CHE 201B – Section A: General Chemistry
Dr. Diana Nabhan (Zahle)
AMERICAN UNIVERSITY OF SCIENCE & TECHNOLOGY
FACULTY OF ENGINEERING
DEPARTMENT OF BIOMEDICAL ENGINEERING
DEPARTMENT OF MECHATRONICS ENGINEERING
DEPARTMENT OF COMPUTER AND COMMUNICATIONS ENGINEERING
CHE 201B: GENERAL CHEMISTRY
Spring-Term 2018-2019
INSTRUCTOR
Diana Nabhan, Ph.D.
LECTURE HOURS
T-TH 4:00 pm - 5:15 pm
Room: 302, Block B
OFFICE HOURS
T
3:00 pm - 4:00 pm
Otherwise by appointment
Room: Instructor’s Lounge
COURSE OBJECTIVES
This course deals with general chemical principles. The goal of this course is to provide
knowledge on the basics of atomic structure, chemical bonds, chemical reactions, gases,
solutions, reaction equilibria, with emphasis on the practical aspects of chemistry in numerous
health-related situations.
COURSE PREREQUISITES
ENG 001: INTENSIVE ENGLISH II
PREREQUISITES BY TOPICS The student should have some competencies in basic
physics and mathematics upon which CHE 201B will be built.
COURSE CREDITS
3 Credit Hours
INSTRUCTION TECHNIQUE
Lectures will be used predominantly. These will be supported by problem sets and problem
solving sessions.
REQUIRED TEXTS
 Stoker H.S. General, Organic, and Biological Chemistry. Sixth Edition. Boston, MA:
Houghton Mifflin Company, 2012.
REFERENCES
 Ebbing D.D. and Gammon S.D. General Chemistry. Ninth Edition. Boston, MA:
Houghton Mifflin Company, 2009.
OTHER REQUIREMENTS
 A scientific calculator - an inexpensive one will do.
 Straight-edge ruler.
 Engineering paper - A4 Notepad.
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CHE 201B – Section A: General Chemistry

