Advanced Placement Chemistry
Course Syllabus
Texts:
Chemistry by Zumdahl and Zumdahl, 6th ed., Houghton Mifflin Company, 2003.
ISBN: 0-616-2605-8.
Hein, Best, Pattison, and Arena: Introduction to General, Organic, and Biochemistry
ISBN: 0-534-37998-2
Course Description:
AP Chemistry is designed to be a freshmen level college course equivalent to a year of
general chemistry suited for science majors. The pre-requisites for enrolling in AP
Chemistry are APP Chemistry and Algebra II. Students taking AP Chemistry are usually
juniors, however an occasional senior is enrolled. Class size averages around 20
students. Most years we have two classes of AP Chemistry.
Our school has a seven period day with each class being 55 minutes long. The first period
of the day is optional, available for those that choose to take seven periods per day. We
are on the year round schedule so we begin school in late July or early August. School
ends during the last week of May. In order to increase class time and meet the demands
of the course we also meet before or after school for an hour each week. Extended lab
time is also available once a week. We do this during zero periods for those that do not
have the optional zero period course, or after school for those that cannot make the zero
hour. Scheduling of AP chemistry is also planned so that we can work through lunch if
we need to in order to complete labs. In the spring semester we meet twice a week
during third quarter and three times a week during fourth quarter after school hours. This
is time is used for labs, AP exam review or just as help sessions.
Several topics required are covered in APP Chemistry and a very short time is spent
reviewing them in AP Chemistry at the beginning of the fall semester. Also, some of the
labs are done in APP Chemistry so that each student has had exposure to all labs by the
time they finish the two-year sequence. Times specified for each unit are approximate
and may vary a few days depending on the class abilities and schedule conflicts.
Our high school has a wide population of learning styles due to our diverse student body.
We have 23 languages spoken among our students. We are very proud of our diverse
population and spend numerous hours learning additional instructional strategies to meet
the needs of our population. Our AP program includes students from many cultures so it
is essential that students be given additional assistance during class (tutors, dictionaries,
etc.) when necessary.
Grades are calculated on a point system where tests count 75% of their final grade.
Homework, quizzes and small projects are assigned regularly and given a point value
relative to the assignment’s difficulty.
Course Objectives:
Students will understand chemical fundamentals and work problems dealing with
chemical concepts. Students will learn to analyze scientific issues using scientific
problem solving skills.
Students will become critical and independent thinkers who do not memorize their way
through science courses.
Students will be able to express their ideas with clarity and logic.
Students will work in pairs in lab and learn to work efficiently with a partner.
Students will use their lab experience to learn to physically manipulate equipment and
materials in order to make relevant observations and collect data. They will use their
results to form conclusions and verify hypotheses. Students must communicate their
results and procedures in a formal written lab report. They must also keep a journal of
their time spent in lab.
Students will be prepared to score well on the AP exam.
Course Outline:
Fall Semester: (approximately 16 weeks when finals week and standardized
testing times are removed)
Review Sessions (1.5 weeks)
Students will review topics covered in APP Chemistry. They will receive an extensive
packet as homework for each topic. Packets are a combination of teacher’s work and
chapter reviews from the supplemental workbook for our text. Packets will be checked
and discussed on the following day in class. Topics included in this review session:
Measurement standards and dimensional analysis
Classification and properties of matter
Atomic theory and structure
Nomenclature and quantitative composition
Chemical Reactions and Equations
Stoichiometry
Chemical Bonds and structure of compounds
After completing these packets the students should be able to successfully:
1. Use the basic vocabulary adequately for each topic.
2. Work easily with the metric system, temperature scales, significant figures, and
scientific notation, density, heat quantities, etc.
3. Distinguish between the three classes of matter.
4. Discuss and distinguish between physical and chemical properties and changes.
5. Describe the structure of the atom complete with extensive electron placement.
Discuss quantum numbers and use them to describe the location of electrons.
Define and identify isotopes, atomic number, and atomic mass.
6. Name compounds and calculate molar mass, moles, percent composition,
empirical and molecular formulas.
7. Name and identify the different types of reactions (Composition, etc.). Write and
Balance equations. Predict products of reactions. Discuss heat content of
reactions.
8. Work stoichiometric problems including those involving limiting reagents and
percent yield. Also work problems dealing with gases and stoichiometry.
