CHEMISTRY 12 SYLLABUS Online 2010 Mr. Lockwood Email: plockwood@sd43.bc.ca Personal: https://my43.sd43.bc.ca/schools/pinetreesecondary/classes/plockwood/default.aspx UserName: Password: WebCT: http://bb.etc.bc.ca/webct/entrypageins.dowebct Username: District: http://public.sd43.bc.ca/district/col/default.aspx Password: RATIONALE: Chemistry is the science, which deals with the properties and reactions of materials; it is concerned with the identification, characterization and transformation of matter and with the energy changes accompanying these transformations. Chemical science focuses on the structure and interaction of matter at the atomic and molecular levels. This course is intended to provide you with a grounding in the discipline of chemistry, as those of you who take it might subsequently engage in further study of the subject. The treatment of the topics is mathematically more rigorous and detailed than in Chemistry 11; therefore, the range of topics is narrower than in Chemistry 11. TEXT: Hebden Chemistry 12 MATERIALS: Scientific Calculator (non-graphing, check http://www.bced.gov.bc.ca/exams/specs/calculator_policy06.pdf) MARKS: 90% Tests/Quizzes (Included in this is a midterm and in-class final) 10% Assignments Optional Provincial Exam 60% School Mark and 40% Provincial Exam = Total Mark STUDENT RESPONSIBILITIES If you are going to be away for any reason, it is your responsibility to email me before class or within 24 hours of not attending class. If you do not you will not be eligible to make missed assignments or tests! Assignments will be due within 1 day of your absence. I expect that you can scan and email your assignments or fax to the school. Tests will only be up during regular day time school hours here at Pinetree. Unit 1 2 3 4 5 Theme Reaction Kinetics Equilibrium Solubility of Ionic Substances Acids/Bases/Salts Oxidation-Reduction Sections in Hebden 1 2 3 4 5 Help/Tutoring: Please use email address as shown above. Session Day Topic to be Completed 1 Sept 15 Introduction Kinetics, Activation assignment due next period 2 Sept 22 Chemistry 11 Review Exam/Kinetics 3 Sept 29 Kinetics Unit test ( A, B and C) 4 Oct 6 Equilibrium 5 Oct 13 Equilibrium Quiz ( D and E), Equilibrium Assignment Due 6 Oct 20 Equilibrium Test ( D, E and F) 7 Oct 27 Solubility 8 Nov 3 Solubility Test ( G, H and I) 9 Nov 10 Midterm ( A I) 10 Nov 17 Acid Base 11 Nov 24 Acid Base Quiz (J and K) 12 Dec 1 Acid Base, Acid Base worksheet due 13 Dec 8 Acid Base Test (J-R) 14 Dec 15 Redox 15 Jan 5 Redox Quiz (S and T) 16 Jan 12 Final (All outcomes) Updated 25 January 2011 Page 1 of 13 Lockwood
Description of Type (Assignment, Exam/Quiz ) Date Completed Mark Activation Assignment (Chem 11 Review and Outcome A) Assignment /35 Chemistry 11 Review Test Exam /35 Kinetics Unit Test ( A, B and C) Equilibrium Quiz ( D and E) Equilibrium Assignment ( D, E and F) Equilibrium Test ( D, E and F) Solubility Test ( G, H and I) Midterm ( A to I) Acid-Base Quiz ( J and K) Acid-Base Assignment ( J - M ) Acid Base Test ( J to R) Redox Quiz ( S and T) Final Exam (All ) Exam /61 Quiz /20 Assignment /30 Exam /60 Exam /49 Exam /53 Exam /26 Assignment /30 Exam /52 Exam /30 Exam /78 Updated 25 January 2011 Page 2 of 13 Lockwood
Reference // Text A: Reaction Kinetics (Introduction) 1. give examples of reactions proceeding at different rates 2 2. describe rate in terms of some quantity (produced or consumed) per unit of time 6 3. experimentally determine rate of a reaction 6 & 7 4. identify properties that could be monitored in order to determine a reaction rate 6 5. recognize some of the factors that control reaction rates 4 6. compare and contrast factors affecting the rates of both homogeneous and heterogeneous reactions 5 7. discuss situations in which the rate of reaction must be controlled 2 #4 B: Reaction Kinetics (Collision Theory) 1. demonstrate an awareness of the following: reactions are the result of collisions between reactant particles not all collisions are successful sufficient kinetic energy (KE) and favourable geometry are required to increase the rate of a reaction one must increase the frequency of successful collision energy changes are involved in reactions as bonds