CHEM-130
Introduction to Chemistry
Winter 2015
Instructor: Sarah Simmons
Phone: 269-294-4205
Email: ssimmons@glenoaks.edu
Office: G-217
Office Hours: Open Door Policy, M,W: 10:30-11:00am, 12:30-1:00pm, 5:00-6:00pm, F: 7:00-8:00am
Classroom: Lecture: M, W 11-12:25pm Rm G-207 Lab: F 11-12:50pm Rm G-221
Website: sarahsimmonschemistry.weebly.com
Course Description: This is an introductory course for those students who have little or no background in
chemistry as well as for those students whose program requires a minimum of hours in a laboratory
science. This is a general survey course dealing primarily with fundamental principles of chemistry
including measurements, atomic structure, nomenclature, balancing equations, stoichiometry,
bonding, gases, thermodynamics, and acids and bases.
PREREQUISITE: Math 100 with a grade of 2.0 or higher or 104 or 151 or equivalent or by placement into
104
Required Materials:
 Introductory Chemistry, A Foundation. 7 th ed. Zumdahl.
 Scientific calculator (log and exponential functions)
Methodology and Activities: This is a lecture/laboratory combination course. Lecture sessions discuss the
main and/or troublesome topics and include sample problems. Lecture sessions are formal to semi-formal
with open and general discussion on a pertinent topic preferred. The laboratory sessions are used to
introduce new concepts or to reinforce concepts discussed in the lecture sessions.
Quizzes: There will be several pop quizzes given in lecture throughout the semester. They will be fairly
short, lasting only 5-10 minutes at the beginning of class, and may deal with topics already discussed or
from the reading assignments.
Exams: There will be 5 in-class exams. Each exam will count for 100 points and will include a
combination of multiple choice, problem solving and short answer questions. There will also be a
cumulative final exam at the end of the semester.
Absences: Due to the complex nature of this course it is important that students attend each lecture. If
absence is unavoidable the student is responsible for obtaining the missed lecture notes from another
student. Make-up exams are not available without a documented emergency. If extra help is needed for
missed information, you must have a copy of the notes before asking the instructor for additional help.
Make-up Policy:
No labs will be dropped when calculating the final grade. There will be one make-up lab available at the
end of the semester.
Two quizzes will be dropped when calculating the final grade. No make-up quizzes will be available.
One exam score will be dropped when calculating the final grade. The final exam will count as 2 exams.
Grading: The final grade will be calculated as follows
 Lecture: quizzes 10%, Exams: 65%
 Laboratory: 25%
Grades will be assigned according to the following scale
Percentage
Grade
100 – 90%
4.0
89 – 85%
3.5
84 – 80%
3.0
79 – 75%
2.5
Percentage
74 – 70%
69 – 65%
64 – 60%
59 – 0%
Grade
2.0
1.5
1.0
0.0
Classroom Etiquette: Proper classroom behavior is expected at all times. Talking in class and disruptive
behavior will not be permitted and may result in dismissal from the class. Please turn off cell phones and
any other noisemaker. No children will be allowed in the classroom. Remember, we are all here to learn
and respect for the instructor and other students is a part of that process.
Incomplete and Withdrawal Policy: An “I” or incomplete for a course grade will not be given unless at
least 75% of the course work has been completed. Withdrawal from class is your privilege and
responsibility. It is necessary for you to follow correct procedures. A grade of W is automatically given
through February 27st. After this date if you stop attending class and do not follow the official procedures
for dropping or withdrawing from the class you shall receive a semester grade of 0.0 or whatever your total
point accumulation permits. The last day a faculty may issue a W is April 26 st.
Assistance: If you are a student with a documented disability and you believe you are entitled to receive
accommodations for this class, please contact me privately so we may discuss your specific needs. You
will also need to contact the Student Support Specialist to schedule an appointment for an intake if you
have not already done so, You may contact the Student Support Specialist by calling 269-467-9945 and ask
for Student Services.
Academic Dishonesty: Academic dishonesty includes, but is not limited to taking, using, or copying
another’s work and submitting it as your own, using notes on exam’s, intentionally falsifying information
or taking another’s ideas with intention of passing in class as one’s own. Academic Dishonesty will not be
tolerated and will result in a zero.
Sensitivity: Glen Oaks Community College is committed to providing equal access to education for all
persons regardless of race, color, sex, age, religion, national origin, sexual orientation, disability, veteran
status, or other status as protected by law. The College is committed to an environment that demonstrates
civility, caring and respect. Harassment of any kind is a barrier to effective work and academic
achievement. Glen Oaks Community College values diversity of expression, collaboration, partnering and
finding ways to communicate effectively across differences in the college community. If you feel that you
have been the focus of discrimination or harassment, you may report the incident
https://glenoaks.ethicaladvocate.com or by phone at 1-877-743-4127. You may also contact a counselor by
calling (269) 467-9945 and asking for Student Services
Emergency Evacuation Procedures: A map of the wing where this classroom is located is posted near the
wing entrances marking evacuation routes and the designated tornado shelter area. This is an area where
emergency service personnel will go first to look for individuals who need assistance in exiting the
building. Please make sure to review the maps to ensure you will know how to evacuate in case of an
emergency. Students who may need assistance should identify themselves to the teaching faculty.
Learning Outcomes:
By the completion of this course, successful students will:
A.
Safety
 Explain a Material Safety Data Sheet (MSDS) (2)
 Identify different types of fire extinguishers and what types of fires they are to be used upon. (2)
 Explain the correct usage of a fire blanket, eye wash and shower. (2)
 Describe proper disposal methods for chemicals. (2)
 Describe the effects of improper disposal methods on the environment. (2)
 Recognize and correctly name laboratory equipment, glassware, and supplies that are used. (5)
B.
Introduction to Chemistry
 Define Chemistry and its sub disciplines (2)
 List the steps of the scientific method and apply it to solve problems (5)

