1. 1 What is a Mole? Mole Video

2. 2 What is a mole? No!! Not that kind of mole! Unit of measure that is important in understanding the relationship between the number of particles in a substance and its’ mass.

3. 3 The Mole No! Not that kind of mole. A mole (mol) is the amount of a substance that contains as many particles as there are atoms in 12g of C-12.

4. 4 Avagadros Number Avagadro’s number- determined experimentally 6.022 x 10 23 units = 1 mole “Units” can be atoms, particles, formula units or molecules

5. 5 Check these out! I have measured exactly 1.00 mol of a bunch of household items. Pass them around.

6. 6 Molar Mass The amount of substance that contains Avogadros number of particles. Units: grams/mol Atomic mass (amu) = Molar mass (g/mol)

7. 7 The Periodic Table So, when we look at the periodic table, we have a bunch of conversion factors that will help us do all sorts of calculations. Yipee!

8. 8 How do I do gram to particle calculations? Flow chart: Gram  Mole  Particle Using the flow chart, we can solve any of these seemingly difficult calculations.

9. 9 Now, let’s determine the number of moles! Fun huh? How many moles in 20.0 g of Boron?

10. 10 Practice makes perfect! How many moles in 68.7g of Lithium?

11. 11 Can we go the other way? How many grams in 2.61 moles of Chlorine atoms?

12. 12 How many moles are present in 8.32 x 10 25 atoms of silver? How many atoms in 2.3 mol of silver?

13. 13 Now let’s take it all the way! How many atoms in 3.0g of Carbon? How many grams in 1.2 x 10 23 atoms of carbon?

14. 14 Work on you WS….

15. 15 Molar Mass A compound is a collection of atoms that are chemically bonded together. Molar mass is the mass in grams of one mole of the compound. You may also hear this quantity referred to as molecular weight.

16. 16 What is the Molar Mass of water? 1. Count how many atoms of each element. 2. Multiply by the atomic mass rounded to the 0.01 place. 3. Add them up!

17. 17 Examples CO 2 1 Carbon atom1(12.01)g 2 Oxygen atoms2(16.00g) = 32.00g 12.01g + 32.00g = 44.01g

18. 18 Easy Huh? Try these! NaOH MnO 4 Cu 3 (PO 4 ) 2

19. 19 NaOH1Na23.00g 1O16.00g 1H1.01g 23.00g + 16.00 g + 1.01g =40.01g

20. 20 Manganese (IV) oxide MnO 2 Mn1(54.94) O2(16.00) 54.94g/mol + 32.00g/mol = 86.94g/mol

21. 21 Copper (II) Phosphate Cu 3 (PO 4 ) 2 Copper 3(63.55) Phosphorus2(30.97) Oxygen8(16.00) 380.59 g/mol

22. 22 How many formula units in 3.45 g of NaOH?

23. 23 How many grams are in 1.06 x 10 27 formula units of MnO 2 ?

24. 24 Now, lets combine what we’ve learned to do a problem you may see on the exam. Methane is a gas. Its molecular formula is CH 4. How many moles are in 20.0g of methane? Steps 1. Determine the molar mass 2. Use the answer in #1 as a conversion factor to change grams to moles.