Chemistry 40S & Honours Course Outline

Chemistry 40S & Honours Course Outline Textbook: van Kessel et al. (2003). Nelson Chemistry 12. Nelson Thomson Learning: Toronto. Website: http://adeakin.pbworks.com OBJECTIVES FOR STUDENTS: To develop an understanding of the basic principles and concepts of science To develop critical thinking and problem solving abilities To develop the skills and understand the processes of science To develop an understanding of the interconnecting ideas and principles that transcend and unify the natural science disciplines To attain the level of scientific awareness essential for all citizens in a scientifically literate society To make informed decisions about further studies and careers in science To develop a positive attitude towards science To develop an understanding and appreciation of the effect technology has on advancements in science and the resulting effects on society GRADING SCHEME TERM WORK WEIGHT Summative Assessment Tests & Quizzes 40% Labs and Activities 30% Formative Assessment SMART Response Anecdotal Non-Academic Achievement Anecdotal Factors FINAL EXAM 30% TOTAL 100% CURRICULUM OVERVIEW* I. Electrochemistry II. Kinetics III. Introduction to Equilibrium IV. Solubility Equilibrium V. Acids & Bases & Aqueous Equilibrium VI. Atomic Structure & Periodicity *order may vary TERM WORK 70% of the course grade has been assigned to term work. Completion of labs, homework, and assignments is the responsibility of the student. Students are expected to have all of their work completed neatly and on time. Typed work is preferred but not required. Furthermore, students are encouraged to keep all of their returned work as the final exam is cumulative and includes concepts from the entire semester. HOMEWORK Homework is assigned with the purpose of reinforcing concepts and pacing the rate of instruction and must be completed before the beginning of classroom instruction. Students are expected to complete assigned homework. Old chemists never die. They merely reach equilibrium.

Chemistry 40S & Honours Course Outline LATE WORK The contents of tests, quizzes, and exams will include ALL classroom and assigned work, with the exception of projects, and, therefore should be completed even if it does not receive a mark. Marks may be lost for assignments submitted late. Late assignments may not receive a mark if submitted after marked work has been handed back to students. ELECTRONIC COMMUNICATION DEVICES Electronic communication devices impact teaching and learning. Use of multi-functioning communication devices including, but not limited to, cellular phones, PDAs, MP3 players, recorders, and digital cameras is prohibited for the entire 68 minutes of classroom instruction, unless sanctioned by the instructor. ABSENCES Missed work must be completed on your own time. Quizzes or tests will be written the day you return to school, unless other arrangements are made with the teacher BEFORE your absence. When more than one day is missed, testing arrangements must be made with the teacher. ACADEMIC DISHONESTY COPYING AND CHEATING Copying and cheating is not tolerated. Marks will be deducted from all students involved in incidents of copying or cheating. LABORATORY SAFETY Laboratory experiments are an important component in the study of chemistry. Students are expected to follow all safe lab procedures when conducting labs. Unsafe behavior will not be tolerated. Students must wear safety goggles over their eyes for all laboratory activities involving gas, glass or chemicals. Removal of safety goggles while conducting labs is not tolerated. Vision is precious and sight cannot be replaced! TEXTBOOKS Students are responsible for the care of textbooks issued to them. All texts should have inside their front cover, neatly written, the current borrower's name. Students must cover the cost of damage or loss to the book issued to them. Payment for lost or damaged textbooks is due at the end of each term. Old chemists never die. They merely reach equilibrium.

