MCCC
Fall 2005
PRINCIPLES OF CHEMISTRY I
(CHE 151)
Welcome to the first semester of Principles of Chemistry. This handout provides information
concerning course policies and procedures. The course syllabus is also attached.
Course description: A study of the fundamentals of chemistry for the science major. An emphasis is
placed on atomic structure, molecular structure, bonding, periodic law, reactions and weight relations,
gases, liquids, solids, changes of state and thermochemistry.
Prerequisite: High school Chemistry or CHE 150 Corequisite: MAT 161 or MAT 170
Teaching Staff:
Dr. Evon Martins
Office: 215-641-6459
SC 335
emartins@mc3.edu
Materials:
1. ”Chemistry", 8th Edition by Chang. Lecture material and homework problems originate in this
book.
2. "Student Solution Manual" J. Cruickshank and R. Chang. Contains detailed solutions for all even
numbered homework problems.
3. General Chemistry Laboratory Manual, by van Koppen, ISBN 0-07-285113-9.
4. Scientific calculator (logarithms, exponential, powers, roots, etc.)
Lectures:
There will be three classes per week, each 2 hours long (Section CC 10:10 – 12:10 or Section
EC 1:30 – 3:30 SC 311). You should attend ALL lectures for your section. Attendance is of utmost
importance since I will be emphasizing and clarifying important and difficult concepts. Unless
informed otherwise, you will at exam time be held responsible for having learned all the assigned
readings whether or not they are explicitly discussed in class. Any changes in the course format and/or
information about exams will be announced in lecture. All CELL PHONES should be turned OFF
during class time.
Laboratory is in SC 314. Attendance and promptness is required in laboratory. If you miss lab
for any reason a written report will replace lab grade. This is allowed one time. Missing two labs, for
any reason, will result in a zero grade for second missed lab. Also, being tardy for lab will result in
minus ten points off lab grade. Tardy means one second past the starting time for your lab based on
the school’s computer clock. Submission of late lab reports will result in minus ten points per week
late.
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Fall 2005
Examinations:
There will be five exams, see syllabus for dates. THERE ARE NO MAKE UP EXAMS! If
you miss one exam your final exam will count double. If you miss two exams, you will receive a zero
on the second missed exam. All necessary constants, the periodic table, and formulas will be provided.
Course grading:
The course grade will be based on the average of the following seven grades:
EXAM I
EXAM II
EXAM III
EXAM IV
EXAM V
Average of LABORATORY Grades
ACS FINAL EXAM
Academic Integrity:
All college polices on academic integrity will be strictly enforced. Any involvement with
cheating, the fabrication or invention of information used in an academic exercise, or facilitating
academic dishonesty of others will result in serious consequences ranging from reprimand to expulsion.
Furthermore, I have the right to give a second test to any student whose performance on a particular
test seems suspicious in my judgment.
Additional Help:
Principles of Chemistry I is considered by many students to be a moderately difficult course. In
order to be successful, you must be conscientious and devote considerable time to the course material.
Your success will depend primarily on your being able to logically analyze the wording in the chemical
problems assigned for homework, given on exams, and relate them to basic concepts and mathematical
expressions. For most students, the best way to learn the material is to work on the homework
problems independently (with the solutions manual closed). Good analytical skills and problem
solving techniques must be acquired in order to pass the exams, which consist mostly of word
problems. Rote memorization of the book will not allow you to pass the course. Chemistry is a
cumulative subject where one principle builds upon another. This course moves along at a fast pace
and you need to stay on top of the material at all times. Experience shows us that students who fall far
behind encounter difficulties and rarely catch up again. If, despite attending all classes and working
out all homework problems, you realize that some difficulties remain with understanding the course
material, then seek help early!
Students with Disabilities:
Students with disabilities may be eligible for accommodations in this course. Please contact the
Director of Services for Students with Disabilities in the Counseling Center, College Hall, at (215)
641-6575/6577 for more information.
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Fall 2005
LEARNING GOALS
Upon completion of this course, the student should be able to:
 Use Dimensional Analysis in all calculations
 Name and identify molecular and ionic compounds
 Perform all forms of stoichiometric calculations: mass-to-mass, limiting reagent and % yield
 Understand acid – base, redox, and precipitation aqueous solutions
 Understand gas laws for ideal and real gases, gas mixtures and gas stoichiometry
 Perform thermochemical and thermodynamic calculations
 Understand electronic structure of an atom by using quantum numbers and electron
configuration
 Understand periodic variation in physical and chemical properties
 Understand ionic and covalent bonding theories and should know how to draw Lewis structures
 Assign molecular geometry and hybridization
 Understand the intermolecular forces in liquids and solid, and be able to read phase diagrams
SYLLABUS*
Lecture
Day/Date
Read
Sections
Homework
1
W 8/31
1.1 – 1.8
2
F 9/2
1.9
2.1 – 2.2
Chemistry: The study of change.
