SCH4U – Grade 12 University Chemistry 2014-15 COURSE OUTLINE
TEACHER: Mrs. Schieck
OFFICE: Room 105
TEXT: Chemistry 12, Nelson
REPLACEMENT COST: $136.00
PREREQUISITE: Grade 11 University Chemistry
PHONE: 416-393-8122 EXT: 20095
Classrooms: # 208, 212
WEBSITE: schieck-chem.blogspot.com
(I update the website every Friday with a description of the work
covered for the week and any evaluation dates. Test Review
sheets and homework answers are also sometimes posted.
Marks are posted by student number after every major test)
Course Description & Outline
The Grade 12 university preparation chemistry course is designed to be a challenging
course in which you will extend you knowledge of chemistry and improve and refine
your learning skills. The course goes beyond the acquisition of facts to concentrate on
giving you an understanding of the principles and applications of chemistry. A further
emphasis is placed on the importance of chemistry in everyday life and evaluating the
impact of chemical technology on the environment.
UNIT 1: STRUCTURE & PROPERTIES
Chapter 3: Atomic Theories
a) Bohr’s atomic theory and atomic spectra,
quantized energy
b) Wave mechanical model of the atom
c) Quantum numbers & spectra, orbitals, shells,
subshells, energy level diagrams, electronic
configurations & the periodic table
d) ion charges, magnetism, unexpected electronic
configurations
Chapter 4: Chemical Bonding
a)
b)
c)
d)
Hydbridization
VSEPR theory & shapes of molecules
Predicting polarity of molecules
Dipole-dipole, London forces, hydrogen
bonding, physical properties of liquids
e) Ionic, metallic, molecular and network covalent
crystals: bonding & properties
UNIT 2: ENERGY & RATES OF REACTION
Chapter 5: Thermochemistry
a) Heat and energy changes, exothermic vs.
endothermic, temperature, open vs. closed
system
b) Calorimetry, q = mcT, Heat transfer and
enthalpy change: physical, chemical & nuclear
change
c) Molar enthalpies H conventions, & calorimetry
calculations, Conventions for indicating heats of
reaction, Enthalpy diagrams
d) Getting molar enthalpies using Hess’s Law,
standard Enthalpies of Formation, and bond
energies.
e) (From chapter 7) First Law of Thermodynamics,
enthalpy, entropy and spontaneity, Predicting
signs for entropy, Second Law of
Thermodynamics, Gibbs Free Energy and the
Gibbs Helmholtz equation
Chapter 6: Rates of Reaction
a) Kinetics, expressing and measuring rates of
reaction
b) 5 factors affecting rate: chemical nature,
concentration, temperature, catalysts, surface
area
b) Rate law, rate constant, orders or reactions
relating reaction rate to time
c) Collision theory, activation energy, potential
energy diagrams, activated complex
d) Reaction mechanisms, elementary process,
rate-determining step, reaction intermediates
e) Maxwell-Boltzmann KE distributions and
theoretical effect of chemical nature,
concentration, temperature, catalysts, surface
area
UNIT 3: CHEMICAL SYSTEMS & EQUILIBRIUM
Chapter 7: Equilibrium State
a) dynamic equilibrium, forward vs. reverse
reactions, solubility, phase & chemical
equilibrium, % reaction at equilibrium, Equilibrium
and G
b) Equilibrium Law, Equilibrium constant, K &
problem solving, Heterogeneous vs.
