SECTION C – CONSERVATION
C.1 – SOURCES OF RESOURCES – see Table 3 pg. 123
¨ Atmosphere : N2, O2, Ar, He, Ne, H2O, CO2
¨ Hydrosphere :H2O, NaCl, Mg, Ca, S
¨ Lithosphere
¨ Crust : Silicates, Al, Na, Fe, Ca, Mg, K, coal, oil, oxides, sulfides, carbonates
¨ Mantle: Mg and Fe silicates
¨ Core: Fe, Ni
¨ Which layer of the planet do the majority of our resources come from? Lithosphere found in the crust
¨ The resources that we use are not evenly distributed in the earth – see Table 4 pg. 124
¨ What is one primary reason we MUST be involved in international trade?
Ø Certain countries control the vast majority of certain resources. Examples:
¨ The development of the U.S. as a major industrial nation can be greatly attributed to what?
¨ Huge amounts of virtually every resource
C.2 – REVIEW of THe LAW OF CONSERVATION OF MATTER
¨ The law of conservation of matter - matter (atoms) can NOT be created or destroyed. You can rearrange atoms in molecules by breaking and/or forming bonds between atoms – but the number of atoms of each element remains the same before and after a chemical reaction.
¨ DIATOMIC elements : Those that exist in nature as doublets when they are not combined with any other elements – BrINClHOF
¨ SUBSCRIPTS – small numbers telling how many atoms of an element are in a molecule
¨ COEFFICIENTS – large numbers written in front of a compound telling how many molecules there are
¨ You may only change COEFFICIENTS when balancing equations – and you may only place them at the beginning of a formula – not in the middle!
Ø BALANCE THE FOLLOWING EQUATIONS
1. C + O2 2CO
2. Fe2O3 + CO Fe + 3CO2
3. Cu2S + O2 CuO + SO2
4. CuO + C Cu + CO2
5. NH3 + O2 NO2 + H2O
6. O3 O2
7. Cu + AgNO3 Cu(NO3)2 + Ag
8. C8H18 + O2 CO2 + H2O
C.3 – ATOM, MOLECULE, AND ION INVENTORY – MOLES, MOLES, MOLES!!
2H2 + O2 2H2O
· Write a sentence to describe what happens in the equation above, in terms of atoms and molecules….
· Atoms and molecules are such small units, we use moles instead for “real life” Counting!
· The Coefficients written in front of the molecules can mean atoms/molecules or moles interchangeably
· 1 mole of anything = 6.02 x 1023 “things” = Avagadro’s Number
Q. – How many eggs are in a dozen? ______
Q. – How many pickles are in a dozen? ______
Q. – How many pickles are in a ton of pickles?______
Q. – How much paper is in a ream?______
Q. – How many eggs are in a ream?______
Q.- How many pickles are in a ream? ______
Q, - How many Helium atoms are in a ream?______
Q. – How many eggs are in a mole? ______
Q. – How many pickles are in a mole? ______
Q. – How many Helium atoms are in a mole?!______
Q. – How long do you think it would take you to drink 1 mole of water?
Q. – How long would it take someone to count out 1 mole of water molecules?
MILLION DOLLAR Q. – Mr. K gave you all exactly 1 mole of water molecules…. How in the world did he find the time to count them all out?!
MILLION DOLLAR A.-
Q. - Is the number of golf balls in a mole of golf balls the same as the number of bowling balls in a mole of bowling balls?
Q. – Is the mass of a mole of golf balls the same as the mass of a mole of bowling balls?
¨ Since it is difficult to count atoms and molecules, it would be nice to be able to weigh them, and relate the weight to the number of atoms or molecules
¨ The atomic masses on the periodic table !
¨ Atomic mass = relative mass of one atom of an element
¨ Units of AMU’s
¨ Ex. – what is the mass of one mole of carbon atoms?
¨ Ex. – what is the mass of one mole of sodium atoms?
¨ Ex. What is the mass of 6.02 x 1023 oxygen atoms?
¨ The atomic masses on the periodic table can be used to find the molar masses of atoms, or compounds!
¨ Molar mass = the mass of one mole of a substance
¨ Units of grams/mole
¨ Ex. – What is the mass of 3 moles of carbon atoms?
¨ Ex. – What is the mass of one mole of sodium chloride (NaCl) molecules?
¨ Ex. – What is the mass of 2 moles of sodium chloride (NaCl) molecules?
¨ Ex. – what is the mass of 2 moles of calcium chloride (CaCl2) molecules?
¨ Given the number of moles of a substance you can find the mass, and conversely given the mass you can find the number of moles – both by using the molar mass from the periodic table and dimensional analysis!!
¨ Ex. – Determine the number of moles in 25 g of NaCl
¨ Ex. – Determine the number of grams in 2.5 moles of NaCl
C.4 - CONSERVATION
¨ Why do metals and petroleum specifically pose such a problem in terms of depletion of these particular resources?
¨ What are the four “R’s” of resource conservation and management?
¨ Rethink
¨ Replace
¨ Reuse
¨ Recycle