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AP Chemistry Syllabus
Text: Chemistry by Zumdahl and Zumdahl, 5th ed., Houghton Mifflin Company, 2000. ISBN# 0395985811f (student version).
Supplemental aids:1. Zumdahl Solutions Guide, 5th ed. (same publisher as above).2. The Princeton Review: Cracking the AP chemistry exam,
20062007 edition.
Laboratory texts: we do not use a specific lab text, instead we utilize lab handouts received from AP chemistry summer institutes and
two day conferences.
Class Format
Our campus is on a Block schedule with classes being 80 minutes in length. Students attend class on an A or B day schedule. Generally we meet five times in a two week period.
Class time is split up between lectures, demonstrations and student problem solving in groups. On the average a class is 15 – 20 minutes of
teacher led discussion followed by individual or group problemsolving of old AP type problems/questions for 30
minutes and then group reporting of answers and reviewing the chemical/mathematical processes in answering the questions for the remainder of the class.
Laboratory Experiences
Labs are usually begun during class utilizing 1 or 2 class periods per two weeks, followed by open lab time before school and after school. After
school lab time is utilized most often allowing students 6090 minutes three days a week. A typical lab would require student/group work of three to four hours over a two week period. All labs require hands on experiences or physical manipulations, understanding of chemical processes and procedures, interpretations and sharing of results.
Each student will be required to keep a Lab book. The lab book will consist of the Table of Contents and reports for each lab done. The grade for each lab will be indicated in the Lab book. Each report will be broken down into the following: Title, purpose, hypothesis, procedure, list of materials, data tables (both observational and data), calculations and a conclusion. Additionally, each report will include a paragraph outlining possible sources of error. Emphasis will be on technique and accuracy of data collection and interpretation and calculations.
Post lab discussion will be led by the teacher and require student/group communication of results.
The following is a list of labs for the year:
1. Review of lab safety/proper taking of measurements such as using analytical balances, volumetric flasks and so on.
2. Identification of an unknown by its physical properties. Students/groups will use corrects procedure for determining boiling/melting points to correctly identify knowns followed by a given unknown.
3. Percent composition of an unknown chlorate. The decomposition of a chlorate will be done using proper technique. The stoichiometric calculation of the products will done and compared to the actual yield.
4. % of water in a hydrated crystal. Measure and calculate the mass of each product and determine the empirical formula.
5. Netionic lab. Through a series of chemical reactions, groups of 3 will utilize knowledge of the periodic table and reaction types to predict the products of each reaction and then write the correct ionic or net ionic equation. Students will be required to calculate and measure quantities to make their own solutions for each reaction. Organization of data and observations into tables is required.
6. Separation techniques. Students will work in pairs to perform various methods of separation including distillation and chromatography. Students will determine which technique is appropriate for given question.
7. Electrochemical Cells. Students will work in pairs to determine the activity series using electrochemical potentials. Based on acquired data, students will organize the series for several metals including zinc copper and lead. Students will then perform calculations using the Nernst. Each group will report its series to the class.
8. Qualitative Analysis. Students will work in pairs. They will record observations of various reactions for cations and anion. Results will be organized into tables. Students will then be given unknown solutions of cations/anions and correctly identify them. Groups will report their findings to the class.
9. Calorimetry. Students will construct a simple calorimeter and determine the heat content of a chosen food item. They will perform the associated calculations and then compare answers with label information.
10. Hess’s Law. Working in small groups, students will determine the enthalpy of an acid/base neutralization. They will determine the
equations and formulate the overall reaction, calculating the enthalpy.Accuracy and sources of error will be emphasized.
11. Atomic spectra analysis. Students will observe the various colors and analyze the spectra of various metallic salts. Emphasis will be on observation and measuring the wavelength using a spectroscope for salt. Students will then be given an unknown and use their data/observations to make the correct analysis. Calculations for frequency of wavelengths will performed.
