AP CHEMISTRY
Course Description AP Chemistry is designed to prepare you for college chemistry. It is intended to be a very fast
moving course, which hopefully will also prepare you for the AP Exam, and give you the opportunity to earn
college credit. Since it is a weighted course, it also has the possibility to boost your GPA. At the beginning of each
unit, you will be given an outline for that unit. We will attempt to stick to a strict schedule in order to cover the
material necessary to prepare you for the AP Exam. Topics to be covered are listed below. Laboratory activities,
which will include the use of the scientific method, measurement, laboratory apparatus, and safety, are an integral
part of the course. You will be required to maintain a laboratory manual with all lab procedures, data, results and
conclusions. Data will be communicated within a group and between groups. Universities may ask to see this
manual for proof of college-level laboratory experiences.
Unit 1: Chemical Foundations
Recall basic chemistry information such as structure of matter, metric units, dimensional analysis, formula writing
and naming; Solve wavelength/frequency/energy problems; Describe a timeline of atomic theory development
Describe the possible quantum numbers for a given atom; Relate an element's position on the periodic table to its
electron arrangement; Explain periodic trends and exceptions to trends in ionization energy, electron affinity,
atomic radii, ionic radii, and electronegativity
Assignments
Ch 1 Chemical Foundations Problems #23,26,32,34,46, 48,50,56,58,62,70,72,74,80,82,89
Ch 2 Atoms, Molecules & Ions Problems #24,26,32,46,50,52,58,60,62,64,66,68,70,72,74,78,87
Ch 7 Atomic Structure & Periodicity Problems #38,40,42,44,46,50, 62,66,68,70,76,78,80,82,
84,86,88,90,94,96,98,102, 106,111,112,114,117, 120,121,122,126,135
Laboratory Experiments:
Chromatography
- Students separate mixtures of metal ions (Cu2+, N?+, Fe3+) by two different chromatographic techniques.
Ions are identified by chemical reactions and by Rf values
Melting and Boiling Points
- Students determine melting points of 3 solids + unknown solid and boiling points of 3 liquids +
unknown liquid using standard techniques as well as Melt-temp apparatus for melting point.
Unit 2: Stoichiometry
Solve stoichiometry problems (including empirical and molecular formulas, combustion analysis, and limiting
reagent problems)
Assignments:
Ch 3 Stoichiometry & Chemical Equations Problems #18,22,26,30,32,36,54,56a,62,68,70,72,74-76,77,78,80,82,86,90,92,94,
98,100,106,108,110,120,123
Lab Experiments:
Determination of % Cu in Post-82 Pennies
-Zn is reacted with HCI to remove inside of pennies and determine %Cu and savings to government.
Analysis of Alum
-Melting point and % H20 are determined in an alum sample
Unit 3: Chemical Reactions
Balance chemical reactions (including redox) Determine oxidation numbers; write net-ionic reactions; State
solubility rules; Solve molarity and dilution problems; Solve solution stoichiometry problems, including titration,
precipitation, and redox; Predict products of reactions using AP reaction prediction format (including complex ion
reactions)
Assignments
Ch 4 Types of Reaction & Solution Chemistry Problems #12,16,18,22,24,26,28,30,32,34,36,38,42,48,54,56,
58,60,62,64, 66, 68, 73,84,86
Lab experiments:
Chemical reactions
-Students perform many redox and metathesis reactions, make observations, and write equations for
reactions
Household Chemicals (qualitative analysis)
-Students identify ammonium, sulfate, carbonate, iodide, and chloride ions present in household chemicals
and in unknowns
Reactions in Aqueous Solution
-Students react 25 combinations of aqueous solutions to produce metathesis reactions. Observations are
recorded and net ionic reactions are written for each reaction that occurs.
Qualitative Analysis (computer) http://web.umr.edu/-gbert/qual/qual.html
-Ag+, Pb2+, and Hg2+ ions are separated and identified
Reactions of Cu
-Solid Cu is taken through several chemical reactions to eventually reclaim solid Cu; % yield is calculated.
Redox Titration #1 (computer)
http://www .chem.iastate.edu/ group/Greenbowe/sections/projectfolder/flashfiles/redoxN e w/redox.html
3 different redox titrations are performed. Reactions are balanced and stoichiometry is calculated to
determine the concentration of solutions.