Dr. Diana Nabhan (Zahle)
Access to the internet.
GRADE DISTRIBUTION
This course involves a number of didactic activities, ranging from lectures, problem sets,
problem solving sessions, to quizzes, exams, and final exam. All of these attributes of the
course are intended to help the student in developing his/her understanding of the material
covered in CHE 201B and in providing the department and the course instructor with
information on how the student is doing. Consequently, all of these activities are considered
to be vital and will be taken into consideration while assigning grades at the end of the term.
When the student is being assigned a course grade, it is imperative that this grade accurately
reflects the student’s level of achievement and his/her mastery of the material covered in CHE
201B. A breakdown of the weighting that will be used in making this assessment is as
follows:
Class Attendance
Quizzes
Problem Sets
Class Exams
Exam No. 1
Exam No. 2
Exam No. 3
Final Exam
ATT
5%
QZS
5%
HWK 15%
EX1
EX2
EX3
FIN
20%
20%
20%
35%
Note: Two out of the three exams will be counted towards the final course grade based on the
highest grades attained. No make-up exams are allowed. Late assignments will be dealt with
according to the distributed course rules and regulations, which are governed by the
Department of Biomedical Engineering. Under severe conditions, only the Final Exam is
allowed to be petitioned; however, students have to realize that in the event that a make-up
Final Exam is granted, it would be unjust that the grantee becomes privileged over his/her
fellow colleagues in terms of extra-time to prepare for the exam and in developing an idea
about the contents of the exam. Accordingly, the make-up Final Exam will carry an increased
level of difficulty of at least 20% from the regular exam.
COURSE COMPETENCIES
This course contributes primarily to the students' knowledge of General Chemistry and
prepares the Biomedical Engineering student for advanced topics in Organic Chemistry,
Biochemistry, and Biomaterials. At the end of the course, the student should be able to
perform the following tasks:
1.
2.
3.
4.
Demonstrate an understanding of what exactly is chemistry about.
Know the common terminology associated with the field of chemistry.
Demonstrate an understanding of measurements in chemistry.
Understand the fundamental types of subatomic particles, how they arrange
themselves within an atom, and the relationship between an atom’s subatomic makeup
and its chemical identity.
5. Understand why atoms tend to join together in larger units and comprehend the
binding forces (chemical bonds) that hold them together – The Ionic and Covalent
Bond Models.
6. Demonstrate an understanding of how to represent chemical reactions by using
chemical equations and how to derive quantitative relationships from these chemical
equations.
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CHE 201B – Section A: General Chemistry
Dr. Diana Nabhan (Zahle)
7. Understand the properties exhibited by matter in the various physical states - solid,
liquid, and gas - and the correlation of these properties with molecular behavior.
8. Demonstrate an understanding of solutions and their characteristic properties.
9. Understand the chemical changes that occur when various types of matter interact, the
various types of chemical reactions, chemical reaction rates, and chemical
equilibrium.
10. Develop an understanding of acids, bases, and salts and their role in biochemical
systems and the chemical industry.
11. Develop an understanding of nuclear reactions and the associated terms: radioactivity,
nuclear power plants, nuclear weapons, and nuclear medicine.
ATTENDANCE
For legitimate reasons only, a student is allowed to absent him/herself for a maximum of 6
contact hours 1 from the course lectures and the tutorial and laboratory sessions.
However, any absence of more than two sessions will be counted toward the 5% evaluation of
the course grade. Absences beyond the specified maximum limit will result in an automatic
AW in the course and possibly other disciplinary measures. An unexcused absence from an
unannounced quiz will result in a zero on that quiz. Should the student be absent from a
lecture during which a problem set is due, it is the duty of the student to make certain that the
homework assignment is handed in on time. Failure to do so will incur a penalty on that
assignment’s grade.
ACADEMIC INTEGRITY
The student should get familiar with the Course Rules and Regulations of the Departments
of Biomedical Engineering (BME), Mechatronics Engineering (MTE) and Computer and
Communications Engineering (CCE) at AUST. These are compiled and distributed to the
student at the beginning of every academic term. In particular, the student should be aware
that plagiarism, abuse of laboratory facilities, and other sorts of academic dishonesty are not
tolerated and can result in unsympathetic penalties.
The Departments of BME, MTE and CCE fully acknowledge the potential significance of
students studying together. In this sense, the BME, MTE and CCE Departments do not have
any reservation to this kind of collaboration, as long as all contestants are involved in all
facets of the work, and not with each individual contributing to a fraction of the assignment.
Specifically, when a student submits an assignment with his/her name on it, the BME , MTE
and CCE Departments take it for granted that the details presented in the assignment are
entirely the student’s own work, and that this student has substantially participated in the
creation of this work. If a portion of the work has been conceived by collaborative work, that
section should be highlighted and the names of the students involved in this collaboration
should be listed next to that section.
PROBLEM SETS
For most part of the course, problem sets will be assigned on a weekly basis. A detailed
description of the problem set assignment timetable is compiled at the end of this handout.
All problem sets are graded on a five-point scale, from 0 to 4. The following table delineates
the effort required to achieve each of these grade points.
Grade
0
1
Description
The student fails to turn in the homework assignment
A contact hour is equivalent to 75 minutes.
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CHE 201B – Section A: General Chemistry
1
2
Dr. Diana Nabhan (Zahle)
The student turns in the homework assignment, but basically, did nothing worthwhile.
The student turns in the homework assignment, however most of the problems are either incomplete
or non-understandable.
The student completes most or all of the problems in the assignment; however, the student still has
some evident mistakes in the worked solution.
The student completes all of the problems in the assignment, with perhaps little insignificant
mistakes; however in general, the student demonstrates a solid understanding of the material.
3
4
Graded assignments will be returned to the students after two lectures from the onset of their
submission.
COURSE OUTLINE BY TOPIC
The day-to-day topics to be covered in the table below may be adjusted as the subject proceeds, but
all examination dates are fixed, and problem set due dates are unlikely to change.

