2. Redox Reactions Or How Batteries Work

3. REDOX Reactions The simultaneous transfer of electrons between chemical species. – Actually 2 different reactions occurring at the same time. Oxidation:a loss of electrons Reduction:a gain of electrons

4. ReDox Na +Cl  NaCl Na o +Cl o  Na + Cl - Which element was Oxidized? Na Which element was Reduced? Cl

5. How do we remember ReDox? mnemonics

6. 5 LEO growls GER Losing Electrons Oxidation Gaining Electrons Reduction

7. Turn to Page 5

8. 7 OIL RIG Oxidation IsIs Losing Reduction IsIs Gaining

9. How do we know if there is a RedOx Reaction occurring? We first must find the Oxidation states.

10. What is the oxidation state of each of the following species? Cl in Cl 2 0 Mg in MgO +2 Na in NaBr +1 F in SrF 2 Sr in SrF 2 +2 O in O 2 0

11. J Deutsch 200310 Regents Question Which particles are gained and lost during a redox reaction? (1)Electrons (2) Protons (3) Neutrons (4) Positrons

12. J Deutsch 200311 Regents Question As a Ca atom undergoes oxidation to Ca 2+, the number of neutrons in its nucleus (1)Decreases (2) Increases (3) Remains the same

13. Turn to Page 6

14. Rules for Determining Oxidation Numbers 1.Free Elements have an oxidation number of zero. Ex: Na, S 8, H 2 2.All Metals in group 1 have a +1 Oxidation # in compounds. Ex: Na, K, Li 3.All Metals in group 2 have a +2 Oxidation # in compounds. Ex: Mg, Ca, Ba 4.Oxygen has a –2 Oxidation Number 1.Unless it is in a Peroxide like H 2 O 2

15. Continued Rules 5.Hydrogen has a +1 oxidation #. 6.Halogens have a -1 oxidation #. 7.For any neutral compound, the sum of the oxidation numbers of the atoms in the compound must equal zero. For ex: H 2 SO 4 8.For a polyatomic ion, the sum of the oxidation #’s must equal the ionic charge of the ion. Ex: SO 4 2-

16. CuF 2 PBr 3 HNO 3 C 2 O 4 -2 SO 4 -2 CO 3 -2 C 12 H 22 O 11 H2OH2O

17. Turn to Page 7

18. Now we will take a deeper look into Oxidation. Can be defined as: – The loss of electrons – The gain of oxygen – The loss of hydrogen

19. OXIDATION The loss of electrons Na (s)  Na + + e - The sodium ion has been oxidized to the sodium cation. Na + Cl Sodium loses electron to chlorine - ClNa + +

20. OXIDATION Gain of oxygen – Combustion reactions are classic examples C (s) + O 2(g)  CO 2(g) (burning of coal) 2Fe (s) + 3O 2(g)  2Fe 2 O 3(s) (rusting of iron)

21. OXIDATION Loss of hydrogen – Oxidation can sometimes be best seen as the loss of hydrogen CH 3 OH (l)  CH 2 O (l) + H 2(g) Methyl alcohol has been oxidized into formaldehyde

22. Which one of the following elements were oxidized? Cl in Cl 2 0 → NO Mg in MgO +2 → YES Na in NaBr +1 → YES F in SrF 2 -1 → NO Sr in SrF 2 +2 → YES O in O 2 0 → NO

23. Turn to Page 8

24. Now we will take a deeper look into Reduction. 3 Definitions – The gain of electrons – The loss of oxygen – The gain of hydrogen

25. Gain of electrons – The process of silver electroplating Ag + + e -  Ag Silver cation has gained an electron and has been reduced to silver metal. REDUCTION

26. Loss of oxygen – Reduction can also be seen as the loss of oxygen in going from reactant to product. Fe 2 O 2 (s) + 3 CO (g)  2 Fe (s) + 3 CO 2(g) Iron ore is reduced to iron metal in a blast furnace with carbon monoxide

27. REDUCTION Gain of hydrogen A reduction can also be described as the gain of hydrogen atoms going from reactant to product. CO (g) + 2 H 2(g)  CH 3 OH (l) Carbon monoxide has been reduced to methyl alcohol

28. One’s loss is another’s gain Neither oxidation or reduction can take place without the other. – When those electrons are lost something else has to gain them. When trying to remember which is which think of LEO the lion goes GEROIL RIG Lose Electrons OxidationOxidation is Losing Gain Electrons ReductionReduction is Gaining

29. Turn to Page 9

30. Use a chart to determine Oxidation States. Elements Oxidation State Number of Atoms Total Charge

31. First we will do K 2 PtCl 6 ElementsKPtClSum of Oxidation States Oxidation State Number of Atoms Total Charge

32. Now do the following: What is the oxidation state of S in MgSO 4 ? What is the oxidation state of N in NaNO 3 ? What is the oxidation state of Cl in KClO 3 ?

