1. Single Displacement and Redox

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3. Single Displacement and Redox: At the conclusion of our time together, you should be able to: 1.Identify a basic single displacement reaction 2.Use the reactivity series table to determine if the reaction will take place 3.Show the change in oxidation numbers for a single displacement reaction

4. Decomposition Simple Reactions Synthesis (Combination) Single Replacement Double Replacement

5. Decomposition Synthesis Single Replacement Double Replacement ABAB + AB AB + ABAB + C + C ABAB + C + CDD

6. Decomposition Synthesis Single Replacement Double Replacement ABAB + AB AB + ABAB + C + C ABAB + C + CDD

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8. Single Replacement Reactions Single Replacement Reactions occur when one element replaces another in a compound. Single Replacement Reactions occur when one element replaces another in a compound. A reactive metal can replace a metal (+) OR a reactive halogen can replace a halogen (-). A reactive metal can replace a metal (+) OR a reactive halogen can replace a halogen (-). element + compound  element + compound element + compound  element + compound A + BC  AC + B (if A is a metal) OR A + BC  BA + C (if A is a ) A + BC  BA + C (if A is a halogen ) (remember the cation always goes first!)

9. Single Replacement Reactions Page 43:3 - For these reactions, you must remember: Page 43:3 - For these reactions, you must remember: When H 2 O splits into ions, it splits into H + and OH - (not H+ and O -2 !!) A single replacement reaction will only occur if the replacement ion has a higher activity than the original ion in the compound To determine this, refer to a relative activity table

10. Relative Activities Metals Decreasing ActivityHalogens Lithium, LiFluorine, F Potassium, KChlorine, Cl Calcium, CaBromine, Br Sodium, NaIodine, I Magnesium, Mg Aluminum, Al Zinc, ZnHydrogen, H Chromium, CrCopper, Cu Iron, FeMercury, Hg Nickel, NiSilver, Ag Tin, SnPlatinum, Pt Lead, PbGold, Au

11. Single Replacement Reactions (note: Li is higher relative activity than H): (note: Li is higher relative activity than H):

12. A Displacement Reaction: metallic copper with silver nitrate Cu + Ag NO 3 Ag + Cu(NO 3 ) 2 Note: Cu is higher relative activity

13. Single Replacement Reactions with Halogens Cl 2 + KBr  KCl + Br 2 1 2 2 1 1 2 2 1 Note: Cl replaces the bromine ion in the reaction because of higher relative activity Br 2 + KCl  NR 2

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15. Single Replacement Reactions Write and balance the following single replacement reaction equation: Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zinc metal reacts with aqueous hydrochloric acid Zn (s) + HCl (aq)  Zn (s) + HCl (aq)  ZnCl 2 + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction because of higher relative activity 2

16. Single Replacement Reactions Now s how the change in oxidation numbers for a single displacement reaction : Now s how the change in oxidation numbers for a single displacement reaction : Zn (s) + 2 HCl (aq)  ZnCl 2 + H 2(g) Zn (s) + 2 HCl (aq)  ZnCl 2 + H 2(g) Each Zn loses 2e - oxidation, reducing agent Zn o -2e -  Zn 2- Each H gains 1e - reduction, oxidizing agent 2 H + +2e -  2 H o

17. Single Replacement Redox Aluminum metal reacts with aqueous copper (II) nitrate Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq)  Al (s) + Cu(NO 3 ) 2(aq)  Al(NO 3 ) 3(aq) + Cu 2 Al (s) + 3 Cu(NO 3 ) 2(aq)  2 Al(NO 3 ) 3(aq) + 3 Cu Each Al loses 3e - oxidation, reducing agent Each Cu(II) gains 2e - reduction, oxidizing agent

18. Interesting Signs:

19. Single Displacement and Redox: Let’s see if you can: 1.Identify a basic single displacement reaction 2.Use the reactivity series table to determine if the reaction will take place 3.Show the change in oxidation numbers for a single displacement reaction

20. Try This… Page 47:3 Zinc reacts with aqueous iron (III) chloride Zinc reacts with aqueous iron (III) chloride Zinc is higher reactivity so… Zinc is higher reactivity so… Zn + FeCl 3  Fe + Z n Cl 2 32 2 3 32 2 3 Each Zn loses 2e - oxidation, reducing agent 3 Zn o -6e -  3 Zn 2+ Each Fe(III) gains 3e - reduction, oxidizing agent 2 Fe 3+ +6e -  2 Fe o

21. I don’t feel so stupid now…