Course Plan Course: Chemistry 12 Teacher: Anthony Tran Email: Anthony.Tran@burnabyschools.ca Phone: 604.760.8685 Burnaby Online Program – School District #41 Burnaby Course Length: 10 months (approx 100 hours) Chemistry 12 Course Description In Chemistry 12, you will develop a deeper understanding of chemical principles introduced in previous courses. The units of study include: Chemical Reactions and their Rates Chemical Equilibria Solubility Acid and Base Chemistry Electrochemistry To be successful in this course a student should have strong mathematics skills and problem-solving abilities as there is an emphasis on applying mathematics to solving problems. Chemistry 12 often serves as a prerequisite for further studies in sciences. How will your mark be calculated? Assignments Labs Unit Tests Final Exam 20% 10% 50% 20% Resources The text used in this course is Hebden: Chemistry 12 Workbook for Students. This text is very useful and will help you gain confidence with the material in this course. You can pick it up anytime during our office opening hours. Please download and print a copy of the data booklet provided as a resource in this introductory section. It is important that you learn how to use the information presented in this booklet. The Course Timeline is a resource that can be used as you work through each unit to ensure you have a sound understanding of the material covered. You may also want to visit the BC government Education website below which may help you prepare for unit tests and the final exam. http://www.bced.gov.bc.ca/exams/ Students are expected to: Contact the teacher by instant messaging or email when help is needed or questions arise. Be actively engaged and submitting work on a regular basis. Inform the teacher when they will be inactive for two or more weeks. Be aware that if they are inactive in a course for four or more weeks they may be removed from that course. Check their email at least twice a week. Create and submit completed solutions for all activities in the unit/chapter before requesting a test. Cite all sources properly. Answer in your own words. Check that their work and tests have been marked. Make time available to come in to Burnaby Online to write tests. Make appointments to write tests at least 2 school days in advance. Communication Communication is key to success in this course. Please be sure to contact your instructor by email or phone anytime a problem arises. We hope you achieve great success in this course. You will be required to complete all assignments and submit them to be marked. When completing each assignment remember to show a good level of understanding of the material covered. All tests and exams will be written at the Burnaby Online centre. 2 Course Learning Activities UNIT Review Unit Unit 1 Chemical Reactions and their Rates Unit 2 Chemical Equilibriums Unit 3 Solubility SECTION Moles and Molarity Review Assignment Stoichiometry Review Assignment 1.1: Reaction Rates 1.2: Collision Theory 1.3: The Potential Energy Diagram 1.4: Heats of Reaction 1.5: Influence of Form of Reaction on Rate 1.6: Kinetic Energy Distribution Curve 1.7: Reaction Mechanisms Unit 1.1 Assignment Unit 1.2 Assignment Unit 1.3 Assignment Lab 1.1 Assignment Lab 1.2 Assignment Unit 1 Practice Exam Unit 1 Test 2.1: Equilibrium: Introduction 2.2: Le Chatelier’s Principle 2.3: The Equilibrium Law 2.4: Four Laws of Thermodynamics 2.5: A Concentration vs. Time Graph Unit 2.1 Assignment Unit 2.2 Assignment Unit 2.3 Assignment Unit 2.4 Assignment Lab 2.1 Assignment Unit 2 Practice Exam Unit 2 Test 3.1: Solubility/Ksp/Vocab 3.2: Predicting Ppt Formation Qualitatively 3.3: Predicting Ppt Formation Quantitively 3.4: Altering Solubility and the Effect of Temperature 3.5: Saturated Solutions 3.6: Separated Dissolved Ions 3.7: Common Ions Unit 3.1 Assignment Unit 3.2 Assignment Unit 3.3 Assignment Unit 3.4 Assignment Unit 3.5 Assignment Lab 3.1 Assignment 3 PRESCRIBED LEARNING OUTCOMES COMPLETED A1 & A2 A3 & A5 A4 A4 A7 & A8 A4 & A7 A6 B1 & B6 B3 B2, B5 & B6 B2 B3 C1 & C6 C4 & C5 C3 & C7 C1 C2 C8 C8 Lab 3.2 Assignment Unit 3 Practice Exam Unit 3 Test Midterm Exam Midterm 4.1: Acids and Bases 4.2: Acid/Base Conjugate Pairs 4.3: The Equilibrium of Pure Water 4.4: Relative Strengths of Acids and Bases 4.5: Measuring Acidity/Basicity with pH and pOH 4.6: Temperature Dependence of pH and pOH 4.7: The pH of Distilled Water 4.8: How to Solve Acid/Base Problems 4.9: Percent Dissociation 4.10: Calculating [H+], [OH-], pH and pOH 4.11: Acidic and Basic Anhydrides 4.12: Indicators 4.13: The Chemistry of Ammonia 4.14: Titration 4.15: Inexact Neutralization Unit 4 4.16: Hydrolysis Acid & Bases 4.17: Buffers Chemistry Unit 