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Chabot College
Fall 2010
Course Outline for Chemistry 1A
GENERAL COLLEGE CHEMISTRY I
Catalog Description:
1A - General College Chemistry I
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. 3 hours lecture, 6 hours laboratory.
[Typical contact hours: lecture 52.5, laboratory 105]
Prerequisite Skills:
A. Mathematics: Before entering the course the student should be able to:
1. operate a scientific calculator, including +, -, x,  exponential notation, log and antilog (base 10
and base e), 1/x, square root of x, xy;
2. find a root or power of any number;
3. add, subtract, multiply, and divide numbers in exponential notation;
4. take the log and antilog of any number in either base 10 or base e;
5. perform chain calculations knowing the hierarchy of functions;
6. add, subtract, multiply, and divide fractions;
7. solve an algebraic equation for an unknown;
8. given a linear equation with two variables, recognize direct and inverse proportionalities;
9. given a statement of a problem, assign variables and construct an algebraic relationship among
them;
10. given a set of data involving two variables, plot a graph of that data;
11. given a straight-line graph, calculate the slope and y-intercept of the line;
12. given a straight-line graph, write the equation relating the variables.
B. Chemistry: Before entering the course the student should be able to:
1. describe matter and energy;
2. classify states of matter and describe phase changes using the kinetic molecular theory;
3. distinguish between elements/compounds/mixtures; physical/chemical, intensive/extensive,
endothermic/exothermic changes and/or properties;
4. solve unit conversion problems, including metric system and metric to English, and density
problems, using dimensional analysis;
5. convert between the three temperature scales Celcius, Kelvin and Fahrenheit;
6. solve mathematical problems using algebraic equations, significant figures and units
correctly;
7. describe basic atomic structure using simple quantum theory, and Bohr Theory;
8. state electron configurations and orbital diagrams, and their relationship to placement on the
periodic table;
9. name salts, common acids and binary molecular compounds by both systematic and
common methods;
10. describe the mole concept and use it in various calculations such as amount conversion
problems, percent composition, and determination of empirical/molecular formulas when
given percent composition;
11. perform all levels of stoichiometric calculations (mass, gas and solution) including limiting
reagent problems;
12. perform calculations using the Gas Laws;
13. define ionic and covalent bonds and give properties of each;
14. draw Lewis structures for simple covalent molecules and polyatomic ions;
15. classify chemical reactions by type, perform mass balance of chemical equations, and predict
products (such as single and double replacement, combination, decomposition and
combustion);
Chabot College
Course Outline for Chemistry 1A, page 2
Fall 2010
16. perform calculations involving molarity and percent concentrations for solutions;
17. classify solutes as electrolytes or nonelectrolytes, and write net ionic equations to determine
if reaction has occurred;
18. define acids and bases by Arrehenius and Bronsted-Lowry theories, write acid dissociation
reactions, including the use of hydronium ion (H 3O+), and identify conjugate acids and
conjugate bases in acid/base reactions;
19. perform precision acid/base titration calculations;
20. perform simple pH calculations;
21. satisfactorily perform the following laboratory procedures and techniques:
a. safely handle chemicals and equipment in the laboratory;
b. read and record measured quantities from various analytical instruments, correctly
recording the certain digits and estimating the uncertain digit;
c. weigh chemicals to 0.001 grams using a top-loading balance;
d. quantitatively transfer solid and liquid chemicals from one container to another;
e. correctly use a Bunsen burner;
f. accurately measure liquid volumes using analytical volumetric glassware such as
graduated cylinders, burets, and volumetric pipets;
g. perform gravity filtrations quantitatively;
h. perform acid/base titrations using known and unknown solutions;
i. measure temperature;
j. accurately and comprehensively observe chemical and physical changes and record
such information in a scientifically correct form;
k. construct models of simple molecules using model kits and Lewis structures;
l. perform error and precision analysis of data by calculating averages, relative ranges and
percent errors.
m. guided experiment design and writing of simple laboratory experiment procedures
n. quality narrative explanations of observations and/or results
Expected Outcome for Students:
Upon completion of the course, the student should be able to:
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solve problems involving the concepts listed under course content;
write balanced chemical equations including net ionic equations;
write balanced chemical equations for oxidation-reduction reactions;
describe atomic theory and structure;
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 including resonance forms and formal charges 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;
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
Fall 2010
Course Content (Lecture):
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Matter and energy
Chemical equations, including net ionic equations
Balancing Oxidation-reduction reactions
Nomenclature
S.I. and metric units
Stoichiometry
Atomic structure
Periodic law
Chemical bonding
a. Lewis structures
b. Molecular geometry
c. Hybridization
d. Molecular Orbital Theory
Thermochemistry
a. Calorimetry
b. Heats of Formation
c. Hess' Law
d. Bond energies
Gases
a. Ideal
b. Non-ideal
Thermodynamics
Liquids, solids and metallic bonding
Solutions
Laboratory safety
Calorimetry experiments
Titration experiments
Gravimetric experiments
Course Content (Laboratory):
1. Techniques:
a. Preparation of standard solutions and use of spectrophotometer
b. Determination of heat of reaction, specific heat of metal, and gas constant
c. Determination of wavelength using atomic spectrum of hydrogen
d. Acid-Base titration
e. Oxidation-Reduction titration
f. Collection of gas by water displacement method
g. Building of 3-D models of molecules
h. Using Microsoft Excel software to plot graphs and find equation of straight line
2. Safety:
a. Safe handling of chemicals and proper techniques for use of scientific instrumentation.
Methods of Presentation:
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Lecture, informal with student questions encouraged
Models, periodic tables, videos, and overhead transparencies
Demonstrations, computer simulations
Safety and proper respect for chemicals and scientific apparatus are constantly stressed
Assignments and Methods of Evaluating Student Progress:
1. Typical Assignments
a. Homework: 10 – 12 homework problems per chapter taken from the text.
Chabot College
Course Outline for Chemistry 1A, page 4
Fall 2010
Example: Complete a worksheet on molecular geometry.
Write correctly balanced oxidation/reduction equations for 20 reactions.
b. Laboratory assignment: In the experiment Determination of the gas constant R, using the
ideal gas law equation, calculate the value of R. Report the average, relative range, and
relative error compared to the accepted value. Calculate from your data the value of molar
volume in L/mole at STP. Would you expect the same % error as you got for your
determination of R? Explain.
2. Methods of Evaluating Student Progress
a. Homework
b. Quizzes
c. A minimum of 12 written laboratory reports based on departmentally approved
experiments and graded on criteria that may include the following
1) Description of experimental procedures
2) Completeness of data collected
3) Quality of data collected
4) Computational precision and accuracy
5) Accuracy and precision of experimental laboratory results
6) Proper use of symbolic notation
7) Quality of analysis of scientific principles explored
8) Quality of narrative explanations and reasoning
9) Representation of data in tables or diagrams
d. Examinations
e. Final examination
f. Written assignments that encourage critical thinking and writing skills
Textbook(s) (Typical):
Chemistry and Chemical Reactivity, Kotz, Treichel, and Townsend, Thomson Brooks/Cole, 2009
Special Student Materials:
1. Safety goggles approved for chemistry laboratory
2. Scientific calculator
3. Laboratory coat/apron (optional)
Revised: 10/17/97; 12/2/97; 11/20/05; 10/1/09
Laurie Dockter/Harjot Sawhney/Wayne Pitcher