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. Calculate the atomic mass of the element made up of the following isotopes: 99.50 % H-1 0.30 % H-2 0.20 % H-3

15. Calculate the atomic mass of the element made up of the following isotopes: 5.0 % Pu-242, 5.0 % Pu-243 80.0 % Pu-244, & 10.0 % Pu-245

16. Convert 7.0 g of silicon to moles

17. Convert 250 g of CaCO 3 to moles

18. Convert 3.0 moles of helium to grams

19. Convert 5.6 L of oxygen gas at STP to moles

20. Convert 0.50 moles of helium to volume at STP

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

22. Convert 3.0 moles of glucose to molecules

23. Convert 250 mL of 0.10 M HCl to moles

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

25. Convert 6.8 g NH 3 to volume at STP

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

27. Calculate the number of oxygen atoms in 32  g of Fe 2 O 3

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

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

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

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

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

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

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

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

36. 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

37. 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

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

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

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

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

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

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

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

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

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

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

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

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