1. Moles and Molecular Mass Meyer 2013

2. Diatomics Di = two Atomic = atoms Diatomics are atoms that are paired under normal conditions

3. The 7 diatomic Atoms

4. What is a Mole Mole Abbreviation = mol The mole is the unit scientists use to represent the amount of a substance. In Chemistry class a mole is not a furry little critter that lives under ground

5. The Mole A mole (mol) is an amount of substance that contains = 6.022 x 10 23 items A dozen is an amount of substance that contains = 12 items Why is the mole such a big number?

6. The Mole Moles of different substances vary in size, mass, and volume

7. The Mole A dozen eggs is smaller than a dozen cars A mole of copper fits in your hand – a mole of oranges (fruit) is larger than the planet Earth

8. The Mole One (1) mole = 6.022 x 10 23 atoms How do you count atoms?

9. Counting Atoms Chemist count atoms by weighing them ( determining the mass) 1 mole is equal to the Atomic Mass (Red Number on your periodic table)

10. Our New Conversions Write this down on your periodic table: 1 mole = Atomic Mass (red number) 1 mole = 6.022x10 23 Atoms (Avogradro’s number)

11. 1 mole = Atomic Mass (red number) 1 mole = 6.022x10 23 Atoms 18.5 grams of sodium = _____ Moles of sodium

12. 1 mole = Atomic Mass (red number) 1 mole = 6.022x10 23 Atoms 2.3 moles of oxygen = _____ grams of oxygen

13. 1 mole = Atomic Mass (red number) 1 mole = 6.022x10 23 Atoms 2 grams of copper = _____ Atoms of copper