1. The Mole the link between the macroscopic gram and the nanoscale  our “scale up”

2. The Mole number of atoms needed to have atomic mass in grams 6.02 x 10 23

3. Using the Mole to Scale Up to Grams When I have 6.02 x 10 23 protons or neutrons (nucleons), I will have a mass of about 1 gram In class, discuss Carbon Consider other atoms –Suppose we have 1 mole (6.02 x 10 23 Na -23 atoms) –Suppose we have 1 mole (6.02 x 10 23 F - 19 atoms)

4. Using the Mole to Scale Up to Grams: Na - 23 = (6.02 x 10 23 x 23) nucleons = (23) x (6.02 x 10 23 nucleons) 1 g = 23 g This is atomic mass of Na - 23 (but in grams) this is 1 mol of Na atoms 23 x

5. Using the Mole to Scale Up to Grams So, when I have 1 mole (or 6.02 x 10 23 atoms) of Na -23, I must have 23 g !!

6. Using the Mole to Scale Up to Grams: F - 19 = (6.02 x 10 23 x 19) nucleons = (19) x (6.02 x 10 23 nucleons) 1 g = 19 g This is atomic mass of F - 19 (but in grams) this is 1 mol of F atoms 19 x

7. Using the Mole to Scale Up to Grams So, when I have 1 mole (or 6.02 x 10 23 atoms) of F - 19, I must have 19 g !! Based on this scale up, whenever I have one mole of atoms of an element, I will have the atomic mass of that element in GRAMS → if I have 1 mole of He atoms, I will have 4 g of He → if I have 1 mole of Cr atoms, I will have 52 g of Cr → etc.

8. Using the Mole The link between macroscopic grams and nanoscale number of particles! If I had 0.750 mol of Pb, –How many grams of Pb must I have? –How many atoms of Pb must I have?