2015-16
Frederick Douglass High School
225 Hamilton Holmes Drive
Atlanta, Georgia 30318
Instructor: Miss K. Dixon
Tutorials: Thursday 3:45-5PM
Email: kdixon@atlanta.k12.ga.us
Phone: (404) 802-3100
Conferences: Thursday 4-5PM
Room Location: 336
Course Description: The AP Chemistry course is designed, according to College Board, to be equivalent of the
general chemistry course usually taken during the first college year. AP Chemistry should meet the objectives
of a good college general chemistry course. Students in each course should attain depth of the understanding of
fundamentals and a reasonable competence in dealing with chemical problems. The course should contribute to
the development of the students’ abilities to think clearly and to express their ideas, verbally and in writing,
with clarity and logic. The college course in general chemistry differs qualitatively from the usual first
secondary school course in chemistry with respect to the kind of textbook used, the topics covered, the
emphasis on chemical calculations and the mathematical formulation of principles, and the kind of laboratory
work done by students. Quantitative differences appear, in the number of topics treated, the time spent of the
course by the students, and the nature and the variety of experiments done in the laboratory.
Course Prerequisites: The AP Chemistry course is designed to be taken only after the successful completion
of a first year course in high school chemistry. In addition, the recommended mathematical prerequisite for an
AP Chemistry class is successful completion of a second-year algebra course.
Textbook: Chemistry: The Central Science 11th edition (Brown, LeMay, Bursten, and Murphy)
Course Goals and Objectives:
1.
2.
3.
4.
To help students develop a conceptual framework for chemistry.
To help students gain an appreciation of science as a process.
To help students develop skills that will enable them to be life long learners.
To help students develop the ability to demonstrate their knowledge and critical thinking skills about
chemistry in written form.
5. To prepare students for the comprehensive AP Chemistry Examination to be given in the Spring.
6. To improve the student’s ability to work, communicate, and learn effectively with others.
7. For the student to recognize that there are common repetitive themes and patterns among the major
topics and themes in chemistry.
Class Structure: The school operates on a four by four schedule with classes meeting every day for 90
minutes. AP Chemistry classes meet for the same amount of time as other classes. Students must be highly
motivated and possess good study habits to do well in the course. Sustaining a solid laboratory program is the
Transforming, Teaching, and Learning to Improve Student Achievement
most difficult aspect of this course. The class meeting does not allow much time over the course of the year to
complete all of the necessary topics and labs, but the labs do reflect major concepts and include a variety of lab
techniques for students to learn. Students, therefore, need to be prepared to conduct labs both in class (90
minutes), after school (2 hours), and on occasional Saturdays (2-3 hours).
The AP Chemistry class will be taught using a varying combination of techniques with the majority of the
material being presented through lecture and laboratory experiences. Instruction will be disseminated using one
of the following formats to include instructional strategies such as high level questioning,
mentorship/apprenticeship, tiered assignments, independent projects, compacting and learning centers, direct
instruction, class discussions and/or Powerpoint presentations, supplemental handouts, videos, technology,
research, special projects, individual and group activities, and weekly/bi-weekly assessments. There will be
opportunities for which guest speakers will be invited to present current research and laboratory techniques
within their fields as it relates to concepts students are expected to master. In addition, field trips will be used as
a means of extended learning and field investigations.
Below please find a tentative schedule for which concepts and calculations will be covered introduced and
covered in depth. The time frame is subsequent to change in regards to unforeseen circumstances (i.e. weather,
assemblies, etc.), however all topics will be covered. Assignments, activities, and laboratory investigations will
be given during the unit lesson in an effort to reinforce and review content.
Topic Outline (according to College Board)
The following is an outline of the topics to be covered in AP Chemistry and the correlating percentage of
multiple choice questions on the annual spring exam (May 4, 2015):
I.
