AP COURSE SYLLABUS
Course Title: AP Chemistry
Textbook: Chang, R. Chemistry. 8th ed. 2005 McGraw - Hill
ISBN: 0-07-251264-4
COURSE OBJECTIVE
 The ultimate goal of this course is for students to gain a solid understanding of
modern chemistry and the principles that govern it in order to successfully solve
mathematically based problems stemming from both the textbook as well as the
laboratory.
COURSE DESCRIPTION
 This course is designed to prepare the student to effectively complete the AP Exam.
The course is set up according to the College Board curricular requirements and the
material covered is in direct alignment with those requirements. Students are
expected to maintain a laboratory notebook which documents all lab work completed
throughout the course. Upon completion of this AP course students will have
received content that is equivalent to a college level first year general chemistry
course.
GRADE MAKEUP
 Student’s will be graded in four areas of assessment; homework, participation,
laboratory work, and tests. Homework and participation comprise about 25% of the
overall grade, while labs makeup approximately 25% and tests are worth 50% of a
student’s final course grade.
o 100 – 90 A
89 – 80 B
79 – 70 C
69 – 60 D
Below 60 F
LABORATORY COMPONET
 All students are required to maintain and submit a complete laboratory notebook that
includes objectives, purposes, and requirements for each lab. Each student is required
to work and collaborate with a lab partner during the course of all laboratory
experiments. At times the students will be required to participate in groups of 4 to
complete certain laboratory experiments and present their findings to the class. Since
our school is on a 50 minute class period which meets 5 days a week, the average
laboratory experiment will require a total of 2 class periods to complete. Throughout
the course of the year the average time spent in the laboratory will average out to
about 2 class periods a week. (C5 & C7)
FALL SEMESTER (Approximately 16 weeks)
C2: States of
Matter (Gases,
Liquids and
solids, Solutions)
TOPIC 1 Matter & Measurement (1 week) (C2)
ALL students should;
 Recall a definition of chemistry
 Understand the process and stages of scientific (logical) problem solving
 Recall the three states of matter, their general properties and the methods for their
interconversion
 Understand and recall definitions for physical and chemical change
C5: Laboratory
(Physical
manipulations;
Processes and
procedures;
Observations and
data
manipulation;
Communication,
group
collaboration, and
the laboratory
report)
C7: The course
includes a
laboratory
component
comparable to
college-level
chemistry
laboratories. A
minimum of one
double-period per
week or its
equivalent is
spent engaged in
laboratory work.
A hands-on
laboratory
component is
required. Each
student should
complete a lab
notebook or
portfolio of lab
reports.








Know the difference between elements, mixtures and compounds including the
difference between heterogeneous and homogeneous mixtures
Understand and be able to use scientific notation (standard form)
Recall and use SI units and prefixes
Be able to convert between units
Understand the concept of derived units and use relationships relating to density
Recall the meaning of uncertainty and understand and be able to use the rules for
determining significant figures and rounding off
Understand the differences between, and be able to apply, the concepts of accuracy
and precision
Learn, and be able to use, formula for the conversion of the three different
temperature units studied in TOPIC 1
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 1 pages 2-37
o Book Work Problems
 6,7,17,21,23,29,39,42,61,82
o Laboratory Experiments
 Determination of the Empirical Formula of Silver Oxide, Taken from
Laboratory Experiments for Advanced Placement Chemistry, By Sally
Ann Vonderbrink, Ph.D. 2nd Edition
TOPIC 2 Atoms, Ions & Nomenclature (2 weeks) (C1)
ALL students should;
 Recall a very brief history of Atomic Theory
 Know and understand the five main aspects of Dalton's Atomic Theory
 Recall some of the experiments that led to the identification of sub-atomic particles
 Know the three particles that make up the atom and their relative charges, masses and
positions in the atom
 Be able to use the Atomic # and Mass # of an isotope to calculate the numbers of
protons, neutrons and electrons present
 Know what the term isotope means and be able to perform simple calculations
relating to isotopic data
 Understand radioactivity and the properties of radioactive particles
 Be able to write nuclear equations
 Understand the concept of half-life and be able to perform calculations related to it
 Recall some uses of radioactivity
 Understand the term mass deficit
 Be able to use neutron: proton ratio to make predictions about stability
 Understand the terms nuclear fission and fusion
