1. The Mole-just as a _____ is always ____, a _______ is always _______, a ______ is always ____, and a _____ is always ____, a _____ is always ____________________________, or __________, and just like it is sometimes easier to buy things by the _______ or by the _____, it is sometimes easier to consider numbers of _________ of _______ by the _____ pairtwodozentwelve gross144ream500 mole602,000,000,000,000,000,000,000 6.02 x 10 23 dozenream particlesmattermole I. Converting Moles to Particles and Particles to Moles How many eggs in 4½ dozen? 4.5 dozenx 12 eggs ________ 1 dozen How do we simplify when we multiply fractions? 3 x __ 4 8 9 = 24 36 = 2__ 3 or 3 x __ 4 8 9 = 2 3 1 31 2 =54 eggs __ conversion factor

2. The Mole I. Converting Moles to Particles and Particles to Moles How many molecules in 4.5 moles of sucrose? 4.5 moles sucrosex 6.02 x 10 23 molecules sucrose _________________________ 1 mole sucrose =2.7 x 10 24 molecules sucrose conversion factor How many moles in 1.75 x 10 25 molecules of water? 1.75 x 10 25 molecules H 2 Ox 6.02 x 10 23 molecules H 2 O _________________________ 1 mole H 2 O =29.1 moles H 2 O 2 significant figures 3 significant figures 2 significant figures

3. The Mole II. Molar Mass-the _______ of ______ are established ________ to the mass of one __________ atom, which has ____ _________ and ____ __________ massesatomsrelative Carbon -12six protonssixneutrons -____-________ of the mass of a __________ atom, or about the mass of a _______ or a ________, is called an _______ _____ _____, or _____ onetwelfthCarbon -12 protonneutron atomicmassunitamu -the ______ _____ is the _____ of one _____ of an element, and is numerically equal to the ________ _____, but with units of ______ per _____, so the _______ _____ of a Carbon-12 atom is ___ ____, and the ______ _____ of Carbon-12 is ___ ______ per _____ molarmass mole atomic massgramsmole mass12amuatomic molarmass12grams mole

4. A. Converting Mass to Moles and Moles to Mass The Mole II. Molar Mass What is the mass of 0.415 moles of Vanadium? 0.415 moles Vx 50.942 grams V _______________ 1 mole V =21.1 grams V 3 significant figures 5 significant figures 3 significant figures How many moles of Tantalum are in 75 grams of Tantalum ? 75 grams Tax 180.948 grams Ta _______________ 1 mole Ta =0.41 grams V 2 significant figures 6 significant figures 2 significant figures

5. The Mole A. Converting Mass to Atoms and Atoms to Mass II. Molar Mass How many atoms are there in 99.838 g Uranium? 3 significant figures 99.838 g Ux 1 mole U _______________ 238.029 g U =2.525 x 10 23 atoms U 5 significant figures 3 significant figures 6.02 x 10 23 atoms U _______________ 1 mole U x 6 significant figures 2.52 x 10 23 atoms U= What is the mass, in grams, of 1.1703 x 10 24 atoms of Niobium? 4 significant figures 1.1703 x 10 24 atoms Nbx 1 mole Nb _______________ 6.022 x 10 23 atoms Nb =1.8055 x 10 2 g Nb 5 significant figures 92.906 g Nb _______________ 1 mole Nb x 4 significant figures 1.806 x 10 2 g Nb=

6. The Mole A. Converting Mass to Molecules and Molecules to Mass II. Molar Mass How many molecules are there in 456 g Silicon dioxide? 456 g SiO 2 x 1 mole SiO 2 _______________ 60.084 g SiO 2 =4.57 x 10 24 molecules SiO 2 6.02 x 10 23 molecules SiO 2 _______________ 1 mole SiO 2 x What is the mass, in grams, of 1.75 x 10 26 molecules of cyclohexane? 1.75 x 10 26 molecules C 6 H 12 x 1 mole C 6 H 12 _______________ 6.02 x 10 23 molecules C 6 H 12 =2.45 x 10 4 g C 6 H 12 84.162 g C 6 H 12 _______________ 1 mole C 6 H 12 x

7. The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition What is the percent composition of Sodium, Sulfur, and Oxygen in Sodium Sulfate? 22.990 g Na 1 mole Na 2 moles Nax=45.98 g Na 32.065 g Na 1 mole S x=32.065 g S 15.999 g O 1 mole O 4 moles Ox=63.996 g O 142.0 g Na 2 SO 4 x100 x x = = = 32.38% 22.58% 45.07%

8. The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition What is the percent composition of Carbon, Hydrogen, and Oxygen in fructose, C 6 H 12 O 6 ? 12.011 g C 1 mole C 6 moles Cx=72.066 g C 1.008 g H 1 mole H 12 moles Hx=12.10 g H 15.999 g O 1 mole O 6 moles Ox=95.994 g O 180.2 g C 6 H 12 O 6 x100 x x = = = 39.99% 6.715% 53.27%

