Naming Compounds and

1

• Naming Compounds and
• Writing Formulas

2
Periodic Table

• Recall that the periodic table is more than a
  list of elements.
• Elements are put in columns because of similar
  properties.
• Each column is called a group.

3
Representative Elements
0
1A
4A
6A
2A
3A
5A
7A

• The group A elements

4
Metals
5
Transition Metals

• The Group B elements

6
Nonmetals
7
Metalloids
8
Systematic Naming

• There are too many compounds to remember the
  names of them all.
• A compound is made of two or more elements.
• The name should tell us how many and what type of
  atoms.

9
Types of Compounds

• There are two types of compounds ionic compounds
  and molecular compounds.

10
Ionic Compounds

• The simplest ratio of the ions represented in an
  ionic compound is called a formula unit.
• The overall charge of any formula unit is zero.
• In order to write a correct formula unit, one
  must know the charge of each ion.

11
Atoms and Ions

• Atoms are electrically neutral.
• They have the same number of protons and
  electrons.
• Ions are atoms, or groups of atoms, with a
  charge.
• Ions have a different numbers of electrons.

12
Anions

• An anion is a negative ion.
• An anion has gained electrons.
• Nonmetals can gain electrons.
• The charge is written as a superscript on the
  right.

F-1
Has gained one electron
O-2
Has gained two electrons
13
Cations

• A cation is a positive ion.
• It is formed by losing electrons.
• There are more protons than electrons.
• Metals form cations.

K1
Has lost one electron
Ca2
Has lost two electrons
14
Ionic Compounds

• The charges of monatomic ions, or ions containing
  only one atom, can often be determined by
  referring to the periodic table or table of
  common ions based on group number.
• The charge of a monatomic ion is equal to its
  oxidation number.

15
Charges on Ions

• For most of the Group A elements, the Periodic
  Table can tell what kind of ion they will form
  from their location.
• Elements in the same group have similar
  properties, including the charge when they are
  ions.

16
Charges on IonsOxidation Numbers
1
2
3
3-
2-
1-
17
Naming Cations

• We will use the systematic way.
• For cations, if the charge is always the same
  (Group A) just write the name of the metal.

18
Naming Cations

• Transition metals (as well as tin and lead) can
  have more than one type of charge.
• Indicate the charge with Roman numerals in
  parenthesis.
• Zinc (Zn2) and silver (Ag1), although
  transition metals, only have one possible charge.
  Roman numerals ARE NOT used for zinc and silver.

19
Example

• Li1

• Li is the symbol for lithium.

• Lithium is a Group 1A metal, so the charge is
  always the same. Write the name of the metal.

• Li1 is called the Lithium ion.

20
Example

• Sr2

• Sr is the symbol for strontium.

• Strontium is a Group 2A metal, so the charge is
  always the same. Write the name of the metal.

• Sr2 is called the Strontium ion.

21
Example

• Fe2

• Fe is the symbol for iron.

• Iron is a transition metal, so the charge is not
  always the same. Write the name of the metal,
  indicating the charge with Roman numerals in
  parenthesis.

• Fe2 is called the Iron (II) ion.

22
Example

• Pb2

• Pb is the symbol for lead.

• Lead is a Group 4A metal, and the charge is not
  always the same. Write the name of the metal,
  indicating the charge with Roman numerals in
  parenthesis.

• Pb2 is called the Lead (II) ion.

23
Problem

• Name the following cations.

• Ca2

Calcium ion
Aluminum ion

• Al3

Tin (IV) ion

• Sn4

24
Problem

• Name the following ions.

• Na1

Sodium ion
Iron (III) ion

• Fe3

Copper (I) ion

• Cu1

25
Writing the Formulas for Cations

• Write the formula for the metal.
• If a Roman numeral is in parenthesis use that
  number for the charge. Indicate the charge with
  a superscript.

26
Writing the Formulas for Cations

• If no Roman numeral is given, find the Group A
  metal on the periodic table and determine the
  charge from the column number.

27
Example

• Nickel (II) ion

• Ni is the symbol for nickel.

