ADVANCED PLACEMENT CHEMISTRY
SYLLABUS
September 2014 - May 2015
Overview:
Niagara Wheatfield offers one section of AP Chemistry, which meets five days a week
for 42 minutes, with an extra period every other day for laboratory.
This course is designed to provide a solid, first-year college chemistry experience, both
conceptually and in the laboratory and should be challenging for every student.
Students receiving a 3 or higher on the AP Exam may be eligible to receive college
credit at some colleges and universities. The labs will serve as a supplement to the
classroom instruction. Sixteen Laboratory hands-on laboratory experiments will be
performed throughout the year accounting for for more than 25% of class time, and
additional class time will be used to help students meet each of the learning goals in
the AP Scientific Practices. Inquiry and Problem and solving skills, both on paper and
in the lab, are emphasized throughout the course. Students will complete two to three
labs a month during the first three quarters of the year. The final quarter will focus
predominately on review, with students will taking several graded practice AP Exams in
order to become familiar with the exam style help increase the students’ awareness of
test-taking strategies.
The course is organized around six “Big Ideas.” Each Big Idea is broken down into
Enduring under standings and Essential Knowledge. Science Practices parallel these
enduring understandings and Essential Questions.
“ Big






Ideas”
Structure of Matter
Properties of Matter
Chemical Reactions
Rates of Reactions
Thermodynamics
Equilibrium
Science Practices:
The science practices for AP Chemistry are designed to get the students to think and
act like scientists. Students will be expected to learn to:
Science Practice 1: use representations and models to communicate scientific
phenomena and solve scientific problems.
Science Practice 2: use mathematics appropriately.
Science Practice 3: engage in scientific questioning to extend thinking or to guide
investigations within the context of the AP course.
Science Practice 4: plan and implement data collection strategies in relation to a
particular scientific question.
Science Practice 5: perform data analysis and evaluation of evidence.
Science Practice 6: work with scientific explanations and theories.
Science Practice 7: connect and relate knowledge across various scales, concepts,
and representations in and across domains.
(*From College Board)
It is highly recommended that students have successfully completed Regents
chemistry and Algebra 1 before taking AP Chemistry, but is. Although all Regent’s
topics are covered in detail in this course, they will be gone over quickly. More time is
necessary to cover the increased complexity of the AP Curriculum.
Suggested Math Skills for students entering AP Chemistry
 Knowledge of basic Algebra and Geometry
 Knowledge of how to measure and collect experimental data with respect to
volume, size, mass, temperature, and pH
 Knowledge of how to determine the rates of chemical reactions
 Knowledge of how to calculate solute concentrations
 Knowledge of scientific notation
 Ability to apply basic concepts of probability and to conduct statistical analysis
 Knowledge of graphing, including how to set up axes and plot data
 *Note: Trigonometry and calculus are not mandatory
Course Requirements:
In this class, the Chemistry: The Central Science, Twelfth addition will be covered at a
rate of approximately one chapter every 5 to 7 school days, with approximately 25
problems assigned and reviewed per chapter. The assignments are on a chapter or
weekly basis. Chapter Exams consist of 20-30 multiple-choice questions and up to 4
free-response questions. A student’s grade is approximately a weighted average of
the following:




Tests
Quizzes
Labs
Homework
Materials:




