DEPARTMENT OF SCIENCE
COURSE INFORMATION SHEET FOR
CHE111 – GENERAL CHEMISTRY I
All members of the Science Department at Clinton Community College use the respective course
templates as a basis for their course syllabi. Faculty may, at their discretion, change the order
of the course content or add course content.
COURSE NUMBER AND TITLE: CHE111 – General Chemistry I
COURSE SECTION: TBA
CONTACT HOURS: 5
CREDIT HOURS: 4
SEMESTER AND YEAR: TBA
INSTRUCTOR’S NAME, TELEPHONE NUMBER, EMAIL ADDRESS, OFFICE
NUMBER, AND OFFICE HOURS: TBA
I. COURSE DESCRIPTION:
This is the first semester course in a two-semester sequence which presents the basic laws and
concepts of general quantitative chemistry. This course will include measurement,
stoichiometry, thermochemistry, the periodic table, an introduction to acids and bases, reduction
and oxidation, ionic and covalent bonding, molecular structure, VSEPR and MO Theory. There
are three hours of lecture and one two-hour laboratory per week.
This course meets the SUNY General Education course requirements for natural sciences.
II. PREREQUISITE: ENG094 – Fundamentals of Composition and MAT101 or equivalent or
higher.
Students receiving credit for CHE111 and/or CHE112 cannot receive credit for CHE101.
III. COURSE OBJECTIVES, SUNY GENERAL EDUCATION KNOWLEDGE AREA
LEARNING OUTCOMES AND ASSESSMENT:
COURSE OBJECTIVES:
As the result of instructional activities, students will be able to:
1. use appropriate chemical terminology and nomenclature to effectively communicate their
understanding of concepts in chemistry
2. describe the phases of matter and their molecular and elemental properties
a. distinguish between solids, liquids, gases and plasmas
3. define the difference between homogeneous & heterogeneous mixtures
a. identify and apply methods of separation of mixtures using physical properties
Revised 9/13
b. apply methods of separation using chemical instrumentation such as HPLC & GC
4. explain atomic theory, atomic structure, atomic mass, atomic number, isotopes and ions
of a given particular element
a. calculate atomic mass from mass spectroscopy data to determine the atomic mass
of an element on the periodic table
b. define the concept of a mole, molar mass and Avagadro’s number
c. calculate conversion between grams to moles and moles to grams
5. describe stoichiometry with respect to reactions and solve related problems
a. write balanced equation
b. determine stoichiometric relationships between reactants and products
c. calculate limiting reactants, excess reactants, theoretical yield, & percent yield
6. explain chemical reactions and distinguish between the different types
a. identify and balance combination, decomposition, displacement, and metathesis
reactions
b. write and balance ionic and net ionic equations, precipitation reactions with
respect to solubility, neutralization reactions, red-ox reactions, and combustion
reactions
7. define acids and bases in terms of Arrhenius
a. calculate molarity
b. describe titrametric methods
8. explain kinetic and potential energy, concept of heat, heat capacity, and enthalpy
a. distinguish between endothermic and exothermic processes
b. calculate specific heats of reactions
c. define and use Hess’s Law to calculate the enthalpy of a reaction
d. calculate standard enthalpies of formation
9. describe the concepts in quantum mechanics to explain electron motion
a. describe a photon and how it is emitted
b. define line spectra and give examples
c. describe the electromagnetic spectrum and how each type of radiation relates to
the others with respect to wavelength, frequency and energy
d. define Heisenberg’s uncertainty principle
e. list the 4 quantum numbers, giving both symbol and name, and explain what each
one means and give an example
f. draw all the orientations of s, p, and d orbitals
10. define electron configuration and periodicity for all elements
a. write electron configuration and orbital diagrams for all elements from H to Ba
and their ions
b. list Aufbar’s filling order
c. define periodic trends with respect to ionization energy, electron affinity and
atomic radii
11. explain bonding and molecular structures using VSEPR and MO theory
a. write complete bond descriptions including hybrid orbital’s of sp, sp2 and sp3
b. draw Lewis structures for molecules, identify the bond directions, geometry and
hybridization
c. describe linear, trigonal planar, tetrahedral, trigonal bipyramidal and octahedral
molecular geometry, sub-classifications of each and the associated vertex angle
for the 5 geometric model
d. draw a Molecular Orbital Diagram (MO) for all diatoms from H2 to Ne2,
determine the bond order, and if the molecule is paramagnetic or diamagnetic
Revised 9/13
LAB OBJECTIVES:
The laboratory experience will reinforce the understanding that experimental work is the
foundation of chemical knowledge and which requires fundamental laboratory skills. Students
will:
1. anticipate, recognize, and respond properly to potential hazards in laboratory procedures
a. complete laboratory safety training as designed by the CCC science department
b. review the contents of MSDS & location of MSDS sheets storage area
2. keep accurate and complete experimental records
a. write all lab records in a bound lab notebook using Proper Lab Documentation
(PLD) as required for Good Lab Practices (GLP)
b. enter all data as it is generated in the lab
3. perform accurate quantitative measurements
a. use properly calibrated instruments (i.e. spectrophotometers) and volumetric
glassware
4. interpret experimental results and draw reasonable conclusions
a. record in the lab notebook all information/data using tables, graphs, formulas and
calculations
b. write a conclusion of results in the lab notebook at the end of each lab to
summarize what was discovered in the laboratory
5. communicate effectively through oral and written reports
a. write 3 formal lab reports – Empirical Formula, Hess’s Law and UV/Vis
Spectroscopy
b. report required information such as tables, graphs, formulas, calculations
background and summary in electronic format
c. use Excel, Word and PowerPoint to present laboratory data and reports to the
instructor and classmates as required
6. analyze data statistically, assess the reliability of experimental results, and discuss the
sources of systematic and random error in experiments
a. use statistical interpretation as needed in the summary of lab information and
required lab reports
b. include correlation of data on all graphs via electronically generate linear trend
lines
7. plan & execute experiments through the use of appropriate chemical literature &
electronic resources
a. research background information required for labs and lab reports from reputable
sources such as American Chemical Society (ACS) or .edu, .org, and .gov
websites
LAB ACTIVITIES:
A complete list of proposed laboratory activities must be submitted with the course syllabus.