• Nickel is a transition metal, which is the reason
  why the charge with Roman numerals in parenthesis
  was included.

• The formula for the nickel (II) ion is Ni2.

28
Example

• Gallium ion

• Ga is the symbol for gallium.

• Gallium is a Group 3A metal and its charge is
  always the same (3).

• The formula for the gallium ion is Ga3.

29
Problem

• Write the formulas for the following cations.

Mg2

• Magnesium ion

Cu2

• Copper (II) ion

• Potassium ion

K1
30
Problem

• Write the formulas for the following ions.

• Silver ion

Ag1

• Chromium (VI) ion

Cr6

• Mercury (II) ion

Hg2
31
Naming Anions

• Naming monatomic anions is always the same.
• Change the element ending to ide
• Example F1-
• F is the symbol for fluorine, F1- is

ide.
fluor
ine.
32
Example

• Cl1-

• Cl is the symbol for chlorine.

• Chlorine is a Group 7A nonmetal, so the charge is
  always the same (-1).

• Cl1- is called the chloride ion.

33
Example

• O2-

• O is the symbol for oxygen.

• Oxygen is a Group 6A nonmetal, so the charge is
  always the same (-2).

• O2- is called the oxide ion.

34
Problem

• Name the following anions.

• S2-

sulfide ion

• Br1-

bromide ion

• N3-

nitride ion
35
Problem

• Name the following anions.

• As3-

arsenide ion

• Te2-

telluride ion
36
Writing the Formulas for Anions

• Write the formula for the nonmetal.
• Find the Group A nonmetal on the periodic table
  and determine the charge from the column number.

37
Problem

• Write the formulas for the following anions.

• iodide ion

I1-

• phosphide ion

P3-
38
Problem

• Write the formulas for the following anions.

• selenide ion

Se2-

• carbide ion

C4-
39
Ionic Compounds

• Oxidation numbers can be used to determine the
  chemical formulas for ionic compounds.
• If the oxidation number of each ion is multiplied
  by the number of that ion present in a formula
  unit, and then the results are added, the sum
  must be zero.

40
Ionic Compounds

• In the formula for an ionic compound, the symbol
  of the cation is written before that of the
  anion.
• Subscripts, or small numbers written to the lower
  right of the chemical symbols, show the numbers
  of ions of each type present in a formula unit.

41
Binary Ionic Compounds

• Binary ionic compounds are composed of a metal
  bonded with a nonmetal.
• Name the metal ion using a Roman numeral in
  parenthesis if necessary.
• Follow this name with the name of the nonmetal
  ion.

42
Example

• Name the following binary ionic compounds.

• NaCl

Sodium chloride

• Ca3P2

Calcium phosphide
43
Example

• Name the following binary ionic compounds.

• CuO

Copper (II) oxide

• SnBr2

Tin (II) bromide
44
Problem

• Name the following binary ionic compounds.

• Fe2S3

Iron (III) sulfide

• AlF3

Aluminum fluoride
45
Problem

• Name the following binary ionic compounds.

• KCl

Potassium chloride

• Na3N

Sodium nitride
46
Problem

• Name the following binary ionic compounds.

• CrN

Chromium (III) nitride

• PbO2

Lead (IV) oxide
47
Writing Formulas for Binary Ionic Compounds

• Write the symbol for the metal. Determine the
  oxidation number from either the column number or
  the Roman numeral and write it as a superscript
  to the right of the metals symbol.

48
Writing Formulas for Binary Ionic Compounds

• To the right of the metals symbol, write the
  symbol for the nonmetal. Determine the oxidation
  number from the column number and write it as a
  superscript to the right of the nonmetals
  symbol.

49
Writing Formulas for Binary Ionic Compounds

• Example potassium fluoride

1
1-
K
F
50
Writing Formulas for Binary Ionic Compounds

• If the two oxidation numbers add together to get
  zero, the formula is a one-to-one ratio of the
  elements.

