1. The Mole
(mol)

2. A Little Review converting units from one form to another.
ex: 1inch = 2.54 cm

3. Dimensional Analysis What units do I have? What units do I want?
How can I get there from here?
How many yards are there in 572 feet?
How many liters are there in 7 milliliters?

4. The Mole
A mole is a unit of measure used to measure tiny amounts like molecules.

5. The Mole (cont.) Basically, a mole is just a number like a dozen.
One dozen is 12
One Mole is 6.02x1023
That’s 602,000,000,000,000,000,000,000

6. For Example A Dozen CD’s = 12 CD’s A mole of CD’s = 6.02x1023 CD’s
You can have a mole of anything in theory
This number (6.02x1023 ) is called Avogadro’s Number

7. Atomic Mass
A sample of any element with a mass equal to that element's atomic weight (in grams) will contain precisely one mole of atoms
eg. The atomic mass of Copper is
6.02x1023 atoms Cu = 1 mol
1 mol Cu = g
This is true for every element.

8. Molar Mass of Compounds
A mole can also be used to represent a compound
Ex.
H2O
H = 2 x 1.01 = 2.02
O = 1 x = 16
18.02 g/mol

9. Examples Ca3(PO4)2 Al2O3 Ca = Al = P = 3 x 40 = 120 O = 2 x 27 = 54
310 g/mol
2 x 27 = 54
3 x 16 = 48
102 g/mol

10. Calculate the Molar Masses
AlCl3
H3AsO4
Ca(OH)2
CO2
Lead (II) Nitride

11. A Little Thought
If you have 4 mols of Calcium how many atoms of Calcium do you have?
How many grams does it weigh?