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Topic/Objective
Unit 1 Matter and measurement
 Measurement and units
 Use of significant figures
 Dimensional analysis
 Classification of matter
Unit 2 Atoms, molecules and ions
 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
 Naming compounds
Unit 3 Stoichiometry
 Stoichiometry
1. Balancing of
equations
2. Mass and volume
relations with
emphasis on the mole
concept, including
empirical formulas
and limiting reactants
 Chemical reactivity
 Percent composition of
compounds
Unit 4 Reactions in water and
stoichiometry
 Precipitation reactions
 Ionic and molecular
species present in chemical
systems: net ionic
equations
 Oxidation-reduction
reactions
a. Oxidation number
b. The role of the
electron in
oxidation-reduction
 Strong, weak and
nonelectrolytes
 Concentration & Stoich
Unit 5 Thermochemistry
 State functions
 First law of
thermodynamics

change in enthalpy
 heat of formation

heat of reaction

Hess’s law;
Unit 6 Thermodynamics
 Entropy

free energy of formation;
Section
Ch
1
1.4-1.5
1.5
1.6
1.2
2
AP Outline: First half
HW
Lab
HW1: Read
Title: Safety and Equipment in lab
Ch1, #1, 25, 37,
45, 65
Objective: To teach students proper safety techniques
and get them familiar with lab equipment
HW1: Read
Ch2, 21, 41, 47,
55,
2.1-2.3
HW2: 59, 65,
61, 89
2.4
Title: Qualitative analysis of cations and anions
(exp14)
Objective: To determine the identity of unknowns by
testing for the presence of various ions.
2.5
2.6-2.8
3
3.1
3.3-3.7
HW1: Read
CH3, 11, 19,
20, 23, 33
HW2: 43, 49,
51, 59, 71,
Title: Soichiometry in synthesis of ionic compound
(exp9)
Objective: Potassium alum is produced and the
percent and theoretical yield of the compound is
calculated
Title: Empirical formula of a hydrate (exp2)
3.2
3.3
Objective: Find the empirical formula of a hydrate
by heating it in a crucible and then determining the
moles of the hydrate from mass measurements.
4
4.2
4.2
HW1: Read Ch
4 : 15, 19, 27,
41, 49
HW2: 61, 67,
69, 85, 92
Title: Finding the ratio of moles of reactants in a
chemical reaction (exp1)
Objective: Find the coefficients for two chemical
reactants that appear in a balanced chemical reaction
Title: An Activity series (exp20)
Objective: The activity series for five metals and
three halogens are determined
4.4
4.4
4.3
4.5-4.6
5
5.1
5.2
5.3
5.4
5.5
5.6
HW2: 63, 67,
72, 75,
19
19.1-19.4
HW 1:Read
Ch5, 39, 45, 53,
61
HW1: Read Ch
19, 31, 37, 39,
47,
Title: Thermochemistry and Hess’s Law. (exp13)
Objective: The enthalpy of a reaction is determined
from its three different chemical reactions using
Hess’s law.
Title: Analysis of a coordination compound (exp15)
Objective: A coordination compound is synthesized
free energy of reaction;
Dependence of change in
free energy on enthalpy
and entropy changes
 Relationship of change in
free energy to equilibrium
constants and electrode
Unit 7 Electrochemistry
 Balancing of redox
reactions
 electrolytic and galvanic
cells

Faraday’s laws; standard
 half-cell potentials
 Nernst equation

prediction of the direction
of redox
reactions
 Batteries & Corrosion
Unit 8 Nuclear chemistry
 nuclear equations

