Nomenclature

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
KClCaCl2Al2O3 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

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
Name Each
CuCl Fe2O3MnO2 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 S2O3N2H4 SO3
21
Nomenclature HW

• Work problems
• 49 - 54
• on page 51

22
Drill Name Each
CaO P2O5Al2S3 SO2
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
• PO4-3 SO4-2
• 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
• PO4-3 phosphate
• Some are unusual

32
CN-1 OH-1 C2H3O2-1C2O4-2
33
H2O H3O1NH3 NH41
34
Polyatomic Ion Endings

• Maximum O -ate
• 1 less than max O -ite
• SO4-2 sulfate
• SO3-2 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
Name Each
CaCO3K2SO4
39
Drill Name
Pb(NO3)2 MgSO3
40
Write Formulas For

• Lead (II) nitrate
• Aluminum sulfate
• Potassium chlorate
• Ammonium phosphite

41
Name the Following

• BaSO4 CuNO3
• SO2 (NH4)3PO4

42
Naming Acids
43

• Binary acids become
• Hydro _____ ic acids
• HCl - Hydrochloric acid

44

• Ternary acids become
• _____ ic acids or
• _____ ous acids
• H2SO4 - Sulfuric acid
• H2SO3 - 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
Name or Give Formulas For

• HBr(aq) H2SO4(aq)
• NaVO3 (NH4)3PO3
• Phosphoric acid
• Nitric acid
• Chloric acid

48
Percent Compositionby Mass
49

• 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

50
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

51
Determine Comp for Each

• Fe2O3
• C3H6O3
• CuSO45H2O

52
EmpiricalFormula
53

• Lowest whole number ratio of elements in a
  compound
• C6H12O6 EF CH2O

54
Determining Empirical formulas from percent
composition
55

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

56

• Substance 30 O 70 Fe
• 30 O --gt 30 g O
• 70 Fe --gt 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 Fe2O3

57
Find empirical for a compound with70.0
Fe30.0 O
58
Find empirical for a compound with40 Ca12
C48 O
59
Find empirical for a compound with40.0 C6.7
H53.3 O
60
MolecularFormula
61

• The actual whole number for each element in the
  compound

62
Molecular FormulaC6H12O6Empirical FormulaCH2O
63
Solving MF from EF

• 1) Solve empirical mass
• 2) Divide EM into MM
• 3) Multiply EF by quotient

64
Name each of the following

• KBr MgS
• BaF2 K3P
• K2O LiH
• Al2O3 H2S

65
Name each of the following
FeO Fe2O3
66
Name each of the following

• CuO MnS
• PbO2 Cu2O
• CrCl2 MnF2
• CrCl3 SnCl4

67
Name each of the following

• SeO CS2
• NO2 Cl2O
• N2O4 PCl3

68
Derive formulas for each

• Cesium oxide
• Barium chloride
• Calcium phosphide
• Aluminum sulfide

69
Derive formulas for each

• Lead(IV)oxide
• Copper(II)sulfide
• Manganese(VII)oxide
• Nickel(II)fluoride

70
Name each of the following

• SO4-2 SO3-2
• PO4-3 NO3-1
• ClO4-1 ClO3-1
• ClO2-1 ClO-1

71
Derive formulas for each

• Chromate
• Arsenate
• Arsenite
• Bromite

72
Name each of the following

• BaCO3
• KNO2
• CuClO3
• Al2(SO4)3

73
Derive formulas for each

• Potassium sulfate
• Lead(II)chromate
• Aluminum hydroxide
• Ammonium cyanide

74
Name each of the following

• Cl2O SO2
• N2O3 P2O5
• CO2 CO
• SO3 N2H4

75
Derive formulas for each

• Silicon dioxide
• phosphorus trichloride
• Sulfur hexafluoride
• Iodine trifluoride

76
Name each of the following
NH4Cl BaSO4 KC2H3O2 K2HPO3 KNO3 CuBrO Li2CO3
MgC2O4
77
Name each of the following
HCl H2SO4 H2S H3PO3 HNO3 HBrO H2CO3 HBrO4
78
Derive formulas for each

• Chromic acid
• Hydroiodic acid
• Sulfurous acid
• Bromic acid

79
Name each of the following
KCl MnSO4 SO2 HI(aq) NaNO3 HClO H2CO3(aq)
NH4BrO4
80
Name each of the following
NaCl MnSO4 S2O3 HBr(aq) Na2CO3
HClO HNO3(aq) NH4IO4
81
Chapter 3 General

• Define all the Key Terms on page 74

82
Nomenclature

• Work problems 43 56
• On Pages 51 52