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A.P. Chemistry (12) (ELCA)

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Syllabus: AP Chemistry Coach King

COURSE OBJECTIVEEdit

AP Chemistry is designed to be the equivalent of a first year college general chemistry course and follows the College Board’s AP Chemistry syllabus. As such, the course is suitable only for high school students who exhibit high levels of commitment, motivation and academic maturity. This course presents a rigorous treatment of the following concepts: the nature of matter, gas laws, thermodynamics, stoichiometry, bonding, chemical kinetics, chemical equilibria, and more. Students are expected to be motivated and spend extra time studying outside of class. The problem-solving strategies obtained during this course will prepare college-bound students for careers in the sciences, medicine, engineering, and other technical areas.

INSTRUCTIONALEdit

Text: Zumdahl/Zumdahl, Chemistry, 7/e, Houghton Mifflin Co., (2007).
ISBN: 0-618-71370-0

MATERIALSEdit

  • Scientific calculator, preferably a TI-83 or 84 series,
  • Notebook for saving tests, quizzes, labs, notes, etc.
  • Three-ring binder
  • Writing utensils: pen or pencil acceptable for most work, pencil preferred
  • Lab notebook (www.labnotebooks.net)


Although not an absolute requirement, it is strongly recommended that students invest in one of the AP Chemistry course preparation books currently on the market. There are several available and each student should peruse the titles and select one based upon personal preference. It is not a good idea to wait until two weeks before the examination to purchase the book, buy it at the beginning of the course and use it regularly throughout the year. Five examples of such books are:

  • Cracking the AP Chemistry Exam, 2008 Edition by Princeton Review Publisher: Princeton Review
  • Barron's AP Chemistry 2008 (Barron's How to Prepare for the AP Chemistry Advanced Placement Examination) by Neil D. Jespersen Publisher: Barron’s Educational Series
  • 5 Steps to a 5 AP Chemistry, 2008-2009 Edition (5 Steps to a 5 on the Advanced Placement Examinations) by John Moore and Richard Langley Publisher: McGraw-Hill


EXPECTATIONSEdit

Homework may be assigned for one or more of the following purposes:

  • Practice -- to help students to master specific skills which have been presented in class;
  • Preparation -- to help students gain the maximum benefits from future lessons;
  • Extension -- to provide students with opportunities to transfer specific skills or concepts to new situations; *Creativity -- to require students to integrate many skills and concepts in order to produce original responses



It is assumed that students will spend at least five hours a week in unsupervised individual study.



Assignments are due at the beginning of your class period.

NO LATE WORK WILL BE ACCEPTED OR GRADED.


GRADINGEdit

Point System (earned points / total points = final grade)
Each class activity will be assigned the following point value:

  • Homework = 10 points
  • Quiz = 25 points
  • Lab Notebook = 50 points per lab
  • Test = 100 points
  • Exam = 200 points

TEST CORRECTIONSEdit

Students may correct questions missed on any test for an additional _ point of credit per question corrected. To receive the additional credit the following information must be presented.

  1. Explanation of the rationale used to arrive at the initial, incorrect response on the test.
  2. Correct answer for the question missed.
  3. Where the information to obtain the correct answer was found.
    1. Any student receiving a test grade below a 74% MUST do test corrections


HELP CLASSEdit

If more extensive help is needed I will schedule review sessions in the evening from 5:00 p.m. – 8:00 p.m.


COURSE OVERVIEWEdit

  • Chapter 1: Chemical Foundations
  • Chapter 2: Atoms, Molecules and Ions
  • Chapter 3: Stoichiometry
  • Chapter 4: Types of Chemical Reactions and Solution Stoichiometry
  • Chapter 5: Gases
  • Chapter 6: Thermochemistry
  • Chapter 7: Atomic Structure and Periodicity
  • Chapter 8: Bonding: General Concepts
  • Chapter 9: Covalent bonding: Orbitals
  • Chapter 10: Liquids and Solids
  • Chapter 11: Properties of Solutions
  • Chapter 12: Chemical Kinetics
  • Chapter 13: Chemical Equilibrium
  • Chapter 14: Acids and Bases
  • Chapter 15: Applications of Aqueous Equilibria
  • Chapter 16: Spontaneity, Entropy and Free Energy
  • Chapter 17: Electrochemistry
  • Chapter 18: The Nucleus
  • Chapter 21: Transition Metals and Coordination Chemistry
  • Chapter 22: Organic and Biological molecules

