1. Ingeniería

AP Chemistry Syllabus
Course Overview
The purpose of Advanced Placement Chemistry is to provide a college level course in
chemistry and to prepare the student to seek credit and/or appropriate placement in
college chemistry courses. This course meets five times per week and with several after
school and Saturday sessions for review and additional laboratory time. There is also a
four day ‘AP Chemistry Boot Camp’ in summer to review first year Chemistry and to
perform some introductory laboratory work. Students are engaged in hands-on laboratory
work, integrated throughout the course that accounts for 25% of instructional time.
This course is structured around the six Big Ideas articulated in the AP Chemistry
curriculum framework provided by the College Board.
Chapters in Zumdahl Chemistry
1. Chemical Foundations
2. Atoms, Molecules, and Ions
3. Stoichiometry
4. Solution Stoichiometry
5. Gases
6. Thermochemistry
7. Atomic structure and Periodicity
8. Bonding – General Concepts
9. Covalent Bonding: Orbitals
10. Liquids and Solids
11. Properties of Solutions
12. Chemical Kinetics
13. Chemical Equilibrium
14. Acids and Bases
15. Aqueous Equilibrium
16. Spontaneity, Entropy, Free Energy
17. Electrochemistry
18. Nuclear Chemistry
19. Organic Chemistry
AP Chemistry Topic Covered
None
Atomic Theory & Atomic Structure (BI 1 & 2)
Stoichiometry (BI 3)
Reaction Types & Stoichiometry (BI 3)
Gases (BI 1 & 2)
Thermodynamics (BI 5)
Atomic Theory & Atomic Structure (BI 1& 2)
Chemical Bonding (BI 1& 2)
Chemical Bonding (BI 1 & 2)
Liquids and Solids (BI 1 & 2)
Solutions (BI 2)
Kinetics (BI 4)
Equilibrium (BI 6)
Equilibrium (BI 6)
Equilibrium (BI 6)
Thermochemistry (BI 5)
Reaction Types (BI 3)
Nuclear Chemistry
Descriptive Chemistry (BI 2)
(BI) refers to Big Ideas. Big Idea 1 – Structure of Matter, Big Idea 2 – Properties of Matter:
Characteristics, States and Forces of Attraction, Big Idea 3 – Chemical Reactions, Big Idea 4 – Rates of
Chemical Reactions, Big Idea 5 – Thermodynamics, Big Idea 6 – Equilibrium.
Texts
Zumdahl, Steven and Susan Zumdahl. (2007) Chemistry 7th Ed. Boston: Houghton
Mifflin Co.
Hague, George and Jane Smith (2001) The Ultimate Chemical Equations Handbook.
Batavia, IL: Flinn Scientific (Supplemental)
Lab Manuals
The lab portion of the course is taken from a variety of sources including the following:
Vonderbrink, Sally Ann. Laboratory Experiments for Advanced Placement Chemistry.
Second edition. (Noted as VDB in Course Outline)
Flinn ChemTopic Labs series. (Noted as Flinn in Course Outline)
College Board. AP Chemistry Guided Inquiry Experiments.
(Noted as CB in Course Outline)
Teacher Generated Labs – labs that I made up or don’t remember where I got them
(Noted as TG in Course Outline)
AP Chemistry Course Outline
Weeks / Dates
Chapter / Topics / Labs
1
01 Foundations of Chemistry
Scientific Method
BI 1.D.1:a
Classification of Matter
1.A.1:b; 1.A.1:c; 1.A.1:d
Chemical/ Physical Changes 3.C.1:b; 3.C.1:c; 5.D:2
Nomenclature
1.E.2:b
02 Atoms, Molecules, Ions
Atomic Number and Mass 1.A.1:a
Periodic Table (Groups)
Moles Concept
1.A.3:b; 1.A.3:c; 1.A.3:d; 1.E.2:b
8/31 – 9/4
Curriculum Alignment
LABS:
Analysis of Alum (VDB 04)
SP 2-6; LO 1.4
Densities of Solids and Liquids (TG) SP 3-6; LO 1.3,1.4
Properties of Elements (TG)
SP 3; LO 1.1
Guided Inquiry: Proving a Solution is
SP 2-7; LO 1.2,2.10
a Homogeneous Mixture (TG)
2
9/7 – 9/11
03 Stoichiometry
Chemical Equations
1.E.1:a; 1.E.1:c; 3.C.1:a
Percent Composition
1.A.2:a
Empirical Formula
1.A.2:b
Balancing Equations
1.A.3:a; 1.E.2:c; 1.E.2:d; 3.A.1:a
Stoichiometric Calculations 1.A.3:a; 1.E.1:b
Limiting Reagent / %Yield 3.A.2:a
2
Sample Activity:
LO 3.6 Use data from synthesis or decomposition of a
compound to confirm the conservation of matter and the
law of definite proportions.