are broken and formed 2. describe the activated complex in terms of its potential energy (PE), stability, and structure 3. define activation energy 4. describe the relationship between activation energy and rate of reaction 5. describe the changes in KE and PE as reactant molecules approach each other 6. draw and label PE diagrams for both exothermic and endothermic reactions, including H, activation energy, and the energy of the activated complex 7. relate the sign of H to whether the reaction is exothermic or endothermic 8. write a chemical equation including the energy term (given a H value) and vice versa 9. describe the role of the following factors in reaction rate: nature of reactants concentration temperature surface area 2 #1 9 11 #3 9 11 // Chemistry 11 4 & 5 #2 Updated 25 January 2011 Page 3 of 13 Lockwood
C: Reaction Kinetics (Reaction Mechanisms and Catalysts) Reference // Text 1. use examples to demonstrate that most reactions involve more than one step 2. describe a reaction mechanism as the series of steps (collisions) that result in the overall 2 & 3 #1 reaction 3. define catalyst 3 & 5 #2 4. compare and contrast the PE diagrams for a catalyzed and uncatalyzed reaction in terms of: reaction mechanism H 9 #3 activation energy 5. identify reactant, product, reaction intermediate, and catalyst from a given reaction mechanism 2 & 3 #1 6. describe the uses of specific catalysts in a variety of situations 5 D: Dynamic Equilibrium (Introduction) 1. describe the reversible nature of most chemical reactions 2. identify the reversible pathways of a chemical reaction on the PE diagram 2 3. relate the changes in rates of the forward and reverse reactions to the changing concentrations of the reactants or products as equilibrium is established. 4 4. describe chemical equilibrium as a closed system at constant temperature: whose macroscopic properties are constant #1 & #6 where the forward and reverse reaction rates are equal 2 & 3 that can be achieved from either direction where the concentrations of reactants and products are constant 5. describe the dynamic nature of chemical equilibrium 6. infer that a system not at equilibrium will tend to move toward a position of equilibrium 2 7. determine entropy and enthalpy changes from a chemical equation (qualitatively) 8. state that systems tend toward a position of minimum enthalpy and maximum randomness (entropy) 9. predict the result when enthalpy and entropy factors: 9 #5 & #6 both favour the products both favour the reactants oppose one another Updated 25 January 2011 Page 4 of 13 Lockwood
E: Dynamic Equilibrium (Le Chatelier's Principle) 1. describe the term shift as it applies to equilibria 2. apply Le Chatelier's principle to the shifting of equilibrium involving the following: temperature change concentration change 8 #4 & #7 volume change of gaseous systems 3. explain the above shifts using the concepts of reaction kinetics 4. identify the effect of a catalyst on dynamic equilibrium 5. apply the concept of equilibrium to a commercial or industrial process 9 F: Dynamic Equilibrium (The Equilibrium Constant) 1. gather and interpret data on the concentration of reactants and products of a system at equilibrium Lab Lab 2. write the expression for the equilibrium constant when given the equation for either a homogeneous or heterogeneous equilibrium system #2 3. relate the equilibrium position to the value of K eq and vice versa 4. predict the effect (or lack of effect) on the value of K eq of changes in the following factors: temperature, pressure, concentration, surface area, and catalyst 5. calculate the value of K eq given the equilibrium concentration of all species 5 7 6. calculate the value of K eq given the initial concentrations of all species and one equilibrium #3 concentration 7. calculate the equilibrium concentrations of all species given the value of K eq and the initial concentrations 8. determine whether a system is at equilibrium, and if not, in which direction it will shift to reach equilibrium when given a set of concentrations for reactants and products Updated 25 January 2011 Page 5 of 13 Lockwood