 Understand, that in very general terms, radioactivity involves the rearrangement of
the nucleus and chemical reactions involve the rearrangement of electrons
 Know the approximate locations of metals, non-metals and metalloids on the periodic
table
 Understand the meaning of the terms Molecule and Ion
C1 Structure of
Matter (Atomic
theory and atomic
structure,
Chemical
bonding)








Learn the lists of common anions and cations (including polyatomic ions) studied in
TOPIC 2
Know how to combine those anions and cations in the correct proportions to form
ionic compounds with no net charge
Be able to name binary ionic compounds of a metal and a non-metal
Be able to name binary molecular compounds of two non-metals
Be able to name simple binary acids
Be able to name ionic compounds containing polyatomic anions
Be able to name oxoacids and compounds containing oxoanions
Be able to name hydrated salts
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter(s) 2 & 23 pages 40-73 & 942-975
o Book Work Problems
 Ch. 2 – 10,11,12,13,15,17,21,27,32,33,34,36,46,55,56,63
 Ch. 23 – 5,6,7,14,23,24,26
o Laboratory Experiments
 Analysis of Alum, Taken from Laboratory Experiments for Advanced
Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd Edition
TOPIC 3 Electronic Configuration (2 weeks) (C1)
ALL students should;
 Understand the Bohr model of the atom
 Understand how line emission spectra are formed
 Appreciate that the electron can be considered to have wave like properties as well as
particle type properties
 Understand and use equations that relate the Energy, frequency, speed and
wavelength of waves including the Rydberg equation
 Understand the concept of electrons in shells and the use of quantum numbers
 Understand the use of the terms s, p, d and f and their use in orbital notation
 Recall and understand the rules for filling orbitals (Aufbau, Pauli and Hund) and
determining electronic configuration including the Pauli exclusion principle, Hund's
rule of maximum multiplicity and notable exceptions
 Be able to construct the electronic configuration of the elements using the s, p and d
and f notation
 Be able to construct the electronic configuration of the elements using the noble gas
core and s, p, d and f notation
 Be able to construct the electronic configuration of simple ions (including d block
ions)
 Recall the shapes of the s, p and d orbitals
 Recall that orbitals are electron probability maps
 Be able to describe electronic configurations using the electrons in boxes notation
 Recall the meanings of the terms paramagnetic, diamagnetic and isoelectronic
o Assignments:
 Worksheets
C1 Structure of
Matter (Atomic
theory and atomic
structure,
Chemical
bonding)
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 7 pages 258-303
o Book Work Problems
 8,18,54,56,58,60,62,64,73,76,80,82,84,86,114
o Laboratory Experiments
 Flame Test Lab – Developed by the teacher
TOPIC 4 Stoichiometry (2 weeks)(C3, C6)
ALL students should;
 Be able to write chemical equations in words
 Be able to write chemical equations using chemical formulae and chemical symbols
(this requires knowledge, and correct use of, chemical nomenclature)
 Understand, and be able to use, state symbols as part of chemical equation writing
 Be able to balance chemical equations
 Understand why balancing chemical equations is important
 Understand the concept of percentage by mass
 Be able to calculate empirical formulae from percentage by mass data
 Be able to convert empirical formulae to molecular formulae by using RMM data
 Understand and be able to apply the concept of the mole in chemical calculations
(including the application of Avogadro's number)
 Be able to use combustion data to calculate empirical formulae of compounds
 Understand the importance of, and be able to apply, the concept of stoichiometric
coefficients relating to reacting ratios
 Know how to calculate the number of moles of a solid substance present in a reaction
from data
 Be able to perform calculations relating to Molarity
 Understand and be able to perform calculations relating to the Beer-Lambert law
 Be able to perform calculations relating to dilution
 Be able to perform calculations relating to Molality
 Be able to calculate the formulae of hydrated salts from experimental data
 Understand, and be able to apply, the concept of a limiting reactant
 Understand, and be able to apply, the concept of percentage yield
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter(s) 3 pages 74-113
o Book Work Problems
 14,16,20,24,28,40,42,50,54,60,64,66,68,70,78,80,82,84,86,87,88,90,92
,93,103,112,116
o Laboratory Experiments
 Finding the Ratio of Moles of Reactants in a Chemical Reaction,
Taken from Laboratory Experiments for Advanced Placement
Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd Edition
 Preparing a Primary Standard Solution – Developed by teacher
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.

