Curriculum Map 2015-2016
AP CHEMISTRY
Pace
Essential Understandings
Big Idea
Chapters
Unit 1
Unit 2
Unit 3
Unit 4
Unit 5
Unit 6
5 weeks
5 weeks
5 weeks
6 weeks
6 weeks
6 weeks
Structure of matter
1a- elements are
made of atoms
1b- atomic structure
1c- periodicity
1d- experimental
data and atomic
models
1e- conservation of
matter
Properties and
bonding
2a- physical
properties
2b- intermolecular
forces
2c- bonding
2d- solids
Chemical Reactions
Reaction Rates
Thermodynamics
Equilibria
3a- balancing
equations
3b- reaction types
3c- evidence of
reactions
4a- reaction rate
factors
4b- collision theory
4c- reaction
mechanisms
4d- catalysts and
effects
5a- heat
5b-energy transfer
5c- bond energy
5d- breaking
intermolecular forces
5e- enthalpy/entropy
6a- equilibrium/
reversible reactions
6b- disturbing
equilibrium
6c- acids and bases
6d- Ka and Gibbs free
energy
6, 19
14, 16, 17, 18
__________________________
2, 7, 8
Revised JUNE 2011
3, 9, 10, 11, 12, 13
4, 5, 6, 20
Science Practices
1: The student can use
representations and
models to communicate
scientific phenomena and
solve scientific problems.
2: The student can use
mathematics
appropriately.
3: The student can
engage in scientific
questioning to extend
thinking or to guide
___________________________ ___________________________ investigations within the
context of the AP course.
___________________________
4: The student can plan
and implement data
collection strategies in
relation to particular
scientific questions.
5: The student can
perform data analysis and
evaluation of evidence.
6: The student can work
with scientific
explanations and
theories.
7: The student is able to
connect and relate
knowledge across various
scales, concepts, and
representations in and
across domains.
15
Chapters
Page 1 of 2
Unit
Pace
Learning objectives
Big Idea
Unit 1
Unit 2
Unit 3
Unit 4
Unit 5
Unit 6
5 weeks
5 weeks
5 weeks
6 weeks
6 weeks
6 weeks
Structure of matter Properties and
bonding
Chemical reactions Reaction rates
Thermodynamics
Equilibria
1.1 definite composition
1.2 empirical formulas
1.3 purity
1.4 qualitative and
quantitative analysis
1.5 electron
configuration
1.6 energy levels
1.7 Aufbau/ Hund’s
rule/ Pauli exclusion
principle
1.8 electron distribution
and Coulomb’s law
1.9 periodicity
1.10 group properties
1.11 binary compounds
and formulas
1.12 atomic theory
1.13 changes to atomic
theory
1.14 mass spectrometry
1.15 spectroscopy
1.16 light absorption
1.17 law of
conservation of mass
1.18 conservation of
mass in reactions
1.19 experimentally
determine solution
concentrion
3.1 evidence of chemical
change
3.2 balancing equations
3.3stoichiometry
3.4 limiting reagents
3.5 synthesis/
decomposition
reactions
3.6 law of definite
proportions/
conservation of matter
3.7 Bronsted-Lowry and
conjugate acid-base
pairs
3.8 redox reactions
3.9 redox titration
experiment
3.10 physical vs.
chemical change
3.11 reaction energy
3.12 half reactions
3.13 electrochemistry
5.1 potential energy
5.2 kinetic energy
5.3 energy transfer
5.4 conservation of
energy and reactions
5.5 energy changes
5.6 enthalpy
5.7 calorimetry
experiment
5.8 enthalpy of
formation
5.9 enthalpy and
intermolecular forces
5.10 changes and
molecular interactions
5.11 molecular shape
and effect on
interactions
5.12 entropy
5.13 spontaneous
reactions
5.14 Gibbs free energy
5.15 energy and
spontaneous reactions
5.16 Le Chatelier’s
principle
5.17 reaction
intermediates
5.18 product formation
6.1 reversible reactions
6.2 reaction quotient
and equilibrium
constants
6.3 rates of reactions
6.4 determine favored
reaction direction
6.5 calculate K
6.6 determine
equilibrium conditions
6.7 ICE tables
6.8 shift in reactions
6.9 manipulating
reactions
6.10 stress and effects
on Q and K
6.11 acid-base strength
and equilibrium
6.12 titrations
6.13 determining pK for
acids or bases from data
6.14 neutral solutions
6.15 pH
6.16 pH, strength and
concentration
6.17acid-base reactions
6.18 buffer solutions
6.19 pH and pKa
6.20 buffer reaction
mechanism
6.21 solubility of salts
6.22 Ksp values
6.23 factors effecting
salt solubility
6.24 salt dissolution
and energy changes
6.25 relationship
between K, ∆G, RT and
reaction favorability
Revised JUNE 2011
2.1 properties and bond
type
2.2 strong/weak
solutions
2.3 states of matter
2.4 KMT
2.5 gases
2.6 gas laws
2.7 chromatography
2.8 solute/solvent
interactions
2.9 concentration
2.10 separation
experiments
2.11 London dispersion
forces
2.12 real vs. ideal gases
2.13 intermolecular
forces
2.14 Coulomb’s law
2.15 solubility
2.16 molecular
compounds
2.17 bond type
2.18 polarity
2.19 ionic bonds and
properties
2.20 bond theories
2.21 Lewis models
2.22 bond properties
2.23 ionic solids
2.24 crystal structure
2.25 metallic bonds
