1. Chapter 11:

2. By count By mass By volume A. Measuring Matter
What are three methods for measuring the amount of something?
By mass
By volume

3. B. Words for Numbers
What are some words you know that are used to identify an amount of something?

4. C. What is a Mole 1 mole = 6.02 x 1023 particles
602,000,000,000,000,000,000,000
Particles = molecules, atoms, or formula units

5. D. Moles to Particles
Use dimensional analysis to answer the following questions (1 mole = 6.02 x 1023 particles)
1. How many moles is 2.17 x 1023 atoms?

6. D. Moles to Particles
2. How many moles is 5.50 x 1048 formula units

7. E. Particles to Moles
How many atoms are there in 3.0 moles of copper atoms?
How many molecules are there in 1.5 moles of water?

8. F. The Definition of the Mole
Avogadro defined the mole as:
1 mole, 6.02 x 1023 particles,
is exactly 12.0 g of carbon – 12
Recall:
12 amu = mass of 1 carbon – 12 atom
The carbon – 12 isotope is used as the standard for both amu and the mole

9. Review!
Using your periodic table…what is the atomic mass of the following elements and compounds? Ca Fe Cu Ar P

10. G. Atomic Mass vs. Molar Mass
Atomic Mass (amu)
Molar Mass (g/mol)
Mass of 1 atom
1 atom of carbon = amu
Mass of 1 mole
1 mole of carbon = g

11. H. Molar Mass of a Compound
To calculate, sum up the atomic mass of each element in the compound.
The atomic mass is the molar mass in g/mol

12. Practice Mg 1 24.305 amu 24.305 amu Cl 2 35.453 amu 70.906 amu Element
Find the molar mass of magnesium chloride
MgCl2
Element
# of Atoms
Atomic Mass (amu)
Total Mass (amu) Mg 1
amu
amu Cl 2
amu
amu
Total Mass (amu) = amu
Molar Mass (g/mol) = g/mol

13. Practice
Calculate molar mass of the following:
KOH
HCl
H2SO4
Ca(OH)2