Determining the Concentration of an Unknown Solution – developed
by teacher
TOPIC 5 Aqueous Chemistry (2 weeks) (C2, C3, C6)
ALL students should;
 Understand that a reaction in aqueous solution is one that is carried out in water
 Understand the terms electrolyte, weak electrolyte and non-electrolyte and be able to
predict which compounds fall into which category
 Be able to calculate the individual ion concentrations when ionic compounds are
dissolved in water
 Understand the difference between, and be able to write, full, ionic and net ionic
equations
 Learn and be able to apply solubility rules
 Recall that an acid is a hydrogen ion donor
 Recall that a base is a hydrogen ion acceptor
 Understand how the degree of ionization/dissociation determines the strength of an
acid and a base
 Understand that in a neutralization reaction an acid and base react to form a salt and
water
 Understand that oxidation and reduction can be described in terms of loss and gain of
electrons respectively
 Be able to find the oxidation number of an element within a compound
 Become familiar with some common oxidizing and reducing agents and the halfequations that represent their action
 Understand and be able to recognize the different types of REDOX reaction. Namely
synthesis (combination), decomposition, combustion, single and double displacement
(replacement) including metal displacement, hydrogen displacement from water and
acids and halogen displacement
 Learn and be able to use the reactivity series as a tool for predicting displacement
reactions
 Understand the concept of disproportionation
 Recall and understand the technique of titration
 Be able to carry out simple quantitative moles calculations relating to REDOX
titration data
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 4 pages 114-159
o Book Work Problems
 6,12,20,22,28,34,40,44,46,47,50,54,80,88,91,92,94,97,101,105
o Laboratory Experiments
 Analysis of a Commercial Bleach, Taken from Laboratory
Experiments for Advanced Placement Chemistry, By Sally Ann
Vonderbrink, Ph.D. 2nd Edition
 Oxidation – Reduction Titration, Taken from Laboratory Experiments
for Advanced Placement Chemistry, By Sally Ann Vonderbrink, Ph.D.
2nd Edition
C2: States of
Matter (Gases,
Liquids and
solids, Solutions)
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
TOPIC 6 Gases (2 weeks)(C2, C6)
ALL students should;
 Be able to convert between different units of pressure
 Be able to convert between different units of temperature
 Recall and be able to use Boyle's law in calculations
 Recall and be able to use Charles's law in calculations
 Recall and be able to use Avogadro's law in calculations
 Recall and be able to use the Combined gas law and the General gas law in
calculations
 Recall and be able to use the Ideal gas law in calculations
 Understand and be able to use the van der Waals equation (modified ideal gas law) in
calculations
 Recall and be able to use Dalton's law of partial pressures in calculations
 Recall the conditions that are used as standard in calculations
 Be able to use molar gas volume in calculations
 Understand the Kinetic theory as applied to gases
 Understand the concept of, and be able to perform calculations involving, the rootmean-square-speed of gases
 Understand the terms effusion and diffusion and be able to perform calculations
relating to those concepts
C2: States of
Matter (Gases,
Liquids and
solids, Solutions)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 5 pages 162-211
o Book Work Problems
 6,12,20,22,28,34,40,44,46,47,50,54,80,88,91,92,94,97,101,105
o Laboratory Experiments
 Determining the Molar Volume of a Gas, Taken from Laboratory
Experiments for Advanced Placement Chemistry, By Sally Ann
Vonderbrink, Ph.D. 2nd Edition
 Determination of the Molar Mass of Volatile Liquids, Taken from
Laboratory Experiments for Advanced Placement Chemistry, By Sally
Ann Vonderbrink, Ph.D. 2nd Edition
TOPIC 7 Periodicity (1 week)(C4)
ALL students should;
 Understand that regular, repeatable patterns occur across periods and within groups
on the periodic table
 Appreciate that these patterns sometimes have notable exceptions
 Recall and understand that the noble gases have full outer shells that represent stable
electronic configurations
 Recall how, and understand why, group I, II, VI and VII elements achieve pseudo
noble gas electronic configurations
 Recall the definition of ionization energy
C4: Descriptive
Chemistry
(Relationships in
the periodic table)







Recall the definition of electron affinity
