Advanced Placement Chemistry 2011-2012
Granbury High School
Instructor and Contact Information
Cindy Jackson
Cindy.jackson@granburyisd.org
School phone: 817-408-4600
Science office: 817-408-4636
Course Description
The AP Chemistry course at Granbury High school emulates the first year of college chemistry in breadth and rigor. The
goal of this course is to prepare the student to become an independent thinker functioning in a scientific, technological
society with an appreciation for the natural world. Through discussions, lecture, and laboratory experimentation, the
aim of AP Chemistry is to sharpen the student’s ability to think critically, solve problems and communicate effectively.
The student will be expected to demonstrate development of these abilities through completing assignments, class
presentations, assessments, informal and formal written reports and ultimately an acceptable score on the AP Chemistry
Examination in May.
Text
Chemistry by Zumdahl and Zumdahl, 5th ed., Houghton Mifflin Company, 2000.
General Chemistry: During Class Inventions & Computer Lab Activities Volumes I & II by Abraham, Gelder, and
Greenbowe, 3rd ed., Hayden-McNeil, 2009.
The Ultimate Chemical Equations Handbook by Hague and Smith, Flinn Scientific, Inc., 2001.
Laboratory Experiments for Advanced Placement Chemistry by Sally Ann Vonderbrink, Flinn Scientific, Inc., 2003
Requirements and Expectations
Students are expected to be in class on time with the required materials. The AP Chemistry class meets five 55-minute
periods each week.
To be successful in this class, it will be necessary for students to study and practice problems in chemistry outside of
class, at the very least, one hour per day. Homework assignments will be assigned to provide students with
opportunities for study and practice. Most of the time, homework will not be graded. Mastery of process skills and
concepts will be assessed based on performance on quizzes and tests. The AP chemistry student is expected to seek help
outside of class if he/she is struggling with a particular concept or problem-solving process. I will be available before and
after school if a student needs help or needs a quiet place to work. I have an open-door policy to all my students, so it is
advised NOT to wait until the day an assignment is due or the day before a test to get help.
In each laboratory experiment, students will physically manipulate equipment and materials, make observations, collect
and analyze quantitative and qualitative data, use the data to form conclusions and verify hypotheses. Also, students
will communicate and compare lab results and procedures through collaboration, presentations, and formal written
reports. Students will be expected to keep a formal laboratory notebook. Each student will be provided with a carboncopy lab notebook. The lab experiments will come from sources equivalent to labs encountered in a first-year college
chemistry course. Approximately 1-2 periods per week will be devoted to time in lab; however, students will be required
to spend time outside of class time in the lab completing practical portions of labs and data collection in many cases.
Test and quiz corrections are encouraged for all students, but are required for any student making a failing grade on an
exam. Points will be awarded on the test grade for corrections completed correctly.
Grading Guidelines
Minor Grades
Daily work
Homework and daily work is self-checked and may sometimes count as a minor grade. It is expected to be on
time, and any late work will only be granted half credit.
Laboratory grade
Labs will be graded with each lab and count as one or two minor grades. Lab work is assessed in many ways,
such as formal/informal lab reports and class presentations of data and results. Any late reports will be docked
10 points per day late.
Quizzes
Quizzes count as a minor grade, and are designed for students to spot areas that need special attention before a
major exam.
Major Grades
Tests
Major tests will count as a major grade. The tests will follow the AP exam format, and questions will come from
previously released AP exams. Generally, students can expect an exam 2-3 times per six-weeks depending on
material being covered.
Projects
Projects may count as two minor grades or one major grade depending on the nature of the project.
Chemistry Topics Covered:
Fall semester
Time
(weeks)
Zumdahl
reference
Topics
2
Chapter
1,2,3
Lab Safety
Nomenclature of simple Compounds
Stoichiometry
 Molecular Weight
 Percent Composition of compounds
 The Mole and Molar Mass
 Balancing Chemical Equations
 Limiting Reactant and Percent Yield
 Empirical and Molecular Formulas from
Experimental Data
 Combustion Analysis
AP Curriculum
requirements
IV 2
Labs V (AP recommended experiments)
1. Empirical formula of an unknown
compound (#1) [CBL- Abraham, Gelder, et
al.]
2.
III B 2,3
Analysis of Alum (#2)
Time
(weeks)
2
Zumdahl
Chapters
Chapter 2
Chapter 3
Chapter7
Topics
AP Curriculum
requirements
Atomic Theory
 History of Atomic Theory
o Early history
o Dalton’s Atomic Theory
o Early Experiments: Evidence for
Atomic Theory
 Modern view of the atom
o Atomic and Mass Number; Isotopes
o Atomic Masses: Determination by
chemical and Physical Means
 Electromagnetic Radiation
 Atomic Spectra
 Electronic Structure
o Bohr Model
o Quantum Mechanical Model
o Quantum Numbers
o Orbital Shapes and Energies
o Pauli’s Exclusion Principle
 Aufbau Principle and the Periodic Table
o Orbital-filling Rules
o Electron Configurations
 Periodic Trends and atomic Properties
o Atomic and Ionic Radii
o Ionization Energy
o Electron Affinity
o Electronegativity
 Review of the Periodic Table
o Ion Formation
o Properties of a group
 Alkali metals
 Alkaline earth metals
 Halogens
 Transition metals
 Noble gases
IA
1,2,3,4,5
Labs V (AP recommended experiments)
1.
Gravimetric Analysis of a Metal
carbonate (#16)
Time
(weeks)
Zumdahl
reference
Topics
Chemical Bonding
2
Chapter 8