12. Effects of Intermolecular forces on boiling points. Students will use CBLs and temperature probes to graph the boiling curves of different liquids. They will analyze the relationship between bonding forces and boiling points. Graphs will be printed and reports shared with the class.
13. Bonding geometries. Students will work in pairs using models to observe the 3dimensional shape of various covalently bonded molecules. Drawing will be incorporated into lab reports. Molecular formulas will be given, predictions made and actual models built.
14. Avogadro’s Law. Students will work in groups to determine the exact amounts of reactants necessary to fill given volume. Stoichiometry calculations will be made, solutions prepared and
measurements taken. Accuracy is necessary as is a thorough knowledge of gas laws. Pressure, room temperature and all variables must be considered in making their predictions and comparing them to their results.
15. Boyle’s Law. Using CBLs and gas sensor probes, students will measure and gather data to construct graphs which will illustrate Boyle’s Law.
16. Molar Mass determination by Freezing point depression of an organic compound. Using concepts of colligative properties, students will calculate the molar mass of a compound. Measurements will be taken and calculations done based on chemical principles.
17. Synthesis and % of Cl in a halide salt. Students will use knowledge of reaction types and separation techniques to measure and calculate the % of Chloride ion in an unknown. Several complex steps are involved and accuracy in imperative. Proper lab technique is emphasized. This lab is usually a part of the semester final grade.
18. Reaction Rate of Cviolet. Using CBLs and colorimeters, student will calculate and graph the rate of the reaction. Proper labeling of the graph and calculation of slope is necessary. Results will be shared and compared with the class.
19. Titration of a strong base and weak acid. Students will work in pairs.
Preparation and standardization of a strong base and the calculated Molarity is the first step, followed the determining the Molarity of an unknown weak acid. Titration curve will be constructed. Various calculations such as Molarity, number of moles of weak acid at
equivalence point will be performed. Determination of equilibria (Ka) and pH will be included. Complete calculations are required.
20. Titration curve of a diprotic acid. Using the CBL, the titration curve of a weak diprotic acid will be graphed.
ExamsAll major exams will include the required components of the AP curriculum. Questions from released AP exams, both multiple choice and free response will be included in each exam.
Unit One
• Review Summer Assignment. o Measurements: review mathematical equations and
processed for conversions of units and typical calculations such as dimensional analysis and significant figures.
o Writing & balancing equations: predicting products, identifying types of reactions.
o % composition, empirical and molecular formulas and the applicable calculations.
o Historical models of the atom; comparing Dalton to Rutherford to Bohr and prelude to Quantum structure of the atom.
o Molar mass problems: determining molar masses and the chemical calculations related to molar conversions.
• Stoichiometry.
o Stoichiometry relationships: understanding molar relationships between reactants and products and the applicable calculations.
o Limiting Reactants: understanding the stoichiometric processes in determining the quantifiable relationships between reactants and products.
o*Assigned problems/questions from the Text and released AP exams.
Unit Two:
• Chemical Reactions
o Identification of different reaction types using previous knowledge.
o Predicting products for each type based on properties of reactants and using the periodic table.
• Aqueous Reactions & Solubility Rules o Solubility Rules and their uses in netionic reactionso Writing Netionic reactions.o Demonstrations of soluble and insoluble ppts.o Identifying and balancing equations in acid and base
solutions.
*Assigned problems/questions from Text and released AP exams.
Unit Three:
• Electrochemistry
o Galvanic/voltaic cells. Drawing conclusions based on voltage potentials such as chemical equilibrium, flow of electrons and related problems.
o Cell diagrams: drawings to show oxidation/reductions, electroplating and standard cell notation.
o Cell potentials: calculations for voltages of various cell possibilities.
o Faraday’s Law problems: mathematical manipulations involved in relating cell voltage to electroplating.
o Nernst equation: calculating the effects of changes in Molarity of electrolytes.
o Electrolytic cells: drawing and identifying parts of the cell and the related calculations.