Recall and understand the variation in ionization energy and electron affinity when
moving about the periodic table
Be able to predict the group an element is in from ionization energy data
Understand and be able to apply the terms diamagnetic and paramagnetic
Recall how and why atomic and ionic size vary when moving about the periodic table
Understand how many physical properties change gradually when moving about the
periodic table
Understand and recall the change in the specific chemical properties mentioned in
TOPIC 7
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 8 pages 304-343
o Book Work Problems
 5,12,16,21,24,37,38,48,55,56,60,61,86,91,98,109,118,120,131
o Laboratory Experiments
 Periodic Table Lab Activity – Developed by Teacher
TOPIC 8 Chemical Bonding (2 weeks)(C1)
ALL students should;
 Understand that when forming chemical bonds atoms are attempting to form more
stable electronic configurations
 Understand the essential difference between intra and inter bonding
 Understand the concept of ionic bonding and the nature of the ionic bond
 Understand the concept of covalent bonding and nature of the covalent bond
 Be able to draw Lewis structures
 Understand the concept of resonance related to Lewis structures
 Understand the concept of formal charge related to Lewis structures
 Be able to predict the shape of, and bond angles in, simple molecules and ions using
VSEPR theory
 Understand the concept of the dative (co-ordinate) bond related to Lewis structures
 Understand that ionic bonding and covalent bonding are at two ends of a sliding scale
of bond type
 Understand the concept of electronegativity
 Understand that polarization caused by small highly charged cations leads to ionic
compounds exhibiting some covalent character
 Understand that differences in electronegativity in covalent molecules causes dipoles
and some ionic character in covalent compounds
 Understand when molecules exhibit polarity
 Be able to predict the shapes of simple molecules and ions using Lewis structures
 Understand the occurrence, relative strength and nature of dipole-dipole interactions,
London dispersion forces and hydrogen bonds
 Understand how solid structure influences properties
 Understand the nature of liquids
 Understand the nature of sigma and pi bonds
 Understand and be able to identify different types of orbital hybridization
C1 Structure of
Matter (Atomic
theory and atomic
structure,
Chemical
bonding)
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter(s) 9,10, & 11 pages 344-383, 384-433, 434-485
o Book Work Problems
 Ch 9 – 8,13,30,34,36,37,45,52,59,60
 Ch 10 – 12,14,20,42,69
 Ch 11 – 9,10,12,17,18
o Laboratory Experiments
 Molecular Models – Developed by Teacher
TOPIC 9 Thermochemistry (2 weeks)(C3, C6)
ALL students should;
 Learn definitions that describe the systems studied in thermochemistry
 Understand, be able to quote a definition and write suitable equations for standard
enthalpy of formation
 Understand, be able to quote a definition and write suitable equations for standard
enthalpy of combustion
 Understand and be able to use a Hess's Law cycle or algebraic methods to calculate a
given enthalpy change
 Understand and be able to use in calculations, average bond energy terms
 Understand the meaning of the terms exothermic and endothermic
 Understand and be able to apply the concept of entropy both in descriptive and
calculation contexts
 Understand and be able to apply the concept of Gibbs Free Energy both in descriptive
and calculation contexts
 Understand and be able to apply the energetics of the ionic bond as described by the
Born-Haber Cycle and associated calculations
 Understand the role of charge density in determining some physical properties of
ionic compounds
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 6, 9, &18 pages 214-255, 344-383, 762-795
o Book Work Problems
 Ch 6 – 10,12,14,24,26,30,34,38,51,53,55,57,58,62,64
 Ch 9 – 69,72
 Ch 18 – 12,14,18,20
o Laboratory Experiments
 Thermodynamics – Enthalpy of Reactions and Hess’s Law, Taken
from Laboratory Experiments for Advanced Placement Chemistry, By
Sally Ann Vonderbrink, Ph.D. 2nd Edition
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
SPRING SEMESTER (Approximately 17 weeks)
TOPIC 10 Transition Metal Chemistry Basics (3-4 days)(C3)
ALL students should;
 Understand and be able to write electronic configurations of transition metals and
their ions
 Recall some colors of transition metals and understand when color occurs
 Be able to recognize and name complex ions
