1. Nomenclature
Naming
Compounds

2. Binary Compounds

3. Compounds with only two elements in any ratio

4. KCl NO2
CaCl2 P2O5
Al2O3 H2S
Na2O etc

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 CaCl2 Al2O3 Na2O

10. Name Each:
CaCl2 CaS
K2O LiF

11. Name Each:
FeCl2
FeCl3

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
Add up the oxidation numbers of all the negative elements
The positive portion must balance out the negative portion
Divide the positive portion by the metal subscript

14. Name Each:
CuCl Fe2O3 MnO2 CrO3

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-mono 5-penta 2-di 6-hexa 3-tri 7-hepta
4-tetra etc

20. Name Each:
CO S2O3 N2H4 SO3

21. Nomenclature HW
Work problems:
on page 51

22. Drill: Name Each:
CaO P2O5 Al2S3 SO2

23. Deriving Formulas Write the symbol for each element
Determine ox #s for each
Determine lowest common multiple to balance the charge
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
PO4-3 SO4-2
A root element bound to oxygen

29. Drill: Name each
CuCl2 KBr
PCl5 MgO
Mn2O7 S2O3

30. Naming Polyatomic Ions

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

32. Name the root element
Change the ending
to -ate
PO4-3 = phosphate
Some are unusual

33. CN-1 OH-1
C2H3O2-1 C2O4-2

34. H2O H3O+1 NH3 NH4+1

35. Polyatomic Ion Endings
Maximum O = -ate
1 less than max O = -ite
SO4-2 = sulfate
SO3-2 = sulfite

36. Naming Ternary Compounds

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

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

39. Name Each:
CaCO3 K2SO4

40. Drill: Name:
Pb(NO3)2 MgSO3

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

42. Name the Following:
BaSO4 CuNO3
SO (NH4)3PO4

43. Naming Acids

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

45. Ternary acids become:
_____ ic acids or
_____ ous acids
H2SO4 - Sulfuric acid
H2SO3 - Sulfurous acid

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

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

48. Name or Give Formulas For:
HBr(aq) H2SO4(aq)
NaVO3 (NH4)3PO3
Phosphoric acid
Nitric acid
Chloric acid

49. Drill: Name each:
KBr MgS
BaF2 K3P
K2O LiH
Al2O3 H2S

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

51. Name each of the following:
SeO CS2
NO2 Cl2O
N2O4 PCl3

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

53. Name each of the following:
SO SO3-2
PO NO3-1
ClO ClO3-1
ClO ClO-1

54. Derive formulas for each:
Chromate Sulfate
Arsenate Nitrate
Arsenite Cyanide
Bromite Acetate

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

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

57. Name each of the following:
CuO MnS
PbO2 Cu2O
CrCl2 MnF2
CrCl3 SnCl4

58. Percent Composition by Mass

59. 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 %

60. MgCl2
Mg = 24.3 g/mole
2 Cl = 2 x 35.5 = 71.0 g/mole
MgCl2 = total = 95.3 g/mole
% Mg =24.3/95.3 x 100%
% Cl = 71.0/95.3 x 100 %

61. Determine % Comp for Each:
Fe2O3
C3H6O3
CuSO4*5H2O

62. Drill: Determine % Comp for Each:
C3H6O3
CuSO4*5H2O

63. Name each of the following:
FeO
Fe2O3

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

65. Name each of the following:
BaCO3
KNO2
CuClO3
Al2(SO4)3

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

67. Name each of the following:
Cl2O SO2
N2O3 P2O5
CO2 CO
SO3 N2H4

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

69. Name each of the following:
KCl MnSO4
SO2 HI(aq)
NaNO3 HClO
H2CO3(aq) NH4BrO4

70. Name each of the following:
NaCl MnSO4
S2O HBr(aq)
Na2CO3 HClO
HNO3(aq) NH4IO4

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

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