Ch 1: 12, 14, 21, 22, 24, 25, 26, 30, 32, 33, 34,
35, 36, 43, 48, 49, 52, 62, 75, 78, 82, 89
#
M 9/5
Labor Day Break
3
W 9/7
2.3 – 2.7
Atoms, Molecules and Ions
Ch 2: 14, 15, 16, 26, 31, 32, 43, 44, 45, 46, 55,
4
F 9/9
2.7
3.1 – 3.3
5
6
M 9/12
W 9/14
3.4 – 3.8
3.9 – 3.10
4.1 – 4.2
7
F 9/16
LAB 1**
56, 57, 63, 69, 78, 86, 87, 88
Mass Relationships in Chemical Reactions
Ch 3: 5, 6, 14, 15, 16, 17, 20, 21, 23, 24, 26, 27, 28,
40, 45, 49, 50, 52, 53, 54, 59, 60, 63, 64, 65, 66, 68, 71,
72, 81, 82, 86, 89, 90, 96, 100, 118, 120, 125
Reaction in Aqueous Solutions
Ch 4: 7, 8, 17, 18, 19, 20, 21, 22,
Chemical Safety and Laboratory Rules
Experiment #1 Introduction to Laboratory Techniques
Glass bending and Fire polishing.
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Fall 2005
8
M 9/19
9
10
11
W 9/21
F 9/23
M 9/26
12
13
14
W 9/28
F 9/30
M 10/3
15
16
W 10/5
F 10/7
17
M 10/10
18
W 10/12
6.6 – 6.7
7.1
19
F 10/14
LAB 3
20
21
22
M 10/17
W 10/19
F 10/21
7.2 – 7.4
7.5 – 7.8
7.9
8.1 – 8.3
23
24
M 10/24
W 10/26
8.4 – 8.6
8.6
9.1 – 9.3
25
F 10/28
LAB 4
26
M 10/31
27
28
W 11/2
F 11/4
9.4 – 9.8
29
30
M 11/7
W 11/9
9.9
9.10
10.1
47, 51, 56, 62, 63,
64, 72, 74, 76, 85, 86, 94, 102, 104, 106, 108
31
F 11/11
LAB 6
Experiment # 7 Reaction Enthalpies and Hess’s Law
martins
Exam I
4.3 – 4.4
4.5 – 4.6
4.7 – 4.8
5.1 – 5.3
5.4
5.6 - 5.8
5.8
6.1 – 6.3
6.4 – 6.5
LAB 2
31, 32, 47, 48, 49,
55, 56, 62, 63, 71, 70, 72,
78, 85, 86, 87, 91, 92, 141, 148
Gases Ch 5: 13, 14,
17, 18, 19, 20, 22, 24, 26, 32, 35, 36, 40, 43, 47, 48, 49,
60, 63, 68, 77, 78,
85, 99, 102, 119, 134
Thermochemistry
Ch 6: 15, 16,
17, 18, 25, 26, 27, 34, 35, 37, 38, 46, 48,
Experiment # 4 Determination of a Chemical Formula
Exam II
53, 54, 57, 58, 62, 63, 64, 72, 78, 82, 92, 121
Quantum Theory and the Electronic Structure of
Atoms. Ch 7: 7, 8,
Experiment #2 Nomenclature and reaction
Stoichiometry. Take home lab
No Class today.
15, 16, 20, 26, 28, 30, 31, 32, 40, 41, 42, 54,
55, 56, 57, 58, 60, 61,
62, 63, 68, 79, 80, 84, 85, 91, 92, 115
Periodic Relationships Among the Elements
Ch 8: 20, 22, 24, 27, 30, 37, 38, 40
43, 45, 46, 52, 55, 56, 62, 64, 68,
72, 74, 84, 90, 126
Chemical Bonding I: Basic Concepts
Ch 9: 16, 17, 18, 20, 23, 30, 36, 38,
Experiment # 5 The Molar Volume of Gases
Exam III
LAB 5
39, 40, 44, 45, 46, 48
Experiment # 6 Thermochemistry
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MCCC
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32
M 11/14
10.2 – 10.4
33
W 11/16
10.5, 10.8
11.1 – 11.2
Chemical Bonding II: Molecular Geometry and
Hybridization of Atomic Orbitals.
Ch 10: 4, 6, 7, 8, 9, 12, 18, 20, 21, 22, 23,
24, 33, 34, 38, 39, 41, 42, 43, 44, 50, 64, 65, 76, 82, 84,
88, 89, 92, 99, 100, 103,
Omit sections 10.6 & 10.7
Intermolecular Forces and Liquids and Solids.
Ch 11: 10,
Experiment # 8 Atomic Spectroscopy
34
F 11/18
35
M 11/21
Exam IV
Thanksgiving Holiday
36
37
38
11/23 –
11/27
M 11/28
W 11/30
F 12/2
39
40
41
M 12/5
W 12/7
F 12/9
42
M 12/12
LAB 7
11.3
11.4, 11.6
LAB 8
11.7 – 11.8
11.9
LAB 9
12,
14, 16, 18, 19, 20, 32, 39, 41, Omit 11.5
Experiment # 17 Recycling Aluminum
42, 44, 54, 56, 78, 80, 86,
88, 94, 100, 102, 104, 112, 127, 134
Experiment # 9 Determination of Avogadro’s Number
Start Alum crystals growing.
Section 12.8 Colloids
Exam V
Review for Final Exam and observe alum crystals.
CC-Morning
Class: F
12/16 @
12:30 – 2:30
ACS National Final Exam
Chapters 1 - 11
ECAfternoon
Class: M
12/19 @ 2:45
– 4:45
SC- Evening
Class: T
12/20 @ 6:00
* Tentative and changes may be made.
** Make up LAB will be written report on scientist studied during first semester.
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MCCC
Fall 2005
I have read the syllabus and understand the rules for successful
completion on Che 151. Of special concern are: keep up in the
textbook at all times, no cell phones during class, no make up
exams or laboratories, and I must be on time for laboratory
class. I understand and will obey these rules.
Print name: _________________________
Sign name: _________________________
Dated: ______________
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