Students present problems to the class in which they
demonstrate how to find the empirical formula of a
compound from data on the percent composition by mass.
LABS:
Guided Inquiry: Empirical Formula of Ag2O (VDB)
35
9/14 – 10/2
SP 2-6; LO 1.4,3.1
04 Chemical Reactions and Solutions Stoichiometry
Properties of Water
2.A.3:h
Molarity / Concentration
1.D.3:c; 2.A.3:i; 2.A.3:j
Precipitation and Solubility 6.C.3:d
Acid-Base Rx/Titration
1.E.2:f; 3.A.2:c
Oxidation-Reduction Rx 3.B.3:a; 3.B.3:b; 3.B.3:c; 3.B.3:d
Gravimetric Calculations
1.E.2:e
Types of rx (add,decomp..) 3.A.1; 3.B.1.a; 3.B.3:e; 3.C.1:d
Sample Activity
LO 1.20 The student can design, and/or interpret data
from, an experiment that uses titration to determine the
concentration of an analyte in a solution.
As a pre-lab, students use sample titration data to calculate
the unknown concentration of an acid that has been titrated
with a base.
LABS:
Properties of Solutions (TG)
SP 1,7; LO 2.1, 2.8
Ratio of Moles of Reactants (VB 05) SP 2,4,5,6; LO 2.9,3.2,3.3,3.4
Analysis of a Metal CO3 (VDB 03) SP 2-6; LO 3.5
67
10/5 – 10/16
05 Gases
Laws: Boyles, Charles, Ideal
Kinetic Molecular Theory
Diffusion and Effusion
Partial Pressures
Gas Stoichiometry
Deviation from Ideal
2.A.2:b; 2.A.2:c
2.A.2:d; 5.A.1
2.A.2:b
3.A.2:b
2.A.2:e; 2.A.2:f; 2.A.2:g;
2.B.2:c; 2.B.2:d
3
LABS:
Gas Law Demonstration Labs (TG) SP 1,7; LO 2.4,2.5
Boyles Law (TG)
SP 1,2,4,7; LO 2.6
Charles's Law and Absolute Zero (Flinn) SP 4,5,6; LO 2.6
Molar Volume of Gases (VDB 08) SP 2,3,4,5; LO 2.6,2.12,3.3,3.4
Guided Inquiry: Using Color to Determine % Cu in Brass (CB2)
SP 4,5; LO 1.16,2.25
89
10/19 – 10/30
06 Thermochemistry
Conservation of Energy, Work
5.B.1; 5.E.2:a
Potential Energy Diagrams 3.C.2; 5.C.2:c; 5.C.2:d; 5.C.2:e
Calorimetry
5.A.2; 5.B.2; 5.B.3:a; 5.B.3:b; 5.B.4
Hess's Law
5.B.3:a
Enthalpy's of Formation
5.C.2:g
Endothermic, Exothermic
3.C.2; 5.B.3:e; 5.B.3:f
Sample Activity:
LO 4.8 Translate among reaction energy profile
representations particulate representations, and symbolic
representations (chemical equations) of a chemical reaction
occurring in the presence and absence of a catalyst.
Students create energy diagrams to explain why catalysts
and raising the temperature can increase the rate of a
chemical reaction.