LABEdit

This course includes a laboratory component comparable to college-level chemistry laboratories. To ensure you are adequately prepared for the AP Exam all labs have been designed by Flinn Scientific, Inc. to meet specific AP requirements. All labs will be hands-on experiences. A minimum of one double-period per week or its equivalent is spent engaged in laboratory work. Labs are scheduled for Wednesday afternoons, any changes to the lab schedule will be announced; labs will start at 1:15 p.m. and continue through 7th period (3:00 p.m.). Each student will be given a lab notebook, and all labs are to be written formally. All students will work within a group of 2 or 3 students. Students work in groups to share lab equipment, but each student is responsible for their individual lab reports
ABSOLUTELY NO FOOD OR DRINK IS ALLOWED IN THE LAB

COURSE OUTLINEEdit

The Advanced Placement Chemistry Topic Outline for 2008 The following list describes the topic outline provided by the College Board. The outline is designed to be a guide to the extent and depth of an AP Chemistry course and is not to be viewed as the absolute syllabus. This syllabus is published at the start of the course and should be viewed as provisional and as such is subject to alteration from time to time. This outline describes the five major areas listed below plus a list of types of chemical calculations one might encounter in an AP Chemistry course.

  • Structure of Matter 20%
  • States of Matter 20%
  • Reaction Types 35-40%
  • Descriptive Chemistry 10-15%
  • Laboratory Work 5-10%



For more information about the AP Test go to the following web page: [1]

Course SequenceEdit

SUMMER WORKEdit

Chapter 1 - Chemical FoundationsEdit

  • Scientific Method
  • Units of Measurement
  • Significant Figures
  • Dimensional Analysis
  • Density
  • Classification of Matter

Chapter 2 – Atoms, Molecules and IonsEdit

  • Fundamental Chemical Laws
  • Dalton’s Theory
  • Modern View of Atomic Structure
  • Molecules and Ions
  • Periodic Table
  • Naming Simple Compounds

FIRST SEMESTEREdit

Chapter 3 – Stoichiometry (2 Weeks)Edit

  • The Mole and Molar Mass
  • Percent Composition
  • Determining Formulas
  • Chemical Equations
  • Stoichiometric Calculations
  • Limiting Reactants
  • LAB – Determination of the Empirical Formula of Silver Oxide
  • LAB – Determination of the Molar Mass of Gases and Volatile Liquids

Chapter 4 – Types of Reactions and Solution Stoichiometry (3 Weeks)Edit

  • Electrolytes
  • Solutions
  • Types of Chemical Reactions
  • Precipitation Reactions
  • Acid-Base Reactions
  • Oxidation – Reduction Reactions
  • LAB – Analysis of Aluminum potassium Sulfate
  • LAB – Molar Mass by Freezing point Depression
  • TEST – Chapters 1-4

Chapter 5 and Chapter 10 – Solids, Liquids and Gases (2 Weeks)Edit

  • Intermolecular Forces
  • Kinetic Molecular Theory
  • Pressure
  • Dalton’s Law of Partial Pressure
  • Gas Laws (Boyle’s Charles, Avogadro’s and Ideal)
  • Gas Stoichiometry
  • Real Gases
  • Vapor Pressure and Changes of State
  • Phase Diagrams
  • LAB – Determining The Molar Volume of a Gas
  • LAB – Oxidation – Reduction Titrations

Chapter 6 – Thermochemistry (2 Weeks)Edit

  • Nature of Energy
  • Enthalpy Changes
  • Calorimetry
  • Hess’s Law
  • LAB – Thermodynamics – Enthalpy of Reaction and Hess’s Law
  • MID-TERM EXAM – Chapters 1-6,10