 Understand and be able to write equations for complex ion reactions (Ligand
exchange & Decomposition)
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
o Assignments:
 Worksheets
 AP Free Response Test Questions
 No Formal Test
o Text Reference
 Chapter 22 pages 910-939
o Book Work Problems
 2,5,13,15
o Laboratory Experiments
 Preparation and Analysis of Tetraamminecopper (II) Sulfate
Monohydrate, Taken from Laboratory Experiments for Advanced
Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd Edition
TOPIC 11 Organic Chemistry Basics (3-4 days)(C3)
ALL students should;
 Be able to name some simple aliphatic organic compounds
 Understand and be able to write equations for some organic reactions (Combustion,
Substitution, Acid Base, Addition & Esterification)
o Assignments:
 Worksheets
 AP Free Response Test Questions
 No Formal Test
o Text Reference
 Chapter 24 pages 978-1010
o Book Work Problems
 26,33,35,41,59,60
o Laboratory Experiments
 Synthesis, Isolation, and Purification of an Ester, Taken from
Laboratory Experiments for Advanced Placement Chemistry, By Sally
Ann Vonderbrink, Ph.D. 2nd Edition
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
TOPIC 12 Equation Writing (1 week)(C3)
ALL students should;
 Be able to write equations for Double Replacement Reactions
 Be able to write equations for Simple REDOX Reactions
 Be able to write equations for Non-Simple REDOX Reactions
 Be able to write equations for Hydrolysis Reactions
 Be able to write equations for Complex Ion (Transition Metal) Reactions
 Be able to write equations for Organic Reactions
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
o Assignments:
 Worksheets
 AP Free Response Test Questions
 No Formal Test
o Text Reference
 NA
o Book Work Problems
 NA
o Laboratory Experiments
 An Activity Series, Taken from Laboratory Experiments for Advanced
Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd Edition
 Predicting the Products of Chemical Reactions and Writing Chemical
Equations, Taken from Laboratory Experiments for Advanced
Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd Edition
TOPIC 13 Chemical Equilibrium (2-3 weeks)(C3, C6)
ALL students should;
 Understand the concept of dynamic equilibrium
 Be able to write an expression in terms of concentrations for the equilibrium constant
Kc given an equation
 Understand that equilibria take a finite time to be achieved
 Be able to calculate values for Kc and associated data from initial concentrations
 Be able to write an expression in terms of partial pressures for the equilibrium
constant Kp given an equation
 Be able to calculate values for Kp and associated data from pressure data
 Recall and understand Le Chatelier's Principle
 Understand the application of Le Chatelier's Principle and be able to predict the shift
in position of equilibria and optimum conditions in reactions
 Understand and be able to apply the relationship of Kc to Kp, the different formats of
Kc (reciprocals and roots) and the relationships in simultaneous equilibria
 Understand and be able to apply to calculations, the concept of solubility product
 Understand and be able to apply to calculations, the concept of common ion effect
 Understand and be able to interpret phase diagrams
 Understand and be able to interpret heating and cooling curves
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter(s) 11, 14, & 16 pages 434-485, 584-625, 678-727
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
o Book Work Problems
 Ch 11 – 94
 Ch 14 – 15,16,18,20,22,30,32,40,42,48,58,60,78,
 Ch 16 – 46,48,50,62
o Laboratory Experiments
 The Determination of Keq for FeSCN2+, Taken from Laboratory
Experiments for Advanced Placement Chemistry, By Sally Ann
Vonderbrink, Ph.D. 2nd Edition
 Determination of the Solubility Product of an Ionic Compound, Taken
from Laboratory Experiments for Advanced Placement Chemistry, By
Sally Ann Vonderbrink, Ph.D. 2nd Edition
TOPIC 14 Acids & Bases (2-3 weeks) (C2, C3, C6)
ALL students should;
 Be able to recall the Bronsted Lowry, Arrhenius and Lewis definitions of an acids and
bases
 Be able to identify acid base conjugate pairs
 Recall the difference between strong and weak acids in terms of ionization
 Be able to calculate pH of strong acids and strong bases
 Be able to calculate pH of weak acids and weak bases using Ka and Kb
 Recall a definition of Kw, the ionic product of water
 Recall the definition of a buffer
 Understand and how a buffer works
 Be able to identify and calculate the pH of a buffer solution