LABS:
Measuring Specific Heat of Iron (TG) SP 2-6; LO 3.11,5.3,5.4,5.5
Determining Unknown by Specific Heat (TG) SP 2-6; LO 5.7
Heat of Combustion of Paraffin (TG) SP2-6; LO 3.11,5.6
Measuring Calories (Flinn)
SP 2-6; LO 3.11,5.6
Guided Inquiry: Hess’s Law (VDB 06) SP 2-6; LO 3.11, 5.3-5.5, 5.7, 5.8
10  11
07 Atomic Structure and Periodicity
Electron Configurations
1.B.2:a
11/2 – 11/13
Valence Electrons/ Lewis Dot 1.B.2:c
Props of Light and Waves
1.C.2:e; 1.D.3:a; 5.E.4:b
Bohr Model
1.B.1:d; 1.B.1:e; 1.D.3:b
Quantum Mechanics
1.C.2:d
Electron Orbitals /Shapes
1.C.2:b; 1.C.2:c
Spectroscopy
1.D.2:a; 1.D.2:b; 1.D.2:c; 1.D.3:b
Arrangement of Per Table
1.C.1:a; 1.C.1:b; 1.C.1:d
4
Periodic Trends
1.B.1:b; 1.B.1:c; 1.B.2:b;
1.B.2:d; 1.C.1:c; 1.D.1:b;
2.C.1:a; 2.C.1:b
LABS:
Flame Tests (Measuring Atomic Emissions) (Flinn) SP 5,6,7
LO 1.12
H Atom and Quantum Mechanics (TG)
SP 1,2,6
LO 1.5,1.6,1.7,1.8
Properties of Metals and Nonmetals (Flinn) SP 3,7
LO 2.20,2.26,3.1
12  14
08 Bonding
Lewis Structures
11/16 – 12/11
Structure and Bonding
2.C.4:a
2.A.1:a; 2.A.1:d; 2.C.3;
2.D.1:a; 2.D.2:a; 2.D.1:b;
2.D.3; 2.D.4
Resonance / Formal Charge 2.C.4:c; 2.C.4:d; 2.C.4:e
Bond Polarity / Dipoles
2.C.1:c; 2.C.1:e; 2.C.1:f
Molecular Shapes
2.C.4:b; 2.C.4:e; 2.C.4:f
Bond Energies
2.C.1:d; 5.C.1; 5.C.2:a; 5.C.2:b
Lattice Energies
1.B.1:a; 1.C.2:a; 2.C.1:d
2.C.2A; 2.C.2:b; 2.D.1:b
09 Molecular Orbitals
Hybridization
2.C.4:g
Molecular Orbital Diagrams 2.C.4:h; 2.C.4:i
Sample Activity:
LO 2.21 Use Lewis diagrams and VSEPR to predict the geometry
of molecules, identify hybridization, and make predictions about
polarity.
Students construct balloon models of the arrangement of pairs of
electrons around a central atom. They the draw 20 pictures of
these arrangements and apply these to predicting the shapes of
molecules.
LABS:
Molecular Models Lab (TG)
Cations and Anions (VDB 19)
15  16
12/14 – 1/8
10 Liquids and Solids
Intermolecular Forces
SP 1,6,7; LO 2.1,2.21
SP 3,6; LO 2.3,2.23,2,24
2.A.1:b; 2.B.1:a; 2.B.1:b
2.B.1:c; 2.B.2:a; 2.B.2:c
2.B.2:d; 2.B.3:a; 5.D.1
5
Heating and Cooling Curves 2.A.1:e; 5.B.3:c; 5.B.3:c
Composition of Solutions 2.A.1:c; 2.A.3:b; 2.A.3:c; 2.B.2:d
Colloids and Suspensions
2.A.3:a; 2.A.3:b; 2.A.3:g
Separation Techniques
2.A.3:e; 2.A.3:f
Effect on Biological Systems 2.B.3:e; 2.D.3; 5.E.4:c
LABS:
Molar Mass of Volatile Liquid (VDB 09) SP 2,5; LO 2.4, 2.5, 5.2
Liquid Chromatography (VDB 10)
17  18
SP 1,3,7; LO 2.9,6.21
11 Properties of Solutions
Electrolytes, Nonelectrolytes
Molarity
Mole fraction
Colligative Properties
1/11 – 1/22
LABS:
Determining Solubility Product Constant
of an Ionic Compound (VDB 18)
19  20
12 Chemical Kinetics
Reaction Kinetics
1/25 – 2/5
Rate Law Expressions
Rate Constant
Activation Energy
Reaction Mechanisms
