AP CHEMISTRY COURSE SYLLABUS 2013-2014
Periods 4,5
Brendan Haynie
brendan.haynie@boyd.kyschools.us
Text
Chemistry: The Central Science by Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten,
and Catherine J. Murphy, Pearson Prentice Hall, 12th edition, 2012.
Schedule
Listed below is the schedule for AP Chemistry. The first semester covers the first six units while
the second semester covers the remaining four units. Tests will typically cover multiple units.
Laboratory Experiments will require 25% of the instructional time. Guided inquiry labs taken
from the College Board lab manual are indicated by **
SUPPLIES: notebook, lab notebook (hard bound), graph paper, calculator
GRADING SCALE:
90-100
80-89
70-79
60-69
0-59
A
B
C
D
F
GRADING PROCEDURE:
1. TESTS - 50%
2. PROBLEM SETS - 15%
3. LAB REPORTS, consisting of purpose, procedure, data, data analysis, error analysis, and
conclusion - 25%
4. TERM FINALS - 10%
TOPICS TO BE COVERED
Unit 1
Reading: Chapters 1-2 of Brown, LeMay, Bursten, and Murphy.
Topics: Welcome back to Chemistry (Atoms, Molecules, and Ions)
1. Atoms and the Periodic Table
2. Molecules and molecular compounds
3. Ions
Unit 2 (Big Idea 3)
Reading: Chapters 3-4 of Brown, LeMay, Bursten, and Murphy.
Topics: Stoichiometry and Predicting Reactions Products
1. Chemical equations
2. Patterns of chemical reactivity
3. Formula weights
4. Avogadro's number and the mole
5. Empirical formulas from analysis
6. Quantitative information from balanced equations
7. Limiting reactants
8. Properties of aqueous solutions
9. Precipitations reactions
10. Acid-base reactions
11. Oxidation-reduction reactions,
12. Concentrations of solutions,
13. Solution stoichiometry and chemical analysis
Labs:
1. Determination of the Empirical Formula of Magnesium Oxide (Science Practices 1,2,3,4,5,6,7)
The determination of the percent composition and empirical formula of
magnesium oxide
2. Finding the Ratio of Moles of Reactants in a Chemical Reaction (Science Practices 1,2,3,4,5,6,7)
The method of continuous variations is used to determine the mole ratio of two
reactants in an oxidation-reduction reaction
3. Paper Chromatography (Science Practices - 1,2,4,5,6,7)
Paper chromatography is used to separate the components of unsweetened
grape Kool-Aid
4. Gravimetric Analysis of a Metal Carbonate (Science Practices - 1,2,3,4,5,6,7)
The identity of a Group 1 metal carbonate is determined gravimetrically using a
double replacement precipitation reaction
Unit 3 (Big Idea 1)
Reading: Chapters 6-7 of Brown, LeMay, Bursten, and Murphy.
Topics: The Electronic Structure of Atoms and Periodic Properties of the Elements
1. Wave nature of light
2. Quantized energy and photons
3. Bohr Model
4. Wave behavior of matter
5. Quantum mechanics and atomic orbitals
6. Many electron atoms
7. Electron configurations and the periodic table
8. History of the periodic table
9. Effective nuclear charge
10. Size of atoms and ions
11. Ionization Energy
12. Electron Affinities
13. Properties of metals, nonmetals, and metalloids
14. Trends for Groups 1A, 2A, 6A, 7A, and 8A
Labs:
1. Atomic Spectra and Atomic Structure (Science Practices - 1,2,3,4,5,6,7)
Examine the emission spectra for a series of Group 1A and Group 2A elements
2. An Activity Series (Science Practices - 1,3,4,5,6,7)
Determine the activity series for five metals and three halogens
Unit 4 (Big Idea 2)
Reading: Chapters 8-9 of Brown, LeMay, Bursten, and Murphy.
Topics: Chemical bonding and Predicting and Understanding Molecular Shapes
1.
2.
3.
4.