4.1 Assignment Unit 4.2 Assignment Unit 4.3 Assignment Unit 4.4 Assignment Unit 4.5 Assignment Unit 4.6 Assignment Unit 4.7 Assignment Unit 4.8 Assignment Unit 4.9 Assignment Lab 4.1 Assignment Unit 4 - Part 1 - Practice Exam Unit 4 - Part 2 - Practice Exam Unit 4 Test 5.1: Electrochemical Cell 5.2: Oxidation Numbers 5.3: Balancing Reactions with Oxidation Numbers 5.4: Balancing Reactions with ½ Reactions Unit 5 5.5: The Standard Reduction Potential Table Electrochemistry/ 5.6: Overpotential Effect/Cathodic Protection Redox Reactions 5.7: Type I Electrolytic Cells 5.8: Type II Electrolytic Cells 5.9: Type III Electrolytic Cells Unit 5.1 Assignment Unit 5.2 Assignment 4 D1 & D6 D2 & D3 E1 D4 & D5 E2 E1 E1 E3 & E4 E2 & E4 D2 F8 F2 E1 F1 F3 F4 & F5 F6 & F7 G1 & H1 H1 G3 G3 G2 H2 & H3 H4 & H5 H4 & H5 H2 & H5 Final Unit 5.3 Assignment Unit 5.4 Assignment Unit 5 Practice Exam Unit 5 Test Final Exam Prescribed Learning Outcomes: Chemistry 12 It is expected that students will: Reaction Kinetics (Unit 1) A1 A2 A3 A4 A5 A6 A7 A8 demonstrate awareness that reactions occur at differing rates experimentally determine rate of a reaction demonstrate knowledge of collision theory describe the energies associated with reactants becoming products apply collision theory to explain how reaction rates can be changed analyse the reaction mechanism for a reacting system represent graphically the energy changes associated with catalyzed and uncatalyzed reactions describe the uses of specific catalysts in a variety of situations Dynamic Equilibrium (Unit 2) B1 explain the concept of chemical equilibrium with reference to reacting systems B2 predict, with reference to entropy and enthalpy, whether reacting systems will reach equilibrium B3 apply Le Châtelier’s principle to the shifting of equilibrium B4 apply the concept of equilibrium to a commercial or industrial process B5 draw conclusions from the equilibrium constant expression B6 perform calculations to evaluate the changes in the value of Keq and in concentrations of substances within an equilibrium system Solubility Equilibria (Unit 3) C1 C2 C3 C4 C5 C6 C7 C8 determine the solubility of a compound in aqueous solution describe a saturated solution as an equilibrium system determine the concentration of ions in a solution determine the relative solubility of a substance, given solubility tables apply solubility rules to analyse the composition of solutions formulate equilibrium constant expressions for various saturated solutions perform calculations involving solubility equilibrium concepts devise a method for determining the concentration of a specific ion Nature of Acid and Bases (Unit 4) D1 identify acids and bases through experimentation D2 identify various models for representing acids and bases D3 analyse balanced equations representing the reaction of acids or bases with water D4 classify an acid or base in solution as either weak or strong, with reference to its electrical conductivity D5 analyse the equilibria that exist in weak acid or weak base systems D6 identify chemical species that are amphiprotic 5 Acids and Bases: Quantitative Problem Solving (Unit 4) E1 analyse the equilibrium that exists in water E2 perform calculations relating pH, pOH, [H3O+], and [OH-] E3 explain the significance of the Ka and Kb equilibrium expressions E4 perform calculations involving Ka and Kb Applications of Acid-Base Reactions (Unit 4) F1 demonstrate an ability to design, perform, and analyse a titration experiment involving the following: – primary standards – standardized solutions – titration curves – appropriate indicators F2 describe an indicator as an equilibrium system F3 perform and interpret calculations involving the pH in a solution and Ka for an indicator F4 describe the hydrolysis of ions in salt solutions F5 analyse the extent of hydrolysis in salt solutions F6 describe buffers as equilibrium systems F7 describe the preparation of buffer systems F8 predict what will happen when oxides dissolve in rain water Oxidation-Reduction (Unit 5) G1 G2 G3 G4 describe oxidation and reduction processes analyse the relative strengths of reducing and oxidizing agents balance equations for redox reactions determine the concentration of a species by performing a redox titration Applications of Redox Reactions (Unit 5) H1 analyse an electrochemical cell in terms of its components and their functions H2 describe how electrochemical concepts can be used in various practical applications H3 analyse the process of metal corrosion in electrochemical terms H4 analyse an electrolytic cell in terms of its components and their functions H5 describe how electrolytic concepts can be used in various practical applications 6