Chapter 9
3
AP Curriculum
requirements
Chapter 4
Octet Rule
Electron configurations of ions
Ionic Bonding
o Lattice energy
o Properties of ionic solids
Covalent Bonding
o Electronegativity & bond polarity
o Lewis Structures
o Exceptions to the octet rule
o Formal Charge
o Bond energy and bond length
o Resonance structures
o VSEPR model
o Valence Bond Theory
o Hybrid Orbital Theory
 Molecular geometry (molecules
& ions)
o Molecular polarity: solubility in water
o Multiple bonds
 Sigma and pi bonds
Labs V (AP recommended experiments)
1.
Finding the Ratio of Moles of
Reactants in a Chemical Reaction (#9)
1.
An Activity Series (#20)
2.
Oxidation-reduction Titration (#8)
I B 1 a,c
IB2
a,b,c
IB3
II B 4
IV 2
Aqueous Solutions and Chemical Reactions








Solutions
Concentration: molarity
Solubility
Precipitation Reactions
o Solubility Rules
o Ionic Equations
REDOX Reactions
o Oxidation Numbers
o Half reactions
o Balancing REDOX equations
o Activity Series
o Single displacement reactions
Synthesis Reactions
Decomposition Reactions
Combustion Reactions
III A 2
III A 3a
III B1
III B 2
IV 1
Time
(weeks)
Zumdahl
Chapters
Topics
Thermodynamics
2
Chapter 6



Chapter 16
2
Chapter 13
Equilibrium





Chapter 16
1
Chapter 22
State Functions
First Law of Thermodynamics
 Enthalpy of Reaction
 Enthalpy change
o Calorimetry
o Hess’s Law
o Enthalpy of Formation
o Average Bond enthalpy
Second Law of Thermodynamics
 Entropy
 Free Energy
o Free energy of reaction
o Dependence of free energy on
enthalpy and entropy changes
o Free energy of formation


Chemical dynamic equilibrium
Law of mass action for systems at
equilibrium
Equilibrium constant and reaction quotient
Equilibrium constants for gaseous reactions
o Involving pressure (Kp)
o Involving concentration(Kc)
LeChatelier’s principle
o Effect of change in concentration
o Effect of change in pressure
Effect of change in temperature
Relationship of equilibrium constant and
change in free energy
Organic Chemistry ***





Alkanes: saturated hydrocarbons
o Isomerism in alkanes
o Nomenclature
o Reactions of alkanes (chemical
properties)
o Cyclic alkanes
Alkenes and alkynes
o Isomerism
o Reactions (chemical properties)
Aromatic hydrocarbons
Functional groups
o Alcohols
o Aldehydes and ketones
o Carboxylic acids and esters
o Amines
Polymers
Labs V (AP recommended
experiments)
AP Curriculum
requirements
III E
1,2,3,4
1.
Thermodynamics – Enthalpy of
Reaction and Hess’s Law (#13)
1.
Spectrophotometric Analysis of the
Cobalt II Ion [AP Solutions] (#17)
2.
The determination of Keq for FeSCN(#10)
IV 1
III C 1,2a
III E 4
IV 1
IB3
IV 3
Time
(weeks)
1.5
Zumdahl
Chapters
Chapter 5
Topics
Gases










