1. Objectives
Describe the chemicals in the Earth’s atmosphere, hydrosphere and lithosphere.
Describe and recognize factors that determine the feasibility of mining.
Define oxidation and reduction.
Identify oxidation and reduction processes.

2. 2.B.1: Sources and Uses of Metals
Human needs for resources must be met by chemical supplies currently present on Earth.
The needs include: creating a new coin, manufacturing of clothing, petroleum products, fertilizer for food and energy needs.
Resources can be cataloged by where they are found on Earth.

3. 2.B Earth’s Mineral Resources

4. Earth’s Resources
Atmosphere: provides nitrogen, oxygen, neon and argon.
Hydrosphere: water and dissolved minerals.
Lithosphere: solid part of the earth which provides the greatest variety of chemical resources. These include petroleum, metals, ores and minerals.

5. Earth’s Resources
Ore: a naturally occurring rock or mineral that can be mined.
An ore contains a mixture of components.
Of these minerals are the most important part of the ore.

6. Lithosphere
Average thickness is 3,840 miles. Most of the mined resources occur in the first 25 miles (crust).
Metals found in the crust include: aluminum, sodium, iron, calcium, magnesium and potassium.
These metals must be mined form the earth.

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

10. Mining Copper Ores

11. Mining Copper Ores
The first copper ores mined were relatively rich in copper metal: 35% to 88%.
Such ores are no longer available.
Today it is possible to mine ores containing less than 1% copper
These ores are chemically processed to produce metallic copper.

12. Properties of Copper

13. Mining Copper Ores
Copper is one of the most familiar and widely used metals in society. Uses include:
Electrical wiring.
Second only to silver in electrical conductivity.
Relatively low cost and corrosion resistance
Ductility – ability to be drawn into wires.
Used to produce brass, bronze, jewelry and artwork.

14. Mining Copper Ores
Will future developments increase or decrease the need for copper?
What copper substitutes are available?

15. B.2 Production vs. Use
Follow the guidelines on page to research the metal you are assigned.
Prepare a PowerPoint presentation answering questions (following slide) about your metal.
Due: Class Presentation – DATE

16. PowerPoint Presentation
Cover slide – name of metal / name of student
Symbol of metal, number of protons, common isotopes of the metal
Where is metal found on earth (countries)
History of metal
How abundant is metal (worldwide production)
The metals properties (shiny, color soft, etc.)
Three current uses of metal

17. B.3: Converting Copper
Lab: Handout and page in textbook

18. Some useful websites for your research
All metals:
Aluminum:
Copper:
Lead:
Nickel:
Silver:
Tin:
Zinc:

19. B.4 Metal Reactivity 2 Cu(s) + O2(g)  2 CuO (s)
Identify the reactant(s).
Identify the product(s).
What do the letters in parentheses represent?

20. Symbols used in chemical equations:
(s) = solid / precipitate
(l) = liquid, typically H2O, Hg and Br
(g) = gas
(aq) = aqueous solutions, the solvent has to be water. Ex. Salt water solution

21. 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.

22. Metal Activity Series
Reactive metals are more difficult to release from their compounds.
Ex.
Can zinc (Zn) replace Magnesium in Mg(NO3)2?
Can Zn ever replace copper (Cu) in a chemical reaction?

23. Please rank the following elements in order of reactivity (based on the activity series chart on page 145). List the most reactive element first.
Gold, copper, chromium, magnesium, potassium

24. B.5: Relative Reactivities of Metals
Lab: Handout and page 142 in textbook

25. B.6: Metals
Certain metals in nature are found in the uncombined stated.
These metals are known as free elements, rather than in combination with other elements.
These metals include gold, copper and silver.
Because they are not combined with other elements they were the first metals used by man.
These metals are also very unreactive.

26. Most metals are usually found in the form of a metallic ore (combined with other elements)
Metallic ores are also known as minerals.
These metals include aluminum and iron.
These metals need to be extracted or separated from their ores to yield the pure metal.
Bronze and brass are a combination of copper with another metal and not a pure metal.
Because these metals need to be extracted from their ores they were used by humans at a later time.