C.
D.
Define Theory and Law (2)
Measurement
 Utilize the metric system for measurements of mass, distance, volume, and energy. (5)
 Convert metric/metric, metric/English, and English/metric. (5)
 Measure mass, distance, and volume with accuracy and precision. (5)
 Solve problems relating to measurement including density and temperature. (5)
 Demonstrate and use dimensional analysis in problem solving. (5)
 Properly use significant figures to show uncertainty in a measurement. (5)
Matter
Identify states of matter and list characteristics for each type. (5)
List the hierarchical organization of matter including mixtures, pure substances, compounds, and
elements. (5)
 Distinguish between chemical and physical properties. (2, 5)
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E.
Atomic Theory
 Explain the structure of an atom and the experiments that led to its discovery. (2)
 Determine the number of protons, neutrons, and electrons in an atom. (5)
 Describe the organization of the periodic table (2)
 Describe ions and isotopes and how they affect the number of subatomic particles in an atom (2, 5)
 Determine the charge of ions using the periodic table (5)
 Determine the chemical formula of ionic compounds (5)
F.
Nomenclature
 Determine the name of ionic compounds (5)
 Determine the name of molecular compounds (5)
 Determine the name of compounds involving polyatomic ions (5)
 Determine the chemical formula from the name. (5)
G.
Chemical Equations and Reactions
 Define reactants and products. (2)
 Balance equations by inspection.(5)
 List, recognize, and illustrate types of reactions. (2, 5)
 Predict reactivity for precipitation and neutralization reactions (5)
 Determine the molecular formula, ionic formula, and net ionic formula for precipitation and
neutralization reactions. (5)
H.
Chemical Composition
 Use Avogadro’s number to determine the number of objects in a sample (5)
 Use molar mass to determine the mass of a sample (5)
 Determine the percent composition from a chemical formula (5)
 Determine the empirical and molecular formulas from the percent composition. (5)
I.
Chemical Quantities
 Use mole to mole relationships to convert between substances in a chemical reaction (5)
 Determine the limiting reactant in a chemical reaction and determine the amount of product that
can be made (5)
 Determine the percent yield of a reaction (5)
J.
Energy
 Determine the difference between potential energy and kinetic energy (2)
 Label a process as exothermic or endothermic (5)


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K.
L.
M.
N.
O.
P.
Use specific heat capacity to determine the heat flow and temperature change (5)
Use enthalpy to determine the heat exchange in a chemical reaction (5)
Use Hess’s Law to determine the enthalpy of an unknown reaction. (5)
Determine the spontaneity of a reaction using enthalpy and entropy. (5)
Modern Atomic Theory
Describe electromagnetic radiation by wavelength, frequency, and energy (5)
Describe emission of electromagnetic radiation by atoms and line diagrams (5)
Describe the Bohr model of the atom and Schrodinger’s wave mechanical model of the atom (2)
Write the electron configuration, condensed electron configuration, and orbital diagram for
elements (5)
 Determine the ionization energy and electron affinity for an atom based on periodic trends. (5)
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
Chemical Bonding
 Explain the difference between ionic, polar covalent, and covalent bonding (2)
 Use electronegativity to determine the type of bonding present in a molecule. (5)
 Write a reasonable Lewis Dot Structure of various molecules (5)
 Determine resonance structures where appropriate (5)
 Determine the molecular geometry and shape of the molecule (5)
Gases
Define pressure and its associated units (5)
Define Boyle’s, Charles’s, and Avogadro’s law and be able to complete calculations involving
these laws (5)
 Successfully complete calculations involving the Ideal Gas Law (5)
 Determine the pressure of gases using Dalton’s Law of Partial Pressure (5)
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
Liquids and Solids
 Distinguish between intermolecular and intramolecular forces (5)
 Define and describe London Dispersion Forces, Dipole-Dipole Forces, and Hydrogen Bonding (2)
 Use the heat of fusion and heat of vaporization to determine the energy associated with phase
changes (5)
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

Solutions
Describe a solution using the terms saturated, unsaturated, concentrated, and dilute (2)
Determine the composition of a solution using mass percent and molarity (5)
Determine how to make a solution using dilution (5)
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Acids and Bases
Define Bronsted-Lowry Acids and Bases (2)
Determine the concentration of hydronium and hydroxide ion in a solution (5)
Determine the pH and pOH of a solution (5)
Define a Buffer and explain its uses. (2)
Q. Instrumentation
 Define instrumentation. (2)
 Describe the principles of paper chromatography and explain advantages and disadvantages. (2)
 Describe the operation of a gas chromatograph.(2)
 Describe the operation of a liquid chromatograph. (2)
 Describe spectrophotometry. (2)
 Operate analytical balances. (5)