1
AP Curriculum
requirements
Labs V (AP recommended experiments)
II A 1a,b
Pressure
Boyle,s, Charles’, and Avogadro’s Law
Ideal gas law: equation of state for gas
Gas stoichiometry
Dalton’s Law of partial pressures
Kinetic molecular theory
o Theory applied to gas laws
o Deriving the ideal gas law
o Dependence of kinetic energy
on temperature and how it
relates to pressure
Graham’s law of effusion
Diffusion
Real gases: deviations from the ideal gas
law
Chemistry in the atmosphere
Review & Final Exams
II A
2a,b,c,d
IV 1
1.
Determination of Molar Mass of
Volatile Liquids (#3)
2.
Molar Volume of a Gas (#5)
Spring Semester
Time
(weeks)
Zumdahl
Chapters
Topics
Intermolecular Forces
2
Chapter
10





Intermolecular forces
o Dipole-dipole forces: hydrogen bonding
o Vander Waals forces: London dispersion
forces
Liquid state: structural model for liquids
Structure and types of solids
o Unit cells and crystal packing
o Crystalline solids
o Structure and bonding in metals
o Calculating density in closest packed solid
o Network solids
o Molecular and ionic solids
o Determining the number of ions in a unit
cell
Vapor pressure and changes of state
o Heat of vaporization and fusion
o Vapor pressure
Changes of state
o Phase diagrams
o Critical and triple point
Solutions
2
Chapter 11


Sections
15.6-15.8





Solution composition
o Mass percent
o molarity
o Mole fraction
o Molality
Solution saturation: physical equilibria
 Solubility equilibria and solubility
product constant
 Relative solubilities
 Effect of hydrolysis on solubility
Application to precipitation of slightly
soluble compounds
Factors effecting solubility
o Structure effects
o Pressure effects: Henry’s Law
o Temperature effects on aqueous
solutions
 Solubility curves
Colligative properties
o Calculations involving boiling point
elevation and freezing point depression
o Vapor pressure of solutions
 Raoult’s Law
o Osmotic pressure
Non-ideal solutions
Aqueous systems: solutions, colloids,
suspensions
AP Curriculum
requirements
I B 1a,b
Labs V (AP recommended experiments
1.
Liquid chromatography (#18)
1.
Molar mass by freezing point
depression (#4)
IB3
II B
1,2,3,4
III E 2
II C
1,2,3,4
III C 1
III C 2b(2)
Time
(weeks)
Zumdahl
Chapters
2
Chapter 17
Topics
Electrochemistry





2
Chapter 12
Galvanic cells
Standard Reduction potentials
o Standard half cell potentials
o Complete description of
galvanic cells: prediction of
direction of redox reaction
Cell potential, electrical work, and free
energy
o Relationship of change in free
energy and electrode potentials
Dependence of cell potential on
concentration
o Concentration cells
o The Nernst equation
o Ion selective electrodes
o Calculation of equilibrium
constants for redox reactions
Electrolysis
o Electrolytic cells
o Faraday’s Laws
Chemical Kinetics







Reaction rates
Rate laws
o Differential rate law
o Integrated rate law
Use of experimental data to determine
rate constants, reactant order, and rate
laws:
o Determining the form of rate
law
 Method of initial rates
 Determining a rate law
o Integrated rate law
 First order rate laws
 Half-life of a first order
reaction
 Second order rate laws
 Zero order rate laws
 Integrated rate laws
for reactions with
more than one
reactant
Factors that change the rate of reaction
o Temperature
o Concentration
o Nature of a substance
Energy of Activation
Relationship between rate-determining
step and the reaction mechanism
Catalysts
AP Curriculum
requirements
Labs V (AP recommended experiments
III A 3b,c
III E 4
1.
Electrochemical cells (#21)
1.
Kinetics of a reaction (#12)
IV 1
III D
1,2,3,4,5
IV 1
Time
(weeks)
Zumdahl
Chapters
5
Chapter 14
Topics
Acids and Bases








Chapter 15




1
Chapter 21
Nature of acids and bases
o Arrhenius
o Bronsted-Lowry model
o Acid dissociation constant (Ka)
Calculations involving pH of strong and weak
acid solutions
Water as an acid and base; amphoterism
Percent dissociation
Calculations involving pH of strong and weak
bases
The Lewis acid-base model
Acid-base properties of salts and oxides
Solutions of acids and bases: equilibrium
calculations
Common ion effect
Buffered solutions including buffer capacity
Complex ion formation
Titration calculations and pH curves
o Strong acid-strong base
o Weak acid-strong base
o Calculation of Ka
o Weak base-strong acid
o Acid-base indicators
Nuclear Chemistry ***




