Chemistry Lesson 10.1

1
ChemistryLesson 10.1

• The Mole

2
I. Measuring Matter

• A. 3 ways
• 1. counting (s)
• 2. mass (gram, pound)
• 3. volume (liter, gallon)
• B. Units of measurement
• 1. pair
• 2. dozen
• 3. ream

2
12
500
3
I. What is a mole?

• A. Def the S.I. unit that measures an amount
  or quantity.
• 1. similar to others dozen, ream, bakers
  dozen, gross, hour, day
• B. 1 mole 6.02 x 1023 particles
• 1. called Avogadros number
• 2. Usually refers to atoms, molecules, or
  formula units (Fe, H2O, CaCl2)

4

• C. Why such a big number?
• 1. Atoms are microscopic
• 2. 602,000,000,000,000,000,000,000
• 3. We need to be precise in chemistry

5

• D. Problems
• 1. How many moles of iron do you have with 2.41
  x 1024 atoms?
• 4.00 moles of iron
• 2. I have 3.3 x 1022 formula units of NaCl.
  How many moles is this?
• 0.055 moles of NaCl
• 3. I have 9.76 x 1025 molecules of N2. How
  many moles is this?
• 162 moles

6

• 4. How many molecules are in 2.12 mol of
  propane (C3H8)?
• 2.12 mol x (6.02 x 1023) propane molecules
• 1 1 mol
• 1.28 x 1024 propane molecules
• 5. How many atoms of propane are found in 1.28
  x 1024 molecules of propane?
• 1.28 x 1024 molecules x 11 atoms
• 1 1 molecule (C3H2)
• 1.41 x 1025 atoms

7

• 7. With a partner create a question similar to
  others used today and answer it.
• Then write the same question down and trade it
  with another group.
• Grade it when they are done.

8
Assignment 7.1

1. How many atoms are in 4.10 mol of C6H12O6?
2. How many molecules are in 0.750 mol of H2O?
3. How many C atoms are in 0.890 mol of C6H12O6?
4. How many H atoms are in 1.23 mol of C6H12O6?
5. How many mol are found in 6.02 x 1027 molecules
   of H2O?

5.92 x 1025 atoms
4.52 x 1023 molecules
3.21 x 1024 Carbon atoms
8.89 x 1024 Hydrogen atoms
1.00 x 104 mol of water
9
II. How much does a mole weigh?

• A. Gram atomic mass (single elements)
• 1. Def how much 1 mole of an element weighs
  in grams.
• 2. Ex Carbon
• 3. Others
• P K Ag
• Fe Ar Li

12.01 g
30.97
39.10
107.87
55.85
39.95
6.94
10

• B. Gram Molecular Mass
• 1. Def the mass of one mole of a molecular
  compound.
• 2. Use atomic values and add together GMM
• 3. Ex SO3
• S 32.06 O 16.00 (3)
• 32.06 48.00 80.06 g

11

• 4. Examples
• PO4 C8H18
• H2O SO4
• PCl3 N2O5

94.97
114.26
18.02
96.06
137.32
108.02
12

• C. Gram Formula Mass
• 1. Def the mass of one mole of an ionic
  compound.
• 2. Just like GMM
• 3. Ex NaCl
• Na 22.99 Cl 35.45
• 22.99 35.45 58.44

13

• 4. Examples
• CaI2 Na3PO4
• Li3N AlCl3
• Fe2O3 Al(OH)3

293.88
163.94
34.83
133.33
159.70
78.01
14

• Assignment Read 10.2 for Thursday.