Structure of Matter (20%)
a. Atomic Theory and atomic structure
i. Evidence for the atomic theory
ii. Atomic masses; determination by chemical and physical means
iii. Atomic number and mass number; isotopes
iv. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
v. Periodic relationships including, for example, atomic radii, ionization energies, electron
affinities, oxidation states
b. Chemical bonding
i. Binding forces
1. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including
London dispersion forces)
2. Relationships to states, structure, and properties of matter
3. Polarity of bonds, electronegativities
ii. Molecular models
1. Lewis structures
2. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
3. VSEPR
iii. Geometry of molecules and ions, structural isomerism of simple organic molecules and
coordination complexes; dipole moments of molecules; relation of properties to structure
c. Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical applications
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II.
States of Matter (20%)
a. Gases
i. Laws of Ideal Gases
1. Equation of state for an ideal gas
2. Partial pressures
ii. Kinetic molecular theory
1. Interpretation of ideal gas laws on the basis of this theory
2. Avogadro’s hypothesis and the mole concept
3. Dependence of kinetic energy of molecules on temperature
4. Deviations from ideal gas laws
b. Liquids and solids
i. Liquids and solids from the kinetic-molecular viewpoint
ii. Phase diagrams of one-component systems
iii. Changes of state, including critical points and triple points
iv. Structure of solids; lattice energies
c. Solutions
i. Types of solutions and factors affecting solubility
ii. Methods of expressing concentration (use of normalities is not tested)
iii. Raoult’s law and colligative properties (nonvolatile solutes); osmosis
iv. Nonideal behavior (qualitative aspects)
III.
Reactions (35-40%)
a. Reaction Types
i. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination
complexes; amphoterism
ii. Precipitation reactions
iii. Oxidation-reduction reactions
1. Oxidation number
2. The role of the electron in oxidation-reduction
3. Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard halfcell potentials; Nernst equation; prediction of the direction of redox reactions
b. Stoichiometry
i. Ionic and molecular species present in chemical systems: net ionic equations
ii. Balancing of equations, including those for redox reactions
iii. Mass and volume relations with emphasis on the mole concept, including empirical
formulas and limiting reactants
c. Equilibrium
i. Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle;
equilibrium constants
ii. Quantitative treatment
1. Equilibrium constants for gaseous reactions: Kp, Kc
2. Equilibrium constants for reactions in solution
a. Constants for acids and bases: pK, pH
b. Solubility product constants and their application to precipitation and the
dissolution of slightly soluble compounds
c. Common ion effect; buffers; hydrolysis
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d. Kinetics
i. Concept of rate of reaction
ii. Use of experimental data and graphical analysis to determine reactant order, rate
constants, and reaction rate laws
iii. Effect of temperature changes on rates
iv. Energy of activation; the role of catalysts
v. The relationship between the rate-determining step and a mechanism
e. Thermodynamics
i. State functions
ii. First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law; heats of
vaporization and fusion; calorimetry
iii. Second law: entropy; free energy of formation; free energy of reaction; dependence of
change in free energy on enthalpy and entropy changes
iv. Relationship of change in free energy to equilibrium constants and electrode potentials
IV.
Descriptive Chemistry (10-15%)
Knowledge of specific facts of chemistry is essential for an understanding of principles and concepts. There,
descriptive facts, including the chemistry involved in environmental and societal issues, should not be
isolated from the principles being studied but should be taught throughout the course to illustrate and
illuminate the principles. The following areas will be covered:
1. Chemical reactivity and products of chemical reactions
2. Relationships in the periodic table: horizontal, vertical, and diagonal with
examples from alkali and alkaline-earth metals, halogens, and the first series of
transition metals.
3. Introduction to organic chemistry: hydrocarbons and functional groups (structure,
nomenclature, chemical properties)
V.
