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AAU
KING ABDULAZIZ UNIVERSITY
ACADEMIC ASSESSMENT UNIT
COURSE PORTFOLIO
FACULTY OF SCIENCE
DEPARTMENT OF CHEMISTRY-
COURSE NAME: GENERAL PHYSICAL CEMISTRY
COURSE NUMBER: 202
SEMESTER/YEAR: FIRST SEMESTER/2008
DATE: 2008
ACADEMIC ASSESSMENT UNIT
PART II
COURSE SYLLABUS
ACADEMIC ASSESSMENT UNIT
Instructor Information
 Name of the instructor: - Dr.Samia Kosa,
 Office location: - Science building, First floor 2-177
 Office hours: - Sat. Mon. & Wed 9-10. Mon. 11−3 & Wed 11−12
 Contact number(s): 02-6400000 Ex. 26403
 E-mail address:- [email protected]
Course Information
 Course name and number: - General Physical Chemistry. 202
 Course meeting times, places:- SA − Sat. Mon. & Wed. 8 − 9 am, Room 1142
SB − Sun. & Tues. 8 − 9.5 am, Room 1142
 Course prerequisites and requirements: - Successful completion of Chemistry 201.
 Description of the course: - This course deals with study of the general principles of
physical chemistry, including thermodynamics, solution, kinetics, thermo chemistry,
spontaneity of reaction, electrochemistry, and nuclear reactions.
 Teaching methodology: - white board, discussions, & solving problems.
 Philosophy: - Save time, economic, & effort.
Course Objectives
 This course is designed to help students to understand the basic principles of physical
chemistry. Topics includes, exothermic & endothermic reactions, Hess law, Calorimetry,
bon energy, solute, solvent, Henry’s & Raolt’s laws, collegative properties, reaction
mechanism, catalyst, electrolytic cells, voltaic cell, electrode potential, nuclear reaction,
radioactivity, radioactive decay, half life, fission & fusion nuclear reaction.
 Upon completion of Chemistry 202 students should be able to:
1. Define energy, entropy, enthalpy, & Gibbs free energy.
2. Balance oxidation-reduction reactions by oxidation number.
3. Apply principles of chemical thermodynamics (entropy & free-energy) to chemical
systems.
4. Describe voltaic and electrolytic cells and calculate cell potentials.
5. Tell us weather the reaction proceeds in the right direction or not.
6. Define Henry’s & Raolt’s laws.
7. Tell us weather the reaction spontaneous or not.
Learning Resources
 Text books:1. Chemistry by Chang, 9th Edition.2007
2. Chemical Principles by Mortimer 6th Eddition
3. Lab. Note can be get from the Teaching assistant in the lab.
A calculator is needed for home work, lab report, exams,
 The lab will be in 2nd floor at science building (lab for chem. 202).
 The time of the lab is according to your section in the transcript.
ACADEMIC ASSESSMENT UNIT
Course Requirements and Grading
 Course Grading:
Two exams (15 marks each)
30 marks
Final exams
40 marks
Class activities
5 marks
Labs
25 marks
Total
100 marks
 Labs Grading:
First exams
4 marks
Second exams
5 marks
Class attendance & activities
10 marks
Practical exams
6 marks
Total
25 marks
Letter grades are assigned based on a range of: ++ = 100%, A+ = 99-95%, A = 94-90%, B+ =
89-85%, B = 84-80%, C+ = 79-75%, C = 74-70%, D+ = 69-65%, D = 64-60%. Below 60% = F.
 If you miss an exam for a very good and justifiable reason (such as a doctor's note), a new
exam will be written for you that it is guaranteed to be harder than the original exam.
 Attendance: Attendance in the lecture is not mandatory, but is ABSOLUTLEY,
POSSITIVELY, COMPLETELY, WHOLEHEARTEDLY, STRONGLY
RECOMMENDED!!! Remember, if you could teach yourself chemistry, you wouldn't be
here.
 Cheating: Cheating or plagiarism in any way, shape, or form is not tolerated in this class.
