Chemistry 202-AS1-AB
Chemistry I
1
John Abbott Arts and Sciences Program 700.A0
Chemistry I
Program:
Course Number:
Ponderation:
Credits:
Competency code:
Prerequisite:
Arts and Sciences
202-AS1-AB
3-2-3
2 2/3
01Y6
Chemistry 534
Semester:
Winter 2013
Lectures:
M/W 10-11:30
Lab:
F 8:30-10:30 or 10:30-12:30
Instructor:
Dr. Michael Lautman
Office:
HS412
Telephone:
514-457-6610, ext 5880
e-mail:
michael.lautman@johnabbott.qc.ca
Office Hours: as posted
Introduction:
The main objectives of the course are to fulfill Competency 01Y6 of the Integrated Arts and
Sciences Program and to prepare students to enter the Organic I course of the Science Program
(202-DCP) after only one semester of chemistry. Elements from both Chemistry NYB and
Chemistry NYA are combined to achieve this objective. Effectively, a student at the end of this
course should be able to:
a) Demonstrate an awareness of the chemical species present in any reaction mixture.
b) Employ Le Châtelier’s principle to manipulate an equilibrium process.
c) Demonstrate an awareness of how reactions take place, using simple Collision Theory
and Reaction Progress Diagrams.
d) Demonstrate the ability to use the mole concept and chemical formulas in carrying out
basic chemical calculations.
e) Demonstrate an appropriate understanding of the Quantum Theory underlying modern
concepts of bonding and atomic and molecular structure and properties.
f) Demonstrate an awareness of Valence Bond Theory, including the concepts of
hybridization and σ- and π- bonding.
Given the chemical formula for a simple organic compound (e.g. C4H6O2):
g) Identify and draw 3-D representations of structural isomers, stereoisomers and
enantiomers.
h) Identify reactive centres within particular isomers, based on bond polarities and
concepts such as resonance and conjugation.
i) Identify a structural isomer that contains the carboxylic acid group, and demonstrate
an awareness of the appropriate acid/base equilibrium in aqueous solution, including
the concepts of conjugate base, Ka and Kb.
The student must also demonstrate the appropriate choice and use of standard laboratory
equipment and techniques. The laboratory is designed to allow the student to practice
basic chemical techniques, and to investigate properties of common chemical species,
primarily in solution. Computers are used to both collect and analyze data. .
Chemistry 202-AS1-AB
Chemistry I
OBJECTIVES
Statement of the Competency
To solve problems related to chemical
transformations of substances
Elements of the Competency
1. Perform analyses of chemical processes
quantitatively.
2. Analyze the properties of the elements
with the help of a probability model.
3. Predict the electronic structure of
molecules.
4. Predict particle interactions in solution.
5. Experiment with chemical processes.
2
STANDARDS
General Performance Criteria:
 Individually
 With the help of a Periodic Table
 With the help of computer software
 In the laboratory, employing proper and
safe procedures
 Occasional production of reports
Specific Performance Criteria:
Specific performance criteria for each of
the elements of the competency are shown
below, with the corresponding Intermediate
Learning Objectives. For the items in the
list of learning objectives, it is understood
that each is preceded by:
‘The student is expected to be able to….’
Chemistry 202-AS1-AB
Specific Performance
Criteria
1. Simple Chemical
Reactions in Solution.
1.1. Use of the particulate
nature of matter and
stoichiometry to describe
and analyze some simple
chemical reactions in
aqueous solution.
Chemistry I
Intermediate Learning Objectives
1.1.1.
1.1.2.
1.1.3.
1.1.4.
1.1.5.
1.1.6.
1.1.7.
1.1.8.
1.1.9.
1.1.10.
1.1.11.
1.1.12.
1.1.13.
1.2. Description of rate of
reaction.
1.2.1.
2.
Describe the following fundamental particles: atom, molecule, ion, electron.
Describe the nature of solids, liquids and gases in terms of the motions of the
fundamental particles.
Define the terms: element, pure substance, mixture, compound, molecular
compound, ionic compound.
Describe the species present when these compounds dissolve in water.
Write formulas for basic chemical substances – chemical nomenclature.
Count amounts of substance present, using the 'mole' concept.
Define molarity and molality.
Describe how to prepare solutions of specific molarity from pure substances and
from other solutions (dilution).
Recognize and classify various essentially irreversible processes, specifically
electron transfer and double replacement reactions.
Write balanced chemical equation representing the processes described above:
‘net ionic equations’.