Rules for Assigning Oxidation Numbers 1. Atoms in their free state have an oxidation number of ZERO. (0) H 2( g ), S 8( s) and Ag (s) 2. The oxidation number of ions is the charge of the ion. ( aq ) (0) (0) ( 2) 2 ( aq ) Na and S 3. The sum of the oxidation numbers of individual atoms in a compound or a complex ion is equal to the charge of the compound or ion. ( 6) ( 2) 2 2 7 ( aq) Cr O where 2(+6)+7( 2) = 2 4. Oxygen is assigned an oxidation number of -2, EXCEPT when it is a diatom (O 2(g) ) or in a peroxide ion where it has an oxidation state of -1. (0) ( 2) ( 6) ( 2) 2 O 2( g ), H 2 O, Mn O 4 ( aq) and H 2 O2 5. Hydrogen in compounds or ions carries a +1 oxidation state, EXCEPT when combined with a metal ca+ion. Na H and ( 3) N H 6. Group 1A and 2A atoms in compounds carry oxidation numbers of +1 and +2, respectively. ( 2) ( 2) Li Cl and Ca O 7. Halogens in binary compounds contain a -1 charge. H Cl, Na I and B F3 8. Given compounds that do not follow rules 1-7, use electronegativity values to assign oxidation numbers. ( 3) N F and 3 3 ( 3) Calculate the oxidation numbers of each atom in the following particles. P 4 SnS 2 HSbO 2 U 3 O 8 C 6 H 12 O 6 ClO 4 - Zn 3 (PO 4 ) 2 H 2 O 2 SF 6 I Cl http://mrdeakin.pbworks.com adeakin@pembinatrails.ca (204) 888-5898 Shaftesbury High School, 2240 Grant Ave, Wpg, MB, R3P 0P7

Chemistry 40S & Honours Net Ionic Equations and Half Reactions For each of the following chemical reactions, a. write the balanced net ionic equation; b. label the oxidizing agent and reducing agents; and c. separate the equation into its balanced oxidation and reduction half reactions. 1. Zinc metal reacts with aqueous hydrochloric acid, formula HCl. 2. Solid calcium reacts with nitric acid, formula HNO3. 3. Potassium iodide solution reacts with diatomic chlorine gas. 4. Freshly polished aluminum reacts with an aqueous bromine solution. 5. Iron metal reacts with chromium (II) sulphate to form two products, one of which includes the iron (II) ion.

Chemistry 40S/PGL Making a Redox Table Interactive Simulation Objectives 1. Construct a table of balanced reduction half-reactions ordered from strongest oxidizing agent to weakest oxidizing agent from four combinations of metals and their ionic solutions. 2. Sketch the labelled molecular scale reaction for any metal reducing agent/oxidizing agent combination and write the balanced net ionic equation. Directions 1. Load the Metals in Aqueous Solutions animation from the following URL: http://group.chem.iastate.edu/greenbowe/sections/projectfolder/flashfiles/redox/home.html. The following screen should appear. Figure 1. Metals in Aqueous Solutions Interactive Simulation Home Screen 2. Click on the button. You should see a picture of eight solutions of ions. Use the magnifying glass to see the dissolved ions in solution. Figure 2. Metals in Aqueous Solutions Solutions of Dissolved Ions Shaftesbury High School 2240 Grant Avenue, Winnipeg, MB, Canada, R3P 0P7 204.888.5898 http://mrdeakin.pbworks.com

Chemistry 40S/PGL Making a Redox Table Interactive Simulation 3. Select and follow the instructions to react each metal with the four solutions of ions. Record your observations in Table 1. Table 1. Metals in Aqueous Solutions Data Table 4. In the box below, construct a table of balanced reduction half-reactions ordered from strongest oxidizing agent to weakest oxidizing agent for each solution of ions. RA Mg(s) OA Mg 2+ (aq) Cu 2+ (aq) Zn 2+ (aq) Ag + (aq) SOA Cu(s) Zn(s) Ag(s) SRA 5. Use the button and sketch the labelled molecular scale reaction for any metal/ion combination and write the balanced net ionic equation. Shaftesbury High School 2240 Grant Avenue, Winnipeg, MB, Canada, R3P 0P7 204.888.5898 http://mrdeakin.pbworks.com

