1. How many eggs are there in 5 dozen? How many moles are in 2.25 grams of the element iron, Fe?

2. Standard: Utilize appropriate mathematical equations and processes to solve chemistry problems. 3221.Math.1 Objective: The learner will convert the amount of a substance by using molar conversions through dimensional analysis.

3. Introduction to the Mole

4. What is a mole? Mole – SI base unit used to measure the amount of a substance What is molar mass? Molar mass – the mass in grams of one mole of a substance (ex. hydrogen 1.0079g/mol) What is the conversion factor for molar mass? 1 mole= mass of an atom (mass number)

5. Grams to Moles 3.50 grams He = __________ mol He 20.0 g of oxygen = _________ mol oxygen How many moles are in 250.0 g of sodium?

6. Practice What is the number of moles found in 50.4 grams of Uranium? Calculate the number of moles of 80.850 g of nitrogen. Calculate the number of moles in 334 grams of lead.

7. Moles to Grams 6.0 moles carbon= __________ grams carbon 4.5 x 10 3 moles K = ___________ grams K Determine the mass in grams of 19.73 moles of the element boron, B.

8. 8.90 mol Ca = ___________ g Ca 2.8 mol Fe = ___________ g Fe 4.59 x 10 2 mol F = _____________ g F 6.000 mol S = ____________ g S

9. PROVE IT!!!!!!!

10. 5.68 g N= ___ mol N

11. 0.405 mol N

12. 0.0821 mol Rb= ___ g Rb

13. 7.02 g Rb

14. 3400 g O= ___ mol O

15. 210 mol O

16. 34.71 mol As= ___ g As

17. 2600. g As

18. Exit slip Determine the number of moles of 46.3 grams of the element, copper, Cu? Evaluate and explain in words how you solve this problem. Tell me step by step in complete sentences (4 to 5 sentences).

19. Homework What is the mass in grams of.375 mol of the element potassium, K. What is the mass in grams of 0.0135 mol of the element, sodium, Na? How many moles of gold, Au, are in 3.6 x 10 -10 g How many moles of copper, Cu, are in 3.22g of copper?

20. Standard: Utilize appropriate mathematical equations and processes to solve chemistry problems. 3221.Math.1 Objective: The learner will convert the amount of a substance by using Avogadro’s number through dimensional analysis.

21. Avogadro’s Number and Molar Conversions

22. Avogadro’s Number Avogadro was born in Italy from 1776-1865 His field of study was physics. He developed Avogadro’s number which is 6.022 x 10 23 6.022 x 10 23 = 1 mol

23. Moles to Avogadro’s Number 0.30 mol of F = ______ atoms F. 2.66 mol of N= ______ atoms N? How many atoms are in 4.2 mol O?

24. Avogadro’s Number to Moles 6.7 x 10 26 atoms of Zn= _______ moles Zn 1.69 x 10 23 atoms of V= _______ moles V? How many moles are in 3.29 x 10 21 atoms Al?

25. Practice Please !!!!!! 0.187 mol Ca = _________ atoms Ca How many atoms are in 1.45 x 10 -17 moles of As? 5.00 x 10 21 atoms of S = __________ moles S How many moles of neon are in 7.60 x 10 24 atoms?

26. PROVE IT!!!!!!!

27. 5.68gN=__mol N

28. 0.0821 mol Rb=__g Rb

29. 0.187molCa=__atoms Ca

30. 7.60 x 10 24 Ne atoms=___ moles Ne

31. Exit Slip How many moles are in 4.5 x 10 24 atoms of Ni? How many atoms are 78.94 moles of iodine?

32. HOMEWORK!!!!! Page 86 Practice Problems 1-3. Write the questions and show your work.

33. Standard: Utilize appropriate mathematical equations and processes to solve chemistry problems. 3221.Math.1 Objective: The learner will convert two step molar conversions. The learner will calculate the molecular weight of a compound, and apply it to molar conversions.

34. Entrance Slip Find the mass in grams of 3.012 x 10 24 atoms of Ca. The molar mass is 40.08 g/mol

35. Converting Grams to atoms Example: 1.Calculate the number of atoms in a 356 g sample of Ti? 2.Determine the number of atoms in 7.60 g of He. 3.841 g Mn = __________ atoms of Mn

36. Converting Atoms to Grams Example: 1.Find the mass in grams of 2.44 x 10 24 atoms of carbon, whose molar mass is 12.01 g/mol. 2.Find the mass in grams of 2.11 x 10 24 atoms of copper, whose molar mass is 63.55g/mol. 3.5.46 x 10 24 atoms Pb = __________g Pb

37. Mole Relay Race Student # 1- Read the problem and set the problem up for the correct number of steps. Student #2- Place the units in the set up. Student #3- Fill in the correct conversion factors. Student #4- Solve and write the answer with the correct number of sig. figs.

