CHEMISTRY 12 SYLLABUS

Transcription

1 CHEMISTRY 12 SYLLABUS Online 2013 Mrs. Lockwood District: 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. MATERIALS: Scientific Calculator MARKS: 60% Exams 20% Assignments/Labs 20% Final Exam Description of Assessment Kinetics Assignment (Outcomes A1- A8) Lab 1 Reaction Rates Type (Assignment/Lab, Exam) Assignment Lab Description of Assessment Acid Base Assignment (Outcomes D1-D6 and E1-E4) Lab 4 Acid Base Strength Type (Assignment/Lab, Exam) Assignment Lab Kinetics Unit Test (Outcomes A1- A8) Equilibrium Assignment (Outcomes B1-B6) Lab 2 - Equilibrium Equilbrium Unit Test (Outcomes B1-B6) Solubility Assignment (Outcomes C1-C7) Lab 3 - Solubility Exam Assignment Lab Exam Assignment Lab Lab 5 - Hydrolysis ph Titration Worksheet (Outcomes F1 F3) Acid Base Unit Test (Outcomes D, E, and F) Lab 6 Oxidation Reduction Redox Assignment (Outcomes G1-G4) Redox Test (Outcomes G1- G4) Lab Assignment Exam Lab Assignment Exam Solubility Unit Test (Outcomes C1-C7) Exam Final Exam (All Outcomes) Exam STUDENT RESPONSIBILITIES This is NOT an at your own pace course. It is a flexibly paced course. The flexibility comes in the time of day and the location you work on the course. Reporting periods occur in November, February, April, and June. You have ten months to complete the course. The first topic should be completed within Page 1 of 16

2 the first month. Assignment and test marks will be returned on an on-going bases as completed. Chemistry 12 Online: Kinetics Resource Page 1. Primary Notes: Chem 12 Unit 1 Notes.pdf 2. Worksheet to be handed in: Chem 12 Online Kinetics Assignment 3. Addition Worksheets: Sample Questions in Kinetics.pdf (with Answers) Kinetics Review Questions.pdf 4. Animations: Collision Flash Animation.swf Activation Energy Flash Animation.swf 5. Video (YouTube links): Title Description Link Reactions Rates (20mins) Overview of Reaction Rates, oldie but a goody. 6. Additional Helpful Websites: Description Link Saskatchewan Prov. Government Science Teacher Personal Page University of Waterloo University of North Carolina Chem Guide Virtual Textbook by SFU Notes from US re: kinetics Virtual Lab from US College Virtual Lab from University of Colorado 7. Labs: Description 1 Rates of Reaction ist=uui05b1kirf0jvuitgsqkwig&v=qvlwhovmed Final Assessment: Kinetics Unit Test Page 2 of 16

3 At the end of this unit students should be able to: Text Reference / Don t Reaction Kinetics A1 demonstrate awareness that reactions occur at differing rates Unit 1 1. give examples of reactions proceeding at different rates Section1 2. describe rate in terms of some quantity (produced or consumed) per time A2 experimentally determine rate of a reaction 1. identify properties that could be monitored in order to determine a reaction rate 2. recognize some of the factors that control reaction rates 3. compare and contrast factors affecting the rates of both homogeneous and Unit 1 heterogeneous reactions Sections discuss situations in which the rate of reaction must be controlled 5. calculate the rate of a reaction using experimental data A3 demonstrate knowledge of collision theory 1. identify the following principles as aspects of collision theory * 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 Unit 1 Section 5 collision * energy changes are involved in reactions as bonds are broken and formed * a KE distribution curve can explain how changing temperature or adding a catalyst changes the rate A4 describe the energies associated with reactants becoming products 1. describe the activated complex in terms of its potential energy (PE), stability, and structure 2. define activation energy 3. correctly describe the relationship between activation energy and rate of reaction 4. describe the Δ in KE and PE as reactant molecules approach each other 5. draw and label PE diagrams for both exothermic and endothermic reactions, Unit 1 including ΔH, activation energy, and the energy of the activated complex Sections relate the sign of ΔH to whether the reaction is exothermic or endothermic 7. write a chemical equation that describe energy effects in two ways: * a chemical equation that includes the energy term, (thermochemcial equation) * a chemical equation using ΔH notation A5 apply collision theory to explain how reaction rates can be changed 1. describe the role of the following factors in reaction rate: * nature of reactants Unit 1 * concentration Section 3 * temperature * surface area Page 3 of 16