27. Metal alloys
An alloy is a mixture of 2 or more elements (one must be a metal)
These are uniform throughout, so a homogeneous mixture
Examples: Brass (copper and zinc); Sterling silver (silver and copper) Bronze (copper and tin)

28. Why have alloys?
Alloys are important because they are combining properties and are often superior compared to the pure elements
Typically, more inexpensive than the pure element:
Sterling silver vs pure silver
$0.95 vs $1.68

29. Why have alloys?
Alloys are important because they are combining properties and are often superior compared to the pure elements
Typically, more inexpensive than the pure element:
Sterling silver vs pure silver
$0.95 vs $1.68

30. B.8: Oxidation – Reduction Reactions
B.8: Reading Guide Worksheet

31. IONS
Atoms are neutral because the protons which are positive and electrons that are negative balance out the charge, so there are the same numbers of protons and electrons in an atom.
An ion is an atom or group of atoms that has a positive or negative charge due to loss or gain of electrons.
There are two forms of ions: cation and anion.

32. B.8: Review of Ions Cation – positive ion Anion – negative ion
Monoatomic ions (1 atom)
Polyatomic ions
(group of atoms)
Cu+2 (loss of electrons)
Cl- (gain of electrons)
Na+, Cl-, Mg2+, O2-, Al3+, N3-
NH4+, CO32-, SO42-, PO43- 32

33. B.8: Review of Ions Cu  Cu2+ + 2e-
29 protons (+) 29 protons (+)
29 electrons (-) 27 electrons (-)
Net charge = Net charge = Net charge = -2
Overall charge on both sides of the reaction arrow are the same

34. B.8:Oxidation – Reduction Reaction
Converting copper cation (+2) to copper metal
requires the addition of 2 electrons
Reduction:
Gain of electrons by a reactant.
Ex.
Cu2+ + 2e-  Cu
The copper cation was reduced, lost its charge by gaining electrons

35. Mining and Refining Oxidation:
Loss of electrons – there are electrons in the products
Ex.
Fe  Fe3+ + 3e-
Iron is oxidized to an iron (III) ion by losing 3 electrons

36. OIL – Oxidation Is Loss (of electrons)
Remember…
OIL RIG
OIL – Oxidation Is Loss (of electrons)
RIG – Reduction Is Gain (of electrons)

37. Oxidation – Reduction Reaction
Oxidation and reduction reactions occur together and are called redox reactions.
Cu2+(aq) + Mg(s)  Cu(s) + Mg2+(aq)
- Which reactant (Cu2+or Mg(s)) is reduced?
- Which is oxidized?

38. Oxidation – Reduction Reaction
In a redox reactions the electrical charge, as well as, the atoms must be balanced on either side of the reaction arrow.
This is known as a balanced equation.
Cu2+(aq) + Mg(s)  Cu(s) + Mg2+(aq)
The total electrical charge on both sides of the reaction arrow is +2 in the above equation.
On the activity series chart, magnesium is above copper allowing the reaction to occur.

39. Oxidation – Reduction Reaction
Classwork: Redox Worksheet (B8)

40. Using Redox Reactions to obtain Pure Metals
Techniques that are used to reduce metal cations to pure metals in industry include:
Electrometallurgy - use of electric current
Pyrometallurgy – use of heat
Hydrometallurgy – use of water

41. Electrometallurgy
This technique involves using an electrical current to supply electrons to the metal ions.
This process is used when no other chemical reducing agent is available.
Also allows for the production of very high-purity metals.

42. Pyrometallurgy The use of heat (blast furnace) is used.
Carbon or carbon monoxide are the common reducing agents supplying the electrons for the reduction reaction.
The oldest method to obtain pure metals from ores.

43. Hydrometallurgy This technique uses water to treat the ores.
Used to recover gold and silver from old mines.
Process is known as leaching.

44. Oxidation – Reduction Reaction
Homework – reading guide
Due: Use as a section review
Homework – B8 Supplement Worksheet
Due: