FIRST SEMESTER:
 ALL LABS ARE STUDENT DIRECTED UNLESS OTHERWISE
MENTIONED
CH.
TIME
CONCEPT
LAB/ASSIGNMENTS
2
4-5
days
ATOMS, MOLECULES AND IONS
Atomic theory and atomic structure
LAB:


3&
4
5-6
days
Evidence for the atomic theory (p. 40-50)
Atomic masses: determination by chemical and
physical means (p. 77-80)
 Atomic number and mass number; isotopes (p.
50-52)
 Formula writing review (p. 52-54)
STOICHIOMETRY: CALCULATIONS WITH
CHEMICAL FORMULAS AND EQUATIONS







4
8-10
days
Ionic and molecular species present in chemical
systems: net ionic equations (p. 132-136, 145151)
Balancing of equations (p. 99-102)
Reaction types (p. 144)
Stoichiometry: Mass and volume relations with
emphasis on the mole concept, including
empirical formulas and limiting reactants (p. 8197, 102-117)
Percent composition (p. 88-90)
Empirical/Molecular formulas (p. 90-97)
Empirical formula from combustion (p. 90-92)
AQUEOUS REACTIONS AND SOLUTION
STOICHIOMETRY
 Types of solutions and factors affecting solubility
(p. 130-136)
 Solution stoichiometry (p. 151-154)
 Methods of expressing concentration (p. 136144)
o Molarity
o Dilution
o Mixing of solutions
o Electrolytic properties
 Weak, strong and non
electrolytes
 Ionic and molecular species present in chemical
systems (p. 132-136, 145-151)
 Net ionic equations (p. 132-136, 145-151)
Atom board practice of atomic and
mass numbers and isotopes
ASSIGNMENTS:
 Formula writing review
 Problems from chapter 2
LAB:
Analysis of a Penny and Chemical
Reactions and Equations
ASSIGNMENTS:


Problems from chapter 3:
pg 110-117
40 equations:
o predict products
o balance
o net ionic form
LAB:


Conductivity of Aqueous
Solutions
Precipitating Calcium
Phosphate
ASSIGNMENTS:


Chapter 3 problems
Worksheet on combining
solutions and calculating
ions in solution.
6
14-16
days
THERMOCHEMISTRY
 State functions (p. 236-242)
 First law: change in enthalpy; heat of formation;
heat of reaction; Hess’s law, heats of
vaporization and fusion; calorimetry (p. 243-262)
LAB:


Energy and Specific Heat
Thermochemistry and
Hess’s law
ASSIGNMENTS:
12
11
days
CHEMICAL KINETICS
 Concept of rate of reaction (p. 540-547)
 Use of experimental data and graphical analysis
to determine reactant order, rate constants and
reaction rate laws (p. 547-562)
 Effect of temperature change on rates (p. 565570)



13
11
days
Energy of activation; the role of catalysts (p.
565-577)
The relationship between the rate-determining
step and a mechanism (p. 562-565)
Half-lifes (p. 554-561)
CHEMICAL EQUILIBRIUM
 Concept of dynamic equilibrium, physical and
chemical, LeChatelier’s principle; equilibrium
constants (p. 594-601, 620-626)
 Quantitative treatment
o Equilibrium constants for gaseous
reactions: Kp,Kc (p. 601-620)
 Book problems
LAB:

Factors affecting Rate (kit
from FLINN)
 Crystal violet Lab with CBL
o Determines order
and activation
energy
ASSIGNMENTS:


Book problems
Determine order of reaction
through graphical analysis
LAB:

LeChatelier principle (kit)
SECOND SEMESTER
4,
14,
& 15
11
days
ACID-BASE EQUILIBRIA (p. 154)
 Equilibrium constants for reactions in solution (p.
640-644)
 Constants for acids and bases: pK; pH (p. 647)
 Bronsted-Lowry Acids and Bases (p. 639-642)
 The auto-ionization of water (p. 645)
 PH scale (p. 647)
 Indicators (p. 728-733)
 Strong acids & bases compared to weak acids
and weak bases (p. 650-657, 661-666)
 Relationship between Ka and Kb (p. 663-666)
 Acid-Base properties of salt solutions (p. 671677)
LAB:


Calculation of Ka of an acid
(indicator)



15 &
16
25
days
Acid-Base behavior and chemical structure (p.
639-642)
Triprotic acids (p. 666-671)
Lewis acids and bases (p. 679-682)
ADDITIONAL ASPECTS OF AQUEOUS EQUILIBRIA
 Common ion effect; buffers; hydrolysis (p. 671677, 698-713)
 Acid-base titration (p. 157-160. 713-727)
 Solubility equilibria; solubility product constants
and their application to precipitation and the
dissolution of slightly soluble compounds (p.
744-759)
 Coordination complexes; amphoterism (p. 759764)
 Precipitation reactions (p. 145-151)
 Qualitative analysis for metallic elements (p.
757-759)
17 &
18
7
days
CHEMICAL THERMODYNAMICS
 Second law: entropy; free energy of formation;
free energy of reaction (p. 773-798)
 Dependence of change in free energy on
enthalpy and entropy changes and temperature
changes (p. 773-798)
 Relationship of change in free energy to
equilibrium constants and electrode potentials
(p. 798-802, 833-842)
4&
18
17
days
ELECTROCHEMISTRY
 Oxidation-reduction reactions; balancing
equations (p. 161, 166-168)
 Oxidation number (p. 162-165)
 The role of the electron in oxidation-reduction (p.
165-166)
 Electrochemistry’ electrolytic and galvanic cells;
Faraday’s Lasw; standard half-cell potentials;
Nernst equation; prediction of the direction of
redox reactions (p. 823-836, 838-842, 847-851)
 Cell EMF under standard conditions (p. 833836)
 Free energy and redox reactions (p. 825-833)
 Cell EMF under nonstandard conditions (p. 836842)
 Electrolysis (p. 847-851)
7
3
days
ELECTRONIC STRUCTURE OF ATOMS