4 Text Reference Assessment A6 analyse the reaction mechanism for a reacting system 1. explain why most reactions involve more than one step 2. describe a reaction mechanism as the series of steps (collisions) that result in the overall reaction and describe the role of the rate-determining step 3. explain the significance and role of a catalyst Unit 1 Section 9 4. identify reactant, product, reaction intermediate, and catalyst from a given reaction mechanism A7 represent graphically the energy changes associated with catalyzed and uncatalyzed reactions 1. compare and contrast the PE diagrams for a catalyzed and un-catalyzed reaction in terms of: * reactants * products * activated complex * reaction intermediates * reaction mechanism *ΔH * activation energy Unit 1 Section 10 A8 describe the uses of specific catalysts in a variety of situations 1. identify platinum in automobile catalytic converters as a catalyst 2. describe the effect of a catalyst on a number of reactions, such as * decomposition of hydrogen peroxide (catalysts: manganese (IV) oxide, raw liver, raw potato) * the reaction of the oxalate ion with acidified potassium permanganate solution (catalyst: Mn 2+ ) * the decomposition of bleach (catalyst: cobalt (II) chloride) Unit 1 Sections Page 4 of 16

5 Chemistry 12 Online: Equilibrium / Solubility Checklist 1. Primary Notes: Chem 12 Notes Unit 2 (Part 1 and Part 2).pdf 2. Worksheets to be handed in: Chem 12 Online Equilibrium Assignment Chem 12 Online Solubility Assignment 3. Addition Worksheets: Sample Provincial Questions in Equilibrium.pdf Equilibrium Review Questions.pdf Sample Provincial Questions in Solubility.pdf Solubility Review Questions.pdf 4. Animations: Le Chatelier.mov Le Chatelier s Flash Animation.swf Temp dep Equil.mov NO 2 N 2 O 4 Eq.mov 5. Video (YouTube links): Title Description Link Equilibrium (19 minutes) Overview of Equilibrium, oldie but a goody. 6. Additional Helpful Websites: Description Link Saskatchewan Prov. Government Virtual Lab from US College Virtual Textbook by SFU Classic Dichromate Equilibria Chem Wiki from UC Davis University of North Carolina Chem Guide 7. Labs: Description 2 Equilibrium 3 Solubility ist=uui05b1kirf0jvuitgsqkwig&v=k6kqmlxf_he Final Assessment: Equilibrium / Solubility Unit Test Page 5 of 16

6 At the end of this unit students should be able to: Page 6 of 16 Text Reference Dynamic Equilibrium B1 explain the concept of chemical equilibrium with reference to reacting systems 1. describe the reversible nature of most chemical reactions and how it can be represented on a PE diagram 2. describe the dynamic nature of chemical equilibrium 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. describe chemical equilibrium as a closed system at constant temperature: Unit II * whose macroscopic properties are constant Sections 1 2 * where the forward and reverse reaction rates are equal * that can be achieved from either direction * where the concentrations of reactants and products are constant 5. infer that a system not at equilibrium will tend to move toward a position of equilibrium B2 predict, with reference to entropy and enthalpy whether reacting system will reach equilibrium 1. explain the significance of enthalpy and entropy 2. determine entropy and enthalpy changes from a chemical equation (qualitatively) 3. predict the result when enthalpy and entropy factors: Unit II * both favour the products Section 3 * both favour the reactants * oppose one another B3 apply Le Chatelier's principle to the shifting of equilibrium 1. describe the term shift as it applies to equilibria 2. describe shifts resulting from the following * temperature change * concentration change * volume change of gaseous systems Unit II Section 4 3. explain equilibrium shifts using the concepts of reaction kinetics 4. identify the effect of a catalyst on dynamic equilibrium B4 apply the concept of equilibrium to a commercial or industrial process Unit II 1. describe the Haber process for the production of ammonia (NH 3 ) Section5 B5 draw conclusions from the equilibrium constant expression 1. gather and interpret data on the concentration of reactants and products of a system at equilibrium 2. write the expression for the equilibrium constant when given the equation for either a homogeneous or heterogeneous equilibrium system 3. explain why certain terms (i.e., pure solids and liquids) are not included in the Unit II equilibrium constant expression Sections relate the equilibrium position to the value of K eq and vice versa 5. 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 / Don t