Plagiarism involves copying data/writing from another source without siting the source (i.e.
copying lab reports). Examples of cheating include: using crib notes (written or stored in a
calculator's memory); copying from another student's paper on a test, altering a test answer
and submitting it for a re-grade, etc. If a student is caught cheating the student will receive
a zero on that exam. If a student is caught a second time, the student will fail this course.
Detailed Course Schedule
ACADEMIC ASSESSMENT UNIT
Course Schedule Model
(meeting three times a week)
Week
#
1
Lecture
Topic
Lec.1
Syllabus + Reference + Quiz times
+ Office hours
Lec.2
Thermochemistry, Energy, kinds of
energy, Types of thermodynamic
systems, types of the process.
Lec.3
Lec.4
2
Lec.5
Lec.6
Lec.7
3
Lec.8
Lec.9
4
Chapter 18
Spontaneous & non-spontaneous
process
Gibbs Free Energy + Standard free
Energies
Absolute Entropies, Gibbs Free
Energy & Equilibrium
Reading Chapter 18

Homework assignment
#2
Lec.11
First Exam
Chapter 6 &18
Lec.12
Solutions, Nature of Solutions, The
Solution Process, Hydrated Ions
Chapter 12
Lec.14
Enthalpy of Solution, Effect of
Temperature & Pressure on
Solubility
Concentrations of Solutions
Lec.15
Vapor Pressure of Solutions
Lec.16
Boiling Point & Freezing Point of
Solutions
Lec.17
Osmosis
Lec.18
Distillation
Lec.19
Solutions of Electrolyte, Interionic
Attractions in Solution
Reading Chapter 6
Homework assignment
#1
Third law of thermodynamics
5
7
Chapter 6
First low of thermodynamics + heat
+ work
Enthalpy + heat capacity +
calorimeter
Thermochemical Equations +
Hess’s Law
Second law of Thermodynamics
What is Due?
Buy Book 
Lec.10
Lec.13
6
Reading
Assignment
First Exam
Reading Chapter 12
Homework assignment
#3
ACADEMIC ASSESSMENT UNIT
Week
#
8
9
10
11
12
Lecture
Topic
Reading
Assignment
What is Due?
Lec.20
Chemical Kinetic, Reaction Rate
Chapter 13
Reading Chapter 13
Lec.21
Rate Law
Lec.22
Concentration & time
Lec.23
Activation energy & temperature
dependence of rate constant
Lec.24
Rate Equation for Single-Step
Reactions
Lec.25
Rate Equations & Temperature
Lec.26
Catalysts
Lec.27
Second Exam
Chapter 12 &13
Lec.28
Electrochemistry, Redox reaction
Chapter 19
Lec.29
, Metallic Conduction, Electrolytic
Conduction
Lec.30
Electrolysis, Stoichiometry of
Electrolytes
Lec.31
Voltaic Cells, Electromotive Force
Lec.32
Electrode Potentials
Lec.33
Gibbs Free Energy Change &
Electromotive Force
Lec.34
Effect of Concentration on Cell
Potentials, Concentration Cells
Lec.35
Lec.36
13
14
Homework assignment
#4
Second Exam
Reading Chapter 20
Electrode Potentials & Electrolysis
The Corrosion of Iron, Some
Commercial Voltaic Cells, Fuel
Cells
Homework assignment
#5
Lec.37
Third Exam
Chapter 13 &19
Third Exam
Lec.38
Nuclear Chemistry, The Nucleus
Chapter 23
Reading Chapter 23
Lec.39
Nuclear Reaction
Lec.40
Radioactivity
Lec.41
Rate of Radioactive Decay
ACADEMIC ASSESSMENT UNIT
Week
#
15
Lecture
Topic
Lec.42
Nuclear Transmittance
Lec.43
Nuclear Fission
Lec.44
Nuclear Fusion
Reading
Assignment
Final Exam all Sections
What is Due?
Homework assignment
#6
Study, study, study…
HOMEWORK ASSIGNMENT
From the book (Chemistry by Chang, 9th Edition.2007)
1. Homework assignment # 1 (Chapter 6)
6.11, 6.12, 6.14, 6.15, 6.17, 6.19, 6.21, 6.22, 6.24, 6.25, 6.27, 6.30, 6.33, 6.37, 6.51,
6.55, 6.57, 6.63, 6.73, 6.75, 6.79, 6.93, 6.95, 6.112, 6.124.
