Download General College Chemistry

Replaced Fall 2010
Fall 2006
Chabot College
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:
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B.
operate a scientific calculator, including +, -, x,  exponential notation, log and antilog (base
10 and base e), 1/x, square root of x,xy;
find a root or power of any number;
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;
solve an algebraic equation for an unknown;
given a linear equation with two variables, recognize direct and inverse proportionalities;
given a statement of a problem, assign variables and construct an algebraic relationship
among them;
given a set of data involving two variables, plot a graph of that data;
given a straight-line graph, calculate the slope and y-intercept of the line;
given a straight-line graph, write the equation relating the variables.
Chemistry: Before entering the course the student should be able to:
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describe 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
problems using dimensional analysis;
convert between the three temperature scales;
solve mathematical problems using significant figures and units correctly;
describe basic atomic structure using simple quantum theory;
state electron configurations and their relationship to placement on the periodic table;
name salts, common acids and binary molecular compounds by both systematic and
common methods;
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;
perform all levels of stoichiometric calculations (mass, gas and solution) including limiting
reagent problems;
perform calculations using the Gas Laws;
define ionic and covalent bonds and give properties of each;
draw Lewis structures for simple covalent formulas;
Chabot College
Course Outline for Chemistry 1A - page 2
Fall 2006
15.
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20.
classify chemical reactions by type and predict products (such as single and double
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;
satisfactorily perform the following laboratory procedures and techniques:
a.
safely handle chemicals 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 g 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 liquids 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 and barometric pressure;
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.
Expected Outcome for Students:
Upon completion of the course, the student should be able to:
1.
solve problems involving the concepts listed under course content;
2.
write balanced chemical equations including net ionic equations;
3.
write balanced chemical equations for oxidation-reduction reactions;
4.
describe atomic theory and structure;
5.
use standard nomenclature and notation;
6.
calculate enthalpies of reaction using calorimetry, Hess's law, heats of formation and bond
energies;
7.
describe hybridization, geometry and polarity for simple molecules;
8.
draw Lewis dot structures including resonance forms and formal charges for molecules and
polyatomic ions;
9.
describe the bonding in compounds and ions;
10.
describe simple molecular orbitals of homonuclear systems;
11.
predict deviations from ideal behavior in real gases;
12.
explain chemical and physical changes in terms of thermodynamics;
13.
describe the nature of solids, liquids, gases and phase changes;
14.
describe metallic bonding and semiconductors;
15.
define all concentration units for solutions and solve solution stoichiometry problems;
16.
collect and analyze scientific data, using statistical and graphical methods;
17.
perform volumetric analyses;
18.
use a barometer;
19.
use a visible spectrophotometer;
20.
perform gravimetric analysis
Chabot College
Course Outline for Chemistry 1A - page 3
Fall 2006
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.
2.
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
Safety:
a.
Safe handling of chemicals and proper techniques for use of scientific
instrumentation.
Methods of Presentation:
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4.
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
Chabot College
Course Outline for Chemistry 1A - page 4
Fall 2006
Assignments and Methods of Evaluating Student Progress:
1.
Typical Assignments
a.
Homework: 10 – 12 homework problems per chapter taken from the text.
Example: Complete a worksheet on molecular geometry.
Write correctly balanced oxidation/reduction equations for 20 reactions.
b.
2.
Laboratory assignment: In the experiment Determination of the gas constant R using 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.
Methods of Evaluating Student Progress
a.
Homework
b.
Quizzes
c.
Written lab reports based on departmentally approved experiments
d.
Accuracy and precision of experimental laboratory results
e.
Midterm examinations
f.
Final examination
g.
Written assignments will encourage critical thinking and writing skills by including essays
which involve analytical reasoning
Textbook(s) (Typical):
Chemistry, Steven S. Zumdahl and Susan A. Zumdahl, Houghton Mifflin Company, 2003
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; 11/20/05
Laurie Dockter/Harjot Sawhney