38. Exit Slip 4.06 x 10 24 atoms Cu = _______ g Cu 702 grams P = ________ atoms P

39. Molar Conversion 2- Step Homework 1. Determine the number of moles of fluorine in 9.23 x 10 -9 g of fluorine. 2. How many atoms of germanium are in 3.00 x 10 6 g Ge? 3. What is the mass in grams of 1.2 x 10 25 atoms of the element bromine, Br? 4.How many atoms of beryllium are in 1.67 x 10 3 g of Be? 5. What is the mass in grams of 9.70 x 10 23 atoms of magnesium, Mg?

40. Molecular Weight

41. What is the molecular weight of HCl?

42. Molecular weight Molecular weight – the mass in grams of one moles of a substance. (g/mol) What is the molecular weight of the following: NaCl H 2 O Ca(NO 3 ) 2 Mg(NO 3 ) 2

43. How many moles are in 67.68 grams of Al 2 S 3 ?

44. 345.0 grams of NaOH= ________ mol of NaOH 5.6 moles of HBr= _______ grams of HBr 200.5 grams of MgCl 2 = _______ mol of MgCl 2

45. 3.40 moles of Ti 2 O 3 = _____ grams of Ti 2 O 3 1.24 moles of AlN = _____ grams of AlN Determine the mass in grams of 89.0 moles of NaNO 3 ? 6.00 moles of B 2 (SO 4 ) 3 = ____ grams of B 2 (SO 4 ) 3

46. 4.5 moles SiCl 4 = _____ molecules SiCl 4 2.3 moles of CaS = _______ formula units CaS Determine the number of moles of F 2 in 5.6 x 10 23 molecules of F 2.

47. Exit Slip How many grams are in 8.9 moles of Li 2 O? How many molecules are in 5.90 moles of CO?

48. 267 grams of LiBr = ______ formula units LiBr 7.8 x 10 24 molecules of CO 2 = _____ grams of CO 2 149.0 grams of OF 2 = ______ molecules OF 2

49. HOMEWORK Determine the mass in grams of 89.0 moles of NaNO 3 ? 6.00 grams of B 2 (SO 4 ) 3 = ____ formula units of B 2 (SO 4 ) 3 7.8 x 10 24 formula units of Ba 3 P 2 = ____ moles of Ba 3 P 2 5.6 x 10 25 formula units V 3 (PO 4 ) 5 = _____ grams V 3 (PO 4 ) 5

50. Standard: Convert among the following quantities of a substance: mass, number of moles, and number of particles. Objective: The learner will review molar conversions.

51. Fine the molecular weight of potassium chlorate.

52. What is the mass in grams of 2.50 moles of oxygen, O 2 ?

53. Ibuprofen, C 13 H 18 O 2, is the active ingredient in many nonprescription pain relievers. Its molar mass is 206.31 g/mol. a. If the tablets in a bottle contain a total of 33 grams of ibuprofen, how many moles of ibuprofen are in the bottle? b. How many molecules are in the bottle? c. What is the total mass of carbon in 33 grams of ibuprofen?

54. How many moles are there in 6.60 grams of (NH 4 ) 2 SO 4 ? How many grams of nitrogen is in 6.60 grams of ammonium sulfate? How many grams of oxygen are in 6.60 grams of ammonium sulfate?

55. How many moles are in 4.5 kg of Ca(OH) 2 ? How many kilograms of calcium are in 4.5 kg of Ca(OH) 2 ? How many kilograms of hydrogen are in 4.5 kg of Ca(OH) 2 ?

56. Practice Problems How many grams of Al are in 43.8 g of Al 2 S 3 ? How many grams of chlorine are there in 0.35 moles of CH 2 Cl 2 ? What is the mass of chlorine in 3.36 grams of MgCl 2 ? What is the mass of phosphorus in 135.0 grams of K 3 PO 4 ? How many grams of nitrogen are in 2.01 moles of N 2 O 5 ?

57. Let’s RACE

58. Mole Relay Race 1. Read the problem and set the problem up for the correct number of steps. 3. Place the units in the set up. 4. Fill in the correct conversion factors. 5. Solve and write the answer with the correct number of sig. figs.

59. Exit Slip How many grams of phosphorus are in 1.02 moles of Ca 3 (PO 4 ) 2 ?

60. Homework How many grams of hydrogen are there in 4.5 g of Ca(OH) 2 ? How many grams of carbon are there in 3.4 grams of C 12 H 22 O 11 ? How many grams of nitrogen are in 0.35 moles of Cu(NO 3 ) 2 ?

61. Standard: Analyze ionic and covalent compounds in terms of percent composition. Objective: The learner will evaluate the percentage composition of atoms in chemical formulas.

