1. Drill: Calculate the % composition of each element in Fe 2 (SO 4 ) 3

2. Molar Conversions

3. Moles The standard unit of measure for the amount of a substance in numbers

4. Dozen = 12 of anything

5. Moles = the amount of a substance that would = its mass in g from the PT

6. Moles = 6.022 x 10 23 of anything

7. Molar Conversions Mass to moles Volume of a gas to moles Particles to moles Volume of a solution to moles

8. Moles First

9. Mass to Moles Use atomic masses from the periodic table NaCl = 58.5 g/mole

10. Gas Volume to Moles At STP: 22.4 L/mole Non-STP: PV = nRT PV RT n =

11. Particles to Moles Use Avogadro’s Number 6.02 x 10 23 atoms, molecules, etc/mole

12. Soln Volume to Moles Multiply molarity times volume n = M x V

13. Solution Measures Molarity (M) = the number of moles of solute per liter of solution Others later

14. Convert 7.0 g of silicon to moles

15. Convert 250 g of CaCO 3 to moles

16. Convert 3.0 moles of helium to grams

17. Convert 11.2 L of oxygen gas at STP to moles

18. Convert 0.20 moles of helium to volume at STP

19. Convert: 2.0 x 10 24 atoms He to moles

20. Convert 3.0 moles of glucose to molecules

21. Convert 250 mL of 0.10 M HCl to moles

22. Drill: Determine the volume required to make 60.0 g NaOH into a 0.75 M solution

23. Convert 6.8 g NH 3 to volume of gas at STP

24. Convert 3.0 x 10 25 molecules of CO 2 to mass in kg

25. Drill: Calculate the number molecules in 32  g of Fe 2 O 3

26. First Test Next Thursday on nomenclature, molar conversions, & reactions.

27. Calculate the number of atoms in 16 ng of Fe 2 (SO 4 ) 3

28. Empirical Formula

29. Lowest whole number ratio of elements in a compound C 6 H 12 O 6 : EF = CH 2 O

30. Determining Empirical formulas from percent composition

31. Assume 100 g Change % directly to grams Use molar conversions to convert grams to moles Divide each molar amount by the smallest molar amount

32. Find empirical for a compound with: 70.0 % Fe 30.0 % O

33. Find empirical for a compound with: 40 % Ca 12 % C 48 % O

34. Find empirical for a compound with: 40.0 % C 6.7 % H 53.3 % O

35. Molecular Formula

36. The actual whole number for each element in the compound

37. Molecular Formula C 6 H 12 O 6 Empirical Formula CH 2 O

38. Solving MF from EF 1) Solve empirical mass 2) Divide EM into MM 3) Multiply EF by quotient

40. Drill: Calculate the mass of solute required to make 40.0 mL of 0.25 M Pb(NO 3 ) 2

41. Test Review on Nomenclature, Molar conversions, & % Composition.

42. Calculate the % composition of each element in Pb(NO 3 ) 2

43. Calculate the empirical formula of a substance containing 62.7 % Po, 28.8 % O, & 8.4 % N.

44. Calculate the molecular formula of a substance with an empirical formula of NH 2 & a molecular mass of 32 g/mole.

45. Name each of the following: SeOMgS PbO 2 Cl 2 O KNO 3 ScCl 3

46. Derive formulas for each: Cesium oxide Barium chloride Calcium phosphate Manganese(II) chlorate

47. Name each of the following: NH 4 ClBaSO 4 KC 2 H 3 O 2 K 2 HPO 3 KNO 3 CuBrO Li 2 CO 3 MgC 2 O 4

48. Name each of the following: HClH 2 SO 4 H 2 S H 3 PO 3 HNO 3 HBrO H 2 CO 3 HBrO 4

49. Calculate the number of hydrogen atoms in 1.8 kg of PH 5.

50. Calculate the volume at STP of 6.0 ng of NO.

51. Calculate the mass of KBr required to make 250 mL of a 0.40 M solution.

52. Chapter 3 General Define all the Key Terms on page 74

53. Atomic Mass Work problems: 1 - 9 on page 75

54. Avogadro’s Num. Work problems: 11 - 18 on page 75

55. Molar Conversions Work problems: 18 - 26 on page 75 & 76

56. % Composition Work problems: 27 - 34 on page 76

57. Empirical Formula Work problems: 35 - 46 on page 76 & 77

58. Balancing Rxns Work problems: 49 & 54 on page 77

59. Stoichiometry Work problems: 55 & 64 on page 77 & 78

60. Limiting Reactant Work problems: 65 & 74 on page 78 & 79