7 B6 perform calculations to evaluate the changes in the value of K eq and in concentrations of substances within an equilibrium system 1. perform calculations involving the value of K eq and the equilibrium concentration of all species 2. perform calculations involving the value of K eq, the initial concentrations of all species and one equilibrium concentration 3. perform calculations involving the equilibrium concentrations of all species, the value of K eq and the initial concentrations 4. 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 Unit II Section 8 Solubility Equilibria C1 determine the solubility of a compound in aqueous solution 1. classify solutions as ionic or molecular given its conductivity or the formula of the solute 2. describe the conditions necessary to form a saturated solution Unit III Section 1 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 C2 describe a saturated solution as an equilibrium system 1. describe the equilibrium that exists in a saturated aqueous solution Unit III 2. describe a saturated solution using a net ionic equation Section 1 C3 determine the concentration of ions in a solution 1. write dissociation equations 2. calculate the concentration of the positive and negative ions given the concentration of a solute in an aqueous solution Unit III Sections 2 & 4 C4 determine the relative solubility of a substance, given solubility tables 1. describe a compound as having high or low solubility relative to 0.1 M by using a solubility chart Unit III 2. use a solubility chart to predict if a precipitate will form when two solutions are mixed, Section 3 and identify the precipitate Page 7 of 16

8 Text Reference C5 apply solubility rules to analyse the composition of solutions 1. use a solubility chart to predict if ions can be separated from solution through precipitation, and outline an experimental procedure that includes * compound added * precipitate formed * method of separation 2. predict qualitative changes in the solubility equilibrium upon the addition of a common ion or the removal of an ion 3. identify an unknown ion through experimentation involving a qualitative analysis scheme 4. devise a procedure by which the contaminating ions in hard or polluted water can be removed Unit III Section 5 C6 formulate equilibrium constant expressions for various saturated solutions 1. describe the K sp expression as a specialized K eq expression Unit III 2. write a K sp expression for a solubility equilibrium Section 6 / Don t C7 perform calculations involving solubility equilibrium concepts 1. calculate the K sp for a compound when given its solubility (e.g., AgCl, Ag 2 S, PbCl 2 ) Unit III 2. calculate the solubility from its K sp Section 6 3. predict the formation of a precipitate by comparing the trial ion product to the K sp value using specific data Unit III 4. calculate the maximum allowable concentration of one ion given the K sp and the Section 7 concentration of the other ion just before precipitation occurs C8 devise a method for determing the concentration of a specific ion 1. determine the concentration of chloride ion (by titration or gravimetric methods) using a Unit III precipitation reaction with silver ion Section 8 Page 8 of 16

