Grade 12, Chemistry
SCH4U
Ms.Yang
Tell me a bit about yourself
• Your name, email address
• Your education background
– What chemistry courses have you taken in the past?
– How long have you been in Canada
– Describe your level of English Proficiency
• What is your goal for this year
• Are you applying for university this year? If so, what
program
• Hobbies, Interest:
• How do you learn best: e.g. lecture? Copy down notes?
Video?
• Anything else that you like me to know?
Course Outline
• This course enables students to deepen their
understanding of chemistry through the study of organic
chemistry, the structure and properties of matter, energy
changes and rates of reaction, equilibrium in chemical
systems, and electrochemistry. Students will further
develop their problem-solving and investigation skills as
they investigate chemical processes, and will refine their
ability to communicate scientific information.
• Emphasis will be placed on the importance of chemistry
in everyday life and on evaluating the impact of chemical
technology on the environment.
Course Outline
Unit Number
Unit Title
Allocated Time
1
Content Review
6 hours
2
Organic Chemistry
21 hours
3
Structure and Properties
21 hours
4
Energy and Rate of Reaction
21 hours
5
Chemical Systems and Equilibrium
21 hours
6
Electrochemistry
18hours
Final Evaluation
3 hours
TOTAL TIME
110 hours
Assessment
•
•
•
•
•
Unit Tests
Quizzes
Assignments
Midterms
Lab reports
• Exam: 30%: Cumulative
• 70% of the grade is based on evaluations conducted
throughout the course.
• 30% is based on a final evaluation.
Assessment Continue
• Assessment will be based on four areas of the
science curriculum
–
–
–
–
Knowledge and Understanding
Inquiry: Problem Solving
Communication
Application
• Learning Skills Learning Skills (organization,
teamwork, work independently, and initiative) will
be evaluated separated from your term work and
will appear on the report card under their own
section.
Expectations for the course
• Attend scheduled classes
• Test policy: If you know ahead of time that
you will be absent, it Is your responsibility
to see me before test
• Extra help: Before or after class or you
could email me to schedule a time a place
Contact: betty.yang@canadahanson.com
• Classroom Policy: respect, leave your
working area clean
What you will need for the course
•
•
•
•
Pencil, Pen, eraser
Notebook or line paper
Nelson Work book
Scientific Calculator
5 min Recall Activity
• In 5 minutes, summarize what you
learn from past chemistry courses
and what you would like to learn in
this course
• You could write your answer in
point form or sentences
How much do you know about the
periodic table
Review the Basic
• Atomic Number= the
number of proton
• Mass number= the
total number of protons
and neutrons in a
nucleus.
• How many protons,
electrons and neutrons
does hydrogen has?
• Key Term: Period, Family, Ionic
Compounds, Covalent Compounds
Definitions
• An IONIC COMPOUND consists of a metal
cation bonded to a nonmetal anion.
Electrostatic attraction holds them together.
• A COVALENT COMPOUND consists of two
nonmetal atoms sharing valence electrons.
• A BINARY compound is one that is made of
just two elements.
Content Review
• Name the following
•
•
•
•
•
•
•
•
•
Ca
NaOH
CO
H2SO4(aq)
Pb
He
CO2
BaBr2
SO3
•
•
•
•
•
•
•
•
•
•
•
(NH4)3PO4
PBr5
MgSO4
CaO
H3PO4
Na2Cr2O7
MgO
SO2
Cu(NO3)2
HI
N2O
• Barium Sulfate
• Potassium oxide
• Magnesium
hydroxide
• Potassium nitrate
• Copper(II) oxide
• Nitric acid
• Sulfuric acid
• Iron (II) Chloride
Type I Binary Ionic Compounds
• The metal cations in these compounds have
only ONE possible charge.
Na+
Zn2+
Al3+
Ca2+
sodium
calcium
zinc
aluminum
The charges are memorized or predicted using a
periodic table!
• The cations are bonded to nonmetal anions:
O2N3FBr oxide
nitride
fluoride
bromide
Notice that simple anions are always named with
the suffix “ide”
• Examples
sodium chloride:
Na+ and Cl- 
NaCl
lithium oxide:
Li+ and O2- 
aluminum bromide:
Al3+ and Br - 
Li2O
AlBr3
zinc nitride:
Zn2+ and N3- 
Zn3N2
potassium iodide:
K+ and I- 
KI
Type II Binary Ionic
Compounds
• These are ionic compounds where the
metal cation can form TWO different
charges.
Fe2+
iron (II)
Fe3+
iron (III)
Ni2+
nickel (II)
Ni3+
nickel (III)
Co2+
cobalt (II)
Co3+
cobalt (III)
Cu+
copper (I)
Cu2+
copper (II)
Au+
gold (I)
Au3+
gold (III)
Sn2+
tin (II)
Sn4+
tin (IV)
Polyatomic (Complex) Ions
• All of the cations and anions so far have been simple
ions - single atoms that have lost or gained electrons.
• A molecule is a particle that forms when two or more
atoms bond together.
• A complex ion is a charged molecule. Complex ions
may be cations or anions.
examples:
nitrate: NO3sulfate: SO42Phosphate PO4 3-
hydroxide: OH-
Things to Notice
perchorate
ClO4-
sulfate
SO42-
chlorate
ClO3-
sulfite
SO32-
chlorite
ClO2-
hypochlorite
ClO-
nitrate
NO3-
nitrite
NO2-
Binary Covalent Compounds
• Covalent compounds are made of two
NONMETAL elements sharing valence electrons.
• Because there are no charges to help us write the
formulas of covalent compounds, prefixes are
used to indicate the number of each atom present
in the formula.
Prefix:
CO2 is named “carbon dioxide”
CO is named “carbon monoxide”
N2O is named “dinitrogen monoxide”
SO3 is named “sulfur trioxide”
mono
di
tri
tetra
penta
Hexa
Hepta
Octa
Nona
deca
Binary Acids
• A simple definition of an “acid” is a substance which
produces H+ ions in water.
• Most acids have hydrogen ions in their formulas.
• A binary acid composed of a hydrogen cation
bonded to one other element:
HCl
HBr
H2S
hydrochloric acid hydrobromic acid hydrosulfuric acid
Binary acids are always named: hydro____ic acid
Oxy-Acids
• An acid can also be made of a hydrogen ion
bonded to a complex ion.
Complex ions whose names end in “ate”:
NO3-
CO32-
SO42-
nitric acid:
HNO3
sulfuric acid:
H2SO4
carbonic acid:
H2CO3
phosphoric acid:H3PO4
PO43-
More Oxy-Acids
• Complex ions ending in “ite”:
NO2SO32nitrous acid:
ClOHNO2
sulfurous acid:
H2SO3
hypochlorous acid:
HClO
chlorous acid
HClO2
ClO2-
Organic Compounds
• Think-Pair-Share
• Individually think about what the
word “organic” means to you and
share with the class
• Organic chemistry: study of
compounds in which carbon is the
main element
• What is special about carbon?
– Carbon can form four bonds
– Bond together to form chains, rings
– Form combination of single, double,
and triple bonds
• Physical, chemical properties
Key terms
• Organic families: group of organic
compounds with common structural
features. E.g. Alkane
• Functional group: a structural
arrangement of atoms that give
molecule a particular characteristic
– E.g. double bond between two carbon atom
– A single bond between carbon and more
electronegative atom
– Double bond between carbon and oxygen
• Carbon-Carbon Multiple Bonds
– Double or triple bonds are more reactive
– Benzene- intermediate between single and
double bond
• Single bond between carbon and more
electronegative atom C-O
– Partial charge
– Hydrogen bonding
– Increase melting/boiling point due to
intermolecular force
– Affect solubility
– C=O has similar properties
Hydrocarbon
• Hydrocarbon: an organic compound that
contains only carbon and hydrogen atoms
in its molecular structure
• Classified based on the type of carboncarbon bonds
– Alkane
– Alkenes
– Alynes
• Aliphatic Hydrocarbon
– A compound that has a structure based on straight or
branched chains or rings of carbon atoms; does not
include aromatic compounds such as benzene
• Cyclic Hydrocarbon
– Hydrocarbon whose molecules have a closed ring
structure
• Aromatic Hydrocarbon
– A compound with a structure based on benzene
IUPAC system of nomenclature
• You will need to
memorize the “prefix”
or the root
• Prefix indicate the
number of carbon that
a molecule has
• There are different
suffix
• Alkane: -ane
• Alkene: -ene
• Alkyne: -yne
• Suffix indicate the type
of hydrocarbon
Alkane
• Hydrocarbon
• Saturated
• Suffix: “-ane”
• General formula: CnHn+2
Nomenclature rules