CHEMISTRY 40S & HONOURS BUILDING A REDOX TABLE LAB Objective Construct a table of reduction half-reactions that are ordered from strongest oxidizing agent to weakest oxidizing agent starting at the top left. SOA Ni 2+ + 2e - Ni (s) WRA WOA SRA Chemicals Cu wire Pb wire Zn wire Al wire 0.1 M Cu(NO 3 ) 2 solution 0.1 M Pb(NO 3 ) 2 solution 0.1 M Zn(NO 3 ) 2 solution 0.1 M AgNO 3 solution

CHEMISTRY 40S & HONOURS BUILDING A REDOX TABLE LAB Lab Setup Al (s) Cu (s) Pb (s) Zn (s) Ag + (aq) Ag + (aq) Ag + (aq) Ag + (aq) Cu 2+ (aq) Cu 2+ (aq) Cu 2+ (aq) Cu 2+ (aq) Pb 2+ (aq) Pb 2+ (aq) Pb 2+ (aq) Pb 2+ (aq) Zn 2+ (aq) Zn 2+ (aq) Zn 2+ (aq) Zn 2+ (aq)

CHEMISTRY 40S & HONOURS BUILDING A REDOX TABLE LAB RA\OA

CHEMISTRY 40S & HONOURS BUILDING A REDOX TABLE LAB Hand in a redox table writing each half-reaction as a balanced reduction half reaction and ordering each from strongest oxidizing agent to weakest, placing each OA on the left hand side of the reaction arrow.

Chemistry 40S & Honours Predicting Redox Reactions Use the table of standard reduction potentials to a) record the balanced net ionic equation; and b) state whether the reaction is spontaneous or non-spontaneous. 1. A gold ring is accidentally dropped into a solution of nitric acid, formula HNO3 (assume complete dissociation into hydrogen ions and nitrate ions). 2. In a car battery, lead and lead (IV) oxide electrodes are exposed to a sulfuric acid, formula H2SO4, electrolyte. (Assume that the sulfuric acid ionizes to produce hydrogen ions and sulfate ions.) 3. An aqueous solution of potassium permanganate was reacted with an acidic meaning H + ions are present solution of sodium bromide and an orange brown substance was formed. 4. A strip of chromium metal is placed in a solution of nickel (II) chloride. 5. A piece of aluminum foil is placed in a solution of blue copper (II) chloride. 6. Liquid mercury is mixed with a paste of acidic means H + ions are present manganese (IV) oxide. 7. Hydrogen peroxide and an aqueous solution of silver nitrate are mixed. 8. A strip of silver metal is placed into a solution of nickel (II) chloride. 9. A nickel coin is dropped into a solution of cadmium nitrate. 10. Potassium metal is placed into a beaker of water. 11. When copper metal was placed in a concentrated nitric acid, formula HNO3, solution a brown gas evolved and the solution turned green and then blue.

Chemistry 40S & Honours Predicting Redox Reactions 1. Spontaneous/ Non-spontaneous? 2. Spontaneous/ Non-spontaneous? 3. Spontaneous/ Non-spontaneous? 4. Spontaneous/ Non-spontaneous? 5. Spontaneous/ Non-spontaneous? 6. Spontaneous/ Non-spontaneous?

Chemistry 40S & Honours Predicting Redox Reactions 7. Spontaneous/ Non-spontaneous? 8. Spontaneous/ Non-spontaneous? 9. Spontaneous/ Non-spontaneous? 10. Spontaneous/ Non-spontaneous? 11. Spontaneous/ Non-spontaneous?

