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AP Chemistry Syllabus
Office Hours: 2:30 pm until 3:10 pm.
I can occasionally be reached from 7:35 am – 8:00 am
AP Chemistry
AP Chemistry is a course designed to provide you with a good background in a first year college chemistry course. There will be many times where outside work will be required. You will need to make arrangements around any extracurricular activities, work, employment, etc. as needed. Homework and laboratory assignments will be provided in the first week of class. It is your responsibility to come prepared each day for class. Lectures will be given three days per week for approximately 1 ½ hours. Two days per week will be spent conducting laboratories. Classes are on block scheduling for a total of 90 minute classes. Tutoring is available with scheduling.
Class will be comprised of lecture, lab procedures, occasional practice problems (to reinforce presented material), group discussion and minimal review. Tests may be given after each unit has been covered. Quizzes will be given and will be both announced and unannounced. Lab notebooks and homework will be graded on effort and accuracy.
Students who enter this class should have a good understanding of the following topics:
· Proficient use of the Metric System
· IUPAC Nomenclature
· Names, Charges, and Formulas for Polyatomic Ions
· Gas laws ( KMT, Boyle’s, Charles’, Avogadro’s Laws)
· Stoichiometry and Molar Relationships
· Electronic Structure (i.e. configurations, Lewis structures, electronegativity, VSEPR)
· Nuclear Chemistry
· Solution Chemistry (i.e. pH, pOH, molarity, dilutions and titrations, colligative properties, Intermolecular and Intramolecular bonding)
· Good laboratory techniques and proper lab notebook format
If you feel you do not have a good understanding of any of these topics please make arrangements to meet with me privately.
Prerequisites
Chemistry I and II are required with no less than a “C” average in both classes. Your lab performances from these classes will also be evaluated for consideration of this course.
Interactive Math I and II are prerequisites with no less than a “C” average in either class. Interactive III is preferred, but arrangements may be made accordingly.
Required Texts
Chemistry the Central Science, Brown, Lemay, Bursten, Murphy, 11th edition, Prentice Hall, 2009. ISBN 0-13-601879-3
Chemistry Matter and Change, Buthelezi, Dingrando, Hainen, Wistrom, Zike, McGrawHill, 2008. ISBN 978-0-07-874637-6
Additional texts may be utilized in the school library.
Course Goals
· Provide students with the knowledge required to function in a scientific setting in order to complete laboratories, participate in group settings and work efficiently with others.
· Each student will be able to write a college-level laboratory report that includes but is not limited to the procedure outline, basis for results, chart, graphs, calculations as necessary, and conclusions.
· Students will produce and maintain a professional laboratory notebook and record pertinent data in an organized manner.
· Students will be able to function in a college setting where an instructor’s input is minimal.
· Students will learn to utilize resources such as the Handbook of Chemistry, other chemistry texts and procedure manuals.
· Each student will complete the AP Chemistry Exam in May and be able to make an acceptable score.
Laboratory Procedures
Proper laboratory safety and procedures will be discussed at the beginning of the class. If a student is unable to follow these guidelines, the following will result:
1st offense – Depending on severity – a warning,
2nd offense – Student will be dismissed from the lab and receive a grade of zero.
Labs will be conducted approximately two days a week. You are allotted one absence from laboratory experiments without penalty. The next absence will need to be made up before school on a date predetermined by the instructor.
Laboratory notebooks will be graded once per term. Lab notebooks will be reduced by 50% if they are late.
Laboratory exercises will require you to work in a group setting. You will not only employ your lab partner, but the group as a whole. It will require you to collect any pertinent data, utilize that data as necessary, research any additional material needed, and formally report your conclusions. All laboratory experiments are hands on. This process will not be one that is completed in only one day or hour. It may take multiple attempts, days and collaborations with other lab groups. Laboratory procedures may also require additional information from references other than your book. You will need to be familiar with the Handbook of Chemistry. If you have forgotten the skills needed to use this book please see me for assistance before the day of lab.
There will be a laboratory examination at the end of the course. Students will need to be able to apply concepts, mathematical data and relationships, and general chemical and laboratory knowledge in order to succeed on this exam.
IT IS YOUR RESPONSIBILITY TO COME TO LAB DRESSED APPROPRIATELY! DO NOT ASK TO BORROW, CHANGE, OR CALL HOME FOR CLOTHES!
INAPPROPRIATE DRESS WILL RESULT IN A ZERO!
Grading Scale and Policy
Students will be graded based on the school’s present system. This scale can be found in the School Policy/Procedures Handbook.
The following content will be evaluated. These percentages are subject to change depending upon the material covered. Other content may be added and evaluated by the instructor.
30% Tests
20% Homework (effort and accuracy)
20% Lab Notebook (neatness, effort, and calculations/results)
15% Laboratory Procedures
15% Quizzes
Grading Scale and Policy cont’d
Students that score below 70% on tests will need to complete test corrections. Simply changing the answer will not be sufficient. The student must explain in a professional manner how they reached the corrected answer. You will need to analyze what you did wrong and how you resolved the problem. These corrections will be due three days after receiving the test back from the instructor. Test corrections are MANDATORY, no exceptions.
Homework is due at the end of each section. We will discuss any problems you had with the homework before the Unit Test. The problems will be provided the first week of class with the laboratory experiment outline. If you are aware you will be absent the day homework is due make sure to turn it in early. Late homework will be reduced by 50%.
