Chapter 11 Outline – The Mole I. Measuring Matter (section 11.1) A. Counting Particles Q: How many do the following counting units equal? What would they be used to count? A: unit # it means example Dozen Pair Trio Six-pack Ream Gross Q: What is a mole? A: In one mole of ANYTHING, there are 6.02 x 1023 representative particles ( atoms, molecules, formula units, ions) WOW, that is a lot. Let’s make sure we understand. o 1 mole of pizza = o 1 mole of cotton = o 1 mole of water = o 1 mole of gold = Avogadro’s number = Q: Who was Amedeo Avogadro? A: Q: What is the difference between a molecule, atom, and formula unit? p. 310 Fig. 11-2 A: molecule = atom = formula unit = B. Converting Moles to Representative Particles and Representative Particles to Moles Q: What is a conversion factor? A: Show an example 1. Convert Moles to Representative Particles 1 mole = representative particles (atoms or molecules or formula units) Q: How many molecules are in 4.2 moles of glucose (C6H12O6) Do Practice Problems p. 311 # 1-3 1. 2. 3. 2. Convert representative particles to moles Use the exact same method a converting moles to representative particles, just use the inverse of the conversion factor. Do Practice Problems p. 312 # 4 4. a. b. c. d. II. Mass and the Mole (section 11.2) A. The Mass of a Mole Q: What is the difference between atomic mass and mass number? A: atomic mass= Mass number = Define molar mass = Molar mass is numerically equal to the . Let’s Practice: Element atomic mass molar mass C Sb Br How easy, the molar mass is the same # as the atomic mass on the periodic table. BUT, with units of g/mol not amu. Molar mass of compounds (section 11.3) Add up the masses from the periodic table for each atom of each element. Let’s Practice: 1. molar mass of glucose, C6H12O6 = 2. molar mass of carbon dioxide = Do Practice Problems p. 322 #25 25. B. Using Molar Mass Read p. 314-315 1. Use molar mass to convert moles to mass(grams) and mass to moles Ex. How many grams of gold are in .215 moles of gold? Step 1: determine the molar mass of the element (this is the conversion factor) Step 2: start with what was given Step 3: Plug in the conversion factor (molar mass) Do Practice Problems p. 316 #11 11 a. b. c. d. Do Practice Problems p. 316 #12 12 a. b. c. d. Do Practice Problems p. 323 # 27-29 27. 28. 29. Do Practice Problems p. 324 # 30a-d 30 a. b. c. d. 2. Convert mass to atoms (massmoles atoms) Step 1: must convert mass to moles FIRST. Step 2: once you have moles, convert to atoms using Avogadro’s # as your conversion factor. Conversion factor = Ex. How many atoms of NH3 are in 62 g of NH3 Convert mass moles Convert moles atoms You can do this all in one problem. Do Practice Problems p. 318 #13 a-d 13 a. b. c. d. 3. Convert atoms to mass (atomsmoles mass) Same as mass to atoms, just in reverse. Do Practice Problems p. 318 #14 a-d 14 a. b. c. d. SUMMARY Converting: 1. moles representative particles (i.e. atoms, molecules, formula units) given moles x 6.02 x 10 23 representative particles 1 mole 2. moles mass (grams) given moles x molar mass (g) 1 mol 3. mass(grams) moles given mass (g) x 1 mol . molar mass (g) 4. mass (grams) atoms (mass moles atoms) given mass (g) x 1 mol x molar mass (g) x 6.02 x1023 atoms 1 mol 5. atoms mass (grams) (atoms moles mass) given atoms III. x 1 mol x 6.02 x 1023 atoms x Moles of Compounds (section 11.3) A. Chemical Formulas and the Mole 1. The subscript tells you how many mole of the compound. molar mass (g) 1 mol of atoms are in 1 Ex. In 1 mol C6H12O6 there are 6 moles of C atoms. In 1 mol C6H12O6 there are of H atoms In 1 mol C6H12O6 there are of O atoms Write each of the above as a ratio (conversion factor) These would be then called mole ratios. 2. Using mole ratios (convert moles moles) Ex. Determine the # of moles of C in 3 mol of sucrose ( C12H22O11) Step 1: determine the mole ratio Step 2: start with the given Step 3: plug in the mole ratio (conversion factor), solve Do Practice Problems p. 321 # 20-22 20. 21 22. B. Convert the Mass of a Compound to Representative Particles (mass moles representative particles) Ex.