Electron energy levels (p. 285-309)
Atomic spectra (p. 312-318)
Quantum numbers (p. 300-304)
Atomic orbitals (p. 305)
LAB:

Titration of strong acid and
strong base;
standardization of a base
 Determination of molecular
mass of a weak acid
through titration
 Construction of a pH curve
through titration
 Descriptive/qualitative
analysis determination of
unknown salts
DEMO:
LABS:


The Potential of
Electrochemical Cells(Salt
bridge)
Electrolysis of KI solution

7&
8
3-5
days
PERIODIC PROPERTIES



2, 8,
9, &
10
5
days






5
days


5-8
days
Binding forces (p. 52-54, 341-344, 357-361,
440-461)
o Ionic
o Covalent
o Metallic hydrogen bonding
o Van der Waals
o London dispersion forces
Relationships to states, structure, and properties
of matter (p. 466-478)
Polarity of bonds (p. 346-349)
Electronegativity (p. 344-346)
Resonance structures (p. 373-378)
Exceptions to the octet rule (p. 369-373)
Strengths of covalent bonds
o Bond energy (p. 341, 353-357, 361-364)
o Bond length (p. 342, 422-423, 362-363)
MOLECULAR GEOMETRY AND BONDING
THEORIES


1, 8
10,
& 11
Relationships in periodic table (p. 318-320, 323327)
atomic & ionic radii, ionization energies, electron
affinities, oxidation states, electronegativity (p.
309-311, 320-323, 344-346, 353)
effective nuclear charge, shielding affect,
metallic character (p. 308-309, 320)
BASIC CONCEPTS OF CHEMICAL BONDING

8, 9,
& 10
Aufbau, Pauli and Hund’s Rule (p. 306-308,
312-318)

Lewis structures (p. 365-373)
Valence Bond: hybridization of orbitals,
resonance, sigma and pi bonds (p. 373-378,
404-416)
VSEPR (p. 378-390)
Geometry of molecules and ions, structural
isomerism of molecules and coordination
complexes, dipole moments and relation of
properties to structure (p. 346-349, 378-390,
440-443, 969-974)
INTERMOLECULAR FORCES, LIQUIDS AND
SOLIDS

LAB:
States of matter (p. 26)
Molecular geometry
structures with balls and
sticks and Styrofoam for the
expanded octets.
LAB:


Triple point of dry ice
Molecular mass




11 &
16
5-8
days
PROPERTIES OF SOLUTIONS










1, 2,
&5
19
5
days
2-3
days
Liquids and solids from the kinetic-molecular
viewpoint (p. 439-440, 565-570)
Phase diagrams of one-component systems (p.
479-483)
Changes of state, including critical points and
triple points (p. 475-479)
Structure of solids; lattice energies (p. 353-357,
445-471)
Solution process (p. 498-504)
Saturated solutions and solubility (p. 744-752)
Factors affecting solubility (p. 504-509)
Ways of expressing concentration (p. 136-144,
498-501)
Colligative properties (p. 516-519, 524-527)
Raoult’s Law (p. 509-515)
Nonvolatile compared to volatile solutes (p. 509515)
Osmosis (p. 520-524)
Nonideal behavior and quantitative methods (p.
513, 525)
Ideal solutions (p. 514-515)
GASES


Characteristics of Gases (p. 26)
Gas Laws of ideal gases: Charles, Boyles,
Grahams, Combined Gas Law, Daltons Law of
Partial Pressures, Guy Lussac, and Graham’s
Law of Effusion (p. 183-194, 199-205, 212-214)
 Equation of State of an Ideal Gas (p. 190-191)
 Kinetic molecular theory of gases (p. 205-212)
o Interpretation of ideal gas laws on the
basis of kinetic theory
 Molecular effusion and diffusion (p. 212-214)
 Real Gases: deviations from ideal behavior (p.
214-217)
 Dependence of kinetic energy of molecules on
temperature (p. 206, 210)
 Avogadro’s hypothesis and the mole concept (p.
45-46, 208)
NUCLEAR CHEMISTRY (p. 873-894)




Nuclear equations
Half-lives
Radioactivity
Chemical applications

determination using
freezing and boiling points
Evaporation and
Intermolecular Attractions
LAB:


Using Conductivity to Find
an Equivalence Point
Vapor Pressure of Liquids
LABS:

Determination of molecular
mass from a gas (butane)