SP 2,4,5,6
LO 2.9,6.21,6.24
4.A.1:a; 4.A.1:b; 4.A.1:c
4.D.1; 4.D.2
4.A.2:a; 4.A.2:b; 4.A.2:c
4.A.3
4.B.2; 4.B.3:c
4.B.1; 4.B.3:a; 4.B.3:b
4.C.1; 4.C.2; 4.C.3
LABS:
Rates of Reaction (Catalyst) (Flinn) SP 4,5; LO 4.2,4.4,4.5
Kinetics of a Chemical Rx (VDB 12) SP 2,5; LO 4.5,4.6
Guided Inquiry: Determining the Rate Law SP 2-6; LO 4.2,4.3,4.4
of a Crystal Violet Rx
21  22
2/8 – 2/19
13 Chemical Equilibrium
Characteristics of Equilibrium 6.A.1; 6.A.3:a; 6.A.3:f
Equilibrium Expressions
6.A.3:b
Factors that Affect Equil
6.A.3:c
LeChateliers Principle
6.A.3:b; 6.B.1; 6.B.2
6.C.3:e; 6.C.3:f
Equilibrium Constant
6.A.3:d; 6.A.3:e; 6.A.4
Solving Equilibrium Problems 6.A.2
6
Sample Activity
LO 6.8 The student is able to use Le Chatelier’s principle to
predict the direction of the shift resulting from various
possible stresses on a system at chemical equilibrium.
Students use Le Chatelier’s principle predict the direction
of the shift when reactants or products are added or
removed from a system at equilibrium.
LABS:
Restoring Balance (Equilibrium) (Flinn) SP 3,5; LO 6.4,6.5,6.6
Determining Keq for FeSCN (VDB 13) SP 2,3,5; LO 3.8,3.9
23  25
14 Acids and Bases
Nature of Acids and Bases
3.B.2; 6.C.1:c; 6.C.1:d
6.C.1:e; 6.C.1:f
Kw and pH
6.C.1:a; 6.C.1:b; 6.C.1:g
Strong - Weak Acids and Bases 6.C.1:h
Polyprotic Acids
6.C.1:n
2/22 – 3/12
15 Aqueous Equilibria
Common Ion Effect
Buffers
Titrations and pH Curves
Ksp Solubility Product
6.C.2
6.C.1:i; 6.C.1:j; 6.C.1:k;
6.C.1:l; 6.C.1:m
6.C.3:a; 6.C.3:b
LABS:
Determination of Ka for
Weak Acids (VDB 14)
Acid-Base Titrations (VDB 15)
Guided Inquiry: How Long Will That
Marble Statue Last?
SP 2,4,5,6
LO 2.2, 6.13
SP 2,4,5,6; LO 2.2,6.13
SP 3,4,5
Sample Activity:
LO 3.2 The student can translate an observed chemical
change into a balanced chemical equation and justify the
choice of equation type (molecular, ionic, or net ionic) in
terms of utility for the given circumstances.
Students conduct an investigation into the major
components of acid rain and write the reactions that occur
between the pollutant and the compounds naturally present.
7
26
16 Spontaneity, Entropy
Gibbs Free Energy
5.E.2:d; 5.E.2:e; 5.E.2:f
6.C.3:c; 6.D.1:a
Spontaneity
5.E.1; 5.E.2:c; 5.E.3
Entropy
5.E.1
Free Energy & Equilibrium5.E.2; 6.D.1:b; 6.D.1:c; 6.D.1:e
Rate and Spontaneity
5.E.2:e; 5.E.5
3/15 – 3/19
Sample Activity:
LO 5.13 The student is able to predict whether or not a
physical or chemical process is thermodynamically favored
by determination of (either quantitatively or qualitatively)
the signs of both ΔH and ΔS, and calculation or estimation
of ΔG when needed.
Students solve problems in which they qualitatively and
quantitatively predict the signs and magnitude of ΔH, ΔS,
and ΔG from a set of thermochemical data.