9 Chemistry 12 Online: Acid - Base Checklist 1. Primary Notes: Chem 12 Notes Unit 3 (Part 1 and Part 2).pdf 2. Worksheets to be handed in: Chem 12 Online Acid-Base Assignment 3. Addition Worksheets: Sample Provincial Questions in Acid-Base.pdf ph graphs.pdf Additional Indicator Questions.pdf AB Sample Final 1.pdf AB Sample Final 2.pdf 4. Animations: Acids Ionization.swf Strong Acid Strong Base Titration.swf Weak Acid Strong Base Titration.swf Weak Base Strong Acid Titration.swf Buffer.swf 5. Video (YouTube links): Title Description Link Acid, Bases and Salt (18 minutes) Indicators (18 minutes) Acid Rain (26 minutes) Titration (4 minutes) Overview of Acid, Bases and Salts. Preparation of Indicators Causes and Effects of Acid Rain Titration Techniques 6. Additional Helpful Websites: Description Link Saskatchewan Prov. Government Chem Tutor University of Guelph Animations UC Davis Chem Wiki Chem Guide Titrations UBC ph Tutorial 7. Labs: Description 4 Acid Base Strength 5 Hydrolysis ist=uui05b1kirf0jvuitgsqkwig&v=z7vs4qg9pqa ist=uui05b1kirf0jvuitgsqkwig&v=dukzrowcq2y ist=uui05b1kirf0jvuitgsqkwig&v=yhbqk4paz0y ist=uui05b1kirf0jvuitgsqkwig&v=9--1spj6tuk Final Assessment: Acid-Base Unit Test Page 9 of 16

10 At the end of this unit students should be able to: Nature of Acids and Bases D1 identify acids and bases through experimentation 1. list general properties of acids and bases 2. write names and formulae of some common household acids and bases 3. write balanced equations representing the neutralization of acids by bases in solution 4. outline some of the uses and commercial names of common household acids and bases Text Reference Sections 1 2 / Don t D2 identify various models for representing acids and bases 1. define Arrhenius acids and bases 2. define Brønsted-Lowry acids and bases Sections 1 & 4 D3 analyse balanced equations representing the reaction of acids and bases with water 1. identify Brønsted-Lowry acids and bases in an equation 2. define conjugate acid-base pair 3. identify the conjugate of a given acid or base 4. show that in any Brønsted-Lowry acid-base equation there are two conjugate pairs present 5. identify an H 3 O + ion as a protonated H 2 O molecule that can be represented in shortened form as H + (aq) D4 classify an acid or base in solution as either weak or strong, with reference to its electrical conductivity 1. relate electrical conductivity in a solution to the total concentration of ions in the solution 2. define and give several examples for the following terms: *strong acid *strong base *weak acid *weak base 3. write equations to show what happens when strong and weak acids and bases are dissolved in water Sections 3 & 5 Section 6 D5 analyse the equilibria that exist in weak acid or weak base system 1. compare the relative strengths of acids or bases by using a table of relative acid strengths 2. predict whether products or reactants are favoured in an acid-base equilibrium by comparing the strength of the two acids (or two bases) 3. compare the relative concentrations of H 3 O + (or OH ) between two acids (or between two bases) using their relative positions on an acid strength table Section 6 Page 10 of 16

11 D6 identify chemical species that are amphiprotic Text Reference 1. define amphiprotic 2. describe situations in which H 2 O would act as an acid or base Section 4 / Don t E1 analyse the equilibrium that exists in water 1. write equations representing the ionization of water using either H 3 O + and OH or H + and OH 2. 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) 3. state the relative concentrations of H 3 O + and OH in acid, base, and neutral solutions 4. write the equilibrium expression for the ion product constant of water, K w 5. state the value of K w at 25 C 6. describe the variation of the value of K w with temperature Section 7 7. calculate the concentration of H 3 O + (or OH ) given the other, using K w E2 perform calculations relating ph, poh, [H 3 O + ] and [OH ] 1. define ph and poh 2. define pk w, give its value at 25 C, and its relation to ph and poh 3. calculate H 3 O + or OH from ph and poh 4. describe the ph scale with reference to everyday solutions Section 11 E3 explain the significance of K a and K b equilibrium expressions 1. write K a and K b equilibrium expressions for weak acids or weak bases 2. relate the magnitude of K a or K b to the strength of the acid or base Sections 8 10 E4 perform calculations involving K a and K b 1. given the K a, K b, and initial concentration, calculate any of the following: * H 3 O + * OH * ph * poh 2. calculate the value of K b for a base given the value of K a for its conjugate acid (or vice versa) 3. calculate the value of K a or K b given the ph and initial concentration 4. calculate the initial concentration of an acid or base, given the appropriate K a, K b, ph or poh values Sections Page 11 of 16

