SUPPLIES: Notebook, Lab Notebook (Hard Bound), Graph Paper, Calculator

SUPPLIES: Notebook, Lab Notebook (Hard Bound), Graph Paper, Calculator

AP CHEMISTRY COURSE SYLLABUS 2013-2014

Periods 4,5

Brendan Haynie

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:

90-100A

80-89 B

70-79C

60-69D

0-59F

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

  1. 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

  1. Paper Chromatography (Science Practices - 1,2,4,5,6,7)

Paper chromatography is used to separate the components of unsweetened grape Kool-Aid

  1. 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

  1. 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. Chemical bonds
  2. Lewis structures, and the octet rule
  3. Ionic bonding
  4. 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

  1. 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

  1. 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

  1. 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)
  1. **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 SCN-

  1. 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

  1. **Can We Make the Colors of the Rainbow? An Application of Le Châtelier’s Principle.(Science Practices - 1,2,3,4,5,6,7)
  1. **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: Thermochemistryand 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. Oxidation states and oxidation-reduction reactions
  2. Balancing oxidation-reduction equations
  3. Voltaic cells
  4. Cell EMF under STP
  5. Free Energy and Redox reactions
  6. Cell EMF under nonstandard conditions
  7. Batteries and fuel cells
  8. Corrosion
  9. 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)
  1. 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. Radioactivity
  2. Patterns of Nuclear stability
  3. Nuclear transmutation
  4. Rates of radioactive decay
  5. General characteristics of organic molecules
  6. Hydrocarbons
  7. Alkanes, alkenes, and alkynes (structures and reactions)
  8. Organic functional groups
  9. 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)02.004.006.008.0010.0012.00∞

[nitrile] / (mol L-1)1.100.860.670.520.410.320.250.00

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 ( 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).

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