9. Predict periodic trends such as ionization energy, electronegativity, atomic size,
and electron affinity.
10. Define and describe ionic and covalent bonds. Predict type of bond using
electronegativity differences. Do Lewis dot structures for ions and compounds,
and predict molecular shape using VSEPR theory.
Labs to begin the AP Chemistry Class (done after review session) (1 week)
The Empirical Formula of an Oxide
The Absorption of Cobalt (II) Chloride
Students will be expected to become familiar with the vocabulary
related to each of the following sections.. Students will be held
responsible for the definitions of the key terms listed in the text for
each section.
Kinetic Molecular Theory and States of Matter: (3 weeks)
Topics covered in this section include:
1. General Properties of Phases of Matter:
2. Kinetic Molecular Theory
3. Gas Laws
a. Boyle’s Law
b. Charles’ Laws
c. Dalton’s Law of Partial Pressures
d. Graham’s Law
e. Henry’s Law
f. Guy-Lussac’s Law
g. Ideal Gas Equation
h. Real Gases
i. Air pollution
4. Water and Properties of Liquids
a. Evaporation, vapor pressure, surface tension, boiling point, and melting
point.
b. Hydrates
c. Physical and chemical properties of water
d. Water pollution
e. Intermolecular forces
f. Water pollution
5. Solids
a. Crystalline forms
b. Amorphous forms
6. Phase Diagrams
The students will:
1. Describe the particles placement, movement and energy level in each of the
three phases of matter.
2. State and discuss the major points of the Kinetic Molecular Theory as it
pertains to solids, liquids, and solids.
3. Work problems with all the gas laws listed above.
4. Discuss intermolecular forces and relate them to physical properties.
5. Interpret heating curves and phase diagrams. Identify triple point, boiling
point, critical temperature, etc.
6. Distinguish between crystalline and amorphous solids.
7. Discuss unit cells and crystalline formations.
8. Discuss the major forms of water and air pollution.
Student will work in pairs and perform the following labs:
Boyle’s Law and Charles’ Law
The Combined Gas Law and Dalton’s Law
Hydrates and the Determination of the Formula of a Hydrate
The Identification of an Unknown Liquid
Solutions: (2 weeks)
Topics covered in this section include:
1.
2.
3.
4.
5.
6.
7.
General properties
Solubility rules
Rates of dissolving
Reaction mediums
Concentrations of solutions
Colligative Properties
Colloids
The student will:
1. Describe the nine types of solutions and list general properties of true
solutions.
2. Use the solubility rules to predict solubility of solids in aqueous solutions.
3. Describe how temperature and pressure affect solubilities.
4. Work problems dealing with moles, mass %, molality and mole fractions.
5. Describe colligative properties and work problems dealing with Raoult’s
Law, boiling and freezing point deviations and osmotic pressure.
6. Describe the Tyndall Effect.
7. Define colloids and describe colloidal suspensions.
Students will work in pairs to perform the following labs:
Solubility Curve of KNO3
Freezing Point Depression with Antifreeze
Chemical Kinetics: (2 weeks)
Topics covered in this section include:
1. Rate of reaction
2. Factors that affect reaction rates
3. Rate Law expression
4. Order of reactions
5. Collision Theory
6. Transition state theory
7. Reaction Mechanisms
8. Catalysts
The student will:
1. List and discuss the factors that determine the rate of a reaction.
2. Work problems using experimental data to determine the rate law.
3. Determine the order of reactions.
4. Use proper units for the rate constant.
5. Compare and contrast zero, first and second order reactions in terms of graphs,
rate constants and slopes, and the half life of the reaction.
6. Work problems involving activation energy and the Arrhenius equation.
7. Discuss the role of a catalyst in the rate and mechanism of a reaction.
The students will work in pairs to perform the following experiments:
Reaction Kinetics
Rates of an Antacid Reaction
Chemical Equilibrium: (2.5 weeks)
Topics covered in this section include:
1. Basic concepts of chemical equilibrium
2. LeChatelier’s Principle
3. Equilibrium constants
a. Kw
b. Ka
c. Kb
d. Ksp
e. Kp
f. Kc
4. Reaction Quotients
5. Calculations involving equilibrium constants
The student will:
1. Describe the meaning of dynamic equilibrium.
2. Use LeChatelier’s Principle to predict in which direction equilibrium will shift
when affected by temperature, pressure, and concentration changes.
