Grade 12, ChemistrySCH4U

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 OutlineUnit 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

• (NH4)3PO4• PBr5• MgSO4• CaO• H3PO4• Na2Cr2O7• MgO• SO2• Cu(NO3)2• HI• N2O

• Ca• NaOH• CO• H2SO4(aq)• Pb• He• CO2• BaBr2• SO3

• Barium Sulfate• Potassium oxide• Magnesium

hydroxide • Potassium nitrate• Copper(II) oxide• Nitric acid• Sulfuric acid• Iron (II) Chloride

• Name the following

Type I Binary Ionic Compounds• The metal cations in these compounds have only ONE possible charge.

Na+ Zn2+ Al3+ Ca2+

sodium zinc aluminum calcium

The charges are memorized or predicted using a periodic table!

• The cations are bonded to nonmetal anions:

O2- N3- F- Br -

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- Li2O

aluminum bromide: Al3+ and Br - 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: NO3-sulfate: SO4

2- hydroxide: OH-

Phosphate PO4 3-

Things to Notice

perchorate ClO4- sulfate SO4

2-

chlorate ClO3- sulfite SO3

2-

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.

CO2 is named “carbon dioxide”

CO is named “carbon monoxide”

N2O is named “dinitrogen monoxide”

SO3 is named “sulfur trioxide”

Prefix:

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- SO4

2- CO32- PO4

3-

nitric acid: HNO3

sulfuric acid: H2SO4

carbonic acid: H2CO3

phosphoric acid:H3PO4

More Oxy-Acids• Complex ions ending in “ite”:

NO2- SO3

2- ClO- ClO2-

nitrous acid: HNO2

sulfurous acid: H2SO3

hypochlorous acid: HClO

chlorous acid HClO2

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 carbon- carbon 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

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

The Rules

Parent vs. branches

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

-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 Alkenes & Alkynes

Naming the Alkene

CH3 CH2 C

CH2

CH2 C

CH2

CH3

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!

C

C

C

CC H

HHH

H

H

HH H

H

Cyclic structures• Cyclic structures are circular• Have “cyclo” in name

• cyclopentaneQuestion- Draw the following:

cyclobutene 1,3-cyclopentadiene cyclopropane

CH2

CH

CH2

CHCC

C CCH

H H

H

H H

CH2

CH2

CH2

Try it yourself

Aromatic Hydrocarbon• Benzene: contain ____ carbon ring

Aromatic nomenclatureCH3

CH3

• Copy the table and complete the empty boxes.

Number of

carbons

Name Alkane or alkene

Formula

5 pentene

8 octane

4 butene

10 decane

alkene C5H10

alkane C8H18

alkene C4H8

alkane C10H22

Identify the compound

• Give examples of saturated and unsaturated hydrocarbon– What are their similarities and differences