62. In what subjects would you most likely use percentages?

63. Percentage Composition

64. What is percentage composition? the percent by mass of each element in a compound

65. Percentage Composition What is the equation for percentage composition? (Number of atoms of an element)(molar mass) X 100 = % of element Molecular weight of the compound in compound

66. Percentage Composition Example 1: Find the percentage composition of copper sulfide, Cu 2 S. Step 1: Write the equation. Step 2: Choose one element to solve. Step 3: Count the number of atoms that the element has. Substitute that number into the equation. Step 4: Find the molar mass of the element. Substitute that number into the equation. Step 5: Calculate the molecular weight of the compound. Substitute that number into the equation. Step 6: Solve Step 7: Check your work by adding the percentages. Your final answer should be at least 100%

67. Problem Calculate the percentage composition of the (NH 4 ) 2 CO 3. Calculate the percentage composition of sodium nitrate, NaNO 3. Calculate the percentage composition of calcium hydroxide, Ca(OH) 2

68. Rally Coach

69. Student 1: Will write the problem and the equation used to solve percentage composition. Student 2 and 3: Will perform the steps to solving the problem. Student 4: Will check the problem and write it on the board. Student 5: Will present the problem to the class. In the presentation explain each step.

70. Group 1: Calculate the percentage composition of Ag 2 SO 4. Group 2: Calculate the percentage composition of Cu(NO 3 ) 2. Group 3: Calculate the percentage composition of NaCl. Group 4: Calculate the percentage composition of FeSO 3. Group 5: Calculate the percentage composition of CaCO 3. Group 6: Calculate the percentage composition of H 2 S. Group 7: Calculate the percentage composition of MgF 2.

71. Student A: Calculate the percentage composition of Ag 2 SO 4. Student B: Calculate the percentage composition of Cu(NO 3 ) 2.

72. Exit Slip Calculate the percentage composition of Al 2 S 3.

73. Classwork Write the statement. FIVE POINTS will be deducted is the statements are not written. TEN POINTS will be deducted if work is not shown. Calculate the percentage composition of SrBr 2. Calculate the percentage composition of CaSO 4. Calculate the percentage composition of Mg(CN) 2. Calculate the percentage composition of Pb(NO 3 ) 2. Calculate the percentage composition of Fe(MnO 4 ) 3.

74. Standard: Convert percentage composition into an empirical formula. Objective: The learner will investigate empirical formulas.

75. Empirical Formula

76. Formulas and Percentage Composition Empirical formulas- a chemical formula that shows the composition of a compound. (ratios of atom)

77. Determine Empirical Formulas from Percentage Composition 1.Percent to mass (grams)-Assume that you have 100g of the substance. 1.Mass (grams) to mole 1.Divide by the least number of moles. 1.Multiply 'til whole

78. Determine Empirical Formulas from Percentage Composition. Example 1.Chemical analysis of a liquid shows that it is 60.0% C, 13.4 %H, and 26.6% O by mass. Calculate the empirical formula of this substance. 2.A dead alkaline battery is found to contain a compound of Mn and O. Its analysis gives 69.6% Mn and 30.4% O.

79. Determine Empirical Formulas from Percentage Composition. 1. A compound is 38.77% Cl and 61.23% O. 2. A liquid compound is 18.0 % C, 2.26% H, and 79.7% Cl.

80. Determine Empirical Formulas from Percentage Composition Exit Slip. 1. A compound contains 5.88% hydrogen and 94.12% oxygen. What is the empirical formula?

81. Determine Empirical Formulas from Percentage Composition Homework. 1. A compound is made up of 92.3% carbon and 7.7% hydrogen. What is the empirical formula? 2. A compound contains 70.0% iron and 30.0% oxygen. What is the empirical formula?

82. Standard: Convert empirical formulas to molecular formulas. Objective: The learner will investigate molecular formulas.

83. Molecular Formula

84. Determine Molecular Formulas from Empirical Formula. Molecular formula- a chemical formula that shows the number and kinds of atoms in a molecule. Steps 1.Write the information that is given. 2.Find the molar mass of the empirical formula. 3.Solve using this formula. n= experimental molar mass of compound molar mass of empirical formula 4. Multiply the empirical formula by n to get the molecular formula.

85. Determine Molecular Formulas from Empirical Formula. Example: The empirical formula for a compound is P 2 O 5. Its experimental molar mass is 284 g/mol. Determine the molecular formula of the compound. Determine the molecular formula of a compound with an empirical formula of NH 2 and a molar mass of 32.06 g/mol.

86. Determine Molecular Formulas from Empirical Formula. Example: A sample with a formula mass of 34.00 g/mol is found to consist of 0.44g H and 6.92g O. Find its molecular formula. A compound with formula mass of 42.08 g/mol is found to be 85.64% carbon and 14.36% hydrogen by mass. Find its molecular formula.

87. Determine Molecular Formulas from Empirical Formula. A compound has an experimental molar mass of 78 g/mol. Its empirical formula is CH. What is its molecular formula? A compound has the empirical formula CH 2 O. Its experimental molar mass is 90.0 g/mol. What is its molecular formula? If 4.04g of N combine with 11.46g O to produce a compound with a formula mass of 108.0 g/mol, what is the molecular formula of this compound?

88. Determine Molecular Formulas from Empirical Formula. Exit Slip Determine the molecular formula of a compound with an empirical formula of C 2 H 4 S and a formula mass of 179 g/mol.