The root indicates the
number of carbon atoms
in the main chain or ring
1.
2.
3.
4.

The main chain is the
longest possible chain
and must include
multiple bonds
5.
6.
7.
8.
9.
10.

If there is a ring, it is
usually the main chain
meth
eth
prop
but
pent
hex
hept
oct
non
dec
Alkyl groups
• Side groups/substituent groups attached to
main carbon chain
• Alkane with hydrogen removed
• Suffix changed from “ane” to yl
• Use the prefix and change the suffix to “yl”
Methyl, ethyl, propyl….
Example: Alkane Nomenclature
Parent vs. branches
The Rules
More than one branch
More than 1 type of branch
Agenda
• Alkene, Alkyne nomenclature
• Properties of Alkane Alkene, Alkyne
• Reaction of Alkane, Alkene and Alkyne
• Quiz next week on:
–
–
–
–
5 binary/covalent nomenclature question
nomenclature of alkane, alkene and alkyne
5 naming question
5 drawing question
notes
• http://bettyxwyang.wikispaces.com/
• Other substituent groups
– Halogen:
• Fluorine
• Bromine
Alkene/ Alkynes
• Unsaturated:
• General formula
• Alkene: CnH2n
• Alkyne: CnH2n-2
Naming Alkenes & Alkynes
-Similar rules as Alkane but have different suffix
-number the double/triple bond so that the
numbers are the lowest possible
Suffix:
Alkene: change the end to ___.
Alkyne names change the end to ____
Naming the Alkene
CH2
CH3 CH2 C
CH2 CH3
CH2 C
CH3
CH3
Two double bonds
Combination of double and triple
bonds
Try it yourself
What do you notice?
Properties of Alkene and Alkyne
• Similar to Alkane
– Non-polar
– Low solubility in water
– Low boiling and melting point
• Much more reactive than Alkane!
Cyclic structures
• Cyclic structures are circular
• Have “cyclo” in name
H
H
H
H
C
C
H
C
C
C
H
H
H
H
H
• cyclopentane
Question- Draw the following:
cyclobutene 1,3-cyclopentadiene cyclopropane
H
H2C
HC
CH2
CH
H
H
C
C
C
H
C
C
H
CH2
H
H2C
CH2
Try it yourself
Aromatic Hydrocarbon
• Benzene: contain ____ carbon ring
Aromatic nomenclature
CH3
H3C
•
Identify the compound
Copy the table and complete the empty boxes.
Number
of
carbons
5
Name
Alkane or
alkene
Formula
pentene
alkene
C5H10
8
octane
alkane
C8H18
4
butene
alkene
C4H8
10
decane
alkane
C10H22
• Give examples of saturated and
unsaturated hydrocarbon
– What are their similarities and differences