1. No category

COURSE PRESENTATION
Summer 2015
Course:
Course:
Classroom:
Lab Room #:
Tel:
Email:
1.
Chem 1110
Richmond (Main) 3310
6042406072
[email protected]
Instructor:
Class Hours:
Lab Hours:
Office Room #
Office Hours:
Dr. Vinay N. Choytun
TR 1400-1550
TBA
TR 1550-1630
COURSE FORMAT
Lecture (4h/Week)
2.
COURSE WEBSITE:
Sign on to your myKwantlen account and then click on myCourses. Select this course, and then click on
“Files” on the left sidebar. (contains lecture notes, solutions to assignments, handouts, sample exams, etc.)
3.
COURSE DESCRIPTION
Students will study the modern view of atomic structure, nuclear chemistry, theories of bonding and molecular structure,
organic chemistry (properties and reactions of the major functional groups and isomerism) after a brief review of
stoichiometry, gases and the treatment of experimental data. Students will also perform experiments in the laboratory.
4.
COURSE OBJECTIVES
A student who successfully completes the course will have reliably demonstrated the ability to:
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Solve a variety of stoichiometric and gas law problems
Solve problems based on the Bohr model of the atom, other 1-electron atomic systems and the photoelectric
effect
Use quantum theory to discuss orbital shapes, energies and electron configurations of atoms and ions
Describe and explain trends in atomic and ionic radii, ionization energies, electron affinities, and
electronegativities with reference to the Periodic Table of Elements
Describe ionic and covalent bonding and explain trends in physical properties based on type of bonding
Use Lewis structures and resonance to describe bonding and Valence Shell Electron Pair Repulsion (VSEPR)
Theory to predict shapes of covalent species
Use Valence Bond Theory and Molecular Orbital Theory to rationalize shapes, stabilities and magnetic
properties of covalent species
Describe the different intermolecular forces and explain effects of intermolecular forces on physical properties
of covalent compounds
Name a variety of organic compounds containing different functional groups
Describe and illustrate different types of isomerism possible in organic compounds
Predict the products of simple reactions involving organic compounds
Discuss the common types of radioactivity and their uses
Solve problems based on the rates of radioactive decay, binding energies of nuclei and energy associated with
nuclear reactions
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Course Presentation
5.
COURSE OUTILINE
You are responsible for all information given in the lectures (lecture notes, examples worked out in the
lectures, and assignment problems). The assignment problems are appended at the end of each set of lecture notes.
Solutions to the assigned problems will be posted on the course website within 24 hours after the corresponding
lecture in order to give you some time to attempt them yourself.
Lecture notes will be posted on the course website the day before each lecture. You are expected to print the notes and
bring them to class.
Introduction and Review of Stoichiometry (Chapter 1)
Measurements; significant figures; scientific notation; classification and nomenclature; chemical formulae;
stoichiometric calculations including solutions; empirical formula and molecular formula.
Gases (Chapter 2)
Properties of gases; empirical gas laws (Boyle’s and Charles’); ideal gas law; STP conditions; Dalton’s law of partial
pressures; calculations using gas laws; gas stoichiometry; kinetic theory of gases; molecular velocities; Graham’s laws of
effusion and diffusion.
Atomic Structure & Quantum Theory (Chapter 4)
Experimental basis for modern concepts of the atom; spectra and electromagnetic radiation; Bohr model of the atom
and emission spectrum of atomic hydrogen and hydrogen-like species; quantum theory; dual nature of matter; wave
mechanical model; Heisenberg uncertainty principle; photoelectric effect; orbitals and quantum numbers.
Electron Configurations & Chemical Periodicity (Chapter 5)
Electron configurations; interpretation of the periodic table; periodic properties; atomic and ionic sizes; ionization
energies; electron affinities.
Models and Theories of Chemical Bonding (Chapters 6)
Ionic and covalent bonding; Lewis structures; resonance; electronegativities; VSEPR theory and molecular geometry;
valence bond theory; electron promotion and hybridization; molecular orbital theory applied to diatomic molecules;
bond order and magnetic properties.
Organic Chemistry (Chapter 10-11)
IUPAC nomenclature; saturated, unsaturated and aromatic hydrocarbons, alcohols, ethers, carbonyl compounds,
amines; cyclic compounds; degree of unsaturation; properties and reactions; structural isomerism, geometrical
isomerism, functional and optical isomerism.
Intermolecular Forces and Liquids (Chapter 8)
Intermolecular forces: H-bonding, dipole-dipole, and London / dispersion forces
Nuclear Chemistry (Chapter 21)
Naturally occurring modes of radioactive decay; equations for nuclear reactions and fission/fusion.
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Course Presentation
6.