Chemical bonds
Lewis structures, and the octet rule
Ionic bonding
Covalent bonding
5. Bond polarity and electronegativity
6. Resonance structures
7. Exceptions to the octet rule
8. Strengths of covalent bonds
9. Molecular shapes
10. VSEPR model
11. Hybrid orbitals
12. Multiple bonds
13. Molecular orbitals and their application to diatomics and simple systems
Labs:
1. Molecular Geometries of Covalent Molecules (Science Practices - 1,3,4,5,6,7)
Examine the Lewis structures, VSEPR models, and three dimensional structures
of a series of simple covalently bonded molecules
2. Computational Models for Diatomics and Simple Systems (Science Practices 1,3,4,5,6,7)
Use ab initio computational methods to compute molecular orbitals for a
selection of diatomics and simple polyatomic molecules
Unit 5 (Big Idea 2)
Reading: Chapters 10-11 of Brown, LeMay, Bursten, and Murphy.
Topics: Gasses, Liquids, and Solids
1. Pressure
2. Gas Laws (Boyle's Law; Charles's Law; Avogadro's Law)
3. Ideal Gas Equation
4. Molar Mass
5. Partial Pressure (Dalton's Law of Partial Pressures)
6. Kinetic-Molecular Theory
7. Effusion & Diffusion (Graham's Law)
8. Real Gases
9. Comparison of gases, liquids, and solids
10. Intermolecular forces & properties of liquids
11. Phase changes
12. Vapor Pressure
13. Phase diagrams
14. Structures and bonding of solids
Labs:
1. Determining the Molar Volume of a Gas (Science Practices - 1,2,3,4,5,6,7)
Determine the volume of one mole of H2 gas at STP
2. Determination of the Molar Mass of Volatile Liquids (Science Practices - 1,2,3,4,5,6,7)
Determine the molar masses of various volatile liquids
3. Analysis of Alum (Science Practices - 1,2,3,4,5,6,7)
Determine the melting point and mole ratio of hydrated water to anhydrous
aluminum potassium sulfate in AlK(SO4)2.12H2O
Unit 6 (Big Idea 4)
Reading: Chapters 13-14 of Brown, LeMay, Bursten, and Murphy.
Topics: Properties of Solutions and Chemical Kinetics
1. The solution process
2. Saturated solutions and solubility
3. Factors affecting solubility
4. Expressing concentration
5. Colligative properties
6. Colloids
7. Description of reactions rates and factors affecting reaction rates
8. The rate law and impact of concentration
9. Change of concentration with time (1st and 2nd order reactions)
10. Temperature and rate
11. Reaction mechanisms
12. Catalysis
Labs:
1. **What Is the Rate Law of the Fading of Crystal Violet Using Beer's Law? (Science
Practices - 1,2,3,4,5,6,7)
2. **How Long Will That Marble Statue Last? (Science Practices - 1,2,3,4,5,6,7)
Unit 7 (Big Idea 6)
Reading: Chapters 15,16,17 of Brown, LeMay, Bursten, and Murphy.
Topics: Chemical Equilibrium, Acid-Base Equilibria, Aqueous Equilibria
1. Concept of equilibrium and the equilibrium constant
2. Interpreting and working with equilibrium constants
3. Heterogeneous equilibria
4. Calculating equilibrium constants
5. Applications of equilibrium constants
6. Le Châtelier's Principle
7. Brønsted-Lowry acids and bases
8. Autoionization of water
9. pH scale
10. Strong acids and bases
11. Weak acids and bases
12. Relationship between Ka and Kb
13. Acid-base properties of salt solutions
14. Acid-base behavior and chemical structure
15. Lewis acids and bases
16. Expressing concentration
17. The common ion effect
18. Buffered solutions
19. Acid-base titrations
20. Solubility equilibria, Ksp
21. Factors affecting solubility
22. Precipitations and separation of ions
23. Qualitative analysis for metallic elements
Labs:
1. The Determination of Keq for FeSCN2+ (Science Practices - 1,2,3,4,5,6,7)
Determine the equilibrium constant for the reaction of Fe3+ and SCN2. The Determination of Ka for a Weak Acid (Science Practices - 1,2,3,4,5,6,7)
To experimentally determine the pKa values for two weak acids
3. **Can We Make the Colors of the Rainbow? An Application of Le Châtelier’s Principle.
(Science Practices - 1,2,3,4,5,6,7)
4. **How Much Acid Is in Fruit Juices and Soft Drinks? (Science Practices - 1,2,3,4,5,6,7)
Unit 8 (Big Idea 5)
Reading: Chapter 5,19 of Brown, LeMay, Bursten, and Murphy.