Syllabus

Basic Concepts About Matter (3 Lectures)
-
Week No.
1
1-2
Physical States of Matter
Properties of Matter
Changes in Matter
Pure Substances and Mixtures
Elements and Compounds
Discovery and Abundance of the Elements
Names and Chemical Symbols of the Elements
Atoms and Molecules
Chemical Formulas

Measurements in Chemistry (2 Lectures)
Measurement Systems
Metric System Units
Exact and Inexact Numbers
Uncertainty in Measurement and Significant Figures
Significant Figures and Mathematical Operations
Scientific Notation
Conversion Factors and Dimensional Analysis
Density
Temperature Scales
2-3

Atomic Structure and the Periodic Table (2 Lectures)
Internal Structure of an Atom
Atomic Number and Mass Number
Isotopes and Atomic Masses
The Periodic Law and the Periodic Table
Metals and Nonmetals
Electron Arrangements within Atoms
Electron Configurations and Orbital Diagrams
The Electronic Basis for the Periodic Law and the Periodic Table
Classification of the Elements
3-4
EXAM No. 1: Tuesday, March 12, 2019

Chemical Bonding: The Ionic Bond Model (2 Lectures)
Chemical Bonds
Valence Electrons and Lewis Symbols
The Octet Rule
The Ionic Bond Model
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CHE 201B – Section A: General Chemistry
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Dr. Diana Nabhan (Zahle)
The Sign and Magnitude of Ionic Charge
Ionic Compound Formation
Chemical Formulas for Ionic Compounds
The Structure of Ionic Compounds
Recognizing and Naming Binary Ionic Compounds
Polyatomic Ions
Chemical Formulas and Names for Ionic Compounds
Containing Polyatomic Ions

Chemical Bonding: The Covalent Bond Model (3 Lectures)
The Covalent Bond Model
Lewis Structures for Molecular Compounds
Single, Double, and Triple Covalent Bonds
Valence Electrons and Number of Covalent Bonds Formed
Coordinate Covalent Bonds
Systematic Procedures for Drawing Lewis Structures
Bonding in Compounds with Polyatomic Ions Present
Molecular Geometry
Electronegativity
Bond Polarity
Molecular Polarity
Naming Binary Molecular Compounds
6-7

Chemical Calculations: Formula Masses, Moles (2 Lectures)
and Chemical Equations
Formula Masses
The Mole: A Counting Unit for Chemists
The Mass of a Mole
Chemical Formulas and the Mole Concept
The Mole and Chemical Calculations
Writing and Balancing Chemical Equations
Chemical Equations and the Mole Concept
Chemical Calculations Using Chemical Equations
7-8
EXAM No.2: Thursday, April 11, 2019

Gases, Liquids, and Solids (3 Lectures)
The Kinetic Molecular Theory of Matter
Kinetic Molecular Theory and Physical States
Gas Law Variables
Boyle’s Law: A Pressure-Volume Relationship
Charles’s Law: A Temperature-Volume Relationship
The Combined Gas Law
The Ideal Gas Law
Dalton’s Law of Partial Pressures
Changes of State
Evaporation of Liquids
Vapor Pressure of Liquids
Boiling and Boiling Point
Intermolecular Forces in Liquids

