1. The Mole

2. The Mole Avagadro’s # - 6.02 x 1023
-The mole (mol) is the SI base unit to measure the amount of substance.
-Through experimentation, it has been determined that 1 mole of anything contains x 1023 representative particles
-A representative particle is any kind of particle
(Ex. Atoms, molecules, formula units, electrons or ions)
Avagadro’s # x 1023
-Extremely large number
to count extremely small numbers

3. Converting Moles to Particles and Particles to Moles
Conversion Factor: 6.02 x 1023 representative particles
1 Mole
Moles to Particles
# of Moles x 6.02 x 1023particles = # of Particles
1 Mole
Ex: How many molecules are in 3.50 Moles of sucrose?

4. Particles to Moles # of representative particles x 1 Mole________
# of representative particles x 1 Mole________
6.02 x 1023 rep particles
Ex: Calculate the number of Moles that contain 4.50 x 1024 atoms of Zinc (Zn).

5. For example: C- 12.011 amu, H- 1.008 amu
Molar Mass
-You can find Atomic Mass on the PT. but notice, it is not an exact integer
For example: C amu, H amu
-This is because these weights are an AVERAGE weight of all naturally occurring isotopes.
Isotope- Atoms of the same element with the same number of proton but different number of neutrons, or different atomic mass
Molar Mass- the mass in grams of one Mole of any pure substance
Molar Mass (mm) is equal to atomic mass
Units- g/mol

6. Ex: Calculate the molar mass of Cl2

7. Ex: How many moles of calcium are in 525g Calcium?
Mass to Moles
# of grams x 1 mole = of moles mm
Ex: How many moles of calcium are in 525g Calcium?

8. Mass to Atoms Conversion -There is no direct conversion Two Steps
1. Covert Mass to Moles
2. Convert Moles to Atoms
Ex: How many atoms of gold are in a pure gold nugget having a mass of 25.0g?

9. Atoms to Mass Conversion
Ex: A party balloon contains 5.50 x 1022 atoms of Helium gas, what is the mass in grams of the Helium?

10. Assignment:
Chemistry Matter and Change – Glencoe Text
Pages 346 – 347 #’s 89-93, 95, , 101, 103

11. Moles of Compounds
Recall: The chemical formula for a compound indicates the types of atom and the number of each atom present.
Ex Freon, CC12F2
C – 1 atom
C1 – 2 atoms
F – 2 atoms

12. How many moles of fluorine atoms are in 5.50 moles of Freon?
Finding Moles of Individual Atoms in a Compound
Ex Freon, CC12F2
We know = C – 1 atom
C1 – 2 atoms
F – 2 atoms
So we can write:
1 mol C atom 2 mol C1 atoms 2 mol F atoms
1 mol CC2F2 1 mol CC12F2 1 mol CC12F2
How many moles of fluorine atoms are in 5.50 moles of Freon?

13. Ex. 2 Determine the mols of aluminum ions in 1
Ex.2 Determine the mols of aluminum ions in 1.25 mols of Aluminum Oxide.

14. Molar Mass of Compounds
- The mass of a mole of compound equals the SUM of the masses of every particle in the compound
Ex. Calculate the molar masses of K2CrO4

15. Moles of a Compound to Mass
Two Steps:
1. Calculate Molar Mass of Compound
2. Convert to Mass
Ex. What is the mass of 2.50 moles of allyl sulfide, (C3H5)2S ?

16. Ex. Calculate the mols of 325 g of Calcium Hydroxide
Converting Mass of Compound to Moles
Two Steps:
1. Calculate Molar Mass of Compound
2. Convert Mass to Moles
Ex. Calculate the mols of 325 g of Calcium Hydroxide

17. Converting Mass of Compounds to number of Particles 3 Steps
3 Steps
1. Calculate the Molar Mass of Compound
2. Convert Mass to Moles
3. Convert Moles to Particles
Ex. Aluminum Chloride is used in refining petroleum and manufacturing rubber and lubricants. A sample of aluminum chloride (AlCl3) has a mass of 35.6g. How many AlCl3 atoms are present?

18. Textbook Assignment:
Page 347 #107, 108, 111
Page 348 #114, 115, 123, 127

19. Converting from Moles to Gas Volume
- Many elements occur naturally in gas form
- Molar volume can be used to convert moles to gas volume and gas volume to moles
1 mole is equal to 22.4 L or 1 mole
22.4 L
Ex. A certain reaction produces 86.5L of hydrogen gas. How many moles of Hydrogen were produced? (Remember: Diatomics, H2)

20. Converting from Moles to Gas Volume
Ex. What Volume does 4.96 moles of O2 occupy?

21. Converting Volume to Mass 3 Steps: 1. Convert Volume to Mass
3 Steps:
1. Convert Volume to Mass
2. Calculate Molar Mass
3. Convert Moles to Mass
Ex. Assume we have 86.7L of N2. What is the mass of nitrogen gas?