Topic: Thermochemistry and Chemical Thermodynamics
1. What is energy?
2. First law of thermodynamics
3. Enthalpy and enthalpies of reactions
4. Calorimetry
5. Hess's Law
6. Enthalpies of formation
7. Spontaneous processes
8. Entropy and the second law of thermodynamics
9. Molecular interpretation of entropy
10. Entropy changes in chemical reactions
11. Gibbs free energy
12. Free energy and the equilibrium constant
Labs:
1. **The Hand Warmer design challenge(Science Practices - 1,2,3,4,5,6,7)
Unit 9 (Big Idea 3)
Reading: Chapter 20 of Brown, LeMay, Bursten, and Murphy.
Topics: Electrochemistry, Nuclear Chemistry, and Organic Chemistry
1.
2.
3.
4.
5.
6.
7.
8.
9.
Oxidation states and oxidation-reduction reactions
Balancing oxidation-reduction equations
Voltaic cells
Cell EMF under STP
Free Energy and Redox reactions
Cell EMF under nonstandard conditions
Batteries and fuel cells
Corrosion
Electrolysis
Labs:
1. **How Can We Determine the Actual Percentage of H2O2 in a Drugstore Bottle of
Hydrogen Peroxide? (Science Practices - 1,2,3,4,5,6,7)
2. Electrolysis (Science Practices - 1,2,3,4,5,6,7)
Use an electrolysis cell to electrolyze an acidic solution of CuSO4
Unit 10
Reading: Chapters 21, and 25 of Brown, LeMay, Bursten, and Murphy.
Topics: Nuclear Chemistry, and Organic Chemistry
1.
2.
3.
4.
5.
6.
7.
8.
9.
Radioactivity
Patterns of Nuclear stability
Nuclear transmutation
Rates of radioactive decay
General characteristics of organic molecules
Hydrocarbons
Alkanes, alkenes, and alkynes (structures and reactions)
Organic functional groups
Chirality in organic chemistry
Labs:
1. Synthesis of Esters (Science Practices - 3,4,5,6,7)
Synthesize a series of esters and determine scent.
Non-lab activities for each Big Idea
Activities for Big Idea #1
1.
Students will graph and interpret several data sets on atomic properties (atomic radius, first
ionization energy and electronegativity) in order to arrive at the periodic table from the jumps in
the graphs
Possible Activities for Big Idea #2
1.
Students will prepare models of the various electron pair arrangements, and complete a table
which shows the Lewis structure, electron pair geometry, molecular structure, and use that
information to predict the presence or absence of a dipole moment.
Possible Activities for Big Idea #3
1.
Students will identify and balance chemical reactions using a variety of techniques on a series of
quizzes from the reactions problem from previous AP exams. Old NIE’s quizzes
Possible Activities for Big Idea #4
1.
Students will demonstrate their knowledge of the determination of kinetics by displaying the
solution to the following problem to the class.
The thermal decomposition of an organic nitrile produced the following data:
t / (103 s)
0
2.00
4.00
6.00
8.00
10.00 12.00 ∞
[nitrile] / (mol L-1)
1.10
0.86
0.67
0.52
0.41
0.32
0.25
0.00
Determine the order of the reaction and the rate constant.
Possible Activities for Big Idea #5
1.
Students will explore an animation on heating and cooling curves (www.kentchemistry.com,
select heating curves) and answer a series of questions regarding their observations of
particulate motion in the various phases.
Possible Activities for Big Idea #6
1.
Students take the data from the spreadsheet “Titrations” on pH against added acid or base, and
interpret the data in terms of the types of acid or base present, endpoints, the presence or
absence of a buffer system, and appropriate indicators with justification based on the data.
Possible Activities for Societal or Technological Impact of Chemistry (lab or non-lab)
1.
Students solve a stoichiometry problem on the amount of carbon dioxide produced in the
burning of a tankful of gasoline (assumed to be octane) with information of the size of the gas
tank of the vehicle, the density of octane (0.7028 g mL-1), and a variety of other conversion
factors. Following the solution of this problem, a discussion of what happens to this carbon
dioxide will ensue encompassing the greenhouse effect, whether the burning of fossil fuels
contributes to global climate change, and if something should be done about the burning of
fossil fuels (especially given current estimates for the amount of fossil fuel remaining in the
earth and the students estimated lifetime).