TENTATIVE SCHEDULE OF TOPICS
SESSION
1
2
3
4
5
6
7
8
9
10
DATE 2015
May 12th/14th
May 19th/21st
May 16th/28th
June 2nd
June 4th/9th/11th
June 16th/18th
June 23rd/25th
June 30th
July 2nd/7th/9th
July 14th/16th
11
July 21st/23rd
/28th
12
13
July 30th
Aug 4th
14
Aug 6th
/11th/13th
Final Exam
15
CONTENT
Note
Introduction and Review of Stoichiometry Chapter (1)
Gases (Chapter 2)
Atomic structure and Quantum theory (Chapter 4)
Midterm 1 (Chap. 1, 2, 4)
Electron Configurations & Chemical Periodicity (Chapter 5)
Models and Theories of Chemical Bonding (Chapters 6)
Models and Theories of Chemical Bonding (7)
Midterm 2 (Chap. 5, 6, 7)
Organic Chemistry (Chapter 10-11)
Intermolecular Forces and Liquids (Chapter 8)
Intermolecular forces: H-bonding, dipole-dipole, and
London / dispersion forces
Intermolecular Forces and Liquids (Chapter 8)
Intermolecular forces: H-bonding, dipole-dipole, and
London / dispersion forces
Midterm 3 (Chap. 10, 11, 7, 8)
Nuclear Chemistry (Chapter 21)
Nuclear Chemistry (Chapter 21)
Aug 20th 1130-1430 (Cumulative)
6. REQUIRED TEXTBOOKS AND MATERIALS and ASSIGNMENT INFO.
1. “Chemistry” Olmsted,J.; Williams, G.; Burk, B.; 2013, 2nd Ed.
2. Chemistry 1110 Lab Manual, Kwantlen Polytechnic University (2010)
Assignments
Due Date*
Assignment 1
Assignment 2
Assignment 3
Assignment 4
Assignment 5
Assignment 6
Assignment 6
May 21
th
Jun 4
th
Jun 18
nd
Jul 2
th
Jul 16
th
Aug 4
th
Aug 13
st
*No exceptions or extensions!
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Course Presentation
SUMMER 2015
LABORATORY
UNKNOWN
PAGE
Introduction to the
Chemistry Lab &
Analytical Balance (**)
-
34
May 26
Use of the Analytical
Balance & Laboratory
Techniques (**)
(View the Powerpoint
presentation called
“Laboratory
Techniques”)
-
37
June 2
Molar Mass
Determination of a Group
IA or IIA Metal Carbonate
(*)
-
41
June 9
Molar Mass of
Magnesium (**)
-
57
June 16
Determination of Mass %
of silver in a copper silver
alloy
EXPERIMENT
SCHEDULE WEEK OF:
May 19
48
.
June 23
LAB EXAM I – Empirical
Formula of a
Compound (*)
Page 4 of 8
45
No lab
June 30
July 7
-
Percent Nickel
(Gravimetric Analysis)
(View the Powerpoint
presentation called
“Quantitative
Determination of
Nickel”)
Yes
54
Course Presentation
July 14
Qualitative Organic
Analysis (*)
Yes
72
July 21
Synthesis of Aspirin and
Methyl Salicylate
-
63
July 28
Determination of Ascorbic Yes
Acid in Vitamin C
Solutions (**)
51
LAB EXAM II
Aug. 2
Aug. 9
Preparation of Geometric
Isomers & Intermolecular
Forces (**)
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68
NOTE: 1. Labs with (*) are done and handed in at the end of the lab period.
2. Labs with (**) require the HAND IN sheets and are done and handed in at the end of the lab period
7. Supplementary Lab Material:
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The following website contains hand in sheets for your lab reports as well as Lab
material: Powerpoint presentations of selected labs. You are responsible for viewing the
Powerpoint presentation and printing the hand in sheets prior to coming to the
corresponding lab.
http://www.kwantlen.ca/science/chemistry/labmat/110Slabmat.htm
8. DETAILED SUMMARY OF EVALUATION SCHEME
Assignment/Quizzes (6)
Mid Term Exams (3)
Class Participation
Final Exam
Lab assignment
TOTAL
Grade
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20%
30%
5%
35%
10%
100%
Grade
Conversion Scale
Points
(%)
Definition
Course Presentation
A+
4.33
90 - 100
A
4.00
85 - 89
A-
3.67
80 - 84
B+
3.33
76 - 79
B
3.00
72 - 75
B-
2.67
68 - 71
C+
2.33
64 - 67
C
2.00
60 - 63
C-
1.67
56 - 59
D
1.00
50 - 55
F
0.00
0 - 49
Exceptional Achievement
Outstanding Achievement
Excellent Achievement
Very Good Achievement
Good Achievement
Good Achievement
Satisfactory Achievement
Satisfactory Achievement
Minimal Achievement. This grade does not
permit student to pursue another course for
which the graded course was a prerequisite.