3. Interpret the position of equilibrium using the value of the constant.
4. Work problems involving the value of the equilibrium constant.
5. Work problems involving the value of the reaction quotient.
The students will work in pairs to perform the following experiments:
Le Chatelier’s Principle
Determining an Equilibrium Constant
Acids, Bases and Salts: (2.5 weeks)
Topics covered in this section include:
1. Definitions and properties of acids and bases. Included are Arrhenius,
Bronsted-Lowry, and Lewis acids and bases.
2. Reactions of acids and bases
3. Definition of salts.
4. Electrolytes and non-electrolytes.
5. Ionization of water.
6. pH and pOH scales
7. Calculation of pH and pOH.
8. Strong and weak acids and bases
9. Hydrolysis
10. Buffers and the Common Ion effect.
11. Writing Net Ionic Equations
12. Acid Base Indicators
13. Titration Curves
14. Acid Rain
The student will:
1. Define and give properties of acids and bases using the three main definitions.
2. Define salt.
3. Describe the acid base reactions.
4. Describe the concept of hydrolysis.
5. Identify weak and strong electrolytes
6. Write net ionic equations.
7. Work problems determining pH, pOH, H ion and OH ion concentrations.
8. Judge salt solutions to be acidic or basic.
9. Explain the common ion effect and the chemistry of buffers.
10. Describe how to use a buffer solution.
11. Work problems dealing with buffers.
12. Select indicators for titrations.
13. Analyze and explain titration curves.
14. Work problems involving titration curves.
15. Discuss what causes acid rain and its effect on the environment.
16. Identify conjugate acid-base pairs.
The students will work in pairs to perform the following experiments:
The Analysis of Vitamin C in Foods
Acids, Bases, pH, Hydrolysis and Buffers
Titration with an Acid and a Base
Fall Final Exam
Spring Semester: (13 weeks before AP exam, removing time for
state wide testing)
Oxidation Reduction: (1.5 weeks)
Topics covered in this section include:
1. Definitions of oxidation and reduction
2. Oxidation numbers
3. Redox reactions
4. Activity series
The student will:
1. Identify oxidation and reduction reactions.
2. Identify oxidizing and reducing agents.
3. Describe what oxidation numbers represent and how to find them on periodic
table.
4. Write and balance redox reactions in acidic and basic mediums.
5. Use the activity series to predict products.
The students will work in pairs to perform the following labs:
An Activity Series of Several Metals
Quantitative Redox Titration
Electrochemistry: (2.5 weeks)
Topics covered include:
1. Electrical conductivity
2. Electrolytic Cells
3. Faraday’s Law
4. Voltaic or Galvanic Cells
a. zinc- copper cell
b. copper-silver cell
5. Standard Electrode Potentials
6. Nernst Equation
7. Lead storage battery
8. Nickel cadmium battery
The student will:
1. Identify cathode and anode.
2. Distinguish between the types of cells in terms of function and G.
3. Use Faraday’s Law to solve problems.
4. Diagram cells using proper notation.
5. Calculate cell voltages using the Standard Reduction Potentials.
6. Discuss standard hydrogen cell.
7. Write half reactions and overall cell reactions for electrolysis processes.
8. Work problems using Nernst Equation.
9. Establish the relationship between the free energy change, the cell potential and
the equilibrium constant.
The students will work in pairs to perform the following labs:
Zinc Plating of Ornaments
Electrolysis of Water
Nuclear Chemistry: (1.5 weeks)
Topics included in this section:
1. Radioactivity
2. Alpha, Beta, and Gamma particles
3.
4.
5.
6.
7.
Radioactive disintegration series
Nuclear fission and fusion
Mass energy relationship in nuclear reactions
Nuclear equations
Effects of radiation
The student will:
