Chabot College
Fall 2006
Replaced Fall 2010
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 laws, 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.
[Typical contact hours: lecture 52.5, laboratory 52.5]
Prerequisite Skills:
Before entering the course, the student should be able to:
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perform basic operations on complex numbers;
solve quadratic equations by factoring, completing the square, and quadratic formula;
find complex roots of a quadratic equation;
sketch the graphs of functions and relations:
a.
algebraic, including polynomial and rational
b.
logarithmic
c.
exponential
d.
circles;
find and sketch inverse functions;
perform function composition;
solve exponential and logarithmic equations;
apply the concepts of logarithmic and exponential functions;
solve systems of linear equations in three unknowns using elimination and substitution;
apply the properties of and perform operations with radicals;
apply the properties of and perform operations with rational exponents;
solve equations and inequalities involving absolute values;
solve equations involving radicals;
graph linear inequalities in two variables;
find the distance between points;
find the midpoint of a line segment.
Expected Outcomes for Students:
Upon successful completion of 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;
Chabot College
Course Outline for Chemistry 31, page 2
Fall 2006
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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;
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 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 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;
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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.
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 of ionic compounds, binary covalent compounds and common acids
The mole concept including amount conversions, and all levels and variations of stoichiometric
calculations
Chemical bonding (ionic and covalent), Lewis structures for simple molecules
The Gas Laws (for ideal gases only)
Reactions: balancing equations, classification, prediction of product
Solutions: definitions, molarity and percent concentrations
Net ionic equations
Arrhenius and Bronsted-Lowry acid-base theories
pH calculations and solution stoichiometry including titration calculations
Measurement of mass, volume, and density
Measurement of % composition and determination of empirical formula
Gravimetric analysis and filtration
Observe, classify and analyze various types of chemical reactions
Construction of molecular models from Lewis structures
Collection of gases; measurement of pressure, volume and temperature
Conductivity of substances and solutions
Preparation of solutions
Acid/Base titration
Chabot College
Course Outline for Chemistry 31, page 3
Fall 2006
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Data analysis, calculation of average, relative range, percent error, including graphical analysis
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
Classroom and laboratory demonstrations
Use of models, animations, movies, interactive software, online homework, periodic tables, films
and overlays
Individual and group work in the laboratory
Safe 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.
Example: Nivaldo J. Tro, Chapter 3 problems 28, 32, 34, 36, 42, 44, 48, 50, 56,
60, 62
b.
Laboratory assignment: design an experiment for separating an unknown mixture
of salt and sand and determine the percentage by weight of salt and sand in the
mixture. Determine the precision and accuracy of the results
2.
Methods of Evaluating Student Progress
a.
Homework
b.
Quizzes
c.
Written laboratory reports based on departmentally approved experiments
d.
Accuracy and precision of laboratory results
e.
Midterm examinations (1-5 per semester)
Typical test questions:
1)
How many significant figures are there in the number 0.00003410?
A. 4
B. 8
C. 7
D. 6
E. 5
2)
An unknown liquid compound with the odor of rotten eggs is analyzed in the lab,
and it is found to contain only the elements carbon, hydrogen and sulfur. It is
47.31% carbon by weight, 10.59% hydrogen and the rest is sulfur. Find its
empirical formula and write it in the form CxHySZ. Show all work and box your
final answer.
f.
Final examinations
Textbook(s)(Typical):
Introduction Chemistry, 2nd edition, Nivaldo J. Tro, Prentice Hall, 2005
In-House Laboratory Manual for Chemistry 31, Donna Gibson, et al, 1999
Special Student Materials:
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Safety goggles approved for chemistry laboratory
Scientific calculator
Laboratory coat/apron (optional)
A, Well:al
Revised: 9-30-2005