1. Nomenclature
Naming
Compounds

2. Compounds with only two elements in any ratio
Binary Compounds
Compounds with only two elements in any ratio

3. Naming Binary Compounds

4. Ionic Compounds

5. Name positive element (cation) first with its normal name
Name negative element (anion) last & change its ending to -ide

6. KCl CaCl2 Al2O3 Na2O

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

8. FeO is Iron (II) Oxide
Fe2O3 is Iron (III) Oxide
CrO3 is Chromium (IV)Oxide

9. 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

10. CuCl Fe2O3 MnO2 CrO3

11. Molecule

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

13. Naming Molecules or Covalent Compounds

14. Same rules as ionic compounds except:
If two elements are from the same group, lower element is first.
SO2 is sulfur dioxide
use geometric prefixes to determine the # of each atom

15. Period 2 stopped here 9/8/06

16. Geometric Prefixes 1-mono 5-penta 2-di 6-hexa 3-tri 7-hepta
4-tetra etc

17. CO S2O3 N2H4 SO3

18. Deriving Formulas Write the symbol for each element
Determine ox #s for each
Determine lowest common multiple to balance the charge
Apply subscripts

19. Polyatomic Ion

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

21. Naming Polyatomic Ions

22. Most are oxoanions
A root element (most are non-metals) bound to oxygen

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

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

25. Naming Ternary Compounds

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

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

28. CaCO3 K2SO4 Pb(NO3)2 MgSO3

29. Naming Acids

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

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

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

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

34. Percent Composition by Mass

35. 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 %

36. 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 %

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

38. Empirical Formula

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

40. Determining Empirical formulas from percent composition

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

42. Substance = 30 % O & 70 & Fe
30 % O --> 30 g O &
70 % Fe --> 70 g Fe
30/16 = moles O
70 / 56 = 1.25 moles Fe
1.25/1.25 = 1 & /1.25 = 1.5
Ratio = 1.5 : 1 x 2 = 3 : 2
Empirical Formula Fe2O3

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

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

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

46. Molecular Formula

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

48. Molecular Formula C6H12O6 Empirical Formula CH2O

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

50. Name each of the following:
KBr MgS
BaF2 K3P
K2O LiH
Al2O3 H2S

51. Name each of the following:
FeO
Fe2O3

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

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

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

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

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

57. Derive formulas for each:
Chromate
Arsenate
Arsenite
Bromite

58. Name each of the following:
BaCO2
KNO2
CuClO3
Al2(SO4)3

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

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

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

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

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

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

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

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

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