NUMBER
LAB 1
LAB 2
TITLE of LAB EXERCISE
Introduction, Lab Safety, MSDS & Orientation (PLD)
Mixtures and Separations
Revised 9/13
LAB 3
LAB 4
LAB 5
LAB 6
LAB 7
LAB 8
LAB 9
LAB 10
LAB 11
LAB 12
LAB 13
LAB 14
LAB 15
Density and Measurement
Empirical Formula
Ions and Polyatomic Ions
Solubility & Net Ionic Equations
Conductivity and pH of Various Solutions
Acid /Base Titration
Hess’s Law
Hess’s Law Calculations
Absorption Spectroscopy
Electron Configuration
Lewis Structures
VSEPR & Molecular Geometry
Final Assessment
SUNY GENERAL EDUCATION KNOWLEDGE AREA LEARNING OUTCOMES:
Students will demonstrate the ability to:
1. understand the methods scientists use to explore natural phenomena, including:
 observation
 hypothesis development
 measurement and data collection
 experimentation
 evaluation of evidence
 employment of mathematical analysis
2. apply scientific data, concepts and models in one of the natural sciences
IV. REQUIRED TEXTBOOK AND MATERIALS:
REQUIRED TEXTBOOK:
Gilbert, Thomas R., Kirss, Rein V., Foster, Natalie, and Davies, Geoffrey, Chemistry, The
Science In Context, 3rd Edition, W.W. Norton’s & Company
ISBN: 978-0-393-93431-1
REQUIRED MATERIALS:
A scientific or graphing calculator, a bound composition notebook with graph paper pages for
lab, safety glasses, and a straight edge are all required for this course.
V. METHODS OF INSTRUCTION/COURSE ORGANIZATION: To be determined by the
respective instructor.
VI. ATTENDANCE PROCEDURE (INCLUDING MAKEUP POLICY): To be determined
by the respective instructor.
VII. BIBLIOGRAPHY OF READINGS (IF APPLICABLE): To be determined by the
respective instructor.
Revised 9/13
VIII. METHODS OF EVALUATION (INCLUDING THE CALCULATION OF COURSE
GRADE): To be determined by the respective instructor. The methods of evaluation shall
include tests (test types, length and weight of each), papers (weight of each), projects (weight of
each), and other forms of evaluation (weight of each).
IX. GRADING SCALE: To be determined by the respective instructor. The grading scale shall
indicate what numerical scores correspond to the following grades: A, A-, B+, B, B-, C+, C, C-,
D+, D, and F.
Please Include: If you have, or suspect you may have, any type of disability or learning problem
that may require extra assistance or special accommodations, please speak to me privately after
class or during my office hours as soon as possible so I can help you obtain any assistance you
may need to successfully complete this course. You should also contact Laurie Bethka, Room
420M in the Academic Assistance Center, for further assistance.
X. GENERAL TOPICS OUTLINE:
1. Matter & Measurement
2. Atoms & Elements
3. Molecules, Ions & Their Compounds
4. Reactions in Aqueous Solutions
5. Principles of Reactivity: Energy & Chemical Reactions
6. Atomic Structure
7. Atomic Electron Configuration & Chemical Periodicity
8. Bonding and Molecular Structure
9. Bonding and Molecular Structures
10. Carbon
XI. ACADEMIC INTEGRITY: Academic honesty is expected of all Clinton Community
College students. It is academically dishonest, for example, to misrepresent another person’s
work as one’s own, to take credit for someone else’s work or ideas, to accept help on a test, to
obtain advanced information on confidential test materials, or to intentionally harm another
student’s chances for academic success.
XII. COURSE CONTINUITY PLAN: In the case that the college officially closes because of
an emergency which causes a short term disruption of this course, we will utilize e-mail to
continue this course in the short term (1-3 weeks). All students need to utilize their campus email to receive course related information.
XIII. TECHNOLOGY STATEMENT: A CCC student should expect that any class may
require some course activity that uses a computer and the internet. Activities could include but
are not limited to accessing the course syllabus, schedule, or other handouts on a website,
completing homework online, taking quizzes or submitting written work, participating in a
discussion or sending/receiving email.
Revised 9/13