half-lives, and
radioactivity;
 chemical applications
19.5

Unit 9 Quantum mechanics
 Electron energy levels:
atomic spectra, quantum
numbers, atomic orbitals
Unit 10 Bonding
 Binding forces
a. Types: ionic, covalent, metallic
b. Polarity of bonds,
electronegativities
c. Bond energies, enthalpy and
chemical reactions
 Molecular models
a. Lewis structures
b. Valence bond:
hybridization of orbitals,
resonance, sigma and pi
bonds
c. VSEPR
Unit 11 Gases
 Laws of ideal gases
a. Equation of state for
an ideal gas
b. Partial pressures
 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
HW2: 51, 53,
55, 63,
19.6
from a transition metal ion that is in solution. The
compound is filtered from the solution and tested in
various ways to determine the composition of the
substance.
19.7
20
20.1-20.2
HW1: Read Ch
20, 9, 11, 13,
19
20.3, 20.9
HW2: 23, 35,
51, 59, 93
20.5
20.4
Title: Electrochemical cells (exp21)
Objective: Half cells are constructed using different
metals with the zinc half cell chosen as a reference
standard with all potentials measured with respects to
it. In addition the Nernst equation is used to measure
the potential of a nonstandard solution and to find the
concentration of a complex ion.
20.6
20.5
20.7-20.8
21
21.1-213
21.4
21.5, 21.9
HW1: Read Ch
21, #11,17, 27
HW2: 29,57, 65
6
HW1: Read
CH6,5,25,49,51
HW2: 53, 67,
71, 73
.
8,9
HW1: Read
Ch8, #7,19, 37,
61, 65, 69
Title: Molecule building
6.1-6.9
8.1-8.3
Hw2: Read 9.19.6, # 35, 43,
47, 51, 96
8.4
Objective: The Lewis dot structure of different
covalent compounds are drawn and the respective
models are built using ball and stick model kits.
Polarity, molecular shape and bond angles are also
determined.
8.8
8.5
8.6,8.7,
9.5, 9.6,
9.1-9.3
10
10.1-10.5
10.6
10.7-10.8
10.3
10.7
10.9
HW1: Read Ch
10, # 31, 35,
39, 53,
HW2: 63, 73
105,
Title: Molecular mass of a volatile liquid (exp3)
Objective: A small amount of a volatile liquid inside
a small test tube and then heated in boiling water until
all the liquid vaporizes and fills the tube as excess
water escapes. After the gas is cooled, the mass,
volume, and pressure is measured to determine the
molecular mass of the substance using ideal gas law
Title: Determination of the molar volume of a gas
(exp 5)
Objective: A sample of a solid substance is heated,
decomposing it into several products, including a gas.
The mass of the gas is determined by the weight
difference before and after heating and is then
converted to moles. The volume of the gas, the
pressure, and the temperature are measured.
Topic/Objective
Section
Ch
Unit 12 Liquids and Solids
11
 Binding forces
11.2
a. hydrogen bonding
11.2
b. van der Waals
(including London
dispersion forces)
11.1
c. Relationships to states,
structure, and
properties of matter
11.3, 11.5,
 Gases, Liquids and solids from
the kinetic-molecular viewpoint 11.8
 Phase diagrams of one11.6
component systems
 Changes of state, including
critical points and triple points
11.4
 Structure of solids; lattice
energies
Second half
HW
Lab
HW1: Read
Ch11, # 6, 19,
25, 33
HW2: 45, 53,
55, 77, 79
11.7
Unit 13 Properties of solutions
 Types of solutions and
factors affecting solubility
 Methods of expressing
concentration (use of
normalities is not tested)
 Raoult’s law and
colligative properties
(nonvolatile solutes);
osmosis
 Nonideal behavior
(qualitative aspects)
Unit 14 Kinetics
 Concept of rate of reaction
 Use of experimental data
and graphical analysis to
determine reactant order,
rate constants, and reaction
rate laws
 Effect of temperature
change on rates
 Energy of activation; the
role of catalysts
 The relationship between
the rate-determining step
and a mechanism
Unit 15 Chemical Equilibrium
 Concept of dynamic
equilibrium, physical and
chemical

Le Chatelier’s principle
 equilibrium constants
 Equilibrium constants for
gaseous reactions: Kp, Kc
13
13.1-13.3
13.4
HW1: Read Ch
13, # 21 27, 35,
41
HW2: 43, 47,
57, 65
13.5
Title: Molecular mass by freezing point depression
(exp4)
Objective: After first determining the freezing point
of a pure substance, the freezing point of a solution is
determined. The change in freezing point allows
calculation of the freezing point depression constant.
This constant is then used to help determine the
molecular mass of an unknown substance.
13.6
14
14.1-14.2
HW1: Read
Ch14, #,21, 23,
27, 29,
14.3-14.4
HW2: 65, 67,
84,
Title: Study of the kinetics of a reaction (exp12)
Objective: The total rate law for the oxidation of
iodide by bromate ion in the presence of an acid is
determined. The order for each of the reactants is
found by varying the concentration of each reactant
individually. Once the rate law is determined then the
rate law is calculated and the activation energy is also
determined.
14.5
14.5,14.7
14.6
15
15.1, 15.4,
15.7
15.2-15.3,
15.5-15.6
15.2
HW1: Read
Ch15, #13, 27,
33, 37
HW2: 43, 45,
49, 51,
Title: Determination of the equilibrium constant of
an ionic compound (exp10)
Objective: The solubility product of calcium
hydroxide is determined using calcium nitrate,
vinegar and sodium hydroxide.
Title: Equilibrium and LeChatelier’s Principle
Objective: Students will apply various stresses to a
system and use LeChatelier’s principle to predict the
effect of the various stresses.
Unit 16 Acids and Bases
 Acid-base reactions

concepts of Arrhenius,
Brønsted-Lowry, and
Lewis
 coordination complexes;
amphoterism
16, 17
16.1
16.2-16.5,
16.11
HW2: 65,87,93,
101
17.5
HW3: Read Ch
17, # 21, 31, 33,
41

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
Unit 17 Organic Chemistry
 Introduction to organic
chemistry: hydrocarbons
and functional groups
(structure,
nomenclature,
chemical properties)
 structural isomerism of
simple organic molecules
and coordination
complexes
Review
Lab Work after exam
HW1: Read
Ch16, # 29, 37,
43, 55
Title: Determination of the dissociation constant of
weak acids (exp7)
Objective: A small amount of unknown acid is
dissolved in distilled water with half of the resulting
solution poured into a different container. Sodium
hydroxide is added to the solution to neutralize it,
forming a solution of the salt of the acid. The acid
and salt solution are then combined and the pH is
measured using a pH meter with the pH equaling the
pKa.
HW4: 65, 73,
81, 96,
16.6-16.8
17.6-17.7
17.1-17.3
25
25.1-25.6
HW1: Read Ch
25, # 11, 17, 21
HW2: 23, 25,
27
Title: Preparation of Esters (exp22)
Objective: A number of different esters are prepared,
distilled, and purified by shaking it with a saturated
solution of sodium carbonate. The theoretical yield is
then calculated and the percent yield determined
based on the amount actually prepared.
25.3
Handouts
AP Exam
Title: Qualitative analysis of anions
Objective: Students will analyze solutions to
determine the presence of 6 common anions.
Title: Liquid chromatography
Objective: A mixture of Kool-Aid is separated using
chromatography and is then measured to allow the
calculation of the resolution, selectivity and
efficiency of the process.
Title: Standardization of a solution using a primary
standard
Title: Redox titration
Title: ID of correct indicator
Title: Buffer solutions
Title: Analytical gravimetric determination