MCCC
P R I N C I P L E S O F C H E
( ( C H E 1 5 2 ) )
M I S T R Y I I
W elcome to the second semester of Principles of Chemistry; a continuation of CHE 151.
This course covers an introduction to organic chemistry, solutions, kinetics, equilibria, electrochemistry, thermodynamics, and nuclear chemistry. The laboratory experiments relate to these topics. Prerequisite: CHE 151
This handout provides information concerning course policies and procedures. The course syllabus is also attached.
Teaching Staff:
Dr. Evon Martins
Office: 215-641-6459 SC 335 emartins@mc3.edu
Materials :
1.”C hemistry" , 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 two classes per week, each 3 hours long (Section EC MW 1:30 – 4:45 or
Section IC TTH 9:15 – 12:30 both in room 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.
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. Submission of late lab reports will result in minus ten points per week late .
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Examinations:
There will be four 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:
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 II 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 of approximately 50% 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 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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LEARNING GOALS
Upon completion of this course, the student should be able to:

Name simple aliphatic and aromatic hydrocarbons.

Identify different functional groups.

Perform calculations for various physical properties of solutions; such as, colligative properties and concentrations.

Understand the effect to temperature and pressure on solubility of different solutes; such as gases, liquids and solids, both electrolytes and non electrolytes.

Perform chemical kinetic calculations for rate of reaction, rate law, and plot concentration vs. time to determine reaction order.

Understand activation energy, the development of reaction mechanisms and catalysis.

Perform chemical equilibrium calculation solving for K.

Understand factors that affect chemical equilibrium.

Perform calculation on weak acids and bases solutions and determine pH of acid, base and salt solutions.

Understand the relationship between weak acids and their conjugate base, acid strength and structure, acid-base properties of salts, oxides and hydroxides.

Perform calculations for acid-base titrations, buffer solutions, common ion effect.

Predict precipitation reactions and calculate the solubility product in simple solutions and solutions with common ion effect.

Perform calculations for entropy, free energy and equilibrium.

Understand the three Laws of Thermodynamics.

Write balanced redox reactions and perform electrochemical calculations for Galvanic cells, concentration cells, and electrolysis.

Determine spontaneity of a Redox Reaction.

Write balanced nuclear equations, and understand nuclear stability, radioactivity and transmutation.

Differentiate between fission and fusion; and the uses of isotopes.
LEARNING ACTIVITIES
The learning activities will include lectures and class discussions of topics with an emphasis on calculations. Laboratory activities and the write up of laboratory report are a significant part of the course experience and cover all major topics from the course outline.
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S Y L L A B U S *
Lecture
#
1
Day/Date Read
Sections
W 1/18
TH 1/19
Homework
24.1-24.3 Chapter 24 : Organic Chemistry: # 11, 25,
2 M 1/23
T 1/24
24.3-24.4
12.1-12.3
26, 27, 32, 36, 60, 66.
Chapter 12 : Physical Properties of Solutions: # 11, 15,
12.3-12.6 17, 18, 19, 20, 22, 24, 37, 51, 52, 54, 58, 59, 60, 61, 3 W 1/25
TH 1/26
4 M 1/30
T 1/31
5 W 2/1
TH 2/2
12.6-12.7
13.1-13.2
64, 65, 66, 68, 81, 88, 100
Chapter 13 : Chemical Kinetics: # 5, 6, 7, 8,
16, 17, 20, 21, 22, 13.2–13.3
LAB 1** Chemical Safety and Laboratory Rules
Exp 22: Synthesis of Aspirin
13.3–13.4 27, 28, 6 M 2/6
T 2/7
7 W 2/8
TH 2/9
8 M 2/13
T 2/14
9 W 2/15
TH 2/16
10 M 2/20
T 2/21
13.4-13.6
LAB 2
14.1-14.2
14.3–14.5
29, 30, 37, 38, 40, 51, 52, 54, 62, 72, 86, 88, 92, 109
Distillation of Salt water
Chapter 14 : Chemical Equilibrium: # 7, 8,
16, 17, 19, 20, 22, 26, 28, 36, 39, 40, 44, 46, 48, 56, 57, 58,
11 W 2/22
TH 2/23
12 M 2/27
T 2/28
13 W 3/1
TH 3/2
14 M 3/6
T 3/7
14.5
LAB 3
64, 66, 68, 70, 88, 92, 103
Exp 10: Colligative Properties: Freezing Point Depression
15.1-15.4 Chapter 15 : Acids and Bases: # 4, 5 , 6, 8, 15, 16, 18,
20, 37,
15.5-15.9 43, 44, 45, 46, 48, 53, 54, 64, 68,
15.10
LAB 4
75, 76, 78, 79, 80, 82, 86, 88, 92, 94, 106, 110
Exp 12: Chemical Kinetics: Rate of Decomposition of
Hydrogen Peroxide
15 W 3/8
TH 3/9
3/13-3/19
16 M 3/2
T 3/21
15.11-
15.12
16.1-6.3
Chapter 16 : Acid-Base Equilibria and Solubility Equilibria: #
5, 9, 10,
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17 W 3/22
TH 3/23
18 M 3/27
T 3/28
19 W 3/29
TH 3/30
16.4-16.6 12, 17, 19, 20, 29, 35,
16.8-16.9
18.1-18.3
45, 47, 48, 50, 53, 59, 64, 68, 87, 91, 96, 110
18.4
Lab 5
Chapter 18
12, 13, 14,
: Entropy, Free Energy, and Equilibrium: # 5, 11,
Exp 13: Reaction Reversibility and Le Chatelier’s Principle
18.5-18.7 17, 18, 20, 23, 25, 26, 27, 28, 30, 38, 40, 52, 60, 64 20 M 4/3
T 4/4
21 W 4/5
TH 4/6
19.1-19.2
LAB 6
Chapter 19 : Electrochemistry: # 1, 2,
Exp 14: Determination of an Equilibrium Constant Using a
Spectrophotometer
22 M 4/10
T 4/11
23 W 4/12
TH 4/13
24 M 4/17
T 4/18
25 W 4/19
TH 4/20
19.3
LAB 7
19.4-19.5
19.8
23.1-23.2
LAB 8
23.3-23.6
23.7-23.8
LAB 9
11, 12,
Exp 15: Antacid Analysis and Determination of % Acetic
Acid in Vinegar
14, 16, 17, 21, 22, 24, 26, 29, 30, 32, 34, 38, 46, 49, 70, 107
Chapter 23 : Nuclear Chemistry: # 5, 6, 14, 15, 16, 18,
Exp 16: Acid-Base Equilibria: Determination of Acid
Ionization Constant
23, 25, 26, 28, 29,33, 26 M 4/24
T 4/25
27 W 4/26
TH 4/27
28 M 5/1
T 5/2
34, 62, 66, 68, 80, 82
Exp 20: Thermodynamics of Electrochemical Cells
Review Topics for Final Exam
National ACS Exam
Chapters 12-16, 18,19, 23, 24
* Tentative and changes may be made.
** Make up LAB will be written report on scientist studied during the semester.
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