HARFORD COMMUNITY COLLEGE
CHEM 135 – Chemistry for Engineers
Course Information
EFFECTIVE DATE
Spring 2009
DATE SUBMITTED
January 2008
COURSE NUMBER
CHEM 135
COURSE TITLE
Chemistry for Engineers
PREREQUISITE(S)/CO-REQUISITES
Completion of MATH 017 or MATH 018, or placement
into College Level math and high school Algebra II and
Trigonometry, or high school precalculus.
DIVISION
STEM
BUDGET ORG
NUMBER
1143
SUBJECT
Chemistry
INITIATOR
Steven Iwanowski
DIVISION LEADER
Deborah Wrobel
NUMBER OF CREDITS
4
TOTAL INSTRUCTIONAL HOURS
90 (45 lecture hours, 45 lab hours)
RECOMMENDED CLASS SIZE
24
START-UP COST
0
COURSE FEE
$40
Course Description: CHEM 135 Chemistry for Engineers (4 credits)
Chemistry for Engineers is a one-semester course, with laboratory, covering general
chemistry topics designed specifically for engineering students. Topics include
atomic/molecular structure, the periodic table, chemical reactions, chemical bonding,
equilibrium, kinetics, thermodynamics, electrochemistry, and gas laws. A mathematical
approach will be used throughout the course emphasizing data acquisition and manipulation,
uncertainty and significant figures. The course includes an introduction to basic laboratory
techniques, obtaining measurements, and safety. This course is for non-chemical
engineering students; science majors need to complete the CHEM 111-CHEM 112
sequence. 45 hours of lecture/discussion and 45 hours of lab. Prerequisite: Completion of
MATH 017 or MATH 018, or placement into College Level math and high school Algebra II
and Trigonometry, or high school precalculus. Recommended: CHEM 010 or high school
chemistry. Course fee.
Student Learning Objectives (previously known as course objectives) Linked to
Relevant Academic Outcomes
Upon satisfactory completion of this course, the student will be able to:
1. Describe the relevance of chemistry to civil, mechanical, and electrical engineering.
(Academic outcomes supported by this learning objective: Science and Technology,
Communication, Critical Thinking)
2. Describe atomic structure, electronic structure of atoms, and periodic trends of the
elements. (Academic outcomes supported by this learning objective: Science and
Technology, Communication, Critical Thinking)
3. Perform stoichiometric calculations based on balanced chemical reactions. (Academic
outcomes supported by this learning objective: Critical Thinking, Computational Skills,
Science and Technology)
4. Differentiate between and define ionic and covalent bonding in chemical compounds.
(Academic outcomes supported by this learning objective: Critical Thinking,
Computational Skills, Science and Technology)
5. Define chemical thermodynamics and the terms ΔG, ΔH, ΔS and use the calculation of
ΔG to predict spontaneity of a reaction. (Academic outcomes supported by this learning
objective: Critical Thinking, Computational Skills, Science and Technology)
6. Calculate pH and equilibrium constants and apply Le Châtelier’s principle to systems at
equilibrium. (Academic outcomes supported by this learning objective: Critical
Thinking, Computational Skills, Science and Technology)
7. Define electrochemistry, draw, label and perform calculations with electrolytic and
galvanic cell reactions. (Academic outcomes supported by this learning objective:
Critical Thinking, Computational Skills, Science and Technology)
8. Perform calculations of reaction rates and explain the factors that affect a reaction rate.
(Academic outcomes supported by this learning objective: Critical Thinking,
Computational Skills, Science and Technology, Communication)
9. Conduct basic data acquisition and analysis using good laboratory practices in a safety
conscious manner. (Academic outcomes supported by this learning objective: Critical
Thinking, Computational Skills, Science and Technology, Communication, Interpersonal
Skills)
Course Outline
I. FUNDAMENTALS OF CHEMISTRY
A. Introduction
B. Matter and its Properties
C. Atomic Theory
D. Molecules and Representations
E. Reactions and Stoichiometry
II. FOUNDATIONS
A. Atomic Structure
B. The Periodic Table
C. Light and the Model of the Atom
D. Electron Configurations
III. PERIODICITY
A. Periodic Table Trends
B. Classifications of the Elements
IV. CHEMICAL BONDING
A. Ionic and Covalent Bonds
B. Bond Polarity
C. Molecular Orbital Theory
V. SHAPE AND INTERMOLECULAR INTERACTION
A. Lewis Dot Structures, Octet Rule
B. Molecular Geometry and Molecular Polarity
C. Intermolecular Forces
VI. THERMODYNAMICS
A. Endothermic vs. Exothermic
B. First Law of Thermodynamics
C. Second Law of Thermodynamics, ΔG, ΔH, ΔS
VII. EQUILIBRIUM
A. Gas Reactions and Gas Laws
B. Solutions, Acid/Base
C. Equilibrium Constants
D. Le Châtelier’s Principle
VIII. ELECTROCHEMISTRY
A. Oxidation Numbers
B. The Activity Series
C. Galvanic Cells and Batteries
D. Redox Reactions
IX. KINETICS
A. Reaction Rates and Temperature
B. Rate Laws
C. Catalysts
Instructional Method(s)
To achieve student learning objectives, instruction includes:
Lecture, demonstrations, process-oriented guided-inquiry learning, problem-solving and
laboratory exercises.
Assessment Method(s)
Quizzes, exams, laboratory assignments and reports.
Textual Material(s)
Title: Chemistry for Engineers, An Applied Approach
Author or Editor: Mary Jane Shultz
Publisher: Houghton Mifflin Company
Date: 2007
Title: Laboratory Manual for Principles of General Chemistry, 8th ed.
Author or Editor: J.A. Beran
Publisher: John Wiley & Sons, Inc.
Date: 2008