33. Now do the following: What is the oxidation state of C in CO 3 - What is the oxidation state of Cl in ClO 2 - What is the oxidation state of Cr in CrO 4 2- What is the oxidation state of Cr in CrO 7 2-

34. Packet Page 10-11

35. Review of Terms oxidation-reduction (redox) reaction: – involves a transfer of electrons from the reducing agent to the oxidizing agent. oxidation: loss of electrons reduction: gain of electrons Reducing Agent get oxidized Oxidizing agent get reduced

36. Packet Page 12-13

37. An oxidation-reduction, (redox), reaction involves the transfer of electrons. The oxidation numbers of the atoms will change…. one goes up (oxidation) and one goes down (reduction) Sodium transfers its electrons to chlorine

38. Reduction is the gain of electrons. Nonmetals gain electrons to form – ions The oxidation number goes down (reduces)

39. A half-reaction can be written to represent reduction. Cl 0 + 1e - Cl -1 In reduction half reactions, electrons are written on the left because electrons are gained

40. Oxidation is the loss of electrons. Metal atoms lose electrons to become + ions The oxidation numbers go up (increases)

41. A half-reaction can be written to represent oxidation. Na 0 Na1 + + 1e - In oxidation half reactions, electrons are written on the right because electrons are lost

42. Half-Reactions Show either the oxidation or reduction portion of a redox reaction and the electrons gained or lost.

43. Steps for Writing Half-Reactions Cu 0 + Ag +1 N +5 O -2 3 Cu +2 (N +5 O -2 3 ) 2 + Ag 0 1.Assign an oxidation number to each element. 2.Write a partial half-reaction to show the change in oxidation state: Oxidation: Cu 0 Cu +2 Reduction: Ag +1 Ag 0

44. Steps Continued… 3. Show the number of electrons needed to explain how the oxidation number changed. Oxidation: Cu 0 Cu +2 + 2e- Reduction: Ag +1 +1e- Ag 0 4. Last, but not least, achieve conservation of charge: 2Ag +1 +2e- 2Ag 0

45. Practice Problems 1.Mg + Cl 2 MgCl 2 2.Cu + 2Ag + Cu 2+ + 2Ag 3.Al 0 + Cr 3+ Al 3+ + Cr 0

46. Mg + Cl 2 MgCl 2

47. Cu + 2Ag + Cu 2+ + 2Ag

48. Al 0 + Cr 3+ Al 3+ + Cr 0

49. Regents Question: Given the reaction: Mg (s) + 2H + (aq) + 2Cl – (aq) Mg 2+ (aq) + 2Cl – (aq) + H 2 (g) Which species undergoes oxidation? (1) Mg (s) (2) H + (aq) (3) Cl – (aq) (4) H 2 (g) LEO growls GER LEO

50. Regents Question: Given the equation: C(s) + H 2 O(g) CO(g) + H 2 (g) Which species undergoes reduction? (1) C(s) (2) H + (3) C 2+ (4) H 2 (g) LEO growls GER GER

51. Regents Question: In any redox reaction, the substance that undergoes reduction will (1) lose electrons and have a decrease in oxidation number (2) lose electrons and have an increase in oxidation number (3) gain electrons and have a decrease in oxidation number (4) gain electrons and have an increase in oxidation number

52. Regents Question: Given the equation: 2 Al + 3 Cu 2+ 2 Al 3+ + 3Cu The reduction half-reaction is (1) Al Al 3+ + 3e – (2) Cu 2+ + 2e – Cu (3) Al + 3e – Al 3+ (4) Cu 2+ Cu + 2e –

53. Worksheet Page 16-17

54. Table J tells us if a redox reaction can occur between an atom and an ion. A more active metal will replace an ion below it on Table J. A more active nonmetal will replace an ion below it on Table J. Any metal above H is more active than H and will react with an acid to produce H 2 (g) – The higher up the table, the more readily the replacement will take place.

55. Regents Question: According to Reference Table J, which of these metals will react most readily with 1.0 M HCl to produce H 2 (g) ? (1) Ca (2) K (3) Mg (4) Zn

56. A more active metal will replace a less active metal from its compound. Zn + CuSO 4 Cu + ZnSO 4 Zinc replaces copper because zinc is more active than copper. Cu + ZnSO 4 No Reaction Copper cannot replace zinc Oxidation is on top Reduction is on bottom

57. Review of Terms oxidation-reduction (redox) reaction: – involves a transfer of electrons from the reducing agent to the oxidizing agent. oxidation: loss of electrons reduction: gain of electrons

58. Half-Reactions The overall reaction is split into two half-reactions, one involving oxidation and one reduction. 8H + + Mn +7 O 4  + 5Fe 2+  Mn 2+ + 5Fe 3+ + 4H 2 O Reduction: Mn +7 + 5e   Mn 2+ Oxidation: 5Fe 2+  5Fe 3+ + 5e 

59. AGENTS To recap – Oxidizing agent = the species that’s being reduced – Reducing agent = the species that’s being oxidized

60. Page 18