12 F1 demonstrate an ability to design, perform, and analyse a titration experiment involving the following: primary standards standardized solutions titration curves appropriate indicators 1. 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 2. demonstrate proper titration technique when performing a titration experiment 3. explain the difference between the equivalence point (stoichiometric point) of a strong acid-strong base titration with the equivalence point of a titration involving a weak acidstrong base or strong acid-weak base 4. interpret titration curves plotted from experimental data 5. select indicators whose transition point coincides with the equivalence point of the titration reaction 6. calculate the concentration of an acid or base using titration data or similar data 7. calculate the volume of an acid or base of known molarity needed to neutralize a known volume of a known molarity base or acid 8. calculate the ph of a solution formed when a strong acid is mixed with a strong base Text Reference Section 16 Section 18 / Don t F2 describe an indicator as an equilibrium system 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 Section 17 F3 perform and interpret calculations involving the ph in a solution and K a for an indicator 1. predict the approximate ph at the transition point using the K a value of an indicator 2. predict the approximate K a value for an indicator given the approximate ph range of the colour change 3. match an indicator s colour in a solution with an approximate ph, using a table of indicators Section 17 F4 describe the hydrolysis of ions in solutions 1. write a dissociation equation for a salt in water 2. write net ionic equations representing the hydrolysis of ions in solution Section 13 F5 analyse the extent of hydrolysis in salt solutions 1. predict whether a salt solution would be acidic, basic, or neutral (compare K a and K b values, where necessary) 2. determine whether an amphiprotic ion will act as a base or an acid in solution (compare K a and K b values, where necessary) 3. calculate the ph of a salt solution from relevant data, assuming that the predominant hydrolysis reaction is the only reaction determining the ph Sections 13 Page 12 of 16

13 F6 describe buffers as equilibrium systems 1. describe the tendency of buffer solutions to resist changes in ph (i.e., able to buffer the addition of small amounts of strong acid or the addition of small amounts of strong base) 2. describe the composition of an acidic buffer and a basic buffer 3. describe qualitatively how the buffer equilibrium shifts as small quantities of acid or base are added to the buffer; the stress being the change in the concentration of the stronger acid (H 3 O + ) or base (OH 1- ) 4. describe in detail a common buffer system (e.g., the blood buffer system) Text Reference Sections / Don t F7 describe the preparation of buffer systems 1. outline a procedure to prepare a buffer solution 2. identify the limitations in buffering action Section 19 F8 predict what will happen when oxides dissolve in rain water 1. write equations representing the formation of acidic solutions or basic solutions from non-metal and metal oxides 2. describe the ph conditions required for rain to be called acid rain (ph 5.0 and lower) 3. relate the ph of normal rain water to the presence of dissolved CO 2 (approximate ph 5.6) 4. describe sources of NO x (automobile engines) and SO x (fuels containing sulfur and smelters of sulfide ores) 5. discuss general environmental problems associated with acid rain Section 21 Page 13 of 16

14 Chemistry 12 Online: Oxidation - Reduction Checklist 1. Primary Notes: Chem 12 Notes Unit 4 (Part 1 and Part 2).pdf 2. Worksheets to be handed in: Chem 12 Online Redox Assignment 3. Addition Worksheets: Practical Applications of Electrochemistry.pdf Sample Provincial Questions in REDOX.pdf Balancing Self Test.pdf Chemistry 12 REDOX Titrations.pdf 4. Animations: Zn H Cell.mov Zn Cu Cell.mov Voltaic Cell.mov Electrolytic Cells.mov 5. Video (YouTube links): Title Description Link Oxidation Reduction (15 minutes) Part 1 Building Blocks Part 2 Electrochemical Cells Part 3 Designing Cells Part 4 Corrosion Part 5 Electroplating Overview of Oxidation Reduction, oldie but a goody. Specific about Electrochemical cells Starts with a review. 5 ten minutes videos on Electrochemistry 6. Additional Helpful Websites: Description Link Saskatchewan Prov. Government Chem Tutor University of Waterloo University of Guelph University of Wisconsin University of North Carolina Chem Guide 7. Labs: Description 6 Oxidation Reduction ist=uui05b1kirf0jvuitgsqkwig&v=a93q9rsagoo ist=uui05b1kirf0jvuitgsqkwig&v=tcjxzfod4sm =ZvGAMR2wbaM =ZvGAMR2wbaM =1q50ojQwVhg ist=uui05b1kirf0jvuitgsqkwig&v=tto1k1l1s Final Assessment: Oxidation - Reduction Quiz (Only G1-G4) Page 14 of 16