2.26 electron sea model
2.27 metallic solids
2.28 metal properties
2.29covalent solids
2.30 covalent
properties
2.31 molecular solids
2.32molecular
properties
4.1 factors affecting
reaction rate
4.2 rate law and order
of reaction
4.3 half-life and rate
constant
4.4 elementary reaction
and rate law
4.5collision theory
4.6 temperature and
reaction rates
4.7 reaction
mechanisms
4.8 catalysts and
activation energy
4.9 catalysts and
reaction rates
Page 2 of 2
AP Chemistry Course Syllabus
Jeff Davison
(770) 651-6034
Jeffery.davison@douglas.k12.ga.us
AP Statement:
AP courses are designed to help better prepare students for college. These classes are at the collegiate level and are much more demanding than the standard
classroom experience. AP chemistry is fast-paced. Students may have to devote additional time and effort to AP work and, in turn, they will have greater
opportunities for learning. Regardless of AP performance, students taking an AP class are better prepared for the rigors of college. Note: students are
encouraged to take the AP Chemistry Test.
Course Description:
The following subjects will be addressed in-depth in AP Chemistry: structure of matter, properties and bonding, chemical reactions, reaction rates,
thermochemistry, and equilibrium. Laboratory work will be completed at the collegiate level with standard AP labs for each topic listed. Lab time will make up a
minimum of 25% of instructional time. All laboratory exercises are “wet” labs; virtual labs & simulations are not currently used in this course. The current
textbook is Chemistry & Chemical Reactivity, Sixth Edition by Kotz, Treichel, and Weaver (Copyright 2006). Laboratory resources include Flinn Scientific
(www.flinnsci.com). The following is a list of the big ideas that will be covered in this class, as developed by the College Board:
Big Idea 1: The chemical elements are fundamental building materials of matter, and all matter can be understood in terms of arrangements of atoms.
These atoms retain their identity in chemical reactions.
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.
Big Idea 3: Changes in matter involve the rearrangement and/or reorganization of atoms and/or the transfer of electrons.
Big Idea 4: Rates of chemical reactions are determined by details of the molecular collisions.
Big Idea 5: The laws of thermodynamics describe the essential role of energy and explain and predict the direction of changes in matter.
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.
Revised JUNE 2011
Page 3 of 2
Labs:
Labs are designed to provide students with the opportunity to design experiments, collect data, apply mathematical routines and methods, and refine testable
explanations and predictions. Laboratory time will make up a minimum of 25% of class time. Labs are designed to allow students to demonstrate the following
Science Practices (sp):
1: The student can use representations and models to communicate scientific phenomena and solve scientific problems.
2: The student can use mathematics appropriately.
3: The student can engage in scientific questioning to extend thinking or to guide investigations within the context of the AP course.
4: The student can plan and implement data collection strategies in relation to particular scientific questions.
5: The student can perform data analysis and evaluation of evidence.
6: The student can work with scientific explanations and theories.
7: The student is able to connect and relate knowledge across various scales, concepts, and representations in and across domains.
The labs planned for this course are listed below:
Big Ideas
1. Structure of matter
2. Properties and bonding
Lab (GI = guided inquiry)
1.
2.
3.
1.
2.
3.
4.
3. Chemical reactions
4. Reaction rates
5. Thermodynamics
6. Equilibrium
Revised JUNE 2011
1.
2.
3.
1.
2.
3.
4.
1.
2.
3.
1.
2.
3.
4.
Spectroscopy
Empirical formula
Percent water in a hydrate (GI);(sp2-6)
Determining molar mass by freezing
point
Molar volume of a gas
Molar mass by vapor density
Paper chromatography
(GI)(sp1,3,4,6,7)
Reactions in ionic species
Activity series
Air bag stoichiometry (GI) (sp1-5,7)
Kinetics of a reaction
Activation energy
Rate determining step
Rate of fading crystal violet (GI) (sp17)
Calorimetry (GI) (sp1-5, 7)
Enthalpy
Hess’s Law
Equilibrium constant
Titrations
Buffers
Colors of the rainbow (GI(sp1,3-7))
Page 4 of 2
AP Chemistry involves application of chemistry knowledge in complex problem-solving. Practicing solving AP Chemistry problems requires time, considerable effort
& often much patience. Students are also expected to read ahead. Daily studying and consistent completion of home work is essential to passing this
course and cannot be stressed enough.