51
Writing Formulas for Binary Ionic Compounds

• Example potassium fluoride

1
1-
K
F
KF
52
Writing Formulas for Binary Ionic Compounds

• Example aluminum sulfide

3
2-
Al
S
53
Writing Formulas for Binary Ionic Compounds

• If the two oxidation numbers DO NOT add together
  to get zero, you will need to criss-cross the
  superscripts. These numbers now become
  subscripts.

54
Writing Formulas for Binary Ionic Compounds

• Example aluminum sulfide

3
2-
Al
S
3
2-
55
Writing Formulas for Binary Ionic Compounds

• Omit all positive and negative signs and omit all
  1s.

56
Writing Formulas for Binary Ionic Compounds

• Example aluminum sulfide

Al
S
Al2S3
2
3
57
Problem

• Write the formulas for the following binary ionic
  compounds.

• Lithium selenide

Li2Se

• Tin (II) oxide

SnO
58
Problem

• Write the formulas for the following binary ionic
  compounds.

• Tin (IV) oxide

SnO2

• Magnesium fluoride

MgF2
59
Problem

• Write the formulas for the following binary ionic
  compounds.

• Copper (II) sulfide

CuS

• Iron (II) phosphide

Fe3P2
60
Problem

• Write the formulas for the following binary ionic
  compounds.

• Gallium nitride

GaN

• Iron (III) sulfide

Fe2S3
61
Ternary Ionic Compounds

• Ternary ionic compounds are composed of at least
  3 elements.
• Name the metal ion, using a Roman numeral in
  parenthesis if necessary.
• Follow this name with the name of the polyatomic
  ion.

62
Polyatomic ions

• Polyatomic ions are groups of atoms that stay
  together and have a charge.
• Examples are on page 7 of the Reference Tables
  for Chemistry and include
• Nitrate NO3-1
• Nitrite NO2-1
• Hydroxide OH-1

63
Ternary Ionic Compounds

• There is one polyatomic ion with a positive
  oxidation number (NH4) that may come first in a
  compound. Name the ion.
• Follow this name with the name of the anion or
  second polyatomic ion.

64
Ternary Ionic Compounds

• Certain polyatomic ions, called oxyanions,
  contain oxygen and another element.

65
Examples

• Name the following ternary ionic compounds.
• LiCN

Lithium cyanide

• Fe(OH)3

Iron (III) hydroxide
66
Examples

• Name the following ternary ionic compounds.

• (NH4)2CO3

Ammonium carbonate

• NiPO4

Nickel (III) phosphate
67
Problems

• Name the following ternary ionic compounds.

• NaNO3

Sodium nitrate

• CaSO4

Calcium sulfate
68
Problems

• Name the following ternary ionic compounds.

• (NH4)2O

Ammonium oxide

• CuSO3

Copper (II) sulfite
69
Writing Formulas for Ternary Ionic Compounds

• Write the symbol for the metal or ammonium ion.
  Write the oxidation number as a superscript to
  the right of the metals/ammonium ions symbol.

70
Writing Formulas for Ternary Ionic Compounds

• To the right of the metals symbol, write the
  symbol for the nonmetal or polyatomic ion. Write
  the oxidation number as a superscript to the
  right of the nonmetals/polyatomic ions symbol.

71
Writing Formulas for Ternary Ionic Compounds

• Example potassium nitrate

1
1-
K
NO3
72
Writing Formulas for Ternary Ionic Compounds

• If the two oxidation numbers add together to get
  zero, the formula is a one-to-one ratio of the
  elements.

73
Writing Formulas for Ternary Ionic Compounds

• Example potassium nitrate

1
1-
K
NO3
KNO3
74
Writing Formulas for Ternary Ionic Compounds

• Example aluminum hydrogen sulfate

3
1-
Al
HSO4
75
Writing Formulas for Ternary Ionic Compounds

• If the two oxidation numbers DO NOT add together
  to get zero, you will need to criss-cross the
  superscripts. These numbers now become
  subscripts.
• Parentheses are to be placed around polyatomic
  ions before criss-crossing.

76
Writing Formulas for Ternary Ionic Compounds

• Example aluminum hydrogen sulfate

1-
3
(
)
Al
HSO4
3
1-
77
Writing Formulas for Ternary Ionic Compounds

• Omit all positive and negative signs and omit all
  1s.

