Download AP Chemistry Syllabus SLPS

AP Chemistry Syllabus
Instructor: Phillip Norris
Phone: (314)776-3300 ext. 13210
Room: 321W
Email: [email protected]
Planning Period: 6th
Website: http://www.slps.org//Domain/2441
Course Description:
In keeping with the objectives of the College Board, students enrolled in AP Chemistry will cover content equivalent to
what is presented in two semesters of college general chemistry. Upon successful completion of this course and
achievement of a satisfactory score on the AP Chemistry Examination, students may have the opportunity to receive
general chemistry credits or place out of general chemistry classes and move into more advanced science courses during
their first years in college.
Students will review concepts presented during their first course of high school chemistry beginning with problem solving
skills, data collection, significant figures, stoichiometry, and the basics of the periodic table and general properties of
matter. Moving from this review foundation, students will study chemical reactions, solutions, properties of gases and
thermochemistry before focusing in on a more in depth examination of the periodic table and chemical bonding. They
will explore the intricate differences between solids and liquids, properties of solutions and reactions of acids and bases,
chemical kinetics, equilibria, spontaneity, free energy, entropy, and electrochemistry.
Throughout both semesters of AP Chemistry, an emphasis will be placed upon problem solving skills, descriptive
chemistry, development and use of models to explain chemical principles, and the prediction of products in chemical
reactions. Laboratory experiments have been aligned with the topics and concepts and will be an integral part of the
course. They will be scheduled for 1 to 2 hours per week and will require a formatted laboratory notebook. The skills and
content offered in this course along with those in the laboratory and review components have been chosen to adequately
prepare students for the AP Chemistry Examination and future success in college science courses.
Course Goals:
1. Students are prepared to be critical and independent thinkers who are able to function effectively in a scientific
and technological society.
2. Students will be able to analyze scientific and societal issues using scientific problem solving based on a
fundamental knowledge of chemistry.
3. Students will emerge from this program with an appreciation of the role that chemistry plays in understanding the
natural world.
4. Students will be able to make an acceptable score on the AP Chemistry Examination in May.
5. In each laboratory experiment, students will physically manipulate equipment and materials in order to make
relevant observations and collect data; use the collected data to form conclusions and verify hypotheses; and
communicate and compare results and procedures (informally to other experimenters, and formally in a written
report).
Text: Brown, Lemay and Bursten, Chemistry: The Central Science, 10th edition
Instructional Resources:
http://www.bozemanscience.com/ap-chemistry/
http://www.worldofteaching.com/chemistrypowerpoints.html
http://www.chalkbored.com/lessons/chemistry-11.htm
http://www.sciencegeek.net/Chemistry/Powerpoints2.shtml
http://adriandingleschemistrypages.com/aplabsummary.pdf
http://www.vernier.com/products/books/chem-a/
Concept Outline
Big Idea 1: The chemical elements are fundamental building material of matter, and all matter can be
understood in terms of arrangements of atoms. These atoms retain their identity in chemical reactions.
… or Atomic Structure
Big Idea 2: Chemical and physical properties of materials can be explained by the structure and the
arrangement of atoms, ions, or molecules and the forces between them.
… or Structure—Property Relations
Big Idea 3: Changes in matter involve the rearrangement and /or reorganization of atoms and /or the transfer of
electrons.
… or Chemical Transformations
Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions.
… or Kinetics
Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the
direction of changes in matter.
… or Thermodynamics
Big Idea 6: Any bond or intermolecular attraction that can be formed can be broken. These two processes are
in a dynamic competition, sensitive to initial conditions and external perturbations.
… or Equilibrium
Teaching Strategies
1. Collaboration. High esprit de corps, similar to that which develops among members of a research team, will
be nurtured by encourage students to work together in order to learn.
2. Limit lectures to allow plenty of time for other learning activities. Formal presentations of conceptual
information will be limited to covering the high points of the theory, deriving any important equations, and
presenting demonstrations that are relevant to the topic. Differential instructional activities and laboratory
experiments will be used to further the student’s comprehension of the chemical concepts.
4. Quizzes and tests. Assessment of the student’s progress will be monitored continuously by one or two
questions quizzes, pre-test, and unit exams.