15 At the end of this unit students should be able to: Text Reference / Don t G1 describe oxidation and reduction processes 1. define and apply the following: * oxidation * reduction * oxidizing agent * reducing agent * half-reaction * redox reaction Section 1 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 * whether an atom has been oxidized or reduced by its change in oxidation Section 2 number 3. relate change in oxidation number to gain or loss of electrons G2 analyse the relative strengths of reducing and oxidizing agents 1. from data for a series of simple redox reactions, create a simple table of reduction half-reactions 2. identify the relative strengths of oxidizing and reducing agents from their positions on a half-reaction table 3. use the Standard Reduction Potentials of Half-Cells table to predict whether a spontaneous redox reaction will occur between any two species Section 3 G3 balance equations for redox reactions 1. balance a half-reaction for * a half-reaction in solutions that are acidic, basic, or neutral * a net ionic redox reaction in acidic or basic solution 2. write the equations for reduction and oxidation half-reactions given a redox reaction Sections identify reactants and products for several redox reactions performed in a laboratory and balance the equations G4 determine the concentration of a species by performing a redox titration 1. demonstrate familiarity with at least two common reagents used in redox titrations (e.g., permanganate, dichromate, hydrogen peroxide) 2. select a suitable reagent to be used in a redox titration in order to determine the concentration of a species 3. calculate the concentration of a species in a redox titration from data (e.g., grams, moles, molarity) Section 7 Page 15 of 16

16 Text Reference / Don t H1 analyse an electrochemical cell in terms of its components and their functions 1. construct an electrochemical cell 2. define and label the parts of an electrochemical cell 3. determine the half-reactions that take place at each electrode of an electrochemical cell, and use these to make predictions about the overall reaction and about * the direction of movement of each type of ion in the cell * the direction of flow of electrons in an external circuit * what will happen to the mass of each electrode as the cell operates 4. predict the voltage of the cell when equilibrium is reached Sections determine voltages of half-reactions by analysing the voltages of several cells, with reference to the standard hydrogen half-cell 6. identify the standard conditions for E values 7. predict the voltage (E ) of an electrochemical cell using the table of standard reduction half-cells 8. predict the spontaneity of the forward or reverse reaction from the E of a redox reaction H2 describe how electrochemical concepts can be used in various practical applications 1. give examples of applications of electrochemical cells, including lead-acid storage batteries, alkali cells, and hydrogen-oxygen fuel cells, and explain how each functions Section 1 H3 analyse the process of metal corrosion in electrochemical terms 1. describe the conditions necessary for corrosion to occur 2. suggest several methods of preventing or inhibiting corrosion of a metal, including cathodic protection, and account for the efficacy of each method Section 12 H4 analyse an electrolytic cell in terms of its components and their functions 1. define electrolysis and electrolytic cell 2. design and label the parts of an electrolytic cell used for the electrolysis of a molten binary salt such as NaCl liquid 3. design and label the parts of an electrolytic cell capable of electrolyzing an aqueous salt (use of over-potential effect not required) 4. predict the direction of flow of all ions in the cell and electrons in the external circuit 5. write the half-reaction occurring at each electrode and predict observations based upon this information 6. write the overall cell reaction and predict the minimum voltage required for it to operate under standard conditions Section 13 H5 describe how electrolytic concepts can be used in various practical applications 1. explain the principals involved in simple electroplating 2. design and label an electrolytic cell capable of electroplating an object 3. demonstrate familiarity with electrolytic cells in metal refining processes, including Section 13 refining of zinc and aluminum Page 16 of 16