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Master Course Outline
CHEM& 121
Introduction to Chemistry w/Lab
Course Description: A survey of general chemical principles, including elements and compounds, atomic
structure and periodic properties, chemical reactions, energy, equilibrium and kinetics, solutions, acids
and bases, and nuclear chemistry. This course is intended for allied health and natural resources majors,
as well as those students pursuing an AA degree. It also serves as the prerequisite for CHEM& 161 for
students who have not completed one year of high school chemistry. This course, with CHEM & 131,
constitutes a terminal sequence in chemistry and does not prepare a student for a second year of
chemistry. 4 lecture hours; 2 lab hours. Students may not receive credit for both CHEM& 110 and
CHEM& 121. Satisfies science or lab requirement area B distribution or specified elective for AA degree.
Credits: 5
Prerequisites: A grade of “C-“or better in MATH 095 or placement in MATH 098
Recommended Preparation: None
Co-requisites: None
Learning Outcomes: Students completing the course will have been instructed in the following topics
and procedures, evaluated on their ability to perform the required functions, and earn a course grade
based on the evaluation of their ability to do the following:
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Define matter
Distinguish between chemical properties and physical properties and also between chemical
changes and physical changes.
Demonstrate an understanding of Dalton’s Atomic Theory.
Classify matter
Make measurements and include the proper units.
Use the Metric System of measurements.
Use scientific notation to represent very small and very large numbers, and to perform
calculations using numbers expressed in scientific notation.
Express measured quantities using the correct number of significant figures.
Use units in calculations.
Perform basic calculations such a percentage, and density.
Use symbols for chemical elements to write formula for chemical compounds.
Identify the characteristics of protons, neutrons, and electrons.
Use the concepts of atomic number and mass numbers to determine the number of
subatomic particles in isotopes.
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Use atomic weights of the elements to calculate molecular weights of compounds.
Use the mole concept to obtain relationships between number of moles, and number of
grams, for elements and compounds and use those relationships to obtain factors for use in
factor-unit calculations.
Locate elements on the periodic table on the basis of period and group designations.
Determine the number of electrons in the designated atomic orbitals, subshells, or shells.
Determine the number of valence shell electrons and the electronic structure for atoms and
relate this information to the location of elements in the periodic table.
Determine the electronic configuration of atoms and the identity of atoms based on electronic
configurations.
Recognize property trends of elements within the periodic table, and use the trends to predict
selected properties of the elements.
Draw correct Lewis structures for elements and covalent molecules.
Use electronic configurations to determine the number of electrons gained or lost by atoms as
they achieve noble gas configurations.
Use the octet rule to correctly predict the ions formed during the formation of ionic
compounds, and write correct formulas for ionic compounds.
Correctly name ionic compounds.
Determine formula weights for ionic compounds.
Use VSEPR theory to predict the shapes of molecules.
Use electronegativities to classify covalent bonds as polar or nonpolar and then classify the
molecules as either polar or nonpolar.
Identify the reactants and products in written reaction equations, and balance the equations
by inspection.
Classify reactions as single replacement, double replacement, combination or decomposition.
Identify the oxidized substance and the reduced substance in a redox reaction.
Write molecular equations in total and net ionic forms.
Classify reactions as endothermic or exothermic.
Use the mole concept to perform calculations based on chemical reaction equations and to
calculate percent yields.
Demonstrate an understanding of the kinetic molecular theory and use the kinetic molecular
theory to explain and compare properties of matter in different states.
Do calculations to convert temperature and pressure values into various units.
Do calculations using the various gas laws.
Classify changes in state as endothermic or exothermic.
Do calculations based on the energy changes that accompany heating, cooling, or changes in
the state of a substance.
Classify mixtures as solutions or nonsolutions based on their appearance.
Demonstrate their understanding of solubility.
Predict the solubility’s of solutes in solvents based on polarity.
Calculate solution concentrations in molarity and percent.
Describe how to prepare solutions from pure solute and solvent and from dilution.
Do stoichiometric calculations based on solution concentrations.
Describe the characteristics of colloids.
Describe the processes of osmosis and dialysis.
Use the concept of molecular collisions to explain reaction characteristics.
Represent and interpret the energy relationships for reactions using energy diagrams.
Explain how factors such as concentrations, temperature, and catalysts affect reaction rates.
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Use Le Châtlier’s principle to predict the influence of changes in concentration and reaction
temperature on the position of equilibrium for a reaction.
Demonstrate knowledge of Arrhenius and Brønsted acid-base theory.
Name common acids and bases.
Do calculations using the concept of the self-ionization of water and the pH concept.
Identify the characteristic reactions of acids.
Write reaction equations that represent neutralization reactions between acids and bases.
Demonstrate an understanding of the words weak and strong as applied to acids and bases.
Do calculations related to the analysis of acids and bases by titration.
Explain how buffers work.
Describe and characterize the common forms of radiation emitted during radioactive decay
and other nuclear processes.
Write balanced equations for nuclear reactions.
Solve problems using the half-life concept.
Describe the medical uses of radioisotopes.
Describe the differences between nuclear fission and nuclear fusion reactions.
Course Resources/Textbooks/Website:
The course will require the use of a student bundle which includes the ebook, a hard cover copy of the
textbook, 24 month access to the online Homework, and a student response device (clicker). This
bundle is available for purchase in the GHC Bookstore.
Textbook: Chemistry for Today: General, Organic, and Biochemistry by Spencer L. Seager and Michael R.
Slabaugh , 7th edition, ISBN-13: 9780538733328
The publisher’s website for this material is:
http://www.cengage.com/search/productOverview.do?Ntt=seager||9135663661620626894760696897
1508500773&N=16+4294922413+4294967052&Ntk=all%7C%7CP_EPI#mainTab_
Optional ancillary materials, such as the Student Solutions Manual, are also available from the publisher.
A scientific calculator is also required for the course. A variety of makes and models have been
successfully used. Cell phones , iPods™, computers, or any other internet connected devices may not be
used as a calculator or for any other purposes during testing due to the obvious potential for cheating.
Academic Integrity: All forms of cheating, falsification, and plagiarism are against the rules of this course
and of Grays Harbor College. Students who are unsure what constitutes academic dishonesty are
responsible for asking the instructor for clarification. Instances of intentional academic dishonesty will
be dealt with severely.
Disabilities: Students who have documented disabilities that require accommodations in compliance
with the Americans with Disabilities Act should contact the Disability Support Services coordinator as
well as the instructor of the course in order to ensure that together we create an optimal environment
for educational achievement.
W Day, the final day to officially withdraw from a course, is the Thursday of the seventh week (Thursday
of the fourth week for summer quarter). Students who do not withdraw by that date will receive the
grades they have earned, regardless of whether they are attending the course or completing the work.
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Students who are considering withdrawal are strongly advised to consult with the instructor, advisor and
financial aid prior to withdrawing. The only withdrawals allowed after W Day are complete withdrawals
from all courses.
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