Solutions (2 Lectures)
Characteristics of Solutions
Solubility
Solution Formation
Solubility Rules
Solution Concentration Units
Dilution
Colloidal Dispersions
Colligative Properties of Solutions
Osmosis and Osmotic Pressure
9-10
10-11
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CHE 201B – Section A: General Chemistry
Dr. Diana Nabhan (Zahle)
EXAM No. 3: Thursday, May 2, 2019
 Chemical Reactions (2 Lectures)
Types of Chemical Reactions
Redox and Nonredox Reactions
Terminology Associated with Redox Processes
Collision Theory and Chemical Reactions
Exothermic and Endothermic Reactions
Factors that Influence Reaction Rates
Chemical Equilibrium
Equilibrium Constants
Altering Equilibrium Conditions: Le Châtelier’s Principle
12-13
 Acids, Bases, and Salts (3 Lectures)
Arrhenius Acid-Base Theory
Brønsted-Lowry Acid-Base Theory
Mono-, Di-, and Triprotic Acids
Strengths of Acids and Bases
Ionization Constants for Acids and Bases
Salts
Acid-Base Neutralization Reactions
Self Ionization of Water
The pH Concept
The pKa Method for Expressing Acid Strength
The pH of Aqueous Salt Solutions
Buffers
The Henderson-Hasselbalch Equation
Electrolytes
Acid-Base Titrations
13-14
 Nuclear Chemistry (3 Lectures)
Stable and Unstable Nuclides
The Nature of Radioactivity
Radioactive Decay
Rate of Radioactive Decay
Transmutation and Bombardment Reactions
Radioactive Decay Series
Chemical Effects of Radiation
Biochemical Effects of Radiation
Detection of Radiation
Sources of Radiation Exposure
Nuclear Medicine
Nuclear Fission and Nuclear Fusion
Nuclear and Chemical Reactions Compared
15-16
READING PERIOD
16
FINAL EXAM WEEK
17-18
Th 30/05/2019
F 31/05/2019
S 01/06/2019
F 14/06/2019
DEVIATIONS: Minor deviations from the syllabus are a normal part of any adaptive teaching and learning
process
DISCLAIMER: Changes may be performed to the above syllabus without any prior notification.
Copyright ©2006-2019 American University of Science & Technology - Faculty of Engineering - Department of Biomedical Engineering, Department of
Computer and Communications Engineering, Department of Mechatronics Engineering. All rights reserved.
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CHE 201B – Section A: General Chemistry
Dr. Diana Nabhan (Zahle)
PROBLEM SETS
The student is responsible for submitting the assignment dues on the indicated dates and at the
beginning of the lecture. The student is as well responsible to preserve this piece of document till
the end of the term.
The solution to each problem set will be available in the afternoon following the submission of the
assignment on the online system.
READ CAREFULLY: Assignments should be made on A4 Note Pad Papers with a grid of 5
mm x 5 mm squares. In every assignment, the student’s name, the course code and title, the
assignment number, and the date should be marked at the top of the first page; the problem
number should be clearly marked on the left hand side margin; and the question should be
reiterated at the beginning followed by a comprehensive solution. Complete sentences should be
