1. Drill: Calculate the % composition of each element in H4N2O3

2. Return Tests & Review Drill & Test

3. 4 H = sum 2 N = = O = 48.0
% H = 4.0/80.0 x 100 % = % H
% N = 28.0/80.0 x 100 % = % N
% O = 48.0/80.0 x 100 % = % O

4. Name each of the following:
CuO MnS
SeO2 Na2O
SnCl2 MnF2
HClO3 CCl4

5. Anyone who missed or failed the test may retake a similar test within a week to bring the grade up to 60.

6. Collect Labs

7. CHM II HW
Review PP 06
Work the problems attached to Poly’s website.

8. Are there any questions on previous material?

9. Molar Conversions

10. The standard unit of measure for the amount of a substance
Moles
The standard unit of measure for the amount of a substance

11. Dozen
= 12 of anything

12. Moles
= x 1023 of anything

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

14. Describe the factor label method of conversions

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

16. Atoms or
molecules
mass
moles
volume
of a gas
solution
volume

17. Moles First

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

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

20. Particles to Moles Use Avogadro’s Number
6.02 x 1023 atoms, molecules, etc/mole

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

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

23. Convert 7.0 g of silicon to moles

24. Convert 250 g of CaCO3 to moles

25. Convert 3.0 moles of helium to grams

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

27. Convert 0.20 moles of helium to volume at STP

28. Convert: 2.0 x 1024 atoms He to moles

29. Drill: Convert 3.0 moles of glucose to molecules

30. Review & Collect Drill & HW

31. CHM II HW Review PP-6 Work the attached problem & turn it in on Monday
We will have a lab on Friday.

32. Are there any questions on previous material?

33. Convert 250 mL of 0.10 M HCl to moles

34. 6.8 g NH3 to volume of gas at STP
Convert
6.8 g NH3 to volume of gas at STP

35. Drill: Determine the volume required to make 60. 0 g NaOH into a 0
Drill: Determine the volume required to make 60.0 g NaOH into a 0.75 M solution

36. Review & Collect Drill & HW

37. CHM II HW
Review PP-6
Complete the attached assignment & turn it in tomorrow.

38. Are there any questions on previous material?

39. 3.0 x 1025 molecules of CO2 to mass in kg
Convert
3.0 x 1025 molecules of CO2 to mass in kg

40. Drill: Calculate the number molecules in 32 mg of Fe2O3

41. Calculate the number of atoms in 16 ng of Fe2(SO4)3

42. Empirical Formula

43. Lowest whole number ratio of elements in a compound
C6H12O6: EF = CH2O

44. Determining Empirical formulas from percent composition

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

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

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

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

49. Molecular Formula

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

51. Molecular Formula C6H12O6 Empirical Formula CH2O

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

54. Drill: Calculate the mass of solute required to make 40. 0 mL of 0
Drill: Calculate the mass of solute required to make 40.0 mL of 0.25 M Pb(NO3)2

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

56. Calculate the % composition of each element in Pb(NO3)2

57. Calculate the empirical formula of a substance containing 62
Calculate the empirical formula of a substance containing 62.7 % Po, 28.8 % O,
& 8.4 % N.

58. Calculate the molecular formula of a substance with an empirical formula of NH2 & a molecular mass of 32 g/mole.

59. Name each of the following:
SeO MgS
PbO2 Cl2O
KNO3 ScCl3

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

61. Name each of the following:
NH4Cl BaSO4
KC2H3O2 K2HPO3
KNO3 CuBrO
Li2CO3 MgC2O4

62. Name each of the following:
HCl H2SO4
H2S H3PO3
HNO3 HBrO
H2CO3 HBrO4

63. Calculate the number of hydrogen atoms in 1.8 kg of PH5.

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

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