AP standards & objectives will be strictly adhered to and can be found at www.apcentral.collegeboard.com
Course Format:There are high expectations of AP students. This is reflected in the classroom format. AP Chemistry classes are taught in a seminar format from
the lab perspective with an emphasis upon peer teaching, review and collaboration. A great deal of time will be spent in the lab—approximately 2-3 days
per week—that is 90-135 minutes per week. (Laboratory work will be documented in a lab notebook---see requirements section on next page.) Students
are expected to collaborate with a partner in the lab. Students should not complete assignments or perform tasks in isolation. Students will be required to not only
complete assigned problems but to present solutions to the entire class including inquiry based labs. Also, detailed written responses will be required for many
assignments. The use of the Internet will also be expected. Additional instructional strategies used in this course will include (but may not be limited to)
lecture/note-taking, practice exercises, graphic organizers, TI83/4 + technology, & traditional chemistry laboratories.
On-line resources:
http://apcentral.collegeboard.com/home
http://www.acs.org/content/acs/en.html
http://www.webelements.com/
http://www.chemthink.com/chemthink.htm
Grading Plan:
Category
Weight
Homework/classwork 25%
Lab Work
30%
Tests
30%
Final Exam
15%
Total
100%
Revised JUNE 2011
Page 5 of 2
Big Ideas
1. Structure of matter
2. Properties and bonding
3. Chemical reactions
4. Reaction rates
5. Thermodynamics
6. Equilibrium
Revised JUNE 2011
Activities
a. Students will construct a periodic
table using periodic trend data to
identify unknown elements
b. Students will use wavelength or
frequency data to calculate wave
energy
a. Students will identify functional
groups in covalent compounds
b. Students will identify molecules as
polar or nonpolar
c. Students will show the
relationships between temperature,
volume, pressure, and moles for
gases
a. Students will balance equations
b. Students will determine what
substances are limiting reagents in
a stoichiometric problem
c. Students will calculate the change
in enthalpy in a reaction
a. Students will determine the rate
and order for a reaction
b. Students will calculate the rate
constant
c. Students will calculate the half- life
of a substance
d. Students will determine the effect
of a catalyst on a reaction
a. Students will use measurements
provided to calculate entropy and
Gibbs free energy
b. Students will determine the effects
of a stress placed on a system at
equilibrium
a. Students will calculate the equilibrium
constant
b. Students will demonstrate the ability to
use ICE tables
c. Students will calculate pH
d. Students will find Ksp
Page 6 of 2
Requirements:

All lab work must be written-up in a stitched composition book filled with graph paper. If you do not have one, you may obtain the required
composition notebook at an office supply store only. (Office Depot and Staples should have these on a regular basis.) See the instructor if you have
trouble finding the appropriate lab composition book. Instructions for lab write-ups will be given in the standard collegiate format—see next item.

Lab Notebook: Lab work is done in collaboration with one or two other students and all work is documented in a stitched composition notebook using
the following format:
o All students will keep records of all lab work. Copies of lab notes are not accepted.
o All entries will be in blue or black ink and written on the right side of the notebook only (do not write on the back of the sheets.)
o Do not use any type of correction fluid—line through mistakes and continue on.
o The first page should be a title page with your name, course name, instructor name, institution name & date.
o The next two pages should be a table of contents.
o All pages must be numbered at the bottom in ink.
o Do not add pages or delete pages.
o Each lab should have:
 Title & date at the top of each page.
 Statement of purpose
 Brief description of procedures used.
 Separate chemicals and materials list with safety concerns.
 Data in tabular format.
 Data analysis & graphs where appropriate.
 Lab questions answered using complete sentences.
 Conclusion that addresses % error or % yield and justifications of error.

A graphing calculator is required. The TI-84+ is preferred as some assignments can only be completed with this version or higher.

An AP Chemistry Resource Book can be purchased at most book stores. (Titles will read like: “Passing the AP Chemistry Test,” “Scoring a 5 on the AP
Chemistry Exam” or something of this nature.)
☻AP Chemistry Exam is Monday, May 2, 2016, at 8:00 am.
The exam is set up as follows:
Section
I
II
Revised JUNE 2011
Question Type
Multiple choice
Free response
Number of questions
60
3 long
4 short
Time allotted
90 minutes
105 minutes
Page 7 of 2