used throughout in narrative questions. A ruler should be used wherever appropriate. Except
for drawings, the assignment should be written in blue ball-point ink. BE AS TIDY AS
POSSIBLE!
Assignment No. 1:
1.3, 1.5, 1.8, 1.9, 1.11, 1.15, 1.19, 1.24, 1.25, 1.28, 1.29, 1.31, 1.33, 1.40, 1.43, 1.54,
1.55, 1.64, 1.65. (Due on Tuesday February 26, 2019).
Assignment No. 2:
2.5, 2.8, 2.10, 2.12, 2.14, 2.16, 2.32, 2.34, 2.36, 2.38, 2.42, 2.48, 2.50, 2.51, 2.56,
2.62, 2.69(a,b), 2.71(a,b), 2.74, 2.78(a,b) , 2.80, 2.82, 2.85, 2.95, 2.98, 2.110. (Due
on Tuesday March 5, 2019).
Assignment No. 3:
3.3, 3.5, 3.7, 3.12, 3.17, 3.25, 3.27, 3.29, 3.33, 3.41, 3.43, 3.45, 3.48, 3.50, 3.51,
3.57, 3.60, 3.61, 3.70, 3.74, 3.75, 3.79, 3.82, 3.100. (Due on Thursday March 07,
2019).
Exam No. 1:
Tuesday March 12, 2019.
Assignment No. 4:
4.5(a,b), 4.7(a,b), 4.13, 4.15, 4.23(a,b), 4.25(a,b), 4.27(a,b), 4.39(a,b), 4.41(a,b),
4.43(a,b), 4.47(a,b), 4.49, 4.53, 4.55(a,b), 4.59,(a,d) 4.61(a,c), 4.79, 4.83, 4.85, 4.87,
4.89(a,b), 4.93, 4.95, 4.101, 4.103, 4.107(a,b), 4.113(a,b), 4.115(a,b), 4.117(a,b).
(Due on Tuesday March 19, 2019).
Assignment No. 5:
5.8, 5.14, 5.16, 5.20, 5.22, 5.26, 5.28, 5.30, 5.32, 5.38, 5.40, 5.48, 5.50, 5.52, 5.54,
5.56, 5.62, 5.66, 5.68, 5.70, 5.78, 5.80, 5.82, 5.89, 5.94. (Due on Tuesday April 02,
2019).
Assignment No. 6:
6.1, 6.5, 6.7(a,b), 6.9, 6.11, 6.13(a,b), 6.15(a,b), 6.21(a,b), 6.23(a,b), 6.25(a,b),
6.29(a,b), 6.31(a,b), 6.35, 6.37, 6.43, 6.45(a,b), 6.47, 6.49(a,b), 6.51, 6.59, 6.61(a,b),
6.75, 6.77, 6.79. (Due on Tuesday April 09, 2019).
Exam No.2:
Thursday April 11, 2019
Assignment No. 7:
7.16, 7.18, 7.20, 7.26, 7.28, 7.32, 7.34, 7.46, 7.48, 7.50, 7.58, 7.60, 7.62, 7.66, 7.68,
7.94, 7.96, 7.100, 7.102. (Due on Tuesday April 16, 2019).
Assignment No. 8:
8.1, 8.3, 8.5, 8.9, 8.11, 8.15, 8.17, 8.19, 8.23, 8.25, 8.33(a,b), 8.35(a,b), 8.37, 8.39,
8.41, 8.43, 8.45(a,b), 8.47, 8.49, 8.53, 8.55(a,b), 8.65 (a,b), 8.67 (a,b), 8.69 (a,b),
8.77, 8.81, 8.83, 8.95, 8.99, 8.103. (Due on Tuesday April 25, 2019).
Exam No. 3:
Thursday May 2, 2019.
Assignment No. 9:
9.4, 9.8, 9.12, 9.14, 9.16, 9.18, 9.28, 9.24, 9.26, 9.40, 9.42, 9.44, 9.48, 9.50, 9.54,
9.60, 9.68, 9.70, 9.72, 9.74, 9.84, 9.86, 9.88. (Due on Tuesday May 14, 2019).
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CHE 201B – Section A: General Chemistry
Dr. Diana Nabhan (Zahle)
Assignment No. 10:
10.4, 10.6, 10.8, 10.10, 10.12, 10.14, 10.16, 10.18, 10.20, 10.22, 10.24, 10.26, 10.34
10.36, 10.38, 10.40, 10.42, 10.44, 10.46, 10.48, 10.50, 10.52, 10.54, 10.56, 10.58,
10.62, 10.64, 10.68, 10.72, 10.82, and 10.84. (Due on Tuesday May 23, 2019).
Assignment No. 11:
11.2, 11.4, 11.6, 11.8, 11.10, 11.12, 11.14, 11.16, 11.20, 11.22, 11.26, 11.28, 11.34,
11.36, 11.38, 11.40, 11.42, 11.44, 11.46, 11.48, 11.50, 11.54, and 11.56. (This
assignment will not be collected; however, the material covered in it will be included
in the Final Exam)
Final Exam:
From Monday June 03, 2019 till Friday June 14, 2019.
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