Define: limiting and excess reactant, theoretical, actual and percent yield,
percent composition and percent purity.
Solve problems involving essentially irreversible processes, using basic
principles of stoichiometry and "IRF" tables.
Define pH with respect for strong acids and bases.
1.2.3.
1.2.4.
1.2.5.
Describe a chemical reaction in terms of Collision Theory and utilizing a
Reaction Progress Diagram.
Define rate of reaction in terms of the rate of disappearance of reactants and the
appearance of products.
Write the general rate law for a given reaction.
Define and interpret 'order' of reaction and 'rate constant' of a reaction.
Determine ‘order’ of reaction and ‘rate constant’ given experimental data.
1.3.1.
1.3.2.
1.3.3.
Define the equilibrium constant, K.
Apply Le Châtelier's principle, qualitatively and quantitatively.
Solve problems involving reversible processes using "IRE" tables.
2.1.1.
Predict when chemical species behave according to classical mechanics and
Coulomb’s Law.
Describe the Rutherford model of the atom.
Describe the properties of the electron, and its dominant effect on the behaviour
of chemical species.
1.2.2.
1.3. Description of chemical
equilibrium in qualitative
and quantitative terms.
3
The Structure of
Chemical Species.
2.1. Description of atomic
structure.
2.1.2.
2.1.3.
2.2. Description of the
hydrogen atom.
2.2.1.
2.2.2.
2.2.3.
Discuss the importance of the Heisenberg Uncertainty Principle in
understanding the behaviour of the electron in the hydrogen atom.
Correctly interpret the line spectra of the hydrogen atom in terms of electron
energy levels.
Show an appropriate understanding of the Principal Quantum Number, the
concept of the ‘boundary surface orbital’ and the concept of electron spin.
Specific Performance Criteria
Chemistry 202-AS1-AB
2.3. Description of multielectron atoms.
2.4. Description of some
atomic properties
related to electron
configurations.
2.5. Description of the
ionic bond.
2.6. Description of the
covalent bond.
2.7. Description of
molecules and
complex ions.
2.8. Description of the
molecules and ions of
organic chemistry.
Chemistry I
4
Intermediate Learning Objectives
2.3.1. Appreciate the approximate nature of the quantum mechanical model of the
helium atom.
2.3.2. Show an appropriate understanding of the quantum numbers ‘l’ and ‘ml’, the
Pauli Exclusion Principal, and Hund’s rule.
2.3.3. Write electron configurations for multielectron atoms, using the appropriate
sequence of energy levels and the ‘aufbau’ principle.
2.3.4. Draw Lewis structures of atoms.
2.4.1. Describe trends in atomic and ionic radii.
2.4.2. Describe trends in ionization energies.
2.4.3. Distinguish between electron affinity and electronegativity, and describe
trends in these properties.
2.5.1. Use a Born-Haber cycle to describe and discuss the formation of an ionic
compound.
2.6.1. Show an appropriate understanding of Valence Bond Theory, including the
concepts of ‘orbital overlap’, the ‘electron pair’ bond and hybridization.
2.6.2. Describe σ and π bonding.
2.6.3. Demonstrate an awareness of valence bond properties such as: bond length,
bond energy and bond polarity.
2.7.1. Draw Lewis structures of simple molecules and complex ions, based on
Valence Bond Theory, including the concept of resonance.
2.7.2. Draw 3-D representations of simple molecules using basic VSEPR theory.
2.8.1. Demonstrate an appreciation of the important capacity of carbon for
‘concatenation’, the tendency to bond to ‘itself’ (i.e., to other carbon atoms).
2.8.2. Demonstrate an understanding of the range of chain structures possible.
2.8.3. Demonstrate an understanding of the nature and importance of isomerism in
molecular species.
3. Bringing it all
together (focus on
organic chemistry).
3.1. Description and
analysis of the system
of chemical species,
C4H6O2.
3.1.1. Draw a series of Lewis Structures and 3-D representations for various C4H6O2
species, illustrating the concepts of structural isomers, diastereomers and
enantiomers.
3.1.2. Indicate, for each species in 3.1.1, any charge asymmetry because of bond
polarities, and suggest the likely point of acid and /or base attack.
3.1.3. Draw a Lewis structure for the C4H6O2 species that is a ‘carboxylic acid’ and
write an equilibrium equation representing its acid/base behaviour.
3.1.4. Identify acid/base ‘conjugates’ appearing in 3.1.3, and discuss the role of
‘resonance’ in stabilizing one species over another.