1. Describe the relationship between proton-neutron ratio and nuclear stability.
2. Describe the particles of radioactive decay.
3. Work problems dealing with binding energy.
4. Balance nuclear equations
5. Work problems dealing with half life.
6. Distinguish between fission and fusion.
7. Describe uses of fission and fusion. Include advantages and disadvantages.
8. Describe the effects of radiation.
Thermodynamics: (2.5 weeks)
Topics included in this section include:
1. Spontaneous Reactions
2. State Functions
3. Laws of Thermodynamics
4. Entropy and the Second Law of Thermodynamics
5. Gibbs Free Energy
6. Free energy and temperature
7. Free energy and Equilibrium constant
The student will:
1. Define state functions
2. State and discuss the laws of thermodynamics
3. Define internal energy, PV work, enthalpy, entropy and free energy.
4. Calculate entropy change.
5. Work enthalpy problems.
6. Calculate free energy changes from enthalpy and entropy changes.
7. Use Hess’s law to solve problems of energy, entropy and free energy.
8. Determine the spontaneity of a reaction.
9. Understand the relationship between free energy change and equilibrium.
The students will work in pairs to perform the following experiments:
Hess’s Law
Entropy and Enthalpy Changes
Thermodynamics of Homemade Ice Cream
Organic Chemistry: (2.5 weeks)
Topics included in this section include:
1. Carbon atom bonding
2. Functional groups of organics
3. Alkanes, alkenes, alkynes, cycloalkanes and aromatics
a. nomenclature
b. bonding and structure
c. isomers
d. reactions
e. sources
f. gasoline
4. Alcohols, ethers, aldehydes and ketones
a. nomenclature
b. bonding and structure
c. general properties
d. common compounds
5. Carboxylic acids and esters
a. nomenclature
b. bonding and structure
c. general properties
d. common compounds
The students will work in pairs to perform the following experiments:
The Structure of Hydrocarbons (done with balloons to show structures)
The Synthesis and Analysis of Aspirin (Calculating % Yield)
The Properties and Preparation of Esters and Soaps
Aldehydes and Ketones (Identifying tests, properties and reactions)
Time remaining will be spent on AP reviews, and practice exams.
Spring Final Exam
Laboratory Portion
Labs done in AP Chemistry have been listed at the end of each section they pertain to. I
have also listed labs completed in the APP course that is a pre-requisite of this course.
That list of labs follows this section. All labs are done with students working in pairs.
Students do pre-lab and post-lab exercises as well as a lab report for each lab and keep a
journal of their lab activities. All labs are student conducted. For those labs that require
more than the time allowed in our 55-minute periods we manage to either do them before
or after school or use our lunch time to complete the labs. With some classes Saturday
labs are done. We assess our needs and time available as a class and make the best
decision for that particular group of students. We spend time in the lab equivalent to a
double period per week.
We are fortunate to be in the same city as a major university and have a great working
relationship with their chemistry department. They frequently furnish us with needed
supplies and loan us equipment if we need it.
Labs completed in APP Chemistry:
Lab Equipment Names and Functions (check in lab)
Lab Safety
Lab Techniques I and II (instruction on how to perform correct measurements using
balance, graduated cylinder, how to light Bunsen burner, how to centrifuge, how to
prepare solutions, how to filter,etc.)
Determination of Density
Physical and Chemical Changes (Perform changes and identify them as physical or
chemical)
Elements, Compounds and Mixtures (Students analyze unknowns and identify the class
of matter)
Simple Chemical Reactions (student performs composition, decomposition, single and
double displacement reactions)
Preparation and Properties of Hydrogen Gas (Determines molar volume of gas and
studies the prepared gas)
Preparation and Properties of Oxygen Gas
Preparation and Properties of Carbon Dioxide Gas
Carbon and its Allotropes (Studies allotropes of carbon, structures and properties)
Solutions (Students prepare different types of aqueous solutions, study factors that
increase dissolving time, etc.)
Separation Using Chromatographic Techniques
Flame Tests
Household Acids and Bases (Determining pH – along with discussion on choosing
indicators and practice exercises)
Analysis of a KClO3-KCl Mixture (Calculations Based on Balanced Equations)
Supplemental Resources:
Chem Lab: Laboratory Experiments in General, Organic, and Biochemistry,
Henrickson, Byrd, and Hunter, 2nd Edition
Experiments in General Chemistry, Wentworth, 4th edition
Chemistry: Connections to our Changing World - Laboratory Manual, Prentice Hall
2002
ChemTopic Labs – Thermochemistry, Cesa, Flinn Scientific, 2002
Chemistry – The Central Science, Brown, LeMay, and Bursten, 10th edition
Test Bank and Instructor’s Manual for Hein, Best, Pattison and Arena’s Introduction to
General, Organic and Biochemistry, 7th edition