1. The Mole Objective 3.02

2. What is a MOLE???? An amount of a substance A unit of measurement specific to chemistry mole mol n

3. The Mole “like a dozen” Specific quantity Does not change Avogadro’s Number: The # of “things” in 1 mole 6.022 x 10 23

4. The Mole How its used in Chemistry: Elements are made up of _______________. 1 mole Cu = 1 mole Na = 1 mole O =

5. The Mole How its used in Chemistry: Compounds are made up of _____________. 1 mole NaCl = 1 mole LiOH = 1 mole CaF 2 =

6. The Mole How its used in Chemistry: 1 mole Ca 3 (PO 4 ) 2 * Subscripts = # of moles of the element in the compound

7. The Mole How its used in Chemistry: 2 H 2 + O 2  2 H 2 O * Coefficients = # of moles of a substance in a reaction

8. Molar Mass (Molecular Weight) 1 mole of each substance has a “molar mass” – a specific weight It is the same as atomic mass only in g Ex: 1 mole Na = 1 mole C = 1 mole Li = The units for molar mass are g/mol

9. Molar Mass (Molecular Weight) 1 mole H 2 O = 1 mole NaCl = 1 mole Pb(NO 3 ) 2 =

11. Mole Conversion Review Problems Convert the following: 1. 4.3g of calcium hydroxide into moles 2. 0.82 moles of aluminum oxide into grams 3. 7.90 x 10 24 molecules of water into moles 4. 2.56 moles of sodium carbonate into molecules 5. 8.73 grams of beryllium bromide into molecules 6. 3.17 x 10 23 atoms of copper into grams of copper. 7. How many atoms of iron are there in 5.6 moles of iron (III) phosphate? 8. What is the mass of cobalt in 0.31 moles of cobalt (II) nitride?