Chemistry 40S Electrochemistry Problem Set: Redox Reactions Electronegativity Trends 1. Place the following fictitious elements on the periodic table in a unique pattern that demonstrates the general trend in increasing electronegativities so that no two elements are located directly beside each other on the table. (2 marks) Relative Electronegativities Ey<Sa<Ju<Zk Assigning Oxidation Numbers 2. Write oxidation numbers in round brackets above each atom in the following chemical formulas. Show the algebra you used to arrive at your answer below the formula. A sample solution is provided. (4 marks) ( 2) H O BaO 2 Na 4 Si 2 O 4 I 3 2 2 ( 2) 0 Identifying Oxidizing and Reducing Agents 3. Write oxidation numbers above each atom and circle and label the strongest oxidizing agent (SOA) and the strongest reducing agent (SRA). You do NOT have to balance the equation. (2 marks) AuCl 4 (aq) + H 2 (g) Au(s) + Cl (aq) + H + (aq) Writing Balanced Net Ionic Equations 4. Write the balanced net ionic equation when an aluminum strip reacts in a solution of copper (II) sulfate. (3 marks) /11 1 P a g e

Chemistry 40S Electrochemistry Problem Set: Redox Reactions Writing Balanced Equations from Half Reactions 5. Given the following half-reactions, write the balanced net ionic equation. (2 marks) Reduction ½ reaction: ClO 2 + e ClO 2 Oxidation ½ reaction: 2Hg + 2Cl Hg 2 Cl 2 + 2e Making a Redox Table 6. Create a redox table of half reactions from the following experimental results. Write all half reactions as balanced reduction half reactions with the strongest oxidizing agent (SOA) located at the top left hand side of the list. (3 marks) Sv(s) + Mc + (aq) Sv 2+ (aq) + Mc(s) St 2+ (aq) + Mc(s) Mc + (aq) + St(s) Dk 3+ (aq) + Sv(s) No Reaction Reading the Redox Table Use the redox table below to answer the next two questions. Reduction ½ Reaction (Volts ) E red Fe 3+ (aq) + 3e Fe(s) 0.04 IO 4 (aq) + 2H + (aq) + 2e IO 3 (aq) + H 2 O(l) +1.60 La 3+ (aq) + 3e La(s) 2.37 ClO 2 (g) + e ClO 2 (g) +0.95 AgCl(s) + e Ag(s) + Cl (aq) +0.22 7. Write the balanced equation that includes the strongest oxidizing and reducing agents. (2 marks) 8. Could a solution containing iron (III) ions be stored in container containing Lanthanum without contaminating the solution? Explain your reasoning. (2 marks) 2 P a g e /9 /20

Chemistry 40S Problem Set: Redox Reactions 1. Order the following atoms from MOST electronegative to LEAST electronegative. (2) Cs, Cl, B, Na 2. Determine the oxidation number of the atoms in bold. Show all of your work for full marks. (2) a) C 7 H 5 O 2 b) Sr(HCO 3 ) 2 3. a) Identify the atoms that are oxidized and reduced in the following equation by indicating their change in oxidation number. (2) b) Label the OA and RA respectively. (1) Al (s) + CuSO 4 (aq) Al 2 (SO 4 ) 3 (aq) + Cu (s) c) Write the complete and balanced net ionic equation. (2) 4. Given the following data, generate a redox table with all half reactions written as reduction half reactions placing the strongest oxidizing agent highest on the left hand side. (3) M + (aq) + Y(s) Y 2+ (aq) + M(s) M(s) + D 2+ (aq) no reaction D(s) + Y 2+ (aq) Y(s) + D 2+ (aq) D(s) + A + (aq) no reaction

Chemistry 40S Problem Set: Redox Reactions 5. Rumplestiltskin is concocting a very pure solution containing copper (II) ions. He must stir the solution to dissolve the copper compound and has access to 3 spoons composed of nickel, iron, and silver. With which spoon can he safely stir his solution without contaminating it with metal ions? Give a reason for your answer. (2) 6. Predict the most likely redox reaction when silver is placed in an aqueous cadmium nitrate solution by a) writing the balanced oxidation and reduction half reactions. (2) b) writing the balanced net ionic equation. (1) c) identifying if it is spontaneous or not. (1) /18