*Assigned problems/questions from Text and problems from released AP exams.
Unit Four:• Thermochemistry
o Relationship between energy, heat & worko Calorimetry problems: using chemical equations for “q”
and calculating heat lost and gained between systems.o Enthalpy and related problems: calculating enthalpy
changes, relating Stoichiometry to enthalpy and determining Molar heat.
o Hess’s Law and related problems. Piecing together data and calculations to determine overall enthalpy changes in multiple step reactions.
o Data will be analyzed to determine answers to text problems and released AP exam questions. Answers will be discussed with and between students working with the teacher and in small groups.
• Thermodynamics o Spontaneous reactions: looking at the relationship
between enthalpy, entropy and temperature. o Entropy and 2nd Law of Thermodynamicso Thermodynamics and Keqo Gibbs Free Energy: performing calculations involving
chemical processes such an entropy and enthalpy and temperature to a reaction to be spontaneous.
o Data from questions and problems assigned in the text and from released AP exams will be analyzed and discussed between the teacher and students.
*Assigned problems from the Text and released AP exams.
• Review of Nuclear Chemistry o Predicting nuclear stabilityo Types of radiation and their relationships.o Transmutation problems: calculating the effects of
nuclear emissions.o Halflife problems and associated calculations.
*Assigned questions/problems from the Text.
Unit Five:
• Atomic Structure o Quantum theory review: Aufbau principal, Heisenberg’s
Uncertainty Principle, Pauli’s exclusion principle.o Quantum number assignments/periodic table:
determining the quantum numbers for an element based on periodic law. Identifying invalid quantum numbers.
o Electromagnetic radiation and equationso Calculations for energy of electron transitions from and
to various energy levels: Rhydberg’s equation, Planks constant and others.
• Periodic Trends : Relating an elements position on the periodic table to the following:
o Ionization energieso Radiio Electronegativitieso Affinitieso Bonding predictionso Physical properties predictions.o Questions from released AP exams will be used to
encourage analysis and discussion between teacher and students. Students will work problems and present answers to the class.
• Bonding types o Ionic & covalent (review)o Dispersion forces & typeso Lewis structures: predicting and drawing shapes.o VESPR modelso Formal chargeso Understanding the relationships between types of
covalent bonds and their properties such as physical points. Models will be shown/shared with the class
*Assigned problems from the Text and released AP exams.
• Final Exam review & finals.
Unit Six:
• Gas Laws o Review the principles of Kinetic Theory and its
influences on particle behavioro Introduce the following gas laws: Boyles, Charles,
Avogadro’s, GayLussac, Ideal and nonIdeal laws.o Students will analyzed data and solve related gas law
problems.o Nonideal gas behavior and calculations.
*Assigned associated problems from Text and answers reviewed in class.
• Kinetic Molecular Theory o Students will review the principles and properties of
solids & liquids.o Analyze Phase diagrams and identify aspects such as
triple point, critical temperature and pressure*Assigned related problems from the text and answers discussed by students in class.
• Intermolecular forces o Students will identify the types of IMFs and the effects
these forces have on particle behavior and properties. o Relate periodic law with predicting types of IMFs
elements typically have.o Organic Review: hydrocarbons and functional groups.o Student will work in groups on identifying and naming
organic compounds based on their knowledge of nomenclature and functional groups.
o Review and rank the different types of Dispersion forces*Assigned questions from the Text and from released AP exams.
• Solution chemistry
o Review the various methods of expressing solutions concentration such as Molarity, molality, Normality and % solutions and how to prepare dilute solutions from concentrated ones.
o Students will work in groups to solve related concentration problems and communicate those answers in class and with the teacher.
o Examine the colligative properties of solvents and how they can predict properties of the solvent such as freezing point and boiling point when concentrations are changed
o Students will analyze data and work solutions to changes in boiling and freezing points due to changes in concentration as well as Raoult’s Law.
o Calculate the Molar Mass of a solution from its freezing point depression or boiling point elevation.
