1. Oxidation-Reduction Reactions An oxidation-reduction (or redox) reaction is a chemical reaction in which electrons are transferred from one reactant to another. Oxidation is the loss of electrons. Reduction is the gain of electrons. Zn(s) + Cu 2+ (aq) → Zn 2+ (aq) + Cu(s) Zn metal loses 2 electrons and is oxidized to Zn 2+ Zn 2+ is called the reducing agent Cu 2+ gains 2 electrons and is reduced to Cu metal Cu is called the oxidizing agent 9.4

2. Oxidation-Reduction Reactions Zn(s) + Cu 2+ (aq) → Zn 2+ (aq) + Cu(s)

3. Oxidation-Reduction Reactions A redox reaction is the sum of an oxidation half-reaction and a reduction half-reaction. Oxidation half-reaction: Zn(s)Zn 2+ (aq) + 2e – Cu 2+ (aq) + 2e – Cu(s) Cu 2+ (aq) + Zn(s)Zn 2+ (aq) + Cu(s) Reduction half-reaction: Overall redox reaction: Zn(s) + Cu 2+ (aq) → Zn 2+ (aq) + Cu(s) Oxidation (lose 2e – ) Reduction (gain 2e – )

4. Oxidation Numbers The oxidation number is the charge an atom would have if electrons were transferred completely. The oxidation number is sometimes called the oxidation state. H 2 (g) + F 2 (g) → 2HF(g) +1–100 Oxidation number: N 2 (g) + 3H 2 (g) → 2NH 3 (g) –3–3+100 Oxidation number:

5. Oxidation Numbers To assign oxidation numbers: 1)The oxidation number of an element, in its elemental form, is zero. 2)The oxidation numbers in any chemical species must sum to the overall charge on the species. must sum to zero for any molecule must sum to the charge on any polyatomic ion the oxidation number of a monoatomic ion is equal to the charge on the ion

6. Oxidation Numbers To assign oxidation numbers: 3)Know the elements that nearly always have the same oxidation number.

7. Alternative: imagine all the electrons in a bond go to the more electronegative atom Oxidation Numbers

8. Assign the oxidation numbers to the elements in the ion ClO 3. Step 1:Start with the oxidation numbers you know: Step 2:The numbers in the boxes (total contribution to charge) must sum to negative one (the chemical species is a –1 anion). Cl O 3 +5 Oxidation number: Total contribution to charge: –2 –6–6 – –

9. Oxidation Numbers Assign the oxidation numbers to the elements in the compound H 2 SO 4. Step 1:Start with the oxidation numbers you know: Step 2:The numbers in the boxes (total contribution to charge) must sum to zero (the chemical species is neutral). H 2 S O 4 +1 +2 Oxidation number: Total contribution to charge: +6 –2 –8

10. Oxidation Numbers Assign the oxidation numbers to the elements in the compound KMnO 4. Step 1:Start with the oxidation numbers you know: Step 2:The numbers in the boxes (total contribution to charge) must sum to zero (KMnO 4 is a neutral compound). K Mn O 4 +1 Oxidation number: Total contribution to charge: +7 –2 –8

11. Oxidation of Metals in Aqueous Solutions In a displacement reaction, an atom or an ion in a compound is replaced by an atom of another element. Zn(s) + CuCl 2 (aq) → ZnCl 2 (aq) + Cu(s) Zinc displaces, or replaces copper in the dissolved salt. Zn is oxidized to Zn 2+. Cu 2+ is reduced to Cu. When a metal is oxidized by an aqueous solution, it becomes an aqueous ion. 0+2–1 +2–1 0 0+2–2+2–2 0

12. Oxidation of Metals in Aqueous Solutions The activity series is a list of metals (and hydrogen) arranged from top to bottom in order of decreasing ease of oxidation. Cu(s) + ZnCl 2 (aq) → no reaction ElementOxidation Half-Reaction ZincZn → Zn 2+ + 2e – IronFe → Fe 2+ + 2e – NickelNi → Ni 2+ + 2e – HydrogenH 2 → 2H + + 2e – CopperCu → Cu 2+ + 2e – SilverAg → Ag + + e – GoldAu → Au 3+ + 3e – Zn(s) + CuCl 2 (aq) → ZnCl 2 (aq) + Cu(s) Metals listed at the top are called active metals. Metals listed at the bottom are called noble metals. An element in the series will be oxidized by the ions of any element that appears below it in the table. Increasing ease of oxidation Activity Series (partial)