45%
15%
25%
15%
3-ring notebook
3 subject notebook
Graphing calculator (everyday)
Test Prep book, (Princeton Review, 5 steps to a 5,
Barron’s, etc.)
 Textbook: Brown, LeMay, Bursten, Murphy, and
Woodward, Chemistry: The Central Science , Prentice
Hall (2012),Twelfth addition.(provided)
Course Outline: Readings and examples should be completed from the
Chemistry Text for the corresponding chapter readings. These should be
done before class meetings. Additional End-of chapter review questions
may be assigned.
Date
Unit
Summer
Introduction,
Calculations and
Uncertainty
Activities
Chapter
Readings
1
Approx.
# DAYS
Summer
2.1,2.2,
2.3, 2.4,
2.5
Summer
2.6, 2.7,
2.8
2.9
4.1
23.1-23.3
7
Assessment
(tentative)
Lab Equipment and
procedures,
physical/chemical
properties/changes,
units, metric
prefixes,
Dimensional
Analysis,
uncertainty,
significant Figures,
separation
techniques, density
Summer
Atoms, Molecules,
and Ions-
o
Students use a mass
spectrometer printout of the
relative masses of isotopes
of an element to determine
the percentages of an
isotope and the average
atomic mass of an element.
Formulas and
Equations-
o
Students will use article”
The Strange Case of Moles
Flight 1023,” from the
Journal of Chemical
Education to determine
empirical Formulas of
various compounds at the
crash site. A report will be
written to explain the
mysteries based on these
calculation and
identifications.
Atomic history,
subatomic particles,
mass number,
atomic number,
atomic mass,
isotopes
9/89/16
Formula Writing,
molecular and
empirical formulas
oxidation states,
nomenclature,
complex ions,
coordination
compounds, types
of reactions,
balancing equations,
net-ionic equations,
simple organic
cmpds.
9/16
9/179/23
9/2410/2
10/510/20
10/2110/29
Periodic Table
and Periodicity-
o
Atomic Structure-
o
groups, periods,
ionization energy,
electronegativity,
atomic radius, ionic
radius, electron
affinity, metals,
nonmetal,
metalloids, Periodic
Trends
PES Spectra,
wave/particle
duality, wave
properties, Bohr,
atomic orbitals,
electron
configurations
Stoichiometry-
structures, ionic
bonding, properties
and character of
bonds, covalent
bonds, octet rule
and exceptions,
resonance, VSEPR
model,
Students will draw Bohr
model diagrams for the first
16 atoms and their most
common ions. Electron
configurations will be
determined for each.
7
5
9/23
7
10/2
6
(not 6.5)
o
Students use a PES spectra
(http://www.chem.arizona.e
du/chemt/Flash/photoelectro
n.html) to determine how
many electrons are present
in each shell (atomic
structure). Students will
also predict what the PES
would look like if the
same/different amount of
energy is required to remove
electrons.
o
Students will develop a
detailed procedure for
making 2.00g of a solid from
two given solid reactants.
(precipitation)
3
11
10/20
o
Students will use model kits
to make molecules and draw
Lewis Structures. Models
will be used to determine
symmetry, and molecular
polarity.
8
7
10/29
mole, atomic
weight, molecular
and empirical
formulas, , limiting
reagents, percent
composition,
percent yield,
Chemical
Bonding-Lewis
Pogil Inquiry Activity –
Periodic Table Trends.
Graphs of Electroneagativity,
Ionization Energy, and
Atomic Radius Vs. Atomic
Number will be created and
interpreted.
10/3011/3
11/4-1113
Thanks
Giving
Break
11/1611/30
Hybridization-
o
Hybridization,
valence bond
theory, bond order
Models of various molecules
with hybrid orbitals already
created, will be studied to
determine hybridization,
molecular geometry,
polarity, Steric number, and
bond angles. Lewis dot
structures will also be
drawn.
Thermochemistry
-Enthalpy, Energy,
9
3
11/3
5
7
11/13
24.1-24.4
3
10
9
Calorimetry,
Thermochemical
equations, heats of
formation, bond
energies, heats of
reactions, Hess’ Law
1st Law of
Termodynamics
Organic
Chemistry-
Classes of
hydrocarbons,
substituted,
branched and closed
chain hydrocarbons,
organic
nomenclature,
combustion,
addition,
substitution,
polymerization,
esterification
Gases- Ideal Gas
Law, Avogadro’s
Law, STP, Dalton’s
Law, Grahm’s Law,
Kinetic Molecular
Theory
o
Students will read the
ChemMatters Article “Green
Gasoline Fuel From Plants.”
( Feb. 2010) Students will
discuss advantages and
disadvantages of Green
gasoline. Students will
present their opinions on the
“Future’ for Green Gasoline.
11/30
12/112/11
12/1212/23
Liquids and
Solids-
o
Students will investigate
several popular alloys.
Students will discuss metallic
structures and how adding a
substance can alter the
properties of that metal.
Properties of
Solutions-
o
Students will design a lab
procedure using various
physical separation
techniques to separate
