1. 2.B Earth’s Mineral Resources

2. Earth’s Composition Atmosphere: (gases) Nitrogen, Oxygen, Neon, Argon Hydrosphere: (water) Comes from water and dissolved minerals Lithosphere: (Geosphere – earth) Solid part of the Earth

3. Ores and Minerals Ores: Naturally occurring rock or mineral Can be mined (profitable) Minerals: Solid compounds made of element(s)

4. Mining Deepest mines don’t even scratch the surface its crust All raw materials are mined from the crust Random distribution of minerals

5. Homework Read pgs. 134-138 Do page 151 #1-8

6. Do Now Fill in the BLANKS 1. 2. 3.

7. Objectives 1. SWBAT analyze the world’s use and production of metals. 2. SWBAT differentiate between reactive and non reactive metals. 3. SWBAT answer questions on reactivity.

8. 2.B Earth’s Mineral Resources Use Table 2.3 (pg. 136) to answer these: 1. What metal might Australia wish to obtain from the US? 2. What metal could Australia trade to the US to obtain the metal in the previous question? 3. From which nation would you expect the US to obtain nickel? Why? 4. Give examples of two trade agreements by which China could obtain iron ore in exchange for a metal it has in abundance. 5. What metals might Canada seek to obtain through trade?

9. Challenges faced in mining:

10. 1. Use of supplies 2. Where should mining occur 3. The quantity of useful ore found at the site 4. The percent of metal in the ore 5. The type of mining and processing needed to extract the metal from its ore 6. The distance between the mine and metal-refining facilities and markets 7. The metal’s supply vs. demand status 8. The environmental impact of the mining and metal processing. 9. Can you think of any others?

11. Mining Copper Ores

12. B.2 Production vs. Use Follow the guidelines on page 138-139 to research the metal you selected for your coin. If you chose to create an alloy make sure to research all the metals involved.

13. Do Now Differentiate between an ore and a mineral.

14. Do Now List 3 things to consider when choosing your metal for the coin project.

15. Objectives 1. SWBAT differentiate between reactive and non reactive metals. 2. SWBAT answer questions on reactivity. 3. SWBAT identify oxidation and reduction reactions 4. SWBAT identify oxidizing agent and reducing agents.

16. B.4 Metal Reactivity 2 Cu(s) + O 2 (g)  2 CuO (s) a. Identify the reactant(s). b. Identify the product(s). c. What do the letters in parentheses represent?

17. Symbols used in chemical equations: (s) = solid (l) = liquid, typically H 2 O, Hg and Br (g) = gas (aq) = aqueous solutions, the solvent has to be water. Ex. Salt water solution

18. Activity Series The ranking of elements according to their chemical reactivity. For example, Au (gold), does not react with any components of air such as oxygen. This is one reason why it is used in jewelry. Therefore it is ranked low on the Metal Activity Series Au, also used for gold plating electrical contacts used in air bags. They are dependable because oxides do not form on gold-plated surfaces.

19. Single Replacement Reactions A + BX AX + B Element A is in competition with B for the formation of a compound with ion X. The compound formed is with the MORE reactive element.

20. Metal Activity Series More reactive metals can replace less reactive metals. (Higher up can replace lower down.)

21. Metal Activity Series Reactive metals are more difficult to release from their compounds. Ex. Can zinc (Zn) replace Magnesium in Mg(NO 3 ) 2 ? Can Zn ever replace copper (Cu) in a chemical reaction?

22. Think-Pair-Share 1. List one metal that can replace potassium in K 2 O 2. Can Calcium (Ca) replace Magnesium in Mg(NO 3 ) 2 ? Can Pb ever replace aluminum (Al) in a chemical reaction?

23. Activity Series The more reactive the metal, the more likely to form a cation

24. Mining and Refining Reduction: Gain of electrons – there are electrons in the reactants Ex. Cu 2+ + 2e -  Cu The copper cation was reduced, lost its charge by gaining electrons Process usually done to obtain metal from it’s ore

25. Mining and Refining Oxidation: Loss of electrons – there are electrons in the products Ex. Fe  Fe 3+ + 3e - Iron is oxidized to an iron (III) ion by losing 3 electrons

26. Remember… OIL RIG OIL – Oxidation Is Loss (of electrons) RIG – Reductions Is Gain (of electrons)

27. Oxidation – Reduction Reaction Oxidation and reduction reactions occur together and are called redox reactions. Cu 2+ (aq) + Mg(s)  Cu(s) + Mg 2+ (aq) - Which reactant (Cu 2+ or Mg(s)) is reduced? - Which is oxidized?

28. Half Reactions Fe+Cu 2+ Fe 2+ +Cu Half Reactions include:

29. Do Now Which do you think will be found in the purest form when mining: Highly Reactive Metal Non Reactive Metal Explain WHY!

30. Objectives SWBAT identify oxidation and reduction reactions SWBAT identify oxidizing agent and reducing agents.

31. Oxidizing agents and Reducing agents Oxidizing agents are the items being reduced. Reducing agents are the items being oxidized.

33. Think-Pair-Share Complete the unit review with a partner

37. Homework Pg. 151 # 9, 12, 13, 16-20 Will be collected

38. Do Now Fe(s) + Cd 2+ (aq) ------> Fe 2+ (aq) + Cd(s) What is being oxidized? What is being reduced? What is the reducing agent? What is the oxidizing agent?

39. Objectives SWBAT review homework problems SWBAT practice redox reagents and identify reduction and oxidation. SWBAT answer questions to help them get ready for their upcoming test.

40. Homework 2.B.Supplement Worksheet #1-8

41. Do Now Would this reaction occur? Why? 2Al + 3ZnCl 2 3Zn(s) + 2AlCl 3

42. Objectives SWBAT review homework problems SWBAT practice redox reagents and identify reduction and oxidation. SWBAT answer questions to help them get ready for their upcoming test.

43. Do Now Write an oxidation–reduction equation for the reaction of silver ions with magnesium atoms. a. Which reactant is oxidized? ________ b. Which reactant is reduced? ________ a. the oxidizing agent _______________ b. the reducing agent _______________

44. Objectives