AP Curriculum
requirements
Labs V (AP recommended experiments
III A 1
1.
Acid – base titrations (#6, 7)
III C
2b(1),(2),(3)
2.
Selecting Indicators for acid-base
titrations (#11)
3.
Preparation and Properties of Buffer
Solutions (#19)
1.
Separation and Qualitative
Determination of Cations and Anions
(#14)
IV 1
IC
Nuclear stability and radioactive decay
o Types of radioactive decay
o Nuclear equations
Kinetics of radioactive decay
o Half-life
Applications
o Nuclear transformations
o Carbo-14 dating
o Medical applications
Nuclear fusion and fission
3
AP Test Review & Exam
1
Final exam, practical or project
AP Curriculum Requirements
I. Structure of Matter (20%)
A. Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by chemical and physical means
3. Atomic number and mass number; isotopes
4. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation
states
B. Chemical bonding
1. Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
b. Relationships to states, structure, and properties of matter
c. Polarity of bonds, electronegativities
2. Molecular models
a. Lewis structures
b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
c. VSEPR
3. 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
II. States of Matter (20%)
A. Gases
1. Laws of ideal gases
a. Equation of state for an ideal gas
b. Partial pressures
2. Kinetic molecular theory
a. Interpretation of ideal gas laws on the basis of this theory
b. Avogadro’s hypothesis and the mole concept
c. Dependence of kinetic energy of molecules on temperature
d. Deviations from ideal gas laws
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular viewpoint
2. Phase diagrams of one-component systems
3. Changes of state, including critical points and triple points
4. Structure of solids; lattice energies
C. Solutions
1. Types of solutions and factors affecting solubility
2. Methods of expressing concentration (use of normalities is not tested)
3. Raoult’s law and colligative properties (nonvolatile solutes); osmosis
4. Nonideal behavior (qualitative aspects)
III. Reactions (35–40%)
A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism
2. Precipitation reactions
3. Oxidation-reduction reactions
a. Oxidation number
b. The role of the electron in oxidation-reduction
c. Electrochemistry: electrolytic and galvanic cells; Faraday’s laws; standard half-cell potentials; Nernst
equation; prediction of the direction of redox reactions
B. Stoichiometry
1. Ionic and molecular species present in chemical systems: net ionic equations
2. Balancing of equations, including those for redox reactions
3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting
reactants
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier’s principle; equilibrium constants
2. Quantitative treatment
a. Equilibrium constants for gaseous reactions: Kp, Kc
b. Equilibrium constants for reactions in solution
(1) Constants for acids and bases; pK; pH
(2) Solubility product constants and their application to precipitation and the dissolution of
slightly soluble compounds
(3) Common ion effect; buffers; hydrolysis
D. Kinetics
1. Concept of rate of reaction
2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate
laws
3. Effect of temperature change on rates
4. Energy of activation; the role of catalysts
5. The relationship between the rate-determining step and a mechanism
E. Thermodynamics
1. State functions
2. First law: change in enthalpy; heat of formation; heat of reaction; Hess’s law; heats of vaporization and fusion;
calorimetry
3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on
enthalpy and entropy changes
4. 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. These 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 should be covered:
1. Chemical reactivity and products of chemical reactions
2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth
metals, halogens, and the first series of transition elements
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:
• making observations of chemical reactions and substances
• recording data
• calculating and interpreting results based on the quantitative data obtained
• communicating effectively the results of experimental work
AP Recommended Experiments
1. Determination of the formula of a compound
2. Determination of the percentage of water in a hydrate
3. Determination of molar mass by vapor density
4. Determination of molar mass by freezing point depression
5. Determination of a molar volume of a gas
6. Standardization of a solution using a primary standard
7. Determination of concentration by acid-base titration, including a weak acid or weak base
8. Determination of concentration by oxidation-reduction titration
9. Determination of mass and mole relationship in a chemical reaction
10. Determination of the equilibrium constant for a chemical reaction
11. Determination of appropriate indicators for various acid-base titrations; pH determination
12. Determination of the rate of a reaction and its order
13. Determination of an enthalpy change associated with a reaction
14. Separation and qualitative analysis of cations and anions
15. Synthesis of a coordination compound and its chemical analysis
16. Analytical gravimetric determination
17. Colorimetric or spectrophotometric analysis
18. Separation by chromatography
19. Preparation and properties of buffer solutions
20. Determination of electrochemical series
21. Measurements using electrochemical cells and electroplating
22. Synthesis, purification, and analysis of an organic compound