2. Homework assignment # 2 (Chapter 12)
12.9, 12.11, 12.15, 12.17, 12.19, 12.23, 12.51, 12.53, 12.57, 12.65, 12.72, 12.77,12.81,
12.89, 12.109
3. Homework assignment # 3 (Chapter 13)
13.5, 13.7, 13.15, 13.17, 13.19, 13.27, 13.29, 13.39, 13.41, 13.45, 13.51
4. Homework assignment # 4 (Chapter 18)
18.4, 18.5, 18.9, 18.11, 18.13,18.17, 18.19, 18.23, 18.27, 18.31, 18.39, 18.57
5. Homework assignment # 5 (Chapter 19)
19.2, 19.11, 19.21, 19.26, 19.29, 19.31, 19.46, 19.51, 19.61, 19.90
6. Homework assignment # 6 (Chapter 23)
23.5, 23.6, 23.14, 23.16, 23.20, 23.55, 23.56
ACADEMIC ASSESSMENT UNIT
Practical Sessions Schedule Model
Reading
Assignment
Lab. #
Date
Exp/Practical title
What is Due?
1
Weak 1
Safety & Regulations
2
Weak 2
Determination of the Heat Capacity of
Calorimeter
Lab Report #2
3
Weak 3
Determination of the Heat of
Neutralization of a Strong Acid with a
Strong Base
Lab Report #3
4
Weak 4
Determination of Distribution Coefficient
of Iodine Between Immiscible Solvents
Lab Report #4
5
Weak 5
Determination of Equilibrium Constant
Using Distribution Coefficient of Iodine
Between Immiscible Solvents
Lab Report #5
6
Weak 6
Determination of the Critical Solution
Temperature of Phenol-Water System
Lab Report #6
7
Weak 7
Preparation & Properties of Buffer
Solution
Lab Report #7
8
Weak 8
Midterm Exam
Midterm Exam
9
Weak 9
Determination of Molal Freezing Point
Depression Constant
Lab Report #8
10
Weak 10
Determination of the Dissociation
Constant of Weak Electrolyte by
Measuring the Conductance
Lab Report #9
11
Weak 11
Conductometric Titration &
Determination the Normality of Unknown
Lab Report #10
13
Weak 12
Final Exam
Study,
study,study…
Lab Report #1
ACADEMIC ASSESSMENT UNIT
PART III
COURSE RELATED MATERIAL
Contains all the materials considered essential to teaching the
course, includes:
Quizzes, lab quizzes, mid-terms, and final exams and their solution set
Paper or transparency copies of lecture notes/ handouts (optional)
Practical Session Manual (if one exists)
Handouts for project/term paper assignments
ACADEMIC ASSESSMENT UNIT
PART IV
EXAMPLES OF STUDENT LEARNING
Examples of student work. (Included good, average, and poor
examples)
Graded work, i.e. exams, homework, quizzes
Students' lab books or other workbooks
Students' papers, essays, and other creative work
Final grade roster and grade distribution
Examples of instructor’s written feedback of student’s work, (optional)
Scores on standardized or other tests, before and after instruction,
(optional)
Course evaluation, self evaluation or students comments (optional)
ACADEMIC ASSESSMENT UNIT
PART V
INSTRUCTOR REFLECTION (optional)
ACADEMIC ASSESSMENT UNIT
Part V. Instructor Reflections on the Course
 General physical chemistry course is one of the most important courses in chemistry
because it is give the student the idea & basic knowledge about the most important part
of physical chemistry. Therefore it is considered as important & long course and need
hard work.
 Questions, discussions in the class, & the result of the exam indicated that the course is
well understood.
 The content of the course is enough to give the student the basic information about
physical chemistry.
 The course was presented using a data show, board, & discussion in the class. The
result of the exam indicated that the course is
ACADEMIC ASSESSMENT UNIT