Chapter 7 –Atomic Structure and Periodicity (2 Weeks)Edit

  • Nature of Matter
  • Bohr Model
  • Quantum Mechanical Model
  • Quantum Numbers
  • Orbital Shapes and Energies
  • Pauli’s Exclusion Principle
  • Aufbau principle
  • Periodic Trends
  • LAB – Gravimetric Analysis of a Metal Carbonate
  • LAB – An Activity Series

Chapter 8 and Chapter 9 – Chemical Bonding (3 Weeks)

  • Types of Bonds
  • Electronegativities
  • Bond Polarity and Dipoles
  • Partial Ionic Character of Covalent Bonds
  • Covalent Bond Energies
  • Lewis Structures
  • VSEPR Model
  • Exceptions to the Octet Rule
  • Resonance
  • Hybridization
  • LAB – Separation and Qualitative Determination of Cations and Anions
  • TEST – Chapters 7-9
  • PROJECT DUE

Chapter 11 – Properties of Solutions (2 Weeks)Edit

  • Energies of Solution Formation
  • Solubility
  • Vapor Pressure
  • Colligative Properties
    • Boiling-Point Elevation
    • Freezing-Point Depression
    • Osmotic Pressure
  • Colloids
  • LAB – Liquid Chromatography

Chapter 12 – Chemical Kinetics (2 Weeks)Edit

  • Reaction Rates
  • Rate Laws
  • Chemical Kinetics
  • Catalysis
  • LAB – Determining the Stoichiometry of Chemical Reactions
  • LAB – Kinetics of a Reaction
  • EXAM – Chapters 1-12

SECOND SEMESTEREdit

Chapter 13 – Chemical Equilibrium (2 Weeks)Edit

  • Equilibrium Conditions and Constants
  • Le Chatelier’s Principle
  • LAB – Determination of Ka of Weak Acids
  • LAB – The Determination of Keq for Iron (III) Thiocyanate

Chapter 14 – Acids and Bases (2 Weeks)Edit

  • Arrhenius Theory
  • The pH Scale
  • Lowry-Bronsted Theory
  • The Effect of Structure on Acid-Base Properties
  • Lewis Acids and Bases
  • LAB – Determination of Concentration by Acid-Base Titration
  • LAB – Selecting Indicators for Acid-Base Titrations
  • TEST – Chapters 13-14

Chapter 15 – Applications of Aqueous Equilibria (2 Weeks)Edit

  • Acid-Base Equilibria
  • Solubility Equilibria
  • Complex Ion Equilibria
  • LAB – Standardization of a Solution Using a Primary Standard
  • LAB – pH Properties of Buffer Solutions

Chapter 16 – Spontaneity, Entropy and Free Energy (1 Week)Edit

  • Effect of Temperature on Spontaneity
  • Entropy Changes and Free Energy in Chemical Reactions
  • Dependence of Free Energy on Pressure
  • Free Energy and Equilibrium
  • Free Energy and Work

Chapter 17 – Electrochemistry (1 Week)Edit

  • Galvanic Cells
  • Standard Reduction Potentials
  • Cell Potential, Electrical Work and Free Energy
  • Batteries
  • LAB – Electrochemical Cells
  • MID-TERM EXAM – Chapters 1-17

Chapter 18 – Nuclear Chemistry (2 Weeks)Edit

  • Nuclear Stability and Radioactive Decay
  • Nuclear Transformations
  • Detection and Uses of Radioactivity
  • Thermodynamic Stability of the Nucleus
  • Nuclear Fission and Fusion
  • Effects of radiation

Chapter 21 – Transition Metals and Coordination Chemistry (1 Week)Edit

  • Transition Elements
  • Coordination Compounds
  • Isomerism
  • LAB – Synthesis and Analysis of a Coordination Compound

Chapter 22 – Organic and Biological Molecules (2 Weeks)Edit

  • Alkanes, Alkenes and Alkynes
  • Aromatic Hydrocarbons
  • Polymers
  • LAB – Synthesis, Isolation, and Purification of an Ester
ELCA SENIOR CLASSES Main Page A.P. EnglishA.P. BiologyA.P. CalculusA.P. ChemistryA.P. GovernmentA.P. Spanish Honors EnglishHonors PhysicsHonors Spanish III Algebra IIIAnatomyEnglish 12Bible WorldviewsPolitical Science

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