Intersection 15: The End

1. Intersection 15: The End 12/12/06

2. The Final Exam Questions • Electron configurations, atomic structure, periodic trends, atomic orbitals. • Quantitative calculations. • Lewis & VSEPR Structures and polarity. • Thermochemistry • Thermochemistry • Thermochemistry • Acid/Base chemistry • Acid/Base chemistry • Oxidation number • Redox reactions • Redox reactions • Electrochemistry

3. Research at the University of MichiganA unique opportunity in your life For Help Finding Research Labs • Women in Science and Engineering (WISE) • http://www.wise.umich.edu/ • Undergraduate Research Opportunities Program • http://www.lsa.umich.edu/urop/ • Your future class professors • Dr. Gottfried and Dr. Banaszak Holl • Send specific request with information about yourself and interests (CV). Use contacts. Blanket emails not great approach.

4. Outline • Vitamin C note • Electrochemistry • Nernst • Ampere • Electrolytic cells • Environmental • Hybrid cars

5. Vitamin C • Which fruit keeps best over a long period of time? • Fruits known to sailors • Orange, lemon ~1400 • Limes 1638 • Shaddock (grapefruit) 1700 • Used lemon or lime juice preserved in brandy

6. M Nernst Picture from: www.corrosion-doctors.org/ Biographies/images/

7. M Is potential always the same? Standard conditions: 1 atm, 25oC, 1 M What will influence the potential of a cell?

8. M Mathematical Relationships: Nernst The Nernst Equation: Eo = standard potential of the cell R = Universal gas constant = 8.3145 J/mol*K T = temperature in Kelvin n = number of electrons transferred F = Faraday’s constant = 96,483.4 C/mol Q = reaction quotient (concentration of anode divided by the concentration of the cathode) E = Eo - RT ln Q nF Cu+2 + Zn(s) → Zn+2 + Cu(s) Q =

9. M Applying the Nernst Equation Cu+2 + Zn(s) → Zn+2 + Cu(s) This cell is operating at 25oC with 1.00x10-5M Zn2+ and 0.100M Cu2+? Predict if the voltage will be higher or lower than the standard potential E = Eo - RT ln Q nF

10. M Cu+2 + Zn(s) → Zn+2 + Cu(s) E = Eo - RT ln Q nF Zn+2 + 2e- -> Zn -0.76 V Cu+2 + 2e- -> Cu 0.34 V Eo = standard potential of the cell R = Universal gas constant = 8.3145 J/mol*K T = temperature in Kelvin n = number of electrons transferred F = Faraday’s constant = 96,483.4 C/mol Q = reaction quotient (concentration of anode divided by the concentration of the cathode) 25oC + 273 = K n = Q = [Zn+2]/[Cu+2] 1.00x10-5M Zn2+ and 0.100M Cu2

11. M Were your predictions correct?

12. A Ampere Picture from: musee-ampere.univ-lyon1.fr/

13. A The Units of Electrochemistry • Coulomb • 1 coulomb equals 2.998 x 109 electrostatic units (eu) • eu is amount of charge needed to repel an identical charge 1 cm away with unit force • Charge on one electron is -1.602 x 10-19 coulomb Problem: An aluminum ion has a +3 charge. What is this value in coulombs? magnitude of charge is same at that of e-, opposite sign 3 x 1.602 x10-19 = 4.806 x 10-19 coulomb Key Point: electrons or ions charges can be measured in coloumbs

14. A The Units of Electrochemistry • Ampere • Amount of current flowing when 1 coulomb passes a given point in 1 second • Units of Amperes are Coulombs per second • Current (I) x time (C/s x s) gives an amount of charge. Problem: How much current is flowing in a wire in which 5.0 x 1016 electrons are flowing per second? The charge transferred each second = (5.0 x 1016 electrons/sec) x (1.602 x 10-19 coulomb/electron) = 8.0 x 10-3 coulombs/sec = amps

15. A The Units of Electrochemistry • Ampere • Amount of current flowing when 1 coulomb passes a given point in 1 second • Units of Amperes are Coulombs per second • Current (I) x time (C/s x s) gives an amount of charge. • We can express electron or ION flow in amps! Problem: If 1 mol Al+3 ions passes a given point in one hour, what is the current flow? = 80 C/s = 80 A

16. From: Moore, Stanitski, and Jurs Chemistry: The Molecular Science 2nd Edition/

17. A Batteries Primary Cells non-reversible, non-rechargeable electrochemical cell "dry" cell & alkaline cell 1.5 v/cell mercury cell 1.34 v/cell fuel cell 1.23v/cell Secondary Cells reversible, rechargeable electrochemical cell Lead-acid (automobile battery) 2 v/cell NiCad 1.25 v/cell Lithium batteries

