CHEMISTRY 30 – Course Outline
A.
Prerequisite:
A minimum pre-requisite mark of 50% is required. But in order to experience success in
Chemistry 30, a recommended mark of 60% in Chemistry 20 is advised.
B.
Textbook:
Nelson Chemistry
Replacement cost is $126.00
C.
Course Outline:
Review from Chemistry 20 will be done as required.
Unit 7: Electrochemistry
(approximately 25 periods)
Chapter 13:
Redox Reactions
Chapter 14:
Electrochemical Cells
Unit 8: Chemical Equilibrium – Focusing on Acid-Base Systems
(approximately 25 periods)
Chapter 15:
Equilibrium Systems
Chapter 16:
Equilibrium in Acid-Base Systems
Unit 6: Chemical Energy
(approximately 15 periods)
Chapter 11:
Enthalpy Change
Chapter 12:
Catalysis
Unit 5: Organic Chemistry
(approximately 15 periods)
Chapter 9:
Hydrocarbons from Petroleum
Chapter 10:
Organic Reactions
1
D.
Mark Breakdown

Unit 7 (Chapters 13 and 14)
Electrochemistry
31 %
Chapter 13 Exam
Chapter 14 Exam

Unit 8 (Chapters 15 and 16)
Acid-base Equilibrium
31 %
Chapter 15 Exam
Chapter 16 Exam

Unit 6 (Chapters 11 and 12)
Chemical Energy
19 %
Unit Exam

Unit 5 (Chapters 9 and 10)
Organic Chemistry
19 %
Unit Exam
The final Chemistry 30 mark is a blended mark of the teacher based mark and the diploma
exam mark.
The final mark in Chemistry 30 must be 50% or over to receive credits.
A mark of 70% or better is suggested for Post-Secondary.
Chemistry 30 Diploma: Monday, June 24, 2013
9:00 a.m. – 11:00 a.m.

(Multiple Choice / Numerical Response ONLY)
Students are permitted an additional ½ hour to complete their examination.
Chemistry 30 Diploma Exam

44 multiple choice questions

16 numerical response questions

You have 2.0 hours (120 minutes) – 2.5 hours (150 minutes) to do 60 questions
120 minutes / 60 questions
= 2 minutes per question
80 minutes / 2.0 minutes/question
= 40 questions
150 minutes / 60 questions
= 2 ½ minutes per question
80 minutes / 2.5 minutes/question
= 32 questions
29 multiple choice
23 multiple choice
11 numerical response
9 numerical response
2
TENTATIVE COURSE OUTLINE BY CHAPTER
Unit 7 - Electrochemisty
Chapter 13 – Redox Reactions
13.1 Oxidation and Reduction (page 558)

Reduction / Oxidation Half-reactions

Oxidized species / Reduced species

Oxidizing agent / Reducing agent

Redox equations
Lab / Demo:
Single Replacement Reactions between metals and aqueous solutions
Writing Complex Half-Reaction Equations
13.2 Predicting Redox Reactions (page 568)
 Introduction to Reduction Half-reaction table

Spontaneity Rule (spontaneous /non-spontaneous reactions)

Predicting Redox reactions using the data book
Constructing Redox Tables - making a redox table from lab results or using the
spontaneity rules
Predicting Redox Reactions by Constructing Half-Reactions
13.3 Oxidation States (page 583)

Rules for determining the oxidation number(state) of atoms

Making up ½ reactions in acidic or basic solutions

Balancing using oxidation numbers
13.4 Redox Stoichiometry (page 596)
Redox Titration Lab / Demo
Redox Titration Stoichiometry Questions
Chapter 13 Exam
3
Unit 7 - Electrochemisty
Chapter 14 – Electrochemical Cells – Voltaic and Electrolytic Cells
14.1 Technology of Cells and Batteries (page 612)
14.2 Voltaic Cells (page 622)

Voltaic Cell Demo

Voltaic Cells

Standard ½ cell

Eo (V) values – calculating
14.3 Electrolysis / Electrolytic Cells (page 639)
 Electrolytic cells - Demo

Electrolytic cells

Electroplating – Demo
14.4 Cell Stoichiometry (page 652)
Corrosion

Prevention

Cathodic protection

Sacrificial anode
STS Connections with regard to cells
Chapter 14 Exam
4
Unit 8 – Chemical Equilibrium Focusing on Acid-Base Systems
Chapter 15- Equilibrium Systems
15.1 Explaining Equilibrium Systems (page 676)
 What is Equilibrium?

