1. What doesn’t belong?
Dozen
Couple
Few
Baker’s Dozen
Ten

2. The Mole

3. Definition Avogadro’s Number
Mole- unit standing for 6.02 x particles
602,000,000,000,000,000,000,000 particles
Avogadro’s Number

4. Why such a BIG unit? Atoms and Molecules are TINY!
A drop of water contains 10 trillion water molecules!

5. Moles and Particles 6.02 x 1023 makes a chemist’s life a lot easier
It’s impossible to keep track of one atom
so scientist discovered this number that gives us the molar mass of an atom
Molar mass is the mass of 6.02 x 1023 particles of a given substance
Mass is given in grams

6. Molar Mass
Luckily 6.02 x 1023 particles, or a mole, adds up to the same number as the avg. atomic mass-but in grams
So a mole of magnesium has a mass of grams!

7. We don’t always have exactly 1 mole, though.
When we have different amounts of moles, we can convert between atoms and moles

8. Mole Calculations Moles Particles Multiply by Avogadro’s Number
Divide by Avogadro’s Number

9. Example 1
A lab experiment calls for 2.00 moles of Calcium. How many particles of Calcium are required?
How can we solve this?
ID what we’re given and what the question’s asking for and set up the T-Chart
6.02 x 1023 particles
2 moles Calcium
1 mole Calcium

10. Example 2
You have 12.04x1023 atoms of sulfur. How many moles of sulfur do you have?

11. Whiteboards
How many moles are 1.20 x 1025 atoms of phosphorous?

12. Whiteboards
How many moles of magnesium is 3.01 x 1022 atoms of magnesium?

13. Whiteboards
How many atoms are in moles of zinc?

14. Converting from grams  mole Mole  grams Calculating molecular mass

15. Molar mass: mass of 1 mole of in grams
1 mole C atoms = _____________________
1 mole of C atoms has a mass of_________ g.
Molar mass of O = ___________
Molar mass of Li = ____________
For any element, the
__________________________________
3.2

16. What is the mass of one mole of:C Hg Cu Fe
3.2

17. Molecular mass (or molar mass) is the sum of
the molar masses of all the atoms in a molecule.
SO2 S
32.06 g/mol O
16.00 g/mol
SO2
64.06 g/mol
SO2 consists of ________
and ______________.
1 mole SO2 = _________________
________________molecules of SO2
has a total mass of ______________
3.3

18. Calculate the molar mass of the following
NO2
C6H12O6
(NH4)3PO4

19. When I bought my fly kicks…
If I had 20 Wolfies, and the cost of one pair of kicks is 4 Wolfies for 1 pair, how many pairs could I have?
What’s my conversion factor?
What unit am I given?
What unit is the question asking for?
20 Wolfie
1 pair
(20/4) pairs
5 pairs
4 Wolfies
Now...

20. If I had 20 grams of helium, and one mole of helium is 4 grams, how many moles of helium could I have?
What’s my conversion factor?
What unit am I given?
What unit is the question asking for?
20 grams He
1 mole He
(20/4) moles He
5 moles He
4 grams He

21. Grams  Mole Conversion
1 mole of Zinc has a mass of g.
Conversion factor:
1 mole Zn
65.39 g Zn OR
65.39 g Zn
How many moles of Zn are in 85 grams?

22. How many moles are found in the following quantities?
10.0 g Fe
8.0 g O
1.15 g Mg
15.63 g Cl
Hint: What are the conversion factors?
Partner work

23. Mole  Gram Conversion 1 mole of Zinc has a mass of 65.39 g.
Conversion factor:
1 mole Zn
65.39 g Zn OR
65.39 g Zn
If I had 2 moles of Zn, how many grams of Zn do I have?
2 moles Zn
65.39 g Zn
1 mole Zn
g Zn

24. Find the mass in grams of the following quantities:
1.35 mol Fe
24.5 mol O
0.876 mol Ca
1.25 mol H
Hint: What are the conversion factors?

25. How many grams are found in 2.3 moles of C3H8? How many molecules?
2.3 moles C3H8
44 g C3H8
2.3 x 44 g C3H8
101.2 g C3H8
1 mole C3H8
2.3 moles C3H8
6.02 x 1023 molecules C3H8
1 mole C3H8
2.3 x (6.02 x 1023 molecules C3H8)
13.2 x 1023 molecules C3H8