 Understand the techniques and procedures associated with titrations
 Be able to sketch titration curves and be able to suggest a suitable indicator for a
particular titration
 Understand the hydrolysis of salts and the effect this has on pH
 Understand the meaning of the term 'equivalence point'
 Understand how indicators work
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 15 & 16 pages 626-675, 678-727
o Book Work Problems
 Ch 15 – 1,5,16,20,24,26,44,54,92
 Ch 16 – 5,7,22,23,24
o Laboratory Experiments
 Acid – Base Titrations, Taken from Laboratory Experiments for
Advanced Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd
Edition
 Selecting Indicators for Acid – Base Titrations, Taken from
Laboratory Experiments for Advanced Placement Chemistry, By Sally
Ann Vonderbrink, Ph.D. 2nd Edition
 Preparation and Properties of Buffer Solutions, Taken from
Laboratory Experiments for Advanced Placement Chemistry, By Sally
Ann Vonderbrink, Ph.D. 2nd Edition
C2: States of
Matter (Gases,
Liquids and
solids, Solutions)
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
TOPIC 15 Chemical Kinetics (2 weeks)(C3, C6)
ALL students should;
 Be able to recall AND understand Collision Theory
 Be able to recall AND understand how temperature, concentration, surface area and
catalysts affect a rate of reaction
 Understand AND be able to interpret a Maxwell-Boltzmann distribution plot
 Understand AND be able to interpret an energy profile plot
 Be able to deduce orders, rate equations and rate constants (including units) from
initial rate data
 Understand the link between the rate determining (slow step) in a reaction mechanism
and the rate equation
 Understand AND be able to interpret graphical data relating to rates
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 13 Pages 530-583
o Book Work Problems
 Ch 13 – 15,17,18,52,54,55,64,72,73
o Laboratory Experiments
 Kinetics of a Reaction, Taken from Laboratory Experiments for
Advanced Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd
Edition
TOPIC 16 Electrochemistry (1-2 weeks)(C2, C3, C6)
ALL students should;
 Recall the definition of oxidation and reduction in terms of electrons
 Understand and recall the definition of standard electrode potential
 Understand and recall how to construct a cell diagram and draw a line diagram
(picture) of the apparatus needed
 Recall the conditions that standard electrode potentials are measured under
 Understand the nature and purpose of a salt bridge
 Be able to predict the likelihood or otherwise of chemical reactions using standard
electrode potentials and understand how those predictions may not prove to be
accurate
 Understand and use the Nernst equation
 Understand the relationship between Gibbs Free Energy, equilibrium constants and
Ecell, and be able to perform related calculations
 Understand electrolysis and be able to perform quantitative calculations relating to it
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 19 Pages 796-839
o Book Work Problems
 Ch 19 – 11,12,16,18,24,30,58,62,86
o Laboratory Experiments
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
C2: States of
Matter (Gases,
Liquids and
solids, Solutions)
C3: Reactions
(Reaction types,
Stoichiometry,
Equilibrium,
Kinetics,
Thermodynamics
)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.

Electrochemical Cells, Taken from Laboratory Experiments for
Advanced Placement Chemistry, By Sally Ann Vonderbrink, Ph.D. 2nd
Edition
TOPIC 17 Colligative Properties (1 week)(C2, C6)
ALL students should;
 Understand the concept of vapor pressure
 Be able to relate changes (both quantitative and qualitative) in vapor pressure to
addition of non-volatile solutes to solvents (Raoult's Law)
 Understand and recall Raoults Law in terms of ideal solutions of two volatile
components AND deviations from ideal behavior
 Be able to recall and use equations relating to quantitative treatments of Boiling Point
Elevation, Freezing Point Depression, Osmotic Pressure and the van't Hoff factor
o Assignments:
 Worksheets
 AP Free Response Test Questions
 Topic Test
o Text Reference
 Chapter 12 pages 486-527
o Book Work Problems
 Ch 12 - 51,52,53,57,65,89,90,109
o Laboratory Experiments
 Molar Mass by Freezing Point Depression, Taken from Laboratory
Experiments for Advanced Placement Chemistry, By Sally Ann
Vonderbrink, Ph.D. 2nd Edition
Approximately 3-4 Weeks are spent reviewing for the AP Exam
All Topics have laboratory experiments associated with them. Below is a list of all
laboratory experiments which meet the standards set by the College Board.