Unit 4: Gases, Liquids and Solids
Use the gas laws (Boyle's, Charles', Gay-Lussac's, Dalton's, Combined, Ideal, Graham's, van der Waal's)
to solve problems; Solve gas stoichiometry problems; State and apply the kinetic molecular theory of
gases;
Explain and calculate deviations caused by molecular size and attractions Write equations to
explain chemistry of air pollution and acid rain
Predict-types of intermolecular forces based on bonding; Predict behavior of matter based on type of intermolecular
forces Calculate energy changes involved in phase changes; Describe role of vapor pressure in changes of state;
Interpret a phase diagram; Calculate Born-Haber Cycle problems
Assignments :
Ch 5 Gases Problems #16,22,24,26,30,32,34,40,42, 48,50,52,56,58,60,62,64,66,68,72,74,
78,80,82,84,94,98,102,104,108,112,113,114
Ch 10 Liquids & Solids Problems #36,38-42,50,51,59,71,72,87,88,90,91,94,102,107
Lab Experiments:
Preparation of Gases
-COz, Oz, and Hz gases are prepared. Properties and reactions of these gases are tested.
Molecular Mass of an Unknown Gas
An unknown volatile liquid is vaporized. Using its volume and mass, the molar mass of the liquid is
calculated.
Unit 6: Thermochemistry # 1
Solve enthalpy and calorimetry problems including use of heats of formation, Hess's Law and stoichiometry
Assignments:
Ch 6 Thermochemistry Problems #18,22,24,30,32,34,38,40,42,44,46,48,50,52,54,56,58,
60,62,64,66,68,80, 82, 84,86, 92
Lab Experiments:
Determination of a Calorimeter Constant
-Heat absorbed by a Styrofoam calorimeter is determined using CBL technology.
Hess's Law
-Enthalpy data from the reactions of Mg + HCI and MgO + HCI is used to determine the heat of combustion
of Mg. CBL technology is used to collect temperature
Unit 7: Bonding
Describe the relationship of bond polarity to bond type; Calculate energy involved in the formation of ionic
compounds including lattice energy; Use bond energies to determine enthalpy of reaction;
Draw Lewis structures, predict molecular shapes and bond angles using VSEPR; Draw resonance structures;
Determine bond hybridization and # of sigma and pi bonds;Use Molecular Orbital Bonding Model to determine
bond order and predict stability of molecules.
Assignments:
Ch 8 Bonding Concepts Problems #20,22,26,28,32,34,36,38,40,41,42,46,48,54,56,74, 77,78,80,84,
85,86,88,90,
Ch 9 Covalent Bonds Problems #16,18,20,22,24,29,30,32,34,36,38,42,44,56,63
-
Unit 8: Properties of Solutions
Calculate solution concentration using normality, molarity, molality, mass percent and mole fraction;
Describe and predict solubility based on structure, pressure and temperature Solve Raoult's Law
problems; Calculate boiling point elevation, freezing point depression, vapor pressure lowering and
osmotic pressure changes.
Assignments:
Ch 11Properties of Solutions Problems# 27,28,32,34,3$,36,39,40,42,43,47,48,50,51,52,54,56,6Q,62,64,66,
68,72,74,76,79,90
Laboratory Experiments:
Freezing Point Depression #1
-students prepare ice cream while measuring freezing point depression of ice/water/salt solution and ice
cream solution
Freezing Point Depression #2
- The freezing point of pure tertiary butyl alcohol is determined (using CBL technology). A known amount of
camphor is added to the alcohol and the new freezing point is determined. The fp depression and molar mass
of camphor is calculated.
Unit 9: Kinetics
Write integrated and differential rate laws; Use experimental data graphically to determine order of a reaction ;
Describe the role and action of catalysts; Write possible reaction mechanisms; Use Arrhenius equation to calculate
activation energy
Assignments:
Ch 12 Chemical Kinetics Problems #19,20,21,24,26,28,29,30,37,38,40,46,48,
50,52,56,68,71,74
Iodine Clock Reaction
-Concentration and temperatures of two reactants are varied to determine the order of the reaction and the effect
of temperature changes.
Crystal Violet Decolorization
-Crystal Violet is reacted with NaOH. The color decrease is monitored over time with a colorimeter and data is
graphed to determine the order of the reaction. (60 minutes)
Unit 10: General Equilibrium
Describe the conditions of equilibrium;
Calculate Kc, Kp, or concentrations given initial conditions for solutions and gases using RICE diagrams
Predict effects of stresses on equilibrium (LeChatelier's Principle)
Assignments:
Ch 13 Chemical Equilibrium Problems #21,24,26,28,30,31,32,34,38,40,42,44,48,50,54,56, 60, 62, 64, 66, 67,69,
70, 75, 76,78,82
Laboratory Experiments:
Determination of an Equilibrium Constant
KSCN is reacted with Fe(N03)3 in varying concentrations. Concentrations of FeSCN2+ are determined
colorimetrically. Equilibrium constants are calculated.