components of a mixture
containing three different
substances.
Intermolecular
forces, metallic
bonding, types of
solids, network
solids, vapor
pressure, phase
changes, specific
heat
Solubility,
Precipitation,
Molarity, mole
fraction,
electrolytes, Henry’s
law
o
Students will research how
Henry’s Law can be applied
to Scuba Divers and “The
Bends”. Connections to
ideal gas law will be
included.
Students will be given a set
of conditions in order to
determine if the situation is
thermodynamically favored
or not by looking at ΔG,ΔH,
and ΔS. Students will
present condition changes
(Temperature) that may
lead to a thermodynamically
favored situation.
1/41/12
Chemical
Thermodynamics-
o
1/131/29
Chemical
Equilibria-
o
Students will read
ChemMatters Article “What’s
so Equal about equilibrium”
(Sept. 2005) Students will
discuss and make
connections between
Equilibrium and Ozone
Production and Destruction
in the Troposphere and
Stratosphere. Students will
discuss substances that can
lead to the destruction of
ozone and make connection
to Global Warming.
o
POGIL Equilibrium Inquiry
Activity
Gibbs’ Free Energy,
Laws of
Thermodynamics,
Enthalpy, Entropy,
energy and work,
exothermic and
endothermic,
Spontaneousvs.
nonspontaneous
Equilibrium
expressions, I.C.E.
Tables and
Calculations, Le
Chatelier’s Principle
11,12
9
12/11
13 (not
13.5)
8
12/23
19
7
1/12
15,
17.1,17.4,
17.5,17.6
12
1/29
4.2,4.5,4.
6
o
Demonstration- Cobalt
Chloride Equilibrium
Solution- Students will
discuss and interpret results
of several stresses
(Temperature/ increasing
concentration, decreasing
concentration) applied to the
equilibrium solution.
Students should be able to
use Le Chatelier’s principle
to explain the observed
color changes. Connections
to color changing objects in
real-life will be made.
Students will view several
online simulations in groups.
They will discuss each
simulation and answer
questions associated with
each equilibrium.
bromine liquid-gas equilibrium
animation
colbalt chloride equilibrium animation
NO2 N2O4 equilibrium animation
(http://group.chem.iastate.edu/Green
bowe/sections/projectfolder/animatio
nsindex.htm)
o
2/12/12
2/223/11
Chemical
Kinetics-Rate
Laws, order of
reactions, collision
theory, rate
constant, half- life,
activation energy,
catalysts, reaction
mechanisms
Acids and Bases-
Acid- base theories,
Strength of
Acids/Bases pH, Ka
and Kb expressions,
Titration, percent
ionization, Kw,
indicators, buffers,
equivalence points, ,
hydrolysis of salts,
common-ion effect
o
Demonstration- Iodine Clock
Reaction. Students will
interpret the results based
on the collision Theory.
Effect of catalyst,
Temperature, and
concentration will be shown.
o
Students will interpret
several PE diagrams.
Students will use the
Maxwell-Boltzman
distribution to explain
Temperature and Catalyst
effects on the rate of
reaction.
o
Students will conduct an
investigation into the major
components of acid rain and
write the reactions that
occur between the pollutant
and the compounds
naturally present (i.e.,
water, carbon dioxide.)
o
Cabbage Juice will be used
as an indicator to determine
pH of household chemicals
and calculation of their
corresponding [H+] or
[OH-].
14
10
2/12
16
(not
16.11)
15
3/11
17.2,17.3,
4.3
3/144/1
Electrochemistry-
Simulation- Voltaic and
Electrolytic Cells
(http://group.chem.iastate.e
20 (not
20.6)
4.4
9
4/1
Nuclear
Chemistry-
21
4
4/8
Review for Exam
–
Additional Labs
----
o
Half-reactions,
Electrochemical
Cells, standard
voltages , Faradays
Law, writing and
balancing redox
equations (also in
acidic and basic
solution)
du/.../animationsindex.ht
m )Students will Set up a
simulation to produce the
desired Voltage (Voltaic Cell)
between electrodes, and
verify the time to
electroplate a mass of a
metal onto a
surface(electrolytic Cell).
o
Students will use the HalfReaction Method and the
Oxidation Number Change
Method to balance redox
reactions. Redox reactions
in acidic and basic conditions
will be explored.
4/4- 4/8
Nuclear equations,
half lives, nuclear
emissions, fission
and fusion, nuclear
benefits and risks
4/10 Exam
AP Chemistry Labs
All Labs are hands-on and student-run. All labs are required and will account for 25% of the
overall quarter grades. All Lab Reports will be turned in and kept in a notebook upon return.
We will complete 16 required labs, 10 of which will be inquiry based.
*Required Lab Notebook Components:
 Objective
 Materials
 Procedure
 Data and Observations
 Analysis (Calculations)
 Questions
 Conclusion
Topic
Introduction,
Calculations,
and Uncertainty
Atoms,
Molecules, and
Ions
Formulas and
Equations
Stoichiometry
Lab