*Assigned questions and problems related to the above from the Text and from released AP exam. Some problems will be worked individually and as groups and reviewed in class together.
Unit Seven
• Kinetics o Discuss the different ways of measure the rates of
reactions such as relative rates, integrated rate laws and order of reactions.
o Review the factors that affect reaction rates such as temperature, concentration, surface area and the role of catalysts.
o Analyze reaction data to perform mathematical calculations based on chemical principles for determining orders of reactions, overall orders and rates of reactions.
o Predict rate laws based on molecularity; know the role of intermediates and elementary steps.
*Assigned problems from Text and released AP exams to analyze information and determine solutions to basic Kinetics questions.
• General Equilibrium
o Introduce the concept of general equilibrium and Keq.o How to calculate Keq from reaction data.o Kc & Kp conversionso Show the relationship between K & Q concepts & solve
related problems using the RICE table and data from text problems and released AP exams.
o Discuss LeChatelier’s principle and how changes in factors such as pressure and concentration affect the equilibrium of a reaction.
o Relate equilibrium back to concepts of Electrochem.o Learn how to correctly write an Equilibrium expression.
*Assign related question and problems from the Text and released AP exams.
• Acids/Bases
o Review the basic definitions of Acids and Bases: Arrhenius, BronstedLowry and Lewis.
o Learn how to identify acids & base using the above definitions.
o Review properties of Acids & Bases.o A/B neutralization and predicting salts; determine
whether the salt is an acid or base salt from the reaction.o Solve calculations for pH and pOH and convert between
the two.o Introduce concepts of Ka and Kb and solve related
problem such as Ka for weak acids and Kb for weak bases.
o Show the relationship of Ka and Kb for weak and strong acids and how to identify weak acids or based from their K values.
o Calculate pH or pOH from reactions data and Ka or Kb values, and how to calculate Ka or Kb from the pH or pOH.
*Assign problems from the text and released AP exams. Students will work on old AP questions and Princeton Review resource book in groups and share answers with the class.
• AcidBase Neutralizationo Review reactions types and identify acidbase
neutralizations. Determine from the reaction and identify/name the resulting salts.
o Review whether A/B salt is neutral, acidic or basic.
o How to calculate the pH of a salt based on hydrolysis of the salt.
o Solve problems and perform calculations on determining the pH and pOH of an acidbase titration.
o Introduce the concept of Buffers and solve related calculations on determining the pH of buffers during and acidbase titration.
o Learn how to determine Buffer systems based on desired pH or pOH.
o Review types of indicators and identify needed indicator for titration of a particular pH.
o Graph titration data and analyze the graph to identify the neutralization point and the concentration of an acid or base from the graphed data. Identify the midpoint and calculate the pH from interpreting the graphed data.
*Assign associated problems from the Text and released AP question/problems, both multiple choice and free response. After school sessions on working through these problems with groups of students and the teacher will be provided. Results will be shared.
• Introduce the concepts of Solubility.o Review solubility rules and reactions types that typically
produce precipitates.o Review how to solve equilibrium problems with the
RICE table using solubility data.o Show the relationship between Ksp and the formation of
a precipitate.o Solve problems calculating the Ksp of a reaction and
identifying which precipitate will form first when comparing two reactions.
o Examine the common ion effect and LeChatelier’s principle and their effects on precipitate formation.
o Review the concept of complex ions
*Assign related problems on aqueous equilibria from the Text and from released AP exams. Students will take problems data and solve problems working in small groups and share with the teacher and class.
AP exam Review: Before and after school sessions will be provided to review for the exam.
AP Exam Reviews:
Class time:1. atomic structure2. ionic reactions; solubility rules3. thermochemistry4. thermodynamics
Outside of class:1. bonding & lewis structures2. electrochemistry3. gases4. equilibrium5. acidbase equilibrium6. Ksp