3.1.5. Demonstrate, using the equilibrium cited in 3.1.3, how an equilibrium system
may be manipulated to advantage (principle of Le Châtelier).
Chemistry 202-AS1-AB
Chemistry I
5
Methodology
The course will be 75 hours, divided into Lecture and Laboratory periods, as follows:
Lectures: 45 hours.
Two 1.5-hour lectures per week, consisting of the introduction of new material, usually accompanied
by the working of sample problems. In addition, preparation for upcoming laboratory sessions will
occasionally be discussed during lecture time.
Laboratory Sessions: 30 hours.
One 2-hour laboratory session per week. These sessions will include practice in the basic techniques
of experimental chemistry, experiments designed to verify certain properties of solutions, and
experiments that illustrate the properties of some reactions that occur in solution. The chemistry
laboratories are equipped with computers interfaced with various instruments and students will be
trained in their use. Periodically, laboratory sessions may be used for workshops that will help the
student cope with course material.
Required Texts
Textbook: Chemistry, A Molecular Approach with Mastering Chemistry (2nd Ed.) (bookstore)
Other materials: Molecular Model Kit (bookstore)
Laboratory Requirements
 Safety glasses must be worn at all times in the laboratory. Good quality safety glasses are
available from the bookstore or from most hardware stores (~ $10-20). Normal prescription
glasses may be worn, but for safety reasons, the use of contact lenses is not permitted.
 A sturdy cotton lab coat is required. These are available from the bookstore (~ $20).
Evaluation




Unit Tests (3 tests of equal value)
Final Exam
Laboratory
Assignments/quizzes
30% (Feb 20, April 10, May 8)
30%
25%
15%
Please Note:
a) A student may drop the lowest test mark if it is lower than the final exam mark, so that the
remaining tests are worth 20% of the final grade, and the final exam is worth 40% of the final
grade. This arrangement is not available for a student who is assigned a grade of zero on a unit
test because of cheating.
b) To pass the laboratory portion of the course, a minimum of 60% of the total laboratory grade
must be obtained. Failing this, a laboratory grade of zero will be given and a maximum grade of
55 will be allowed for the course.
c) Notwithstanding other class grades, if a student passes the laboratory portion of the course, a
grade of 60% or more on the final exam will guarantee a pass in the course.
Course Costs
The major course costs are specified above. However, an instructor may require the student to
purchase additional materials, such as a laboratory notebook (approx. $10) or course notes (approx.
$10).
Chemistry 202-AS1-AB
Chemistry I
6
Regulations
a) Regular attendance is expected. If lectures are missed, it is the responsibility of the student to
cover the material missed and to be aware of any announcements made concerning assignments,
quizzes, tests or changes to the laboratory schedule.
b) Students must attend the laboratory session in which they are officially registered.
c) There will be no make-up tests, quizzes or laboratory periods. If you miss an evaluation session
or deadline due to illness, you must notify your instructor as soon as possible. A valid medical
note is required to prove absence for a medical reason. If a test is missed for a valid reason, then
the final exam mark will be used as a basis for a substitute for the missed test mark. Late
homework will not be accepted.
d) Periodically there may be workshops held during the laboratory period. Attendance is required.
Quizzes or assignments may be given during these workshops.
e) A special note concerning the use of chemicals: this course uses chemicals as part of its
normal teaching practices. If a student has experienced allergic reactions in the past due to any
particular chemical or chemicals, or for any other reason the student feels that exposure to
chemicals may result in harm, he or she must inform the instructor. In the event that an allergic
reaction is experienced at the college, the student should report to Campus Security immediately
(local 5226, 5231, or 9-514-398-7770).
f) Cell phones and computers may only be used during class for pedagogical purposes.
College Policies
a) Cheating and Plagiarism: The College has a universal policy on cheating and plagiarism, which
is upheld in this course. The student is referred to the IPESA for further information.
b) Mid-semester Assessment: All students will receive a mid-semester assessment, to give them
some idea of how they are progressing in the course. This assessment has no percentage value in
calculating the final grade.
c) It is the responsibility of all students to keep all assessed material for at least one month past the
grade review deadline in the event that they would want to request a grade review. Students can
learn more about their rights and responsibilities by reading the IPESA.
d) Students must inform their instructor, in advance, of anticipated absences, including religious
holidays. Students who wish to observe religious holidays must inform their teacher of their
intent, in writing, within the first two weeks of the semester.