Throughout the year students will complete, in addition to the recommended labs, other
labs and activities that serve to enhance their chemistry experience. (C5, C7)
C5: Laboratory (Physical
manipulations; Processes and
procedures; Observations and data
manipulation; Communication,
group collaboration, and the
laboratory report)
C7: The course includes a laboratory component
comparable to college-level chemistry
laboratories. A minimum of one double-period per
week or its equivalent is spent engaged in
laboratory work. A hands-on laboratory
component is required. Each student should
complete a lab notebook or portfolio of lab
reports.
C2: States of
Matter (Gases,
Liquids and
solids, Solutions)
C6: The course
emphasizes
chemical
calculations and
the mathematical
formulation of
principles.
Recommended Experiments
Experiments that meet the recommended
experiments
1.
Determination of the Formula of a Compound
1.
Determination of the Empirical Formula of Silver
Oxide; (Student Conducted – 50 min)
2.
Determination of the percentage of Water in a Hydrate
2.
3.
Determination of Molar Mass by Vapor Density
3.
Analysis of Alum; (Student Conducted – 2 - 50 min
periods)
Determination of the Molar Mass of Volatile Liquids;
(Student Conducted – 50 min)
4.
Determination of Molar Mass by Freezing point
Depression
4.
Molar Mass by Freezing Point Depression; (Student
Conducted – 50 min)
5.
Determination of the Molar Volume of a Gas
5.
Determining the Molar Volume of a Gas; (Student
Conducted – 50 min)
6.
Standardization of a Solution Using a Primary Standard
6.
Acid – Base Titrations; (Student Conducted – 2 - 50 min
periods)
Preparing a Primary Standard Solution – Developed
by teacher; (Student Conducted – 50 min)
7.
7.
Determination of Concentration by Acid-Base Titration,
Including a Weak Acid or Weak Base
8.
8.
Determination of Concentration by Oxidation-Reduction
Titration
9.
9.
Determination of Mass and Mole Relationship in a
Chemical Reaction
Acid – Base Titrations; (Student Conducted – 3 - 50 min
periods)
Analysis of a Commercial Bleach; (Student Conducted
2 – 50 min periods)
10. Oxidation – Reduction Titration; (Student Conducted –
2 -50 min periods)
11. Finding the Ratio of Moles of Reactants in a Chemical
Reaction; (Student Conducted – 50 min)
10. Determination of the Equilibrium Constant for a
Reaction
12. The Determination of Keq for FeSCN2+; (Student
Conducted – 2 - 50 min periods)
13. Determination of the Solubility Product of an Ionic
Compound (Student Conducted – 50 min)
11. Determination of the Appropriate Indicators for Various
Acid-Base Titrations, pH Determination
14. Selecting Indicators for Acid – Base Titrations;
(Student Conducted – 50 min)
12. Determination of the Rate of Reaction and its Order
13. Determination of Enthalpy Change Associated with a
Reaction
15. Kinetics of a Reaction; (Student Conducted – 2- 50 min
periods)
16. Thermodynamics – Enthalpy of Reactions and Hess’s
Law; (Student Conducted – 50 min)
14. Separation and Qualitative Analysis of Cations and
Anions
17. Completed during first year of Chemistry(4 – 5 - 50
min periods)
15. Synthesis of a Coordination Compound and its
Chemical Analysis
18. Preparation and Analysis of Tetraamminecopper (II)
Sulfate Monohydrate; (Student Conducted – 2 - 50 min
periods)
19. Completed during first year of Chemistry (2 – 50 min
periods)
20. The Determination of Keq for FeSCN2+; (Student
Conducted – 50 min periods)
16. Analytical Gravimetric Analysis
17. Colorimetric or Spectrophotometric Analysis
18. Separation by Chromatography
21. Completed during first year of Chemistry(50 min)
19. Preparation and Properties of Buffer Solutions
22. Preparation and Properties of Buffer Solutions;
(Student Conducted – 2 -50 min periods)
20. Determination of Electrochemical Series
23. An Activity Series; (Student Conducted – 50 min)
21. Measurements Using Electrochemical Cells and
Electroplating
24. Electrochemical Cells; (Student Conducted – 50 min)
22. Synthesis, Purification, and Analysis of an Organic
Compound
25. Synthesis, Isolation, and Purification of an Ester;
(Student Conducted – 2 - 50 min periods)