18. A “Flash Light” Batteries Primary Cells "Dry" Cell Zn(s) + 2 MnO2(s) + 2 NH4+ Zn+2(aq) + 2 MnO(OH)(s) + 2 NH3 Alkaline Cell Zn(s) + 2 MnO2(s) ZnO(s) + Mn2O3(s)

19. A Leclanche “Dry” Cell

20. A Mercury Battery Primary Cells Zn(s) + HgO(s) ZnO(aq) + Hg(l)

21. A Fuel Cells anode H2(g) + 2 OH-(aq)→ 2 H2O(l) + 2 e- cathode O2(g) + 2 H2O(l) + 4 e-→ 4 OH-(aq) Picture from: http://www.bpa.gov/Energy/N/projects/fuel_cell/education/fuelcellcar/

22. A Lead-Acid (Automobile Battery) Secondary Cell Pb(s) + PbO2(s) + 2 H2SO4 2 PbSO4(s) + 2 H2O 2 v/cell thus 12 volt battery = 6-2 volt cells

23. A Nickel-Cadmium (Ni-Cad) Secondary Cell Cd(s) + 2 Ni(OH)3(s)↔ Cd(OH)2(s) + Ni(OH)2(s)

24. M Lithium Batteries • Lithium batters (developed in 1970; used in watches, pacemakers, etc.) • The 4-volt lithium battery, which has up to 33 percent higher energy density and 60 less weight than a nickel-metal hydride battery of the same size, has made possible the miniaturization of the current generation of electronic devices

25. M Lithium chemistry • What is the ½ reaction involving lithium? • Is this a reduction or oxidation reaction? • Does it take place at the anode or cathode?

26. M The other ½ of the battery: • Co+3 + e- →Co+2 (+1.92 V) • What is the standard potential of the cell? [Li+ + e- → Li (-3.045 V)] • A lithium battery has a potential listed at 4V. Does this differ from the number you calculated? Why?

27. M Alternative Anodes • Which elements would you predict to have oxidation potentials similar to lithium? (no peeking at the table of standard reduction potentials!) Is what way is lithium preferable to these elements?

28. M Alternative Cathodes • Co+3 + e- →Co+2 • Disadvantage: Use of cobalt oxide can lead to thermal runaway. Increased temperature and pressure cause case of battery to break and fumes are released. Lithium is exposed to oxygen and hydrogen in the air. • What are the alternatives and why aren’t they being used in conjunction with lithium to build a battery with higher potential?

29. M Table of Standard Reduction Potentials

30. M Other commercially viable batteries • Besides cobalt, two other reduction reactions used in lithium batteries are shown below. What is the potential of these batteries? • Fe+2 + 2e-→ Fe (-0.41 V) • ½ I2 + e-→ I- (0.54 V)

31. M Other cathode reactions being explored • Al and Mg are also being explored as materials for the cathode. What are the advantages and disadvantages of these materials?

32. A

33. A Corrosion: A Case of Environmental Electrochemistry • Facts about formation of rust • Iron does not rust in dry air: moisture must be present • Iron does not rust in air-free water: O2 must be present • The loss of iron and the deposition of rust often occur at different places on the same object • Iron rusts more under acidic conditions (low pH) • Iron rusts more quickly in contact with ionic solutions • Iron rusts more quickly in contact with a less active metal (such as Cu) and more slowly in contact with a more reactive metal (such as Zn)

34. Balance the Redox Reaction Fe(s) + O2 (g) Fe+2(aq) + H2O(l) in acid

35. A Corrosion: A Case of Environmental Electrochemistry O2(g) + 4 H+(aq) + 4 e-=> 2 H2O(l) Eo = 1.23 V Fe(s) => Fe+2(aq) + 2 e- Eo = 0.44 V 2 Fe(s) + O2(g) + 4 H+(aq)=> 2 H2O(l) + Fe+2(aq) Eo = 1.67 V 2Fe2+(aq) + ½O2(g) + (2+n)H2O(l)  Fe2O3.nH2O(s) + 4H+(aq)

36. A Corrosion: A Case of Environmental Electrochemistry • Sacrificial cathode

38. Evaluations • Please fill out both an evaluation for Dr. Banaszak Holl and Dr. Gottfried and put them in the correct envelopes! • Constructive comments very helpful! Thanks for a great semester!