27  28
17 Electrochemistry
Balancing Redox
3.B.3:a-d
Cell potential
3.C.3:a; 3.C.3:b; 3.C.3:c; 5.E.4:a
Nernst Equation
3.C.3:d
Spontaneous/ Nonspontaneous 3.C.3:e
Chemical Applications
3.C.3:f
3/22 – 4/9
LABS:
Electrochemical Cells (VDB 22)
SP 2,4,5,6; LO 3.12,3.13,3.14
Electrolysis (VDB 23)
SP 2,4,5,6; LO 3.12,3.13,6.25
Oxidation-Reduction Titrations (VDB 20) SP 2,5,6 LO 3.8,3.9
29
18 Nuclear Chemistry
Radioactive Decay
Half Life
Nuclear Fission and Fusion
4/12 – 4/16
30
19 Coordination Compounds
Complex Ions
4/29 – 4/30
LABS:
Analysis of Tetraamine CuSO4 (VDB 24)
31
4/26 – 4/30
SP 5
20 Organic Chemistry
Hydrocarbons
Functional Groups
Polymers
8
Biological Molecules
Isomerism
LABS:
Molecular Models (TG)
Purification of an Ester (VDB 25)
32
33  40
SP 1,6,7; LO 2.1,2.21
SP 5
AP Exam May 5
LABS:
Unknowns Lab (TG)
SP 3,4,5
Lab Schedule and Descriptions
All of the laboratory experiments in this course are hands-on. Students work individually
or in a group of two depending upon the lab. They collect, process, manipulate, and
graph data from both qualitative and quantitative observations. Inquiry is emphasized in
many of the experiments that students complete. The lab work requires students to
design, carry out, and analyze data using guided inquiry principles. For all labs, students
are required to report the purpose, procedure, all data, data analysis, error analysis,
results, and conclusions in a lab report that is submitted for grading. A laboratory
notebook is required for the course. All completed lab reports documenting all lab
experiences must be included in the notebook. The notebook is checked every nine
weeks and at the end of the course.
These are the labs that will be performed over the course of the year:
Analysis of Alum (VDB 04)
Students perform a series of experiments to determine the chemical and physical
properties of aluminum potassium sulfate (alum). Analyses include percent
composition, water of hydration, and molecular formula.
Densities of Solids and Liquids (TG)
Students determine the densities of various solids and liquids and then use density
to identify and unknown substance.
Properties of Elements (TG)
Students observe the properties of several Group I and Group II elements,
including their reactivity with water.
Proving a Solution is a Homogeneous Mixture (TG)
Students are asked to design and perform an experiment to prove that a 1.0 M
NaCl solution is a homogeneous mixture.
9
Empirical Formula of Silver Oxide (VDB 01)
Students determine the percent composition and empirical formula of silver oxide.
Properties of Solutions (TG)
In a series of short experiments students will observe and measure the effects of
certain conditions on solvation and solubility. Some examples are solubility of
gases versus temperature, heat of solution, and effect of particle size on speed of
dissolving.
Ratio of Moles of Reactants (VDB 05)
Students determine the mole ratio of 2 reactants by using the method of
continuous variations. The change of temperature is the property that is
measured.
Gravimetric Analysis of a Metal Carbonate (VDB 03)
Students will determine the identity of a Group I metal carbonate compound by
gravimetric analysis.
Activity Series (VDB 07)
Students will determine the activity series for 5 metals and for 3 halogens.
Gas Law Demonstration Labs (TG)
Students will perform a series of demonstrations of the properties of gases and use
the kinetic molecular theory to generate plausible explanations for the observed
behaviors.
Boyles Law (TG)
Students verify Boyle’s Law by adding weights to the plunger of a closed syringe.
Charles’s Law and Absolute Zero (Flinn)
Students verify Charles’s Law using air trapped inside sealed syringes that are
placed in cold and hot water baths.
Molar Volume of Gases (VDB 08)
Students will determine the volume of one mole of hydrogen gas at STP.
Using Color to Determine % Cu in Brass (CB 2)
Students use spectrophotometry and Beer’s law to determine what percent of a
brass screw is copper.
Guided Inquiry: Hess’s Law (Based on VDB 06)
Students will design and perform an experiment to verify Hess’s law by
measuring the temperature change for 3 acid-base reactions.
10
Measuring Specific Heat of Iron (TG)
Students will calculate the specific heat of iron by measuring the increase in
temperature of a known mass of water.
