Chemical Behavior of Metals

1. Chemical Behavior of Metals Chapter 3: Activity 3

2. Solutions • Solid copper chloride is added to water • CuCl2(s) → Cu+2(aq) + 2Cl-1(aq)

3. Which Metals Won’t Corrode? What would happen if solid metal ZINC was placed in a copper chloride solution? Zn (s) + Cu(Cl)2 (aq)?

4. Single Replacement Reaction When solid ZINC was placed in a copper chloride aqueous solution….. Zn (s) + Cu(Cl)2 (aq) ZnCl2 (aq)+ Cu (s)

5. Single Replacement Reaction When 1 reactant replaces another reactant of the same type. -Metals will replace Metals -Nonmetals will replace Nonmetals

6. Online animation

7. Single Replacement Reaction Why do Metals Replace Each Other? Some metals want to lose electrons. Some metals want to gain electrons.

8. Use the Activity Series of Metals to determine if a reaction will occur

9. Is Zn higher than Cu on the list? Use the Activity Series of Metals to determine if a reaction will occur Li K Ba Sr Ca Na Mg Al MnZn Fe Cd Co Ni Sn Pb HCu Ag Hg Au

10. Activity Series of Metals YES Zn is Higher than Cu Decreasing Activity Li K Ba Sr Ca Na Mg Al MnZn Zn + CuCl2 → ZnCl2 + Cu Fe Cd Co Ni Sn Pb HCu Ag Hg Au

11. So what is happening? • Zn is more reactive than Cu • It will lose it’s outer most electrons (valence electrons) easier than Cu will and will become a Zn+2.

12. Cl-1 Cl-1 Cu+2 Cl

13. So what is happening? .

14. Cl-1 Zn+2 Cl-1 Cl-1 Cl-1 Cl

15. Recap • In solution, metals are floating around by themselves as ions • Metals that are higher on the Activity Series are more reactive than metals lower on the list • Metals that are higher are more reactive and want to lose their valence electrons

16. Yesterday’s Activity • Solid aluminum was added to a solution of copper chloride • Al(s) + CuCl2(aq) → Cu(s) + AlCl3(aq) • So, solid aluminum went into solution and copper came out of solution!!!! • WHY???????

17. Some practice • Will this reaction happen? Cu + AgNO3→ ? • Yes, Cu is higher on the list • Cu + AgNO3→ Ag + Cu(NO3)2 • So, after the reaction, silver is now the solid!

18. Some practice • Will this reaction happen? Cu + Pb(NO3)2→ ? • No, Cu is lower on the list • Cu + Pb(NO3)2 → No Reaction • So, copper is still a solid

19. Batteries • A device that converts chemical energy to electrical energy. • Metals that are farther apart on the activity series will produce a more efficient battery

20. Batteries Li KBaSr Ca Na Mg AlMnZn FeCd Co NiSnPb HCu Ag Hg Au 0.51

22. How Batteries Work Video

23. Car Battery

26. Why do metals react? • Metals that are more reactive want to LOSE electrons • This is called OXIDATION Cu + AgNO3→ Ag + Cu(NO3)2 • When the less reactive metal GAIN these lost electrons • This is calledREDUCTION • SO… Cu Lost Electrons =Oxidation Ag Gained Electrons = Reduction 0 +1 0 +2

27. REDOX REACTIONS • LEO the lion goes GER • Losing Electrons is Oxidation • Gaining Electrons is Reduction

29. Oxidation Mg + S MgS Mg lost electrons 0 +2 Mg has been oxidized OXIDATION

30. Reduction Mg + S MgS S gained electrons 0 -2 Sulfur has been reduced REDUCTION

31. Leo the lion goes Ger Mg + S MgS S is REDUCED 0 -2 0 +2 Mg is Oxidized

32. Applications of Metal corrosion reactions What is this???

33. Applications of Metal corrosion reactions MRE

34. The idea behind a flameless heater is to use the oxidation of a metal to generate heat. Magnesium metal works better than iron because it rusts much more quickly. To make a flameless heater, magnesium dust is mixed with salt and a little iron dust in a thin, flexible pad about the size of a playing card. To activate the heater, a soldier adds a little water. Within seconds the flameless heater reaches the boiling point and is bubbling and steaming. To heat the meal, the soldier simply inserts the heater and the MRE pouch back in the box that the pouch came in. Ten minutes later, dinner is served!

35. MRE

36. Daniels Electrochemical Cell Video