G: Solubility Equilibria (Concept of Solubility) 1. classify solutions as ionic or molecular given the formula of the solute 2. describe the conditions necessary to form a saturated solution 3. describe solubility as the concentration of a substance in a saturated solution 4. use appropriate units to represent the solubility of substances in aqueous solutions 5. measure the solubility of a compound in aqueous solution 6. describe the equilibrium that exists in a saturated aqueous solution 7. write a net ionic equation that describes a saturated solution 8. calculate the concentration of the positive and negative ions given the concentration of a solute in an aqueous solution 10 & Chemistry 11 #15 H: Solubility Equilibria (Solubility and Precipitation) 1. describe a compound as having high or low solubility relative to 0.1 M by using a solubility chart 2. use a solubility chart to predict if a precipitate will form when two solutions are mixed, and identify the precipitate 11 3. write a formula equation, complete ionic equation, and net ionic equation that represent a precipitation reaction 4. use a solubility chart to predict if ions can be separated from solution through precipitation, and outline the process 10, 11 & 16 5. predict qualitative changes in the solubility equilibrium upon the addition of a common ion 14 6. identify an unknown ion through experimentation involving a qualitative analysis scheme 7. devise a procedure by which the contaminating ions in hard or polluted water can be Lab & 16 removed #11 I: Solubility Equilibria (Quantitative Aspects) 1. describe the K sp expression as a specialized K eq expression 2. write a K sp expression for a solubility equilibrium 3. calculate the K sp for AB and AB 2 type compounds when given the solubility of a compound 4. calculate the solubility of AB and AB 2 type compounds from the K sp 11 13 #8 & #9 5. predict the formation of a precipitate by comparing the trial ion product to the K sp value using specific data 6. calculate the maximum concentration of one ion given the K sp and the concentration of the other ion 7. demonstrate and describe a method for determining the concentration of a specific ion Lab Updated 25 January 2011 Page 6 of 13 Lockwood
J: Acids, Bases, and Salts (Properties and Definitions) 1. identify acids and bases through experimentation Lab 2. list general properties of acids and bases 3. write balanced equations representing the neutralization of acids by bases in solution 2 4. define Arrhenius acids and bases 5. write names and formulae of some common acids and bases and outline some of their common properties, uses, and commercial names Lab 6. define Brønsted-Lowry acids and bases 2 7. identify Brønsted-Lowry acids and bases in an equation 2 8. write balanced equations representing the reaction of acids or bases with water 2 & 3 9. identify an H 3 O + ion as a protonated H 2 O molecule that can be represented in shortened form as H + (aq) 3 10. define conjugate acid-base pair 2 & 3 11. identify the conjugate of a given acid or base 3 12. show that in any Brønsted-Lowry acid-base equation there are two conjugate pairs present 3 K: Acids, Bases, and Salts (Strong and Weak Acids and Bases) 1. relate electrical conductivity in a solution to the concentration of ions 2. classify an acid or base in solution as either weak or strong by comparing conductivity 2 3. define a strong acid and a strong base 4. define a weak acid and a weak base 5 & 7 5. write equations to show what happens when strong and weak acids and bases are dissolved in water (dissociation, ionization) 6 6. compare the relative strengths of acids or bases by using a table of relative acid strengths 7. identify and explain why the strongest acid in aqueous solutions is H 3 O + and the strongest base in aqueous solutions is OH 1-8. predict whether products or reactants are favoured in an acid-base equilibrium by comparing the strength of the two acids (or two bases) 9 bases) using their relative positions on an acid strength table 9. compare the relative concentrations of H 3 O + (or OH 1- ) between two acids (or between two 6 10. define amphiprotic 11. identify chemical species that are amphiprotic 7 & 9 12. describe situations in which H 2 O would act as an acid or base #1 #1 Updated 25 January 2011 Page 7 of 13 Lockwood
