1. Introduction to the Mole

2. Common Core Connection
Objectives:
Today I will be able to:
Apply the mole conversion factor to calculations relating to the quantity of atoms in a sample
Calculate the quantity of atoms in my name by completing a lab
Informal assessment – monitoring student interactions as they complete the practice
Formal assessment – analyzing student responses to the practice and the exit ticket
Common Core Connection
Make sense of problems and persevere in solving them
Reason abstractly and quantitatively
Build strong content knowledge

3. Lesson Sequence Evaluate: Warm-Up Explain: Intro to the Mole Notes
Elaborate: Mole Practice
Evaluate: Exit Ticket

4. Warm-Up What makes an atom neutral? Why would an atom not be neutral?
Define mass number
Describe the overall structure of an atom
Can an atom gain or lose electrons? If it can, what is it called?

5. Objective Today I will be able to:
Apply the mole conversion factor to calculations relating to the quantity of atoms in a sample
Calculate the quantity of atoms in my name by completing a lab

6. Homework
Have a great afternoon 

7. Agenda
Warm-Up
Intro to the Mole Notes
Mole Practice
Exit Ticket

8. Introduction to the Mole

9. How can we make a large quantity easier to count?
Example
Instead of counting eggs individually we can count the number of dozens
1 dozen = 12 eggs OR 12 eggs = 1 dozen
If a baker buys 6 dozen eggs, how many eggs does he have?
6 dozen 1
12 eggs
1 dozen
= 72 eggs x

10. The Mole
Atoms are too small and too numerous to count so we needed to develop a constant value of atoms to make it more reasonable to work with.
The Mole (Avogadro's Number)
6.02 x 1023
602,000,000,000,000,000,000,000

11. Example
If you took a mole of dollar bills and placed them next to each other around the circumference of the earth, they would go around the earth how many times?
2.34 x 1015
That’s Huge!
Bring paper with dollar calculation

12. Particles = Atoms, Molecules, Formula Units
1 Mole = 6.02 x Particles
Particles = Atoms, Molecules, Formula Units

13. We will use this when we get to the gas law unit
1 mole = 22.4 Liters
We will use this when we get to the gas law unit

14. Example 1
How many formula units of AgCl are in 2 moles of AgCl?

15. Example 2
How many Mg atoms are in 0.5 moles of Mg?

16. Converting from Mass to Moles
Atomic mass is based on the mass of one mole of an element or compound
1 mole = atomic mass unit of an element or compound in grams (molar mass)
Example: Carbon
1 mol of carbon = 12 grams carbon
12 grams of carbon has 6.02 x 1023 atoms of carbon

17. Molar Mass What is the mass of one mole of Chlorine?
35.45 grams of chlorine = 1 mole of chlorine
35.45 grams of chlorine has 6.02 x 1023 atoms
This is the Molar Mass of an element
It can be used as a conversion factor!
35.45 grams Cl
1 mole Cl
1 mole Cl
35.45 grams Cl OR

18. Molar Mass of Compounds
The formula mass of the elements can be used to find the molar mass of a compound
Example: Water (H2O)
18.0 grams of water = 1 mole of water
18.0 grams of water has 6.02 x 1023 molecules of water
Element
Number
Mass (g/mol) H 2
1.01 O 1
16.0
Total mass of Water
18.0

19. The Mole
If there was 20.0 g of iron, how many moles in that amount?
20.0 g Fe 1 x
1 mol
56 g Fe =
.357 mol Fe

20. The Mole
If you have 10.0 g of water, how many molecules in that amount?
10.0 g H2O 1
6.02 x 1023 molecules
1 mol
1 mol
18 g H2O x x =
3.34 x 1023 molecules of H2O

21. The Mole
If you have 25.0 g of copper (II) sulfate, CuSO4, how many formula units are in that mass?
1 mol
160 g CuSO4
6.02 x 1023 formula units
1 mol
25.0 g CuSO4 1 x x
9.41 x 1022 formula units of CuSO4 =

22. Exit Ticket
How many moles are in 6.02 x 1025 molecules?