Homogeneous equilibria
c) Le Chatelier’s Principle & Concentration vs time
graphs: temperature, concentration and gas
volume changes, changes not affecting
equilibrium: catalysts, inert gases
d) Reaction Quotient & problem solving, Solubility
Product constant Ksp, predicting precipitation,
common ion effect
Chapter 8: Acid-Base Equilbria
a) Arrhenius Acids & Bases
b) Bronsted-Lowry theory, amphiprotic/amphoteric,
strong vs. weak acids, acids and their conjugate
bases
c) Dissociation of water, Kw, Strong Acids, Strong
Bases, Kw, Hydrogen ion concentration & pH,
pOH, pKw for strong acids and bases
d) Weak acids and bases, % ionization, Ka, Kb,
Organic bases, Ka x Kb = Kw, Calculations
involving pH, Ka, Kb for weak acids and bases
e) Lewis Acids & Bases
f) Acid-Base titrations - strong acid/strong base
titration curves, pH at the equivalence point and
related calculations
g) Buffers
UNIT 4: ELECTROCHEMISTRY
Chapter 9: Electric Cells
a) oxidation & reduction, oxidation numbers &
electron transfers
b) balancing redox equations using oxidation
number method, half reaction method
c) predicting redox equations, oxidizing agent,
reducing agent, use of redox tables, Left hand
spontaneity rule
d) Cells vs. Batteries, basic cell design, Galvanic
Cells, Standard Cells & cell potential, the
hydrogen half-cell, Consumer, commercial &
industrial cells
e) Corrosion & sacrificial anodes
Chapter 10: Electrolytic Cells
a) Electrolysis
b) refining metals and electroplating
c) Quantitative electrolysis calculations
UNIT 5: ORGANIC CHEMISTRY
Chapter 1: Organic Compounds
a) organic vs. inorganic compounds, functional groups
& multiple carbon-carbon bonds, hydrocarbons,
aliphatics, alkanes, alkenes, alkynes, cyclics,
aromatics, isomers
b) nomenclature of alkanes, enes & ynes, benzene
compounds, physical properties of hydrocarbons
c) chemical reactions of hydrocarbons: combustion,
substitution with halogens, addition (with H2,
halides, hydrogen halides, water) & Markinov’s
Rule
d) substitution reactions of Aromatic hydrocarbons
(with halides, nitric acid, alkyl halides)
e) Organic Halides; nomenclature, properties, uses,
preparation from hydrocarbons, elimination
reactions Alcohols (1st, 2nd & tertiary);
nomenclature, uses, properties, Reactions:
preparation from hydrocarbons, combustion,
elimination
f) Ethers: nomenclature, properties, Reactions:
preparation from alcohols (condensation)
g) Aldehydes and Ketones: nomenclature, properties,
Reactions; preparation from alcohols (oxidation),
hydrogenation to form alcohols
h) Carboxylic Acids: nomenclature, properties,
Reactions: oxidation of aldehydes to acids,
esterification,
Esters: nomenclature, properties, Reactions:
hydrolysis
i) Amines: nomenclature, properties, Reactions:
preparation from alkyl halides,
Amides: nomenclature , properties, Reactions:
preparation from carboxyl group + amine,
hydrolysis
j) polymers (addition & condensation)
Further information about this course can be found at the
Ontario Ministry of
Education Website:
http://www.edu.gov.on.ca/eng/curriculum/secondary/200
9science11_12.pdf
Assessment and Evaluation
Ongoing assessment will occur to allow
students the opportunity to be
successful. Students will be evaluated in
four categories of the achievement
chart. These will be in the form of
quizzes, labs, tests, culminating lab
activity and a compulsory final exam.
Quizzes: At least one day of notice will
be given.
Labs: For most labs, the
experimental data collection and the
analysis are done in class in the form
of a lab quiz. You cannot receive
marks for an experiment you did NOT
perform. Follow up with your teacher
promptly regarding missed labs.
During
Course
Final
Mark
Knowledge & Understanding of
chemistry
35%
24.5
Ability to Communicate
Chemistry
30%
Inquiry & Analysis Skills
20%
14%
Applications – Connections
between Chemistry,
Technology & Society
15%
10.5%
Culminating lab activity
Final Examination
21%
6%
24%
70% of final
grade based
on course
work
30% final
evaluation
Tests: You will be given at least one weeks notice of a major test. You are expected to give the highest
priority to writing all tests on the assigned day. Missing a test is a serious matter.
Unless there are extenuating circumstances, no more than 2 makeup tests will be allowed to any
student.