L: Acids, Bases, and Salts (K w, ph, poh) 1. write equations representing the ionization of water using either H 3 O + and OH 1- or H + and OH 1-2. write the equilibrium expression for the ion product constant of water, K w 3. predict the effect of the addition of an acid or base to the equilibrium system: 2H 2 O(1) H 3 O + (aq) + OH 1- (aq) 4. state the relative concentrations of H 3 O + and OH 1- in acid, base, and neutral solutions 5. state the value of K w at 25 C 6. describe the variation of the value of K w with temperature 7. calculate the concentration of H 3 O + (or OH 1- ) given the other, using K w 8. describe the ph scale with reference to everyday solutions 9. define ph and poh 10. define pk w, give its value at 25 C, and its relation to ph and poh 11. perform calculations relating ph, poh, H 3 O +, and OH 1-12. calculate H 3 O + or OH 1- from ph and poh M: Acids, Bases, and Salts (K a and K b Problem Solving) 1. write K a and K b equilibrium expressions 2. relate the magnitude of K a or K b to the strength of the acid or base 3. given the K a, K b, and initial concentration, calculate any of the following: H 3 O + OH 1- ph poh 4. calculate the value of K b for a base given the value of K a for its conjugate acid (or vice versa) 5. calculate the value of K a or K b given the ph and initial concentration 3 4 4 & 5 6 8 #2 #3 & #4 N: Acids, Bases, and Salts (Hydrolysis of Salts) 1. write a dissociation equation for a salt in water 2. write net ionic equations representing the hydrolysis of salts 3. predict qualitatively whether a salt solution would be acidic, basic, or neutral 4. determine whether an amphiprotic ion will act as a base or an acid in solution 12 & 13 #6 Updated 25 January 2011 Page 8 of 13 Lockwood
O: Acids, Bases, and Salts (Indicators) 1. describe an indicator as a mixture of a weak acid and its conjugate base, each with distinguishing colours 2. describe the term transition point of an indicator, including the conditions that exist in the equilibrium system 3. describe the shift in equilibrium and resulting colour changes as an acid or a base is added to an indicator 4. predict the approximate ph at the transition point using the K a value of an indicator 5. predict the approximate K a value for an indicator given the approximate ph range of the colour change P: Acids, Bases, and Salts (Neutralizations of Acids and Bases) 1. demonstrate an ability to design and perform a neutralization experiment involving the following: primary standards standardized solutions titration curves indicators selected so the end point coincides with the equivalence point 2. calculate from titration data the concentration of an acid or base 3. calculate the volume of an acid or base of known molarity needed to neutralize a known volume of a known molarity base or acid 4. write formula, complete ionic, and net ionic neutralization equations for: a strong acid by a strong base a weak acid by a strong base a strong acid by a weak base 5. calculate the ph of a solution formed when a strong acid is mixed with a strong base 6. contrast the equivalence point (stoichiometric point) of a strong acid-strong base titration with the equivalence point of a titration involving a weak acid-strong base or strong acidweak base 12 #5 10 & 11 #5 Updated 25 January 2011 Page 9 of 13 Lockwood
Q: Acids, Bases, and Salts (Buffer Solutions) 1. describe the tendency of buffer solutions to resist changes in ph 2. describe the composition of an acidic buffer and a basic buffer 3. outline a procedure to prepare a buffer solution 4. identify the limitations in buffering action 5. describe qualitatively how the buffer equilibrium shifts as small quantities of acid or base are added to the buffer 6. describe common buffer systems present in industrial, environmental, or biological systems R: Acids, Bases, and Salts (Acid Rain) 1. write equations representing the formation of acidic solutions or basic solutions from nonmetal and metal oxides 2. describe the ph conditions required for rain to be called acid rain 3. relate the ph of normal rain water to the presence of dissolved CO 2 4. describe sources of NO x and SO x 5. discuss general environmental problems associated with acid rain 14 & 15 #7 16 & 17 #13 Updated 25 January 2011 Page 10 of 13 Lockwood