Determining Unknown By Specific Heat (TG)
Students will identify an unknown metal by determining its specific heat and
comparing to a table of known specific heats.
Heat of Combustion of Paraffin (TG)
Students will use a calorimeter to calculate the heat of combustion in calories per
mole for candle wax.
Measuring Calories (Flinn)
Students will measure the calories contained in various food products (Fritos) by
calorimetry.
Flame Tests (Measuring Atomic Emissions) (Flinn)
Students will observe the characteristic flame test colors of different metal
compounds and calculate the wavelengths and frequencies of the various light
emissions.
H Atom and Quantum Mechanics (TG)
Students will calculate and graph the relative energies of principle energy levels
in an H atom and prepare a ruler to measure the amounts of energy given off for
each possible level change. Then students will determine which transitions are
responsible for the 4 bands in the H spectrum.
Properties of Metals and Nonmetals (Flinn)
Students will test the properties of various metals and nonmetals.
Molecular Models Lab (TG)
Students will determine the Lewis structure of 20 different molecular compounds
and construct and ball and stick model to help them determine their geometries
and polarities.
Determination of Cations and Anions (VDB 19)
Students will analyze a solution that contains an unknown combination of anions
and cations and determine the formula.
Molar Mass of Volatile Liquids (VDB 09)
Students will determine the molar masses of various volatile liquids.
Liquid Chromatography (VDB 10)
Students will use liquid chromatography to separate the components of Kool-Aid
using Sep-Pak C18 columns.
11
Determining Solubility Product Constant of an Ionic Compound (VDB 18)
Students will determine the Ksp for Ca(OH)2 through a series of dilutions and
precipitations.
Proving a Solution is Homogeneous (TG)
Students design and execute a procedure to prove that a 1.0 M NaCl solution is
homogeneous.
Rates of Reaction and Effect of Catalyst (Flinn)
Students will determine the effect of a catalyst on reaction rate.
Determining the Rate Law of a Crystal Violet Reaction (CB11)
Using calorimetry and Beer’s law, students determine the order of a reaction and
its rate law.
Kinetics of a Chemical Reaction (VDB 12)
Students will determine the total rate law for the oxidation of iodide ions by
bromate ions in the presence of an acid.
Restoring Balance (Le Chatelier’s Principle) (Flinn)
Students will determine the effects of reaction conditions on the reversible
formation of cobalt complex ions. The effects that will be studied and addition of
a reactant or product, removal of a reactant or product, and changing temperature.
Determining Keq for FeSCN (VDB 13)
Students will calculate the equilibrium constant for the reaction of iron (III) ions
with thiocyanate ions.
Determination of Ka for Weak Acids (VDB 14)
Students will determine the pKa values for ionization of two unknown weak acids.
Acid – Base Titrations (VDB 15)
Students will standardize a sodium hydroxide solution and use the standard
solution to titrate an unknown solid acid.
How Long Will That Marble Statue Last? (CB 10)
Students investigate how the speed of the chemical reaction between solid
calcium carbonate and a solution of hydrochloric acid is affected by changing
variables relating to the two reactants.
Electrochemical Cells (VDB 22)
Students will construct a “standard” table listing the reduction potentials of a
series of metal ions and then use the Nernst equation to measure the voltage of a
cell.
12
Electrolysis (VDB 23)
Students will set up an electrolysis cell and electrolyze an acid solution of copper
sulfate and calculate the value of Avogadro’s number and the value of the
faraday.
Oxidation – Reduction Reactions (VDB 20)
Students will standardize a solution of potassium permanganate by redox titration
with a standard solution of iron (II) ions. Then the standard solution is used to
determine the concentration of an oxalic acid solution.
Analysis of Tetraamine CuSO4 (VDB 24)
Students will prepare a solution of tetraamine copper sulfate and analyze it by
plotting its absorbance spectrum at various wavelengths. Then the solid will be
crystallized and students will calculate the percent yield.
Organic Molecular Models (TG)
Students will use ball and stick models to build and observe the geometries of
basic hydrocarbons and functional groups.
Purification of an Ester (VDB 25)
Students will produce ethyl acetate through an esterification reaction and
determine its percent yield.
13