. Mole Ratios in a Chemical Reaction

12. Activity Series of Metals

13. The Flame Test of various metal nitrates

14. Analyzing Line Spectra using spectroscopes

15. Turning Baking Soda into Salt

16. Thermochemical analysis of the Reaction of Zn with CuSO4

17. Measuring the heat content of a peanut and walnut: Calculating the mass of peanuts to run from Boston to Los Angeles ( 3000 miles).

18. Measuring the Heat of Fusion of Water.

19. Molar Volume of a Gas

20. Determining the Molar Mass of Butane

21. Boyles Law

22. Charles Law

23. Paper Chromatography

24. Sulfur Clock: Chemical Kinetics

25. Chemical Equilibrium – LeChatelier’s Principle – Color Changes of CoCl2 (aq)

26. Acid – Base Titration and Determining the Percentage of Acetic Acid in Vinegar

AP CHEMISTRY COURSE MATERIALS AND SOURCES

Student Textbook including Complete Solutions Guide and Study Guide

Zumdahl. Steven, and Susan Zumdahl. Chemistry. 7th ed. 2007. Boston: Houghton Mifflin.

Zumdahl, Steven, Susan Zumdahl, and Paul Kelter. Study Guide for Chemistry. 7th ed.

Boston: Houghton Mifflin.

Hummel, Thomas J., Steven Zumdahl, and Susan Zumdahl. Complete Solutions Guide to Chemistry 7th ed. 2007. Boston: Houghton Mifflin.

Supporting Textbooks

Brown, Theodore, Eugene LeMay, and Bruce Bursten. Chemistry: The Central Science. 9th ed. 2003. Upper Saddle River, NJ , Prentice Hall.

Kotz, John, Paul M. Treichel, and Gabriela C. Weaver. Chemistry and Chemical Reactivity. 6th ed. 2006. Pacific Grove, CA, Brooks/Cole Thomson Learning.

Laboratory Reference Books

Sally Ann Vonderbrink. Laboratory Experiments for Advanced Placement Chemistry. Batavia, IL, Flinn Scientific, Inc.

Szafran, Zvi, Ronald M. Pike, Mono M. Singh. Microscale Chemistry for High School.

1996. Dubuque, IA. Kendall/Hunt Publishing Co.

Hall, James F. Experimental Chemistry. 4th ed. 1997. Boston, MA. Houghton Mifflin.

Internet-Based Supporting Literature

ChemTeam – dbhs.wvusd.k12.ca.us/webdocs/ChemTeamIndex.html

Contains links to a library of Local, National, and International Chemistry Olympiad Tests.

Collegeboard AP Chemistry Free Response Questions and Answer Guidelines



South Pasadena High School AP Chemistry



AP CHEMISTRY STUDY GUIDES

“Preparing for the AP Chemistry Examination” to accompany the Zumdahl text.

Barrons and Princeton Review AP chemistry preparation books are also used by students to prepare for the AP Chemistry examination.

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