9. The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for Ibuprofen if the molar mass is 206 g/mole and the percent composition of 75.7% C, 8.80% H, and 15.5% O? 12.011 g C 1 mole C75.7 g Cx=6.30 moles C 1.008 g H 1 mole H8.80 g Hx=8.73 moles H 15.999 g O 1 mole O15.5 g Ox=0.969 moles O -the empirical formula is the lowest whole number mole ratio of elements in a compound 0.969 =1.00 mole O =9.01 moles H =6.50 moles CEmpirical Formula = C 13 H 18 O 2 Molecular Formula = C 13 H 18 O 2 Molar mass of Empirical Formula Molar mass of Ibuprofen

10. The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for Glycerol if the molar mass is 92.11 g/mole and the percent composition of 39.12% C, 8.75% H, and 52.12% O? 12.011 g C 1 mole C39.12 g Cx=3.257 moles C 1.008 g H 1 mole H8.75 g Hx=8.68 moles H 15.999 g O 1 mole O52.12 g Ox=3.257 moles O -the empirical formula is the lowest whole number mole ratio of elements in a compound 3.257 =1.000 mole O =2.66 moles H =1.000 moles CEmpirical Formula = C 3 H 8 O 3 Molecular Formula = C 3 H 8 O 3 Molar mass of Empirical Formula Molar mass of Glycerol 92.09 g/mole C 3 H 8 O 3 92.11 g/mole C ? H ? O ?

11. The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for Naphthalene if the molar mass is 128 g/mole and the percent composition of 93.7% C and 6.3% H? 12.011 g C 1 mole C93.7 g Cx=7.80 moles C 1.008 g H 1 mole H6.3 g Hx=6.25 moles H -the empirical formula is the lowest whole number mole ratio of elements in a compound 6.25 =1.00 moles H =1.25 moles CEmpirical Formula = C 5 H 4 Molecular Formula = C 10 H 8 Molar mass of Empirical Formula Molar mass of Naphthalene 64.09 g/mole C 5 H 4 128 g/mole C ? H ?

12. The Mole III. Empirical and Molecular Formulas B. Determining Empirical Formula from Percent Composition What are the empirical and molecular formulas for a Lead chloride compound if the molar mass of the compound is 349.0 g/mole and the percent composition is 59.37% Pb? 207.2 g Pb 1 mole Pb59.37 g Pbx=0.2865 moles Pb 35.453 g Cl 1 mole Cl40.63 g Clx=1.146 moles Cl -the empirical formula is the lowest whole number mole ratio of elements in a compound 0.2865 =4.00 moles Cl =1.000 moles PbEmpirical Formula = PbCl 4 Molecular Formula = PbCl 4 Molar mass of Empirical Formula Molar mass of Lead chloride 349.0 g/mole PbCl 4 349.0 g/mole Pb ? Cl ?

13. The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition-lab 1. Hypothesis-How does the mass of chewed bubblegum compare to the mass of chewed bubblegum? 2. Prediction 3. Gathering Data -safety a. Carefully unwrap one piece of bubblegum. Using the wrapper as weighing paper, place the unchewed gum on the top-loading balance to determine and record its mass to the nearest 0.1 gram. _____________ g. Save the wrapper. b. Chew the bubblegum for 5 minutes. - procedure a. Carefully avoid contaminating the unchewed gum on any surface before chewing

14. The Mole III. Empirical and Molecular Formulas A. Calculating Percent Composition-lab 3. Gathering Data c. After chewing for 5 minutes, remove the gum from mouth and, using the wrapper as weighing paper again, carefully place the wad of chewed gum on the top-loading balance to determine and and record its mass to the nearest 0.1 gram. _______________ g -procedure 4. Analyzing Data mass of chewed gum mass of unchewed gum x100=percent composition -calculate the percent composition of bubblegum x100=_________% 5. Drawing Conclusions

15. The Mole IV. Hydrates A. Naming Hydrates -hydrates are __________ that have a specific number of ______ molecules attached to them compounds water FormulaName (NH 4 ) 2 C 2 O 4 ·H 2 O CaCl 2 ·2H 2 O NaC 2 H 3 O 2 ·3H 2 O FePO 4 ·4H 2 O CuSO 4 ·5H 2 O CoCl 2 ·6H 2 O MgSO 4 ·7H 2 O Ba(OH) 2 ·8H 2 O Na 2 CO 3 ·10H 2 O Ammonium oxalate monohydrate Calcium chloride dihydrate Sodium acetate trihydrate Iron(III) phosphate tetrahydrate Copper(II) sulfate pentahydrate Cobalt(II) hexahydrate Magnesium sulfate heptahydrate Barium hydroxide octahydrate Sodium carbonate decahydrate

16. The Mole IV. Hydrates B. Calculating the Formula for a Hydrate What is empirical formula and for a hydrated compound of Copper(II) sulfate, if 2.50 grams of blue CuSO 4 ·nH 2 O is heated in a crucible until 1.59 grams of white anhydrous CuSO 4 remains ? 159.6 g CuSO 4 1 mole CuSO 4 1.59 g CuSO 4 x=0.00996 moles CuSO 4 18.02 g H 2 O 1 mole H 2 O0.91 g H 2 Ox=0.050 moles H 2 O 0.00996 =5.0 moles H 2 O =1.00 moles CuSO 4 Empirical Formula = CuSO 4 ·5H 2 O Mass of hydrated Copper(II) sulfate - 2.50 g 1.59 gMass of anhydrous Copper(II) sulfate 0.91 g Copper(II) sulfate pentahydrate