13. Oxidation of Metals in Aqueous Solutions Which of the following reactions will occur? ?Co(s) + BaI 2 (aq) ?Sn(s) + CuBr 2 (aq) ?Ag(s) + NaCl(aq) ElementOxidation Half-Reaction BariumBa → Ba 2+ + 2e – SodiumNa → Na + + e – CobaltCo → Co 2+ + 2e – TinSn → Sn 2+ + 2e – CopperCu → Cu 2+ + 2e – SilverAg → Ag + + e – GoldAu → Au 3+ + 3e – Increasing ease of oxidation Activity Series (partial)

14. Oxidation of Metals in Aqueous Solutions

15. Balancing Simple Redox Equations Redox reactions must have both mass balance and charge balance. Before adding half-reactions, the electrons must balance. Cr(s) + Ni 2+ (aq) → Cr 3+ (aq) + Ni(s) Cr(s)Cr 3+ (aq) + 3e – Oxidation half-reaction: Ni(s)Ni 2+ (aq) + 2e – Reduction half-reaction:

16. Other Types of Redox Reactions Combination reactions can involve oxidation and reduction. Hydrogen is oxidized from 0 to +1. Nitrogen is reduced from 0 to –3. N 2 (g) + 3H 2 (g) → 2NH 3 (g) –3–3+100 00–3–3+3

17. Other Types of Redox Reactions Decomposition can also be a redox reaction. Na + is reduced to Na. H – is oxidized to H 2. NaH(s) → 2Na(s) + 3H 2 (g) –100+1 0–1–10

18. Other Types of Redox Reactions Disproportionation reactions occur when one element undergoes both oxidation and reduction. Oxygen in H 2 O 2 (and other peroxides) has an oxidation number of –1. 2H 2 O 2 (aq) → 2H 2 O(l) + O 2 (g) –10+1 +2 –2–20 oxidation reduction –2

19. Other Types of Redox Reactions Combustion is also a redox process. CH 4 (g) + 2O 2 (g) → CO 2 (g) + 2H 2 O(l) +1 0 –4 +2+4 0 –2 +4 –2 –4

20. Study Guide for Section 9.4 DAY 24, Terms to know: Section 9.4 oxidation, reduction, redox, half-reaction, oxidation number or oxidation state, activity series DAY 24, Specific outcomes and skills that may be tested on exam 4: Given a redox reaction, be able to identify which reactant is oxidized and which is reduced, and be able to identify which reactant is the oxidizing agent and which is the reducing reagent Given a simple redox reaction, be able to write two correct half reactions that add together to give the net equation Given a compound, be able to determine the oxidation number for each atom in the formula Given a reaction, be able to determine how the oxidation number changes or remains the same for each atom involved Be able to use the activity series to predict products in redox reactions and whether the reaction will be product or reactant favored

21. Extra Practice Problems for Section 9.4 Complete these problems outside of class until you are confident you have learned the SKILLS in this section outlined on the study guide and we will review some of them next class period. 9.43 9.45 9.47 9.49 9.147 9.157

22. Prep for Day 25 Must Watch videos: https://www.youtube.com/watch?v=AN4KifV12DAhttps://www.youtube.com/watch?v=AN4KifV12DA (aq solutions, crash course chemistry) http://www.youtube.com/watch?v=0cPFx0wFuVshttp://www.youtube.com/watch?v=0cPFx0wFuVs (solvation, Tyler DeWitt) https://www.youtube.com/watch?v=cnSTsLvyuOk https://www.youtube.com/watch?v=cnSTsLvyuOk (dissolving, Tyler DeWitt) https://www.youtube.com/watch?v=wxvERNlUdBQhttps://www.youtube.com/watch?v=wxvERNlUdBQ (equations, Bozeman) https://www.youtube.com/watch?v=IIu16dy3ThIhttps://www.youtube.com/watch?v=IIu16dy3ThI (ppt reactions, crash course chemistry) Other helpful videos: http://www.learnerstv.com/video/Free-video-Lecture-29341-Chemistry.htmhttp://www.learnerstv.com/video/Free-video-Lecture-29341-Chemistry.htm (solutions, Bozeman) http://www.youtube.com/watch?v=gxmpr09Xk4Yhttp://www.youtube.com/watch?v=gxmpr09Xk4Y (solvation, Brightstorm) https://www.youtube.com/watch?v=9h2f1Bjr0p4https://www.youtube.com/watch?v=9h2f1Bjr0p4 (solutions, crash course chem) https://www.youtube.com/watch?v=Q8cxPofGKCMhttps://www.youtube.com/watch?v=Q8cxPofGKCM (solubility, Isaacs) http://ps.uci.edu/content/chem-1p-preparation-general-chemistryhttp://ps.uci.edu/content/chem-1p-preparation-general-chemistry (UC-Irvine, lectures 16-17) Read Sections 13.2, 13.1, 13.4, 9.1-9.2