S: Oxidation- Reduction (Introduction) 1. define and apply the following: oxidation reduction oxidizing agent 2 & 3 #3 reducing agent half-reaction redox reaction 2. determine the following: the oxidation number of an atom in a chemical species the change in oxidation number an atom undergoes when it is oxidized or reduced 4 #1 & #3 whether an atom has been oxidized or reduced by its change in oxidation number 3. relate change in oxidation number to gain or loss of electrons 4 #1 4. from data for a series of simple redox reactions, create a simple table of reduction halfreactions Lab Lab 5. identify the relative strengths of oxidizing and reducing agents from their positions on a half-reaction table 6. use a table of reduction half-reactions to predict whether a spontaneous redox reaction will occur between any two species 3 #3 3 #3 T: Oxidation- Reduction (Balancing Redox Equations) 1. balance a half-reaction in solution (acid, base, neutral) 2. balance a net ionic redox reaction in acid and base solution 3. write the equations for reduction and oxidation half-reactions given a redox reaction 4. identify reactants and products for several redox reactions performed in a laboratory and balance the equations 5. select a suitable reagent to be used in a redox titration in order to determine the concentration of a species 6. determine the concentration of a species by performing a redox titration 5 & 6 #2 Lab Lab Updated 25 January 2011 Page 11 of 13 Lockwood
U: Oxidation-Reduction (Electrochemical Cells) 1. define, construct, and label the parts of an electrochemical cell 2. identify the half-reactions that take place at each electrode 3. predict the direction of movement of each type of ion in the cell 4. predict the direction of flow of electrons in an external circuit 5. predict which electrode will increase in mass and which will decrease in mass as the cell operates 6. predict the voltage of the cell when equilibrium is reached 7 & 8 7. assign voltages to the reduction half-reactions of oxidizing agents by comparison of several cells 8. describe the significance of the E of an electrochemical cell 9. predict the voltage (E ) of an electrochemical cell using the table of standard reduction halfcells 10. predict the spontaneity of the forward or reverse reaction from the E of a redox reaction 11. describe how electrochemical concepts can be used in various practical applications 12 #4 & #6 V: Oxidation- Reduction (Corrosion) 1. describe the conditions necessary for corrosion to occur 2. analyse the process of metal corrosion in electrochemical terms 3. suggest several methods of preventing or inhibiting corrosion of a metal 4. describe and explain the principle of cathodic protection 11 #6 W: Oxidation-Reduction (Electrolytic Cells) 1. define electrolysis and electrolytic cell 2. design and label the parts of an electrolytic cell capable of electrolyzing an aqueous salt (use of overpotential effect not required) 9 & 10 3. predict the direction of flow of all ions in the cell 4. write the half-reaction occurring at each electrode 5. demonstrate the principles involved in simple electroplating 6. construct an electrolytic cell capable of electroplating an object Lab 7. describe the electrolytic aspects of metal refining processes 13 8. draw and label the parts of an electrolytic cell used for electrolysis of a molten binary salt 9 & 10 #5 & #6 Updated 25 January 2011 Page 12 of 13 Lockwood
Student Name PEN # P Individualized Course Learning Plan for Chemistry 12 (Fall 2010) As part of any online course, it is important to set goals for yourself. Please complete the following information, which will serve as your plan for completing Chemistry 12, as well as a reference for your teacher in supporting your learning goals. Planned Course Start Date: Planned Course Completion Date: September 15, 2010 January 12, 2011 Your goal for a grade in this course: Please list any areas where you feel you will need extra support from your teacher in this course: Student Signature: Date: Last Updated 25 January 2011 Page 13 of 13 Lockwood