Seperation of a
dye mixture using
chromatography
( inquiry)
 Analysis of Food
dyes in Beverages
(inquiry)

Acivity Series
Green Chemistry
Analysis of a Mixture
(inquiry)
Gravimetric analysis of
a Metals Carbonate
Chemical
Bonding
Properties of
Solutions
Chemical
Thermodynamics

Qualitative
Analysis and
Chemical Bonding
(inquiry)
Percent Copper in Brass
(inquiry)
Designing a Hand
Warmer(inquiry)
L.O-Learning
Objectives S.P.Science Practices
L.O2.7, 2.10,2.13
S.P1.4,4.2,4.3,5.1,5.2,5.3,
6.2,6.4
L.O1.15,1.1
S.P2.2,4.1,4.2,5.1,6.4
L.O1.9,1.10,3.12,3.8
S.P2.2,2.3,6.1,6.4
L.O1.18,3.3,3.5
S.P1.4,2.1,4.2,5.1,6.4
L.O1.19,1.3, 1.2,3.3
S.P2.2,4.3,5.1,6.1
L.O2.22,2.24,2.28,2.32
S.P1.4,2.2,4.2,5.3
L.O1.16,3.4
S.P4.1,5.1,6.4
L.O2.8,3.11,5.6
S.P1.4,2.2,4.2,5.3
Chemical
Kinetics
Rate of decomposition
of Calcium Carbonate
(inquiry)
Kinetics of Crystal
Violet Fading (inquiry)
Chemical
Equilibria
Applications of Le
Chatelier’s Principle
(inquiry)
Determination of Keq for
FeSCN2+
Acids and
Bases
 Acidity of
Beverages(inquiry)

Acid Base
Titrations
 pH Properties of Buffer
Solutions
Electrochemistry
Oxidation Reduction
Titrations
L.O4.1,4.2
S.P4.1,4.2,5.1,6.1,6.2
L.O4.1,4.2
S.P1.4,2.1,2.2,4.2,5.1,6.4
L.O3.11,6.3,6.8,6.9
S.P1.4,1.5,4.2,4.4,5.1
L.O1.0,1.16,6.9
S.P2.2,4.3,5.1,6.1
L.O1.20,3.3
S.P2.2,3.1,4.2,5.1,6.4,7.1
L.O1.20,3.3,3.7,6.11,6.12,
6.13,6.14,6.15,6.16,
6.17
S.P1.4,2.2,2.3,5.1,6.1,6.2,
6.4
L.O3.7,6.12,6.16,6.18,6.19,
6.20
S.P2.2,2.3,4.2,5.1,6.1,6.4,
7.2
L.O1.20,1.4,3.3,3.8,3.9
S.P1.4,2.2,4.2,5.1,6.1,
6.4,7.1