Electrochemical Cells For the following questions, perform the following: 1. Label the anode and cathode. 2. Show the direction of electron flow. 3. Label the direction of ion movement and the electrolytes as cations and anions. 4. Write the balanced oxidation and reduction half-cell reactions. 5. Calculate the standard cell potential (E cell) from the standard oxidation (E ox) and reduction (E r) values that would appear on the voltmeter. 6. Record the balanced net ionic equation. A. Fe(s) Fe 2+ (aq) Sn 2+ (aq) Sn(s)

Electrochemical Cells B. Co(s) Co 2+ (aq) Zn 2+ (aq) Zn(s) C. Ni(s) Ni 2+ (aq) Ag + (aq) Ag(s)

Electrochemical Cells D. Pt(s) Fe 3+ (aq), Fe 2+ (aq) H + (aq), ClO4 - (aq), Cl - (aq), C(s) E. Al(s) Al 3+ (aq) MnO4 - (aq), H + (aq) C(s)

Electrochemical Cells F. Cr(s) Cr 2+ (aq) Cr2O7 2- (aq), H + (aq) Pt(s)

Galvanic Cells Lab 1. Construct three functional galvanic cells with a positive voltage reading. 2. Sketch the functional cell using a labelled diagram. Include the following terms: (7 marks) 1. Anode & Cathode 2. Movement of ions through salt bridge 3. Direction of electron flow 4. + and - electrodes 5. Salt bridge 6. Anions & Cations (AKA electrolytes) 7. Voltmeter 3. Write balanced oxidation & reduction half-cell reactions, the overall reaction, and represent each cell using cell notation. (3 marks)

Lab Setup Cu (s) Pb (s) Zn (s) Cu(NO 3 ) 2(aq) Pb(NO 3 ) 2(aq) Zn(NO 3 ) 2(aq)

Electrolysis Lab 1. Construct a functional electrolytic cell from distilled water and sodium chloride with phenolphthalein indicator. 2. Write the balanced half-reactions, overall reaction, calculate the minimum positive emf required for the reaction to proceed. (3 marks) 3. Sketch a labelled electrolytic cell including the following labels: Anions & Cations Anode & Cathode, (6 marks) Direction of electron and ion flow including chemical symbol Battery Symbol Positive & Negative terminals Sites of Oxidation & Reduction 4. Write the cell notation that represents the reaction. (1 mark)

Chemistry 40S Electrolysis Problem Set 1. Why is a power supply required for electrolysis? (1 mark) 2. Compare and contrast electrochemical cells and electrolytic cells by completing the following table. (4 marks) Galvanic Cells Electrolytic Cells Spontaneity Standard Cell Potential ( Ceii) Cathode Positive Strongest oxidizing agent present undergoes reduction Negative electrode Anode Strongest agent present undergoes oxidation Direction of Electron Movement Direction of Ion Movement Anode to cathode Anions move to anode Cations move to cathode 3. a. Sketch the electrolysis apparatus for the aqueous electrolysis of calcium bromide and include the following labels. (3 marks) I. Power source II. + and - electrodes III. Anode and cathode IV. Movement of ions V. Site of oxidation VI. Movement of electrons through the solution and reduction through the wires

Chemistry 40S Electrolysis Problem Set b. Write the balanced oxidation and reduction half reactions, and the overall equation. (2 marks) e. What is the minimum voltage required to drive the reaction forward? (1 mark) 4. a. Write the balanced oxidation and reduction half reactions, and the balanced overall equation for the molten electrolysis of aluminum chloride. (2 marks) b. Calculate the masses of solid aluminum and chlorine gas produced on an industrial scale if a current of 300 ka is drawn five full days. (3 marks) 5. A battery delivers 0.300 A of current for 20 minutes. a. How many moles of electons were transferred? (2 marks) b. If the mass of the zinc casing was originally 2 grams, what mass of the casing remains? (2 marks)