1
Common and
Systematic Names
2
Chemical nomenclature is the
system of names that chemists use
to identify compounds. Two classes
of names exist: common names and
systematic names.
3
• Common names are arbitrary names.
– They are not based on the composition of
the compound.
– They are based on an outstanding chemical
or physical property.
• Chemists prefer systematic names.
– Systematic names precisely identify the
chemical composition of the compound.
– The present system of inorganic chemical
nomenclature was devised by the
International Union of Pure and Applied
Chemistry (IUPAC).
4
Common Names, Formulas, and Chemical Names of Familiar Substances
Common Names
Formulas
Chemical Names
Acetylene
C2H2
Ethyne
Lime
CaO
Calcium Oxide
Alumina
Al2O3
Aluminum oxide
Baking soda
NaHCO3
Sodium bicarbonate
Table sugar
C12H22O11
Sucrose
Brimstone
S
Sulfur
Limestone
CaCO3
Calcium carbonate
Laughing gas
N2O
Dinitrogen monoxide
Lye
NaOH
Sodium hydroxide
Milk of magnesia
Mg(OH)2
Magnesium hydroxide
Muriatic acid
HCl
Hydrochloric acid
Vinegar
HC2H3O2
Acetic acid
Washing soda
Na2CO310 H2O
Sodium carbonate decahydrate
Wood alcohol
CH3OH
Methanol
5
Elements and Ions
6
The formula for most elements
is the symbol of the element.
Sodium
Potassium
Zinc
Argon
Mercury
Lead
Calcium
Na
K
Zn
Ar
Hg
Pb
Ca
7
These 7 elements are found
in nature as diatomic molecules.
Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine
H2
N2
O2
F2
Cl2
Br2
I2
8
Ions
9
Positive Ion Formation:
Loss of Electrons From a Neutral Atom
Na  Na+ + e-
Ca  Ca2+ + 2eAl  Al3+ + 3e-
10
Naming Cations
11
Cations are named the same
as their parent atoms
12
Atom
Cation
Name of
Cation
sodium (Na)
+
Na
sodium ion
13
Atom
Cation
Name of
Cation
calcium (Ca)
2+
Ca
calcium ion
14
Atom