78
Writing Formulas for Ternary Ionic Compounds

• Example aluminum hydrogen sulfate

Al
(HSO4)
Al(HSO4)3
3
79
Problems

• Write the formulas for the following ternary
  ionic compounds.
• Ammonium chloride

NH4Cl
(NH4)2S

• Ammonium sulfide

80
Problems

• Write the formulas for the following ternary
  ionic compounds.
• Barium nitrate

Ba(NO3)2
Zn(IO3)2

• Zinc iodate

81
Problems

• Write the formulas for the following ternary
  ionic compounds.
• Sodium hypochlorite

NaClO

• Chromium (III) acetate

Cr(CH3COO)3
82
Problems

• Write the formulas for the following ternary
  ionic compounds.
• Iron (II) dichromate

FeCr2O7

• Mercury (I) bromate

HgBrO3
83
STOP HERE
84
Molecular Compounds

• Writing Names and Formulas

85
Molecular Compounds

• Molecular compounds are made of molecules.
• They are made by joining nonmetal atoms together
  into molecules.

86
Naming is Easier

• A molecular compounds name tells you the number
  of atoms through the use of prefixes.

87
Prefixes

• 1 mono-
• 2 di-
• 3 tri-
• 4 tetra-
• 5 penta-

• 6 hexa-
• 7 hepta-
• 8 octa-
• 9 nona-
• 10 deca-

88
Prefixes

• The name will consist of two words.

Prefix
name
prefix
name
-ide

• One exception is we dont write mono- if there is
  only one of the first element.

89
Prefixes

• The following double vowels cannot be used when
  writing names
• (oa)
• (oo)

90
Example

• NO2

• There is one nitrogen

• mononitrogen

• But, you cannot use mono- on the first element,
  so drop the prefix.

• mononitrogen

• nitrogen

91
Example

• NO2

• There are two oxygens

• dioxygen

92
Example

• NO2

• dioxygen

• You need the suffix -ide

• diox

ygen
ide
93
Example

• NO2

• nitrogen dioxide

94
Example

• N2O

• There are two nitrogens

• dinitrogen

• There is one oxygen

• monooxygen

95
Example

• N2O

• monooxygen

• You cannot run (oo) together, so

• monoxygen

96
Example

• N2O

• monoxygen

• You need the suffix -ide

• monox

ygen
ide
97
Example

• N2O

• dinitrogen monoxide

98
Problem

• Name the following molecular compounds.

• Cl2O7

dichlorine heptoxide

• CBr4

carbon tetrabromide
99
Problem

• Name the following molecular compounds.

• CO2

carbon dioxide

• BCl3

boron trichloride
100
Naming Molecular Compounds

• You will not need to criss-cross oxidation
  numbers.
• Molecular compounds name tells you the number of
  atoms through the use of prefixes.

101
Example

• diphosphorus pentoxide

• The name implies there are 2 phosphorous atoms
  and 5 oxygens.

P2O5
102
Example

• sulfur hexaflouride

• The name implies there is 1 sulfur atom and 6
  fluorines.

SF6
103
Problem

• Write the formulas for the following molecules.
• tetraiodide nonoxide

I4O9
NO3

• nitrogen trioxide

104
Problem

• Write the formulas for the following molecules.
• carbon tetrahydride

CH4
PF3

• phosphorus trifluoride

105
Types of Compounds
Ionic
Molecular
Smallest piece
Formula Unit
Molecule
Types of elements
Metal and nonmetal
Nonmetals
Solid, liquid or gas
State
Solid
Melting Point
High gt300ºC
Low lt300ºC
106
Acids

• Writing Names and Formulas

107
Acids

• Acids are compounds that give off hydrogen ions
  (H) when dissolved in water.
• Acids will always contain one or more hydrogen
  ions next to an anion.
• The anion determines the name of the acid.

108
Naming Binary Acids

• Binary acids contain hydrogen and an anion whose
  name ends in ide.
• When naming the acid, put the prefix hydro- and
  change -ide to -ic acid.

