1. Nomenclature Naming Compounds

2. Binary Compounds

3. Compounds with only two elements in any ratio

4. KClNO 2 CaCl 2 P 2 O 5 Al 2 O 3 H 2 S Na 2 Oetc

5. Binary compounds can be either ionic or covalent

6. Naming Binary Compounds

7. Naming Ionic Compounds

8. Name positive element first with its normal name Name negative element last & change its ending to -ide

9. KCl CaCl 2 Al 2 O 3 Na 2 O

10. Name Each: CaCl 2 CaS K 2 OLiF

11. Name Each: FeCl 2 FeCl 3

12. If the Positive element is not from columns I or II its ox # must be determined and written in roman numerals

13. Determining the Charge 1)Add up the oxidation numbers of all the negative elements 2)The positive portion must balance out the negative portion 3)Divide the positive portion by the metal subscript

14. CuClFe 2 O 3 MnO 2 CrO 3 Name Each:

15. Molecule

16. A covalent compound that can exist as a separate unit Non-metals bond to form molecules

17. Naming Molecules or Covalent Compounds

18. Same rules as ionic compounds except: use geometric prefixes to determine the # of each atom

19. Geometric Prefixes 1-mono5-penta 2-di6-hexa 3-tri7-hepta 4-tetraetc

20. COS 2 O 3 N 2 H 4 SO 3 Name Each:

21. Nomenclature HW Work problems: 49 - 54 on page 51

22. CaOP 2 O 5 Al 2 S 3 SO 2 Drill: Name Each:

23. Deriving Formulas 1)Write the symbol for each element 2)Determine ox #s for each 3)Determine lowest common multiple to balance the charge 4)Apply subscripts

24. Write formulas for: Sodium sulfide Lead (II) iodide Diphosphorus pentoxide

25. Write formulas for: Chromium(III) oxide Aluminum carbide

26. Polyatomic Ion

27. A group of atoms chemically combined that together have a charge

28. Most are oxoanions PO 4 -3 SO 4 -2 A root element bound to oxygen

29. Naming Polyatomic Ions

30. Learn the polyatomic table on page 42 & 43 Learn how to use the periodic table to determine polyatomic ions

31. Name the root element Change the ending to -ate PO 4 -3 = phosphate Some are unusual

32. CN -1 OH -1 C 2 H 3 O 2 -1 C 2 O 4 -2

33. H 2 O H 3 O +1 NH 3 NH 4 +1

34. Polyatomic Ion Endings Maximum O = -ate 1 less than max O = -ite SO 4 -2 = sulfate SO 3 -2 = sulfite

35. Naming Ternary Compounds

36. Ternary Compounds Compounds containing more than two different elements Most contain polyatomic ions

37. Follow ionic rules for naming the compound Name the polyatomic ion as the positive or negative portion

38. CaCO 3 K 2 SO 4 Name Each:

39. Pb(NO 3 ) 2 MgSO 3 Name Each:

40. Write Formulas For: Lead (II) nitrate Aluminum sulfate Potassium chlorate Ammonium phosphite

41. Name the Following: BaSO 4 CuNO 3 SO 2 (NH 4 ) 3 PO 4

42. Naming Acids

43. Binary acids become: Hydro _____ ic acids HCl - Hydrochloric acid

44. Ternary acids become: _____ ic acids or _____ ous acids H 2 SO 4 - Sulfuric acid H 2 SO 3 - Sulfurous acid

45. ____ ic acids form from polyatomic ions ending with ___ ate ____ ous acids form from polyatomic ions ending with ___ ite

46. ___ ide ions become: hydro ___ ic acids ___ ate ions become: ___ ic acids ___ ite ions become: ___ ous acids

47. Percent Composition by Mass

48. Determine the atomic mass of each element in the compound Determine the molecular mass of the compound by adding Divide each elemental mass by molecular mass Multiply by 100 %

49. MgCl 2 Mg = 24.3 g/mole 2 Cl = 2 x 35.5 = 71.0 g/mole MgCl 2 = total = 95.3 g/mole % Mg =24.3/95.3 x 100% % Cl = 71.0/95.3 x 100 %

50. Determine % Comp for Each: Fe 2 O 3 C 3 H 6 O 3 CuSO 4 *5H 2 O

51. Empirical Formula

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

53. Determining Empirical formulas from percent composition

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

55. Substance = 30 % O & 70 & Fe 30 % O --> 30 g O & 70 % Fe --> 70 g Fe 30/16 = 1.875 moles O 70 / 56 = 1.25 moles Fe 1.25/1.25 = 1 & 1.875/1.25 = 1.5 Ratio = 1.5 : 1 x 2 = 3 : 2 Empirical Formula Fe 2 O 3

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

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

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

59. Molecular Formula

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

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

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

63. Name each of the following: KBrMgS BaF 2 K 3 P K 2 OLiH Al 2 O 3 H 2 S

64. Name each of the following: FeO Fe 2 O 3

65. Name each of the following: CuOMnS PbO 2 Cu 2 O CrCl 2 MnF 2 CrCl 3 SnCl 4

66. Name each of the following: SeOCS 2 NO 2 Cl 2 O N 2 O 4 PCl 3

67. Derive formulas for each: Cesium oxide Barium chloride Calcium phosphide Aluminum sulfide

68. Derive formulas for each: Lead(IV)oxide Copper(II)sulfide Manganese(VII)oxide Nickel(II)fluoride

69. Name each of the following: SO 4 -2 SO 3 -2 PO 4 -3 NO 3 -1 ClO 4 -1 ClO 3 -1 ClO 2 -1 ClO -1

70. Derive formulas for each: Chromate Arsenate Arsenite Bromite

71. Name each of the following: BaCO 3 KNO 2 CuClO 3 Al 2 (SO 4 ) 3

72. Derive formulas for each: Potassium sulfate Lead(II)chromate Aluminum hydroxide Ammonium cyanide

73. Name each of the following: Cl 2 OSO 2 N 2 O 3 P 2 O 5 CO 2 CO SO 3 N 2 H 4

74. Derive formulas for each: Silicon dioxide phosphorus trichloride Sulfur hexafluoride Iodine trifluoride

75. 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

76. 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

77. Derive formulas for each: Chromic acid Hydroiodic acid Sulfurous acid Bromic acid

78. Name each of the following: KClMnSO 4 SO 2 HI (aq) NaNO 3 HClO H 2 CO 3(aq) NH 4 BrO 4

79. Name each of the following: NaCl MnSO 4 S 2 O 3 HBr (aq) Na 2 CO 3 HClO HNO 3(aq) NH 4 IO 4

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

81. Nomenclature Work problems 43 – 56 On Pages 51 & 52