Minimal achievement. This grade does not permit
student to pursue another course for which the
graded course was a prerequisite.
Unsatisfactory achievement. Student did not
meet minimum course requirements.
9. INSTRUCTOR/CLASSROOM POLICIES:
•
There are NO makeup exams given in this course. If you miss a midterm exam for a
legitimate reason, the weight of the missed exam will be put on the final exam. You must
contact me (preferably by e-mail) before the scheduled exam time and provide valid
documentation such as a doctor’s note. If I do not hear from you or if I do not receive valid
documentation of your absence, you will receive a zero for the missed midterm exam.
Final exams must be written on the designated date and time.
10. POLICY ON LATE ASSIGNMENTS:
•
•
Attendance at all labs is mandatory. If you miss a lab, you must phone the lab instructor
before the start of the lab. If the lab instructor is unavailable, leave a voicemail message,
including a phone number where you can be reached. As soon as you return to class, you
must provide valid documentation (e.g., doctor’s note, ICBC report) to the lab instructor.
Labs missed without valid documentation will result in a zero assigned for the lab. If you
miss three or more labs, the laboratory portion of this course will be considered
incomplete.
Marks will be deducted for late submission of lab reports. If your overall lab mark is less than
50% or if the laboratory portion of the course is incomplete, the maximum grade that you
can achieve in this course is a C–.
FIELD TRIPS
Nil
10. ADDITIONAL COSTS TO STUDENTS
Nil
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Course Presentation
11. WITHDRAWAL DATES (see http://www.kpu.ca/registration/dates/full-semester)
May 10th 2015
May 17th 2015
May 17th 2015
May 18th 2015
May 22nd 2015
Last day to drop courses with 100% reduction in assessed fees, less
registration deposit (varies for international students)
Last day to drop courses with a 70% reduction in assessed fees, less
registration deposit (varies for international students)
Last day to drop courses without a "W" on academic records
Withdrawal/no refund period commences
Arrears deadline
Withdrawing From a Course
Students may withdraw from open enrolment and most limited enrolment courses until the end of the
eighth week of a semester (or 50% of a course has elapsed). To officially withdraw from a course, a
student must do so by the published deadline. The deadline for withdrawing is published in each
semester's online Registration Guide and Timetable.
Non-attendance by itself does not constitute withdrawal from a course. A student is considered fully
registered until she or he has either withdrawn using the online registration system or submitted a
Course Status Change form (if registration in the program is not done online). A student who stops
attending class but does not withdraw by the deadline will be assigned a grade based on the work
completed in the course.
Before withdrawing from a course, recipients of student loans should confirm whether their status will
be affected by the withdrawal. To be eligible for a student loan, a student must be enrolled in at least
sixty (60) percent of a full course load for her or his program.
If a student withdraws during the second to eighth week of classes in a semester, the course(s) will
appear on the student's official transcript with a grade of "W". Withdrawals will not be permitted after
the end of the eighth week of classes.
A student who withdraws from all courses in a semester may need to apply for re-admission by the
application deadline in order to register again at the University. Students will remain eligible for up to
two additional consecutive semesters after applying and/or registering in an open access program.
12. STUDENT POLICIES - http://www.kpu.ca/policies
POLICY No. C.8 - PLAGIARISM AND CHEATING
Definitions
Cheating, which includes plagiarism, occurs where a student or group of students uses or attempts to
use, unauthorized aids, assistance, materials or methods. Cheating is a serious educational offense.
Plagiarism occurs where a student represents the work or ideas of another person as his or her own.
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Course Presentation
POLICY
Kwantlen Polytechnic University condemns all forms of cheating. If it is determined that a student has
cheated, the University will proceed with discipline in the following manner:
1. For most first offences, a grade of zero will be awarded for the affected assignment, test, paper,
analysis, etc.;
2. For most second offences, a failing grade will be assigned in the affected course;
3. Depending upon the circumstances surrounding a first or second offense, a more severe level of
discipline may be imposed by the University;
4. Where deemed appropriate in the circumstances, for any third offence, the matter must be
referred to the University Vice President Academic under Policy No. C.21 Student Conduct for the
assignment of discipline, which may include suspension or expulsion from the University.
5. Any student who contributes to an act of academic dishonesty by another student may face
disciplinary action.
The following information is provided to help students avoid plagiarism and cheating:
http://libguides.kwantlen.ca/academicintegrity
http://www.kpu.ca/calendar/2014-15/academic-affairs/academicregulations.html
http://www.kpu.ca/sites/default/files/Policies/c08.pdf
Appeals of Academic Decisions
http://www.kpu.ca/appeals-and-complaints
http://www.kpu.ca/sites/default/files/Policies/L06.pdf
Student Evaluation and Grading
http://www.kpu.ca/sites/default/files/Policies/c20.pdf
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Course Presentation