LeChatelier's Principle
Various small-scale experiments are performed that involve creating and stressing equilibrium systems.
Unit 11: Acids and Bases
State 3 definitions of an acid and a base; Calculate pH and pOH of strong acid and base solutions Calculate
pH,pOH, Ka, and Kb for weak acid and base solutions; Calculate pH of polyprotic acids; Relate structure of acids
to strength of acids
Assignments :
Ch 14 Acids/BasesProblems #28,30-36,38,39,42,44,46,50,52, 54,57,60,62,63,66,68,70,74,76,
77,78,79,80,82,88,90,92,94,96,98,100,102,103,104,106,108,110, 112,116-118,122,
124,126,130,134,138,142,153
Unit 12: Applications of Aqueous Equilibria
Calculate pH when a common ion is present Write equations for buffer reactions; Predict and calculate acid-base
properties of salts Calculate pH of buffer solutions; Calculate pH at several points during a titration process Choose
correct indicators for titrations; Calculate solubility or Ksp for sparingly soluble salts
Assignments:
Ch 15Aqueous Equilibria Problems #21,22,23,27,29,31;34,36,38,40,42,44,46, 47,50,52,54,55, 56,58, 59,60
70,72,74,76,78,80,82,84,86,88,90,92,94,96,98,101,117 ,119,121
Laboratory Experiments:
Determination of the Ka of Weak Acids
Various weak acids are titrated to the half-equivalence point to determine Ka (using electronic pH meters
Standardization of a NaOH solution
Students prepare a dilute solution of NaOH and standardize it by titrating with potassium phthalate. (90 minutes)
Determination of the Ka and Equivalent Mass of an Unknown Acid
A diprotic acid is titrated with the standardized NaOH. The pH is monitored and graphed with the aid of computer
technology to determine Ka values and equivalent mass.
Determination of the % Acetic Acid in Mustard (Inquiry Lab)
Students titrate mustard packets with NaOH to determine % acetic acid.
Unit 13: Thermochemistry #2
Describe entropy and the 2nd Law of Thermodynamics Calculate entropy; Calculate free energy
Solve free energy-equilibrium problems
Assignments:
Ch 16 Spontaneity, Entropy & Free Energy Problems #18,22,23,24,27,28,30,32,34,36,38,40,42,44,45,50,52, 56,
58,60,61, 64, 72, 74, 77
Unit 14 : Electrochemistry
Sketch and describe galvanic cells Calculate cell potentials; Use reduction potentials to predict reactivity; Use the
Nernst equation; Describe types of batteries; Predict reactions occurring in electrolysis; Calculate current or mass of
substance consumed or plated out in electrolysis problems; Calculate free energy and cell potential relationships
Assignments:
Ch 17 Electrochemistry Problems # 14,16,26,28,30,32,34,36,38,40,44,48,50,52,55,57,62,
64,70,71,74,79,80,81,84,86,90,93,94,99,100,102
Laboratory Experiments:
EleCtrochemical Cells
Small-scale voltaic cells are prepared with Zn, Cu, Ag, Fe, AI, and Mg. Standard cell potential is measured to
determine relative electrode potentials. Concentrations are varied to investigate the Nernst equation. Reactions
are performed to determine Ksp and Kfvalues from voltages.
Analysis of Bleach
Bleach is diluted and titrated with sodium thiosulfate to determine the % NaOCl. The end point is determined
by the decolorization of an iodine-starch complex.
Unit 15: Orga,nic, Nuclear, and Descriptive Chemistry
Write equations for nuclear reactions; List properties of various types of radioactivity; Compare and contrast
nuclear fusion and fission; Predict stability of isotopes; Name hydrocarbons; Identify functional groups; Name
simple hydrocarbon derivatives such as alcohols, ketones, aldehydes, amines, ethers and esters; Draw isomers of
organic compounds; Identify colors of solutions, precipitates, flame tests, indicators, etc.; Investigate descriptive
chemistry in greater detail, including periodic relationships
Assignments:
Worksheets on nuclear, organic and descriptive chemistry
Laboratory Experiments:
Preparation of Aspirin
Aspirin is prepared. % Yield is calculated and melting point is determined.
Tye-Dyeing
Students tye dye items of their choosing with fiber reactive dyes.
Nuclear .Shielding
Alpha, beta and gamma emitters are tested with various sources of shielding using radiation
monitors.