Culminating lab activity: scheduled for late April (see school calendar), this four hour titration lab will be
evaluated on the basis of experimental technique, lab results and a report and will be worth 6% of the final
mark.
Expectations - Students are expected to:
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attend classes regularly and be punctual.
be respectful towards others and their property
obtain and complete missed class work during absences
come prepared and be ready to work
do their homework on a daily basis.
keep a complete set of notes
be safety conscious at all times in the lab. (Back packs and coats are not permitted in class - see
separate lab safety handout)
Chemistry requires more understanding than memorization, and many of the concepts build on each other.
It is essential that you keep up with the course. Discipline yourself to budget 35-40 min. every other day to
do homework questions and review the lessons no matter what other tests or deadlines you have in other
classes. If you apply this approach to all your classes you will reduce your stress and increase your success.
Credit Rescue in Senior Science Courses: Credit Rescue is the prevention of course failure and loss of the
credit. Due to the increased depth and breadth of the senior science courses, Credit Rescue does NOT occur
after the final exam. For those students that performing at below 60 %, interventions will occur during the
course that may include homework contracts, weekly teacher-student appointments, lunch tutorials or peer
tutoring. This Credit Rescue intervention may be initiated by the teacher or the student.
THE SCHIECK PLAN FOR SUCCESS:
Spend at least 35-40 minutes on Chemistry after every class (every other day).
1. Complete any assigned homework questions or reading. (By the end of the assignment you should
work towards being able to do it without relying on your notes.)
2. Spending some time reviewing your notes from the last couple of lessons.
Good Ways to review:
a) Writing is better than reading for review: Write some terms or questions on a piece of paper, and then
close your book and try to answer/explain them.
b) Try to teach a friend/sibling/parent about a concept you have learned.
c) Do an extra problem that wasn’t assigned for homework
d) Bring homework solution to Mrs Schieck during class or at her office to check for clarity and
completeness
3. Stop by Mrs. Schieck’s office at lunch or after school for help if you are confused about something.
Absences
If you know you are going to be absent for an evaluation (appointment, field trip, sports event), then you must
inform the teacher beforehand. The sooner you discuss the conflict, the more likely an acceptable alternate
arrangement can be made. Failure to do so will jeopardize any consideration.
Missed
Action Student Should Take
Regular
Class
Obtain notes, homework, and/or assignments from the teacher or a classmate BEFORE the
following class.
Quiz
You must follow-up with the teacher and provide confirmation (parental note or parents
call teacher or on an official field trip or team list) that the absence was excused. For most
legitimate absences the teacher will not count the quiz or offer a make-up quiz.
Test
MISSING A TEST IS A SERIOUS MATTER. In the case of appointments that conflict with
the test date, you must let the teacher know IN ADVANCE. The sooner you discuss the
conflict, the more likely an acceptable alternate arrangement can be made. In the case of a
sudden illness, the teacher should be informed as soon as possible and consulted the first
morning of your return to school. For a legitimate absence for a test, a note specifically for
me, explaining why you missed my test must be provided. It will be up to the discretion of the
teacher as to whether a make up test will be offered.
Lab
You will not receive marks for an experiment that you have NOT performed. If you are
absent for a lab, make arrangements to make up the experiment and evaluation ASAP. Lab
experiments are time sensitive; as soon as the marked lab quizzes/reports are passed back,
you can no longer make up the lab and may receive zero for the experiment.
Plagiarism: Plagiarism is the act of taking ownership of written material or ideas belonging to someone else, whether
knowingly or unknowingly. At Humberside Collegiate Institute, plagiarism is strictly dealt with. A student caught plagiarizing
an assignment in this course will receive an automatic mark of zero. A second chance will not be granted.
Deadlines: In accordance with the school’s policy on assessment and evaluation, any assignment or lab report handed in
after the deadline will receive a penalty of 5% per day, up to a maximum of 10%. Exceptions for extenuating
circumstances may apply at the discretion of the teacher.