Chabot College December 1997
Replaced Fall 2006
Course Outline for Chemistry 1A
GENERAL COLLEGE CHEMISTRY
Catalog Description:
1A - General College Chemistry 5 units
Introduction to atomic structure, bonding, stoichiometry, thermochemistry, gases, matter and energy, oxidation-reduction, chemical equations, liquids and solids, solutions, chemical energetics and equilibrium. Laboratory includes both quantitative and qualitative experiments. Prerequisite:
Mathematics 55 or 55B; Chemistry 31 (all courses completed with a grade of C or higher) or appropriate skill level demonstrated through the Chemistry Placement Process; knowledge of safe
B. laboratory procedure as demonstrated through completion of Chemistry 31 or the laboratory safety evaluation. 3 hours lecture, 6 hours laboratory.
Prerequisite Skills:
A. Mathematics : Before entering the course the student should be able to:
1. operate a scientific calculator, including +, -, x,
10 and base e), 1/x, square root of x,x y
; find a root or power of any number;

exponential notation, log and antilog (base
2.
3.
4.
5.
6.
7. add, subtract, multiply, and divide numbers in exponential notation; take the log and antilog of any number in either base 10 or base e; perform chain calculations knowing the hierarchy of functions; add, subtract, multiply, and divide fractions;
8.
9. solve an algebraic equation for an unknown, including both first and second order equations
(quadratic solution); give a linear equation with two variables, recognize direct and inverse proportionalities; give a statement of a problem, assign variables and construct an algebraic relationship
10.
11.
12. among them; give a set of data involving two variables, plot a graph of that data; give a straight-line graph, calculate the slope of the line; give a straight-line graph, write the equation relating the variables.
Chemistry : Before entering the course the student should be able to:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11. define matter and energy; classify states of matter and describe phase changes using the kinetic molecular theory; distinguish between elements/compounds/mixtures; physical/chemical, intensive/extensive, endothermic/exothermic changes and/or properties; solve conversion problems, including metric system and metric to English, and density, using dimensional analysis; convert between the three temperature scales; solve mathematical problems using significant figures correctly; describe basic atomic structure using simple quantum theory; state electron configurations and their relationship to placement on the periodic table; name common salts, acids and molecular compounds by both systematic and common methods; describe the mole concept and use it in various calculations such as percent composition, determination of empirical/molecular formulas when given percent composition; perform all levels of stoichiometric calculations (mass, gas and solution) including limiting reagent problems;

Chabot College
Course Outline for Chemistry 1A - page 2
December 1997
Prerequisite Skills - continued:
12.
13.
14. perform calculations using the Gas Laws; Define ionic and covalent bonds and give properties of each; draw Lewis structures for simple covalent formulas; classify chemical reactions by type and predict products (such as single and double
15.
16.
17.
18.
19.
20.
21.
22. replacement, combination, decomposition and combustion); perform calculations involving molarity and percent concentrations for solutions; classify solutes and write net ionic equations to determine if reaction has occurred; define acids and bases by Arrehenius and Bronsted-Lowry theories; perform simple pH calculations; take measurements correctly from laboratory glassware and instruments; safely handle chemicals in the laboratory; perform basic laboratory techniques (such as filtration, titration) in an efficient and safe manner; perform error and precision analysis of data.
C. Health and Safety : Before entering the course the student should be able to:
1.
2.
3. know and follow self protection procedures; know and follow basic laboratory safety rules; know and follow procedures for safe handling of chemicals and glassware.
More information is available in the handout "Laboratory Safety".
Expected Outcome for Students:
Upon completion of the course, the student should be able to:
1.
2.
3.
4.
5.
6.
7. solve problems involving the concepts listed under course content; write short explanations describing various chemical phenomena studied; write balanced chemical equations including net ionic equations; write balanced chemical equations for oxidation-reduction reactions;
8.
9.
10.
11.
12.
13.
14.
15. describe the different models of the atom; use standard nomenclature and notation; calculate enthalpies of reaction using calorimetry, Hess's law, heats of formation and bond energies; describe hybridization, geometry and polarity for simple molecules; draw Lewis dot structures for molecules and polyatomic ions; describe the bonding in compounds and ions; describe simple molecular orbitals of homonuclear systems; predict deviations from ideal behavior in real gases; explain chemical and physical changes in terms of thermodynamics; describe the nature of solids, liquids, gases and phase changes; describe metallic bonding and semiconductors;
16.
17.
18.
19.
20.
21. define all concentration units for solutions and solve solution stoichiometry problems; collect and analyze scientific data, using statistical and graphical methods; perform volumetric analyses; use a barometer; use a visible spectrophotometer; perform gravimetric analysis.

Chabot College
Course Outline for Chemistry 1A, page 3
December 1997
Course Content:
1. Matter and energy
8.
9.
2.
3.
4.
5.
6.
7.
10.
Chemical equations, including net ionic equations
Oxidation-reduction reactions
Nomenclature
S.I. and metric units
Stoichiometry
Atomic structure
Periodic law
Chemical bonding a. b. c. d.
Lewis structures
Molecular geometry
Hybridization
Molecular Orbital Theory
Thermochemistry a. b. c. d.
Calorimetry
Heats of Formation
Hess' Law
Bond energies
11.
12.
13.
14.
Gases a. b.
Ideal
Non-ideal
Thermodynamics
Liquids, solids and metallic bonding
Solutions
15.
16.
Laboratory safety
Calorimetry experiment
17.
18.
Titration experiment
Gravimetric experiment
Methods of Presentation:
1.
2.
3.
4.
Methods of Evaluating Student Progress:
1.
2.
3.
4.
5.
6.
7.
Lecture, informal with student questions encouraged
Models, periodic tables, films, overlays
Demonstrations
Safety and proper respect for chemicals and scientific apparatus are constantly stressed
Homework
Quizzes
Written lab reports based on departmentally approved experiments
Accuracy and precision of experimental laboratory results
Midterm examinations
Final examination
Written assignments will encourage critical thinking and writing skills by including essays which involve analytical reasoning

Chabot College
Course Outline for Chemistry 1A, page 4
December 1997
Textbook(s) (Typical):
Chemistry , Steven S. Zumdahl, D.C. Heath Publishers, 1993
Special Student Materials:
1.
2.
3.
Safety goggles approved for chemistry laboratory
Scientific calculator
Laboratory coat/apron (optional)
Revised: 10/17/97; 12/2/97
Laurie O'Connor