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

22. 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

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

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

25. Polyatomic Ion

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

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

28. Drill: Name each CuCl 2 KBr PCl 5 MgO Mn 2 O 7 S 2 O 3

29. Naming Polyatomic Ions

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

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

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

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

34. Naming Ternary Compounds

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

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

37. CaCO 3 K 2 SO 4 Name Each:

38. Pb(NO 3 ) 2 MgSO 3 Drill: Name:

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

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

41. Naming Acids

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

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

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

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

46. Name or Give Formulas For: HBr (aq) H 2 SO 4(aq) NaVO 3 (NH 4 ) 3 PO 3 Phosphoric acid Nitric acid Chloric acid

47. Drill: Name each: KBrMgS BaF 2 K 3 P K 2 OLiH Al 2 O 3 H 2 S

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

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

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

51. 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

52. Derive formulas for each: ChromateSulfate ArsenateNitrate ArseniteCyanide BromiteAcetate

53. 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

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

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

56. Percent Composition by Mass

57. 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 %

58. 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 %

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

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

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

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

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

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

65. 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

66. 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

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

68. 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