Chabot College
November 1997
Replaced Fall 2006
Course Outline for Chemistry 31
INTRODUCTION TO COLLEGE CHEMISTRY
Catalog Description:
31 – Introduction to College Chemistry
4 units
Elementary concepts of chemistry with emphasis on mathematical calculations; includes
nomenclature, stoichiometry, atomic structure, gas lawa, and acids and bases. Designed for majors
in science and engineering. Prerequisites: Mathematics 55 or 55B (completed with a grade of “C” or
higher). 3 hours lecture, 3 hours laboratory.
Prerequisite Skills:
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, and square root of x and 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, including both first and second order equations
(quadratic solution);
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 of the line;
12. given a straight-line graph, write the equation relating the variables.
Expected Outcomes for Students:
Upon completion of the course, the student should be able to:
1. define 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 conversion problems, including metric system and metric to English, and density, using
dimensional analysis;
5. convert between the three temperature scales;
6. solve mathematical problems using significant figures correctly;
7. describe basic atomic structure using simple quantum theory;
8. state electron configurations and their relationship to placement on the periodic table;
9. name common salts, acids and molecular compounds by both systematic and common methods;
10. describe the mole concept and use it in various calculations such as percent composition,
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 formulas;
15. classify chemical reactions by type and predict products (such as single and double replacement,
combination, decomposition and combustion);
Chabot College
Course Outline for Chemistry 31, Page 2
November 1997
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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.
Course Content
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Review of relevant mathematics; scientific notation, significant figures, dimensional analysis;
Definitions and classifications of matter and energy;
Atomic structure and periodicity;
Chemical nomenclature;
The mole concept including all levels and variations of stoichiometric calculations;
Chemical bonding (ionic and covalent), Lewis structures for simple molecules;
The Gas Laws (for ideal gases only);
Classifications of reactions and use to predict products;
Solution concentration in terms of molarity and percent concentrations;
Net ionic equations;
Arrhenius and Bronsted-Lowry acid-base theories;
pH calculations and solution stoichiometry including titration calculations;
basic laboratory techniques (such as filtration, measurements, titrations);
Data analysis;
Laboratory safety.
Methods of Presentation:
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Lecture, informal with student questions encouraged;
Use of demonstrations;
Use of models, periodic tables, films and overlays;
Safe and proper respect for chemicals and scientific apparatus are constantly stressed.
Methods of Evaluating Student Progress:
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Homework;
Quizzes;
Written laboratory reports based on departmentally approved experiments;
Accuracy and precision of laboratory results;
Midterm examinations;
Final examinations.
Textbook(s) (Typical):
Chemical Principles, Peters and Kowerski, Saunders Publishing
Special Student Materials:
1. Safety goggles approved for chemistry laboratory;
2. Scientific calculator;
3. Laboratory coat/apron (optional).
October 6, 1997
Donna Gibson