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Curriculum Map Coordinated with Understanding By DesignCourse: AP Chemistry
# of Weeks / Unit/Major Topic / Subtopic(s) / AP Standards / Laboratory Experiments
2 / Introduction and Review / Laboratory Safety
Metric Conversions
Atomic Structure and Models
Nomenclature
Stoichiometry ( Percent Composition, Limiting Reactants, Empirical/Molecular Formulas)
Net Ionic Equations
General Solution Chemistry / I. A. Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by chemical and physical means
3. Atomic number and mass number; isotopes
II. States of Matter
C. Solutions
2. Methods of expressing concentration (use of normalities is not tested)
B. Stoichiometry
1. Ionic and molecular species present in chemical systems: net ionic equations
3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants / Using Metric Equipment for Measurements
Synthesis of Alum
1 / Gases / Boyle's, Charles' and Avogadro's Law
Ideal Gas Law
Partial Pressures, Combined Gas Law Kinetic Molecular Theory
Van der Waals Equation / II. States of Matter
A. Gases
1. Laws of ideal gases
a. Equation of state for an ideal gas
b. Partial pressures
2. Kinetic molecular theory
a. Interpretation of ideal gas laws on the basis of this theory
b. Avogadro’s hypothesis and the mole concept
c. Dependence of kinetic energy of molecules on temperature
d. Deviations from ideal gas laws / Grahams Law
# of Weeks / Unit/Major Topic / Subtopic(s) / AP Standards / Laboratory Experiments
1 / Reactions in Aqueous Solutions -- Oxidation and Reduction / Oxidation States
Balancing Oxidation-Reduction Equations / I. Structure of Matter
A. Atomic theory and atomic structure
5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
III. Reactions
A. Reaction types
2. Precipitation reactions
3. Oxidation-reduction reactions
a. Oxidation number
b. The role of the electron in oxidation-reduction
B. Stoichiometry
2. Balancing of equations including those for redox reactions / Determining Iron by Redox Titration
2 / Thermochemistry / State Functions
Enthalpy
Hess's Law
Heat of Formation and Reaction
Constant Pressure Calorimetry
Alternative Fuel Sources
Coal and Our Region
Entropy and Free Energy
Calculating Free Energy
through Enthalpy and Entropy / III. Reactions
E. Thermodynamics
1. State functions
2. First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law; heats of vaporization and fusion; calorimetry
3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes / Calorimetry Constants and
Determining Specific Heat through Calorimetry
Heats of Metal/Acid Reactions
Enthalpy of Sodium Hydroxide
and Hydrochloric Acid
# of Weeks / Unit/Major Topic / Subtopic(s) / AP Standards / Laboratory Experiments
2 / Bonding / Quantum Mechanical Model (VSEPR)
Trends in the Periodic Table (electronegativity, ionization, atomic radii)
Lewis Structures & Electron Configuration Review
Hybridization of Orbitals (Atomic & Molecular) / I. Structure of Matter
A. Atomic theory and atomic structure
4. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
c. Polarity of bonds, electronegativities
2. Molecular models
a. Lewis structures
b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
c. VSEPR
3. Geometry of molecules and ions, dipole moments of molecules
II. States of Matter
B. Liquids and solids
4. Structure of solids; lattice energies / Molecular Structure and Models
1 / Liquids and Solids / Dipole Moments
Van der Waals Forces
Phase Change Diagrams
Solubility Conditions
Ideal Solutions
(Raoult's Law)
Colligative Properties
Osmosis / I. Structure of Matter
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
b. Relationships to states, structure, and properties of matter
II. States of Matter
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular viewpoint
2. Phase diagrams of one-component systems
3. Changes of state, including critical points and triple points
C. Solutions
3. Raoult’s law and colligative properties (nonvolatile solutes); osmosis
4. Nonideal behavior (qualitative aspects) / Molecular Mass by Freezing Point Determination
# of Weeks / Unit/Major Topic / Subtopic(s) / AP Standards / Laboratory Experiments
1 / Kinetics / Reaction Rates and Laws
Mechanisms
Homogeneous and Heterogeneous Catalysts / III. Reactions
D. Kinetics
1. Concept of rate of reaction
2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws
3. Effect of temperature change on rates
4. Energy of activation; the role of catalysts
5. The relationship between the rate-determining step and a mechanism / Clock Reaction
1 / Equilibrium / Equilibrium Constants
Calculating Equilibrium Positions and Solving Problems / II. States of Matter
C. Solutions
1. Types of solutions and factors affecting solubility
III. Reactions
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle; equilibrium constants / Determination of Equilibrium Constant for the Formation of FeSCN
1 / Electrochemistry / Brief Review of Oxidation Reduction
Galvanic Cells
Reduction Potentials
Nernst Equation and Faraday's Laws
Batteries / III. Reactions
3. Oxidation-reduction reactions
c. Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
E. Thermodynamics
4. Relationship of change in free energy to equilibrium constants and electrode potentials / Electrode Potential Lab
1 / Representative and
Transition Metals / Group Presentation Project
Coordination Compounds
Naming and Bonding in Coordination Compounds / I. Structure of Matter
B. Chemical bonding
1. Binding forces
b. Relationships to states, structure, and properties of matter
3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes;; relation
of properties to structure / Qualitative Analysis of Cations and Anions
Qualitative Determinations
# of Weeks / Unit/Major Topic / Subtopic(s) / AP Standards / Laboratory Experiments
1 / Organic Chemistry / Review Nomenclature of Hydrocarbons and Functional Groups
Isomers
Enantiomers
Addition Reactions / I. Structure of Matter
B. Chemical bonding
3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; relation of properties to structure / Synthesis of Esters
1 / Test Review / Review Test Format
Practice Test Questions for Essay Questions / Optional Weekend Review
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