109
Example

• HCl

• The acid contains the hydrogen ion and chloride
  ion.

• Begin with the prefix hydro-, name the
  nonmetallic ion and change -ide to -ic acid.

hydro
chlor
ide
ic acid
110
Example

• H2S

• The acid contains the hydrogen ion and sulfide
  ion.

• Begin with the prefix hydro- and name the
  nonmetallic ion.

hydro
sulf
ide
111
Example

• H2S

• The next step is change -ide to -ic acid, but for
  sulfur the ur is added before -ic.

hydro
sulf
ide
ic acid
ur
112
Problem
Name the following binary acids.

• HF

(hydrofluoric acid)

• H3P

(hydrophosphoric acid)
113
Writing the Formulas for Binary Acids

• The prefix hydro- lets you know the acid is
  binary.
• Determine whether you need to criss-cross the
  oxidation numbers of hydrogen and the nonmetal.

114
Example

• Hydrobromic acid

• The acid contains the hydrogen ion and the
  bromide ion.

115
Example

• Hydrobromic acid

H1Br1-

• The two oxidation numbers add together to get
  zero.

HBr
116
Example

• Hydrotelluric acid

• The prefix hydro- lets you know the acid is
  binary.
• The acid contains the hydrogen ion and the
  telluride ion.

117
Example

• Hydrotelluric acid

H1Te2-

• The two oxidation numbers do NOT add together to
  get zero, so you must criss-cross.

H2Te
118
Problem

• Write the formulas for the following binary
  acids.
• Hydrocyanic acid

HCN
H2Se

• Hydroselenic acid

119
Naming Ternary Acids

• The acid is a ternary acid if the anion has
  oxygen in it.
• The anion ends in -ate or -ite.
• Change the suffix -ate to -ic acid
• Change the suffix -ite to -ous acid
• The hydro- prefix is NOT used!

120
Example

• HNO3

• The acid contains the hydrogen ion and nitrate
  ion.

• Name the polyatomic ion and change -ate to -ic
  acid.

nitr
ate
ic acid
121
Example

• HNO2

• The acid contains the hydrogen ion and nitrite
  ion.

• Name the polyatomic ion and change -ite to -ous
  acid.

nitr
ite
ous acid
122
Example

• H3PO4

• The acid contains the hydrogen ion and phosphate
  ion.

• Name the polyatomic ion and change -ate to -ic
  acid.

phosph
ate
orous acid
123
Problem
Name the following ternary acids.

• H2CO3

(carbonic acid)

• H2SO4

(sulfuric acid)
124
Problem
Name the following ternary acids.

• H2CrO4

(chromic acid)

• HClO2

(chlorous acid)
125
Writing the Formulas for Ternary Acids

• The lack of the prefix hydro- from the name
  implies the acid is ternary, made of the hydrogen
  ion and a polyatomic ion.
• Determine whether you need to criss-cross the
  oxidation numbers of hydrogen and the polyatomic
  ion.

126
Example

• Acetic acid

• The polyatomic ion must end in ate since the
  acid ends in -ic.
• The acid is made of H and the acetate ion.

H1C2H3O21-
127
Example
H1C2H3O21-

• The two charges when added equal zero.

HC2H3O2
128
Example

• Sulfurous acid

• Again the lack of the prefix hydro- implies the
  acid is ternary, made of the hydrogen ion and a
  polyatomic ion.

129
Example

• sulfurous acid

• The polyatomic ion must end in ite since the
  acid ends in -ous.
• The acid is made of H and the sulfite ion.

H1SO32-
130
Example
H1SO32-

• The two charges when added do not equal zero, so
  you must crisscross the oxidation numbers.

131
Example
H1SO32-

• Ignore the negative sign and ones are understood.

H2SO3
132
Problem

• Write the formulas for the following ternary
  acids.
• perchloric acid

HClO4

• iodic acid

HIO3
133
Problem

• Write the formulas for the following ternary
  acids.
• perchloric acid

HClO4

• iodic acid

HIO3