1. Metal Characteristic: Example: Nonmetal Characteristic: Example: What do you know about different elements?

2. Physical properties: properties that can be determined without altering the chemical makeup of the material. Color, density, odor, melting point, boiling point, bendable etc. Material remains the same after you test for certain physical properties. A.1 PROPERTIES MAKE THE DIFFERENCE

3. Kind of chemical changes it undergoes. Substance doesn’t stay the same after a chemical change. Ex. Rusting of iron, burning etc. Combustion – burning, involves oxygen. Chemical properties

4. 1.Pure metals have a high luster. 2.Surfaces of some metals become dull when exposed to air 3.Nitrogen gas, forms nitrogen oxides at the high temperatures of an operating automobile engine. 4.Milk turns sour if left too long at room temperature 5.Diamonds are hard enough to be used as a coating for drill bits 6.Metals are ductile 7.Bread rises 8.Argon is used to fill light bulbs to prevent the metal filament wire inside the bulb from being destroyed through oxidation. 9.Metals conduct heat and electricity. Physical or chemical?

5. What is a concern when manufacturing coins? – Cost, durability, reactivity of metal A.3 properties matter: designing the penny

6. 1980s copper became too expensive to be used as the primary metal in pennies. 1943-zinc-plated steel pennies., corroded easily 1982 zinc replaced copper, copper coating. More chemically reactive. 97.5% zinc History of the penny

7. Metals – conducts electricity & heat, malleable, ductile Nonmetals – brittle, bad conductors Metalloids (properties of metals and nonmetals) A.4 The Chemical Elements

8. Mendeleev – arranged according to atomic mass Mosley – arranged according to atomic number Periodicity Pg119 Atomic number - #protons Atomic mass - #protons + #neutrons isotopes The Periodic Table

9. Alkali Alkali earth Transition metals Metalloids Halogens Noble gases Lanthanides actinides Groups

10. Arrangement of electrons Metals tend to give electrons Results in cations What determines properties?

11. http://www.youtube.com/watch?v=7jggPpaLy Kk http://www.youtube.com/watch?v=7jggPpaLy Kk A.13 It’s Only Money

12. Section A Quiz

13. Sources and uses of metals: coin, clothing, engines, fertilizer… Earth’s composition – Atmosphere – N, O, Ar, He, Ne, C – Hydrosphere – water, salt, Mg, S, Ca – Lithosphere – silicates, coal, oil, carbonates, oxides, sulfides, – Mantle – silicates, Mg, Fe – Core – Fe, Ni SecB Earth’s Mineral Resources

14. Lithosphere – solid part, chemical resources, petroleum, ore Ore – naturally occurring rock or mineral that can be mined Minerals – naturally occurring solid compounds containing the element or group of elements of interest. Mines:

15. Africa – chromium 95%, cobalt 52%, manganese 80% China – Aluminum 17% Pg. 136 ques.1-5 World’s Mines

16. Ductility – drawn into wires Brass, bronze Alloy – mixture of metals melted together Not very corrosive Element handbook worksheet Copper

17. Most metals are found combined with other elements in nature. Mined and refined Formation of copper metal: reduction Reduction – gain one or more electrons Cu2+  Cu Reduced comes from the ion charge number. 2+  0 Gets smaller B.8 Mining and Refining

18. Cu  Cu2+ + 2e- Oxidized – lose one or more electrons. 0  2+ ion charge number Formation of Copper(II) ions : oxidation

19. One reactant loses e- and the other gains e-. Another name = redox reactions Cu + 2Ag+  Cu2+ + 2Ag Which is reduced? Ag Which is oxidized? Cu Oxidation-reduction rxn.

20. Cu 2+ (ion blue) + Mg (metal)  Cu (metal) + Mg 2+ (colorless ion) Refining example

21. Electrometallurgy – using an electrical current to supply e- to metal ions. Reducing them 2+  0 Pyrometallurgy – treating metals and their ores with heat, carbon and carbon monoxide to provide e- Hydrometallurgy – treating with reactants in a water solution. Ex. Redox rxns. Redox Rxn. To obtain Pure metals

22. Law of conservation of matter: matter is neither created nor destroyed in a chemical reaction. Balanced chemical equation: number of atoms of each element is the same on the reactant and product sides. C + O 2  CO 2 Diatomic – same element bonded to another of the same. GEN-U-INE Sec. C Conserving Matter

23. 2Cu + O 2  __CuO Coefficients – indicates the number of units of each substance involved in the chemical reaction. Formula unit – smallest unit of an ionic compound. Ionic compounds are called formula units because they form large crystals. Molecules – name for compounds made up of nonmetal+nonmetal.

24. 1.Never touch subscripts! 2.Balance polyatomic molecules first. 3.Balance metals 4.Balance nonmetals (save hydrogen and oxygen for last) 5.Make sure coefficients are in lowest ratio. Rules for balancing equations

25. Make a chart and list number of atoms of each element. Reactants Products 3 C1 C 8 H2 H 2 O3 O C 3 H 8 + O 2  CO 2 + H 2 O

26. The Mole A way to group an amount of atoms together so to not deal with huge numbers. Amount of a substance that contains as many particles as there are atoms in exactly 12 g of carbon-12. Just like: dozen, gross, … 1 mole = 6.022 x 10 23 atoms Avogadro’s number = 6.022 x 10 23 Number of particles in exactly one mole of a pure substance.

27. How many atoms are in 3 moles of Silicon (Si)?

28. How many moles is 5.43 x 10 38 atoms of Na?

29. Molar Mass The mass of one mole of a pure substance. g/mol The molar mass of an element = atomic mass unit Ex. Carbon 12g  12g/mol Example: 2.00 mol He = _____g He 2.00 mol He x 4.00 g He = 8.00 g He 1 mol He

30. What is the mass in grams of 3.50 mol of the element copper, Cu?

31. A chemist produced 11.9 g of Al. How many moles of aluminum were produced?

32. Calculation How many atoms are in 3moles of H 2 ?

33. C.7 Equations and Molar Relationships Stoichiometry – using the chemical equation to solve for amount of products or reactants unknowns. 2CuO + C  2Cu + CO 2 23g ?g 23gCuO x 1moleCuO x 2moleCu x 63.5gCu =18.4g 79.5gCuO 2mole CuO 1mole

34. C.9 Composition of Materials Percent composition – percent by mass of each material found in an item such as a coin. A post-1982 penny with a mass of 2.500 g is composed of 2.4375 g zinc and 0.0625 g copper. What is its percent composition? 2.4375g zinc x 100% = 97.50% zinc 2.500g total 0.0625g copper x 100% = 2.50% copper 2.500g total

35. Practice question Cu 2 S What is the percentage of Copper? Contains 2 moles of Cu and 1 mole of S. %Cu = mass of Cu x 100% mass of Cu 2 S 127.10g Cu x 100% = 79.85% Cu 159.17gCu 2 S

36. Pg 169 Retrieving Copper

37. C.12 Conservation in the Community Depleting Resources Renewable resources – can be replenished by natural processes. Nonrenewable resources – cannot be readily replenished. Petroleum is declining Metal mining is becoming less profitable because the ore contains a smaller percentage of the metal.

38. Conserving Resources 4 R’s Rethinking Reusing Replacing Recycling

39. Poster Design Give examples (2 pts each) with sketches (1 pt each) of each of the R’s. Explain each one of the R’s (2 pts each). Creativity (3pts) Spelling and Grammar (2pts). Rethinking Reusing Replacing Recycling 25 points total