Fall Semester
Unit 1: Calculations and Uncertainty
1. Metric System
2. Dimensional Analysis
3. Significant Figures
4. Scientific Notation
Laboratory: Volume, Mass, and Density
Unit 2: Atoms, Molecules, and Ions
1. Atoms and the Atomic Theory
2. Components of the Atom
3. Introduction to the Periodic Table
4. Molecules and Ions
5. Formulas of Ionic Compounds
6. Names of Compounds
Laboratory: Safety video, Determination of the Formula of a Compound; Classifying Elements
Unit 3: Stoichiometry
1. Atomic Masses
2. The Mole
3. Mass Relations in Chemical Formulas
4. Mass Relations in Reactions
Laboratory: Determination of the Percentage of Water in a Hydrate; Mass and Mole Relationship in a
Chemical Reaction; Percent of Copper in Copper (II) Sulfate Pentahydrate
Unit 4: Reactions in Aqueous Solution/Unit 18: Electrochemistry
1. Solute Concentrations; Molarity
2. Precipitation Reactions
3. Acid-Base Reactions
4. Oxidation-Reduction Reactions
5. Voltaic Cells
6. Standard Voltages
Laboratory: pH, Buffers, and their Properties; Chemical Reactions and Electricity: Cabbage pH Chemistry
Unit 5: Gases
1. Measurements on Gases
2. The Ideal Gas Law
3. Gas Law Calculations
4. Stoichiometry of Gaseous Reactions
5. Gas Mixtures: Partial Pressures and Mole Fractions
6. Kinetic Theory of Gases
7. Real Gases
Laboratory: Determination of Molar Mass by Vapor Density; Determination of the Mass of a Piece of
Magnesium
Unit 6: Electronic Structure and the Periodic Table
1. Light, Photon Energies, and Atomic Spectra
2. The Hydrogen Atom
3. Quantum Numbers
4. Atomic Orbitals; Shapes and Sizes
5. Electron Configurations in Atoms
6. Orbital Diagrams of Atoms
7. Electron Arrangements in Monatomic Ions
8. Periodic Trends in the Properties of Atoms
Laboratory: Periodic Table (online activity); Trends in the Periodic Table
Unit 7: Covalent Bonding
1. Lewis Structures; The Octet Rule
2. Molecular Geometry
3. Polarity of Molecules
4. Atomic Orbitals; Hybridization
Laboratory: Bonds, Molecular Structure and Shapes
Review for 1st Semester Final (Dec. 9--13)
1st Semester Final (week of Dec.16)
Spring Semester
Unit 8: Thermochemistry/Unit 17 Spontaneity of Reaction
1. Principles of Heat Flow
2. Measurements of Heat Flow; Calorimitry
3. Enthalpy
4. Thermochemical Equations
5. Enthalpies of Formation
6. Bond Enthalpy
7. The First Law of Thermodynamics
8. Spontaneous Processes
9. Entropy
10. Free Energy
11. Standard Free Energy Change, ∆Go
Laboratory: Specific Heat and Calorimetry
Unit 9: Liquids and Solids
1. Liquid-Vapor Equilibrium
2. Phase Diagrams
3. Molecular Substances; Intermolecular Forces
4. Network Covalent, Ionic, and Metallic Solids
5. Crystal Structure
Laboratory: Intermolecular Forces and Viscosity; Paper Chromatography
Unit 10: Solutions
1. Concentration Units
2. Principles of Solubility
3. Colligative Properties of Nonelectrolytes
4. Colligative Properties of Electrolytes
Laboratory: Colligative Properties of Water; Replacement Reactions; Polymers
Unit 11: Rate of Reaction
1. Meaning of Reaction Rate
2. Reaction Rate and Concentration
3. Reactant Concentration and Time
4. Models for Reaction Rate
5. Reaction Rate and Temperature
6. Catalysis
7. Reaction Mechanisms
Laboratory: Rates of Reactions
Unit 12: Gaseous Chemical Equilibrium
1. The N2O4-NO2 Equilibrium System
2. The Equilibrium Constant Expression
3. Determination of K
4. Applications of the Equilibrium Constant
5. Effect of Changes in Conditions of an Equilibrium System
Laboratory: Carbon Dioxide generated from Yeast
Review for AP Exam (April 21—May 2)
**AP Exam (Monday, May 5)**