DEPARTMENT OF SCIENCE
COURSE INFORMATION SHEET FOR
CHE112 – GENERAL CHEMISTRY II
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: CHE112 – General Chemistry II
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 second semester course in a two-semester sequence which presents the basic laws and
concepts of general quantitative chemistry. This course will focus on the principles of reactivity
of solids, liquids and gases with respect to chemical kinetics, chemical equilibrium, acid-base
chemistry, precipitation reactions, entropy, free energy, red-ox chemistry, and an introduction to
nuclear chemistry. There are three hours of lecture and one two-hour laboratory per week.
II. PREREQUISITE: CHE 111
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. define the Basic Gas Laws
i. perform calculations using Boyle’s, Charles, Gay-Lussac’s and the Ideal
Gas Laws
ii. define partial pressure and Dalton’s Law
iii. define the Kinetic-Molecular Theory of Gases
iv. define the Real Gas Law behavior
b. describe the difference between diffusion & effusion
c. define the properties of liquids
revised 3/12
i. define surface tension, capillary action & viscosity
ii. define vapor pressure
iii. define boiling
d. distinguish between the intermolecular forces involving polar molecules
e. distinguish between the intermolecular forces involving non-polar molecules
f. distinguish between different types of solids
g. draw a phase diagram and label it completely
3. define the units of concentration
a. calculate molarity, molality, mole fraction, weight percent, and ppm
b. convert concentrations from one unit to another
4. explain solubility of solutions
a. describe the process of liquids dissolving in liquids
b. describe the process of solids dissolving in liquids
c. define factors that affect solubility of gases dissolved in liquids in terms of
Henry’s Law
d. calculate the enthalpy of solutions from thermodynamic data
5. describe colligative properties of solutions
a. calculate Raoult’s Law for changes in vapor pressure
b. determine the boiling point elevation, freezing point depression and use
colligative properties to calculate variables present in these relationships (molar
mass and molality)
6. distinguish between the different types of colloids
a. identify and explain how a surfactant works
b. define osmotic pressure
7. determine rates of chemical reactions
a. determine order of reactions
i. calculate and graph first-order reaction kinetic data
ii. calculate and graph second-order reaction kinetic data
iii. calculate and graph zero-order reaction kinetic data
iv. calculate and graph half-life for first, second & zero-order reactions
b. write a rate equation
c. determine the rate constant (k)
i. calculate R (rate) using a rate law expression and k
d. describe reaction conditions that determine reaction rates
8. explain Collision Theory
a. distinguish between the effect concentration and temperature has on reaction rates
b. calculate activation energy using the Arrhenius Equation
c. define the function of a catalyst and the effect it has on reaction rates
9. describe reaction mechanisms
a. describe molecularity and rate equations for elementary steps
b. define molecularity and reaction order
c. determine reaction mechanisms from kinetic data
10. define chemical equilibrium
a. write an equilibrium constant expression for a balanced equilibrium reaction
b. define the meaning of the equilibrium constant K
c. determine the reaction quotient Q for a reaction
d. use equilibrium constants in calculations
11. explain Le Chateliers Principle
a. explain the effects of the addition or removal of reactants or products
b. explain the effects of volume changes on gas-phase equilibria
revised 3/12
c. explain the effects of temperature changes on equilibria
12. define acids and bases in terms of Arrhenius, Bronsted-Lowry and Lewis
a. describe basic properties of acids & bases
b. determine conjugate acid base pairs
c. explain cationic & molecular Lewis acids and Lewis bases
13. describe the self ionization of water and Kw
a. describe and calculate Ka & Kb in acid base equilibria
i. predict the direction of an acid base equation
14. define the pH scale and calculate pH using logarithms and Kw
a. determine the relationship of acid-base reactions with respect to strength of each
reactant
b. perform an acid base titration
15. define pKa and calculate using the Henderson-Hasselbach equation
16. determine the molecular structure, bonding and behavior of acids and bases
a. determine the acid strength of metal halides
b. compare strengths of oxoacids
c. describe carboxylic acids and draw its functional group
17. define the common ion effect
a. calculate concentration and pH of buffered solutions
i. construct a pH titration curve
18. define solubility of slightly soluble salts and determine Ksp
a. explain the effect of basic anions on salt solubility
19. define entropy & free energy
a. calculate standard enthalpy values
b. summarize spontaneous reactions
c. calculate Gibbs free energy
i. define standard free energies of formation
20. define oxidation-reduction reactions
a. balance red-ox equations
21. describe simple and commercial voltaic cells
a. draw a voltaic cell from electrochemical cell notation