Equilibrium Law Expression based upon balanced equations

Equilibrium constant, (K / Kc), value calculations

Equilibrium concentrations of reactants or products

ICE Tables
15.2 Qualitative Change in Equilibrium Systems (page 690)

Manipulating Equilibrium systems

Le Chatelier’s Principle: changes in concentration, temperature, volume,
catalyst, and inhibitors
Chapter 15 Exam
5
Unit 8 – Chemical Equilibrium Focusing on Acid-Base Systems
Chapter 16 – Equilibrium in Acid-Base Systems
Arrhenius Definition of Acids and Bases
Revised (Modified) Arrhenius Definition of Acids and Base
16.1 Water Ionization and Acid-Base Strength (page 712)
Water Equilibrium Systems
 Calculations of [H3O1+(aq)] and [OH1-(aq)]

Calculations of pH, and pOH
Strong Acids vs. Weak Acids
 % reaction of acids
16.2 Bronsted-Lowry Theory of Acid-Base Concept (page 722)

Predicting Bronsted-Lowry Acid/Base Reactions (using the data book)

Building Acid-Base Tables
16.3 Acid-Base Strength and the Equilibrium Law (page 737)

Acid Ionization Constant, Ka, for weak acids

Approximate rule for determining [H3O1+(aq)]

Base Strength and the Ionization Constant, Kb

Approximate rule for determining [OH1-(aq)]
16.4 Interpreting pH Curves (page 751)

Buffering regions

Endpoints / equivalence point

Acid-base indicators

Polyprotic species / polybasic entities

Buffer solutions
Chapter 16 Exam
6
Unit 6 – Chemical Energy
Chapter 11 – Enthalpy Change
11.1 Energy Demands and Sources (page 480)
11.2 Calorimetry (page 486)
Q = m c t = rH

Heat Transfer and Enthalpy Change

Molar Enthalpies and Calorimetry
rH = n rHm
Law of Heat Exchange (total enthalpy lost = total enthalpy gained)
11.3 Communicating Enthalpy Changes (page 495)
 Method 1: Molar Enthalpies of Reaction, rHm

Method 2: Enthalpy Changes, rH

Method 3: Energy Terms in Balanced Equations (thermochemical
equations)

Method 4: Chemical Potential Energy Diagrams
11.4 Hess’s Law (page 502)
 Predicting rH: Hess’s Law
11.5 Molar Enthalpies of Formation (page 510)

Molar Enthalpies of Formation

Molar Enthalpies of Decomposition

Molar Enthalpies of Combustion
Unit 6 – Chemical Energy
Chapter 12 – Explaining Chemical Changes
12.1 Activation Energy (page 524)
12.2 Bond Energy and Reactions (page 532)
12.3 Catalysts and Reaction Rates (page 535)
Chapter 11 / 12 Exam
7
Unit 5 – Organic Chemistry
Chapter 9 – Hydrocarbons from Petroleum
9.1 Fossil Fuels (page 358)
9.2 Alkanes from Natural Gas (page 362)
Straight Chain Hydrocarbons
 alkanes

alkenes

alkynes
9.3 Alkenes and Alkynes – Cracking Natural Gas
Branched Hydrocarbons
 alkanes

alkenes

alkynes
Cyclic Hydrocarbons
 cycloalkanes

cycloalkenes

cycloalkynes
9.4 Aromatics (page 381)
 benzene
9.5 Crude Oil Refining (page 386)
Reactions of Hydrocarbons
9.6 Complete and Incomplete Combustion Reactions (page 398)
8
Unit 5 – Organic Chemistry
Chapter 10 - Hydrocarbon Derivatives, Organic Reactions, and Petrochemicals
10.1 Petrochemicals in Alberta (page 412)
10.2 Organic Halides and Addition and Substitution Reactions (page 417)
10.3 Alcohols and Elimination Reactions (page 425)
10.4 Carboxylic Acids, Esters, and Esterification Reactions (page 436)
10.5 Polymerization Reactions – Monomers and Polymers (page 445)
Chapter 9 / 10 Exam
9