Laboratory (5-10%)
The differences between college chemistry and the usual secondary school chemistry course are especially
evident in the laboratory work. The AP Chemistry Exam includes some questions based on experiences and
skills students acquire in the laboratory:
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Making observations of chemical reactions and substances
Record data
Calculating and interpreting results based on the quantitative data obtained
Communicating effectively the results of experimental work
Instructional Schedule:
August 2015
Chapters 1-2 Introduction, Matter and Atoms (Lab: Density; Separation by Chromatography)
Chapter 3
Stoichiometry (Nomenclature and Balancing Equations)
(Lab: Hydrates; Cu to Cu)
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September 2015
Chapter 4
Chapter 6
Aqueous Reactions and Solution Stoichiometry
(Labs: Preparation of Sodium Bicarbonate and Sodium Carbonate;
Reactions in Aqueous Solutions: Metathesis Reactions and NIEs)
Electronic Structure of Atoms (Independent Study)
October 2015
Chapter 7
Chapter 5
Chapter 10
Periodic Properties of Elements (Independent Study)
Thermochemistry
(Lab: Hess’ Law)
Gas Laws
(Labs: Behavior of Gases: Molar Mass of a Vapor; Determination of R)
November 2015
Group Presentations (Dates: TBD)
Chapter 8
Basic Concepts of Chemical Bonding (Group Presentations)
Chapter 9
Molecular Geometry and Bonding Theories (Group Presentations)
Chapter 11
Intermolecular Forces, Liquids, and Solids (Group Presentations)
December 2015
Chapter 13
Chapter 14
Properties of Solutions
Kinetics
(Labs: Rates of Chemical Reactions I and II)
January 2016
Chapter 15
Chapter 16
February 2016
Chapter 17
Chapter 19
Equilibrium
(Labs: LeChâtelier’s Principle;
Acid-Base Equilibria
Additional Aspects of Aqueous Equilibria
(Labs: Hydrolysis of Salts and pH of Buffer Solutions;
Chemical Thermodynamics
March 2016
Chapter 20
Electrochemistry
(Labs: Electrochemical Chemistry and Thermodynamics)
April 2016
**Review for AP Exam**
Complete Practice AP Exam
May 2, 2016
AP Chemistry Exam
**SCHEDULE IS SUBJECT TO CHANGE AS NEEDED TO BEST BENEFIT INSTRUCTION**
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Computation of Grades:
Daily Grades/Quizzes/Homework……..……....25%
Research Articles/Projects/Lab Reports……….20%
Tests………………………………………….…35%
Mid-Term/Final………………………………...20%
GRADING SCALE
A = 90-100
B = 80-89
C = 70-79
F = 69 and below
Lab Report Write-Up:
**Students will be using Thread Bound Composition Lab Notebooks**
Students will be responsible for completing the all components of the lab on the pages provided in the Thread
Bound Composition Lab Notebook. The lab write-up will comprised using the following format:
I.
II.
III.
IV.
V.
VI.
VII.
Title of Laboratory Experiment
Introduction and Purpose of Laboratory Experiment
Materials
Procedure (steps/methods used should be extremely detailed as to possible replication without
any assistance being needed)
Analysis/Results (all mathematical and graphical components should be included in this section)
Conclusion
Discussion (students will discuss errors made while completing lab; any changes that may need
to be made; possible extension of lab, etc.)
Materials Required Daily:
1.
2.
3.
4.
5.
6.
7.
8.
Textbook (Chemistry: The Central Science 11th Edition)
Three ring binder
Pencils (#2)
Black/Blue Pens
Scientific Calculators
Notebook Paper
Graphing Paper
Supplemental study material for assistance with comprehension of topics/units
taught in course. Title to be given to students by instructor. Study guide can
usually be found at Barnes and Noble bookstores or ordered online at
Amazon.com.
9. A jump drive/thumb drive for saving respective assignments.
Attendance:
It is truly imperative that all students attend class daily. Please refer to the student handbook addressing student
absences and grading policy. It is expected that all students will complete assignments given by instructor and
submit them according to the given due date. LATE ASSIGNMENTS MAY BE ACCEPTED ONLY AT
THAT SOLE DISCRETION OF THE TEACHER!! If accepted late assignments submitted will be penalized 10
points per day.
Make-up assignments will only be administered no later than five (5) calendar days from when the assignment
was missed provided proper documentation (illness, family emergency, school related activities, etc.) is
submitted. THERE WILL NOT BE MAKE-UP LABS DUE TO THE NATURE OF THE LABORATORY
EXPERIENCES. You will however be given an alternative lab to complete—virtual labs or small scale hands
on activities.
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