b. define dry cells and alkaline batteries
c. describe a fuel cell
22. determine standard electrochemical potentials
a. use a table of standard reduction potentials
b. describe relative strengths of oxidizing and reducing agents
c. define the Nernst equation
23. define natural radioactivity
a. determine rates of nuclear decay
b. write balance nuclear equations
c. describe the difference between nuclear fission and nuclear fusion
24. describe the kinetics of nuclear decay
a. calculate half-life of a nuclear reaction
b. describe carbon dating
c. define nuclear medicine and explain its uses
25. define the processes, pros and cons of nuclear energy
LAB OBJECTIVES:
revised 3/12
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 5 formal lab reports – Freezing Point Depression, Iodine Clock, Le
Chatelier’s Principle, Acid/Base Titration of an Unknown Acid, and pH Titration
Curve
b. write 2 Standard Operating Procedures (SOP’s) – Calibration of a pH Meter and
Calculations of Buffered Solutions
c. perform 2 oral laboratory presentations/demonstrations – Solids, Liquids & Gases
and Electrochemistry
d. report required information such as tables, graphs, formulas, calculations
background and summary in electronic format
e. 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)
Solids, Liquids & Gases
revised 3/12
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
Freezing Point Depression
Solutions – Units of Concentration
Preparation of Solutions for Iodine Clock
Iodine Clock Reaction
Iodine Clock Calculations
Le Chatelier’s Principle – Haber-Bach Process
Standardization of NaOH
Acid /Base Titration of an Unknown Acid
Calibration of a pH Meter
pH Titration Curve
Preparation & Calculations of Buffered Solutions
Presentations in Electrochemistry
Chernobyl & the Nuclear Regulatory Commission
IV. REQUIRED TEXTBOOK AND MATERIALS:
REQUIRED TEXTBOOK:
Kotz, John C. and Treichel, Paul Jr., Chemistry & Chemical Reactivity, seventh edition,
Thomson Brooks/Cole, 2009. ISBN# 978-0-495-38703-9
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, but must include a literature project of the students choice that meets the
following criteria.
A six to ten page term paper on any current research being done in CHEMISTRY that interests
the student is to be organized and written over the semester. The paper must have at least 5 juried
references, 2 may be from the Internet. The other three sources must be from a current book
and/or scientific journal. All sources must be properly referenced by APA, MLA, or ACS and
depending on choice, must be consistent throughout the paper.
The paper should answer a question concerning a specific “current” research topic in chemistry.
The paper is developed by answering a specific question. It should be focused on a “narrow”
topic rather than staying too broad. Some topics of interest are but not limited to
chemical/industrial processes, forensic chemistry, atmospheric chemistry, nutrition, health,
medicine, genetics, environmental issues, nanotechnology or other chemical technology.
Bibliographic instruction should be presented to the students during the first 2 weeks of the
semester. The topic of the term paper should be approved by the instructor about 2 weeks into
revised 3/12
the semester, an outline should be submitted before mid-semester and the final paper due before
finals week.
The paper should be structured in the following way and appear so in the outline.
1. Introduction – This should contain a discussion of the question or problem that is to be
presented in the paper. ex. What is being done on "state-of-the-art control technology" used
to sequester CO2 in coal-fired electrical power generation?
2. General Background – This section should include a discussion of the chemicals pertinent to
the topic. Chemical structure, molecular weight, physical and chemical properties, general
reactivity, and reaction mechanisms are all part of this section.
3. Current Research & Theoretical Perspectives– The student will discuss the current research
being done on this topic as well as theories that are used to explain the research topic as
presented by the researcher. (This is the bulk of the paper.)
4. Opinion – This section includes the student’s perspective on the "science" of this topic and
should emphasis agreement or disagreement with the information, research, and approach
with respect to the current research and theoretical perspectives. A discussion on ethics
relative to this topic could also take place in this portion of the paper if applicable.
5. Conclusion – The student will wrap the paper up into a final discussion or summary that
serves as an overview of the question or statement made in the introduction.
6. Bibliography - must be complete and follow the style writing chosen to use in the paper.
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. Gases & Their Properties
2. Intermolecular Forces & Liquids
3. Chemistry of Solids
4. Solutions & Their Behavior
5. Chemical Kinetics
6. Chemical Equilibrium
7. Acids & Bases & Other Aspects of Aqueous Equilibria
8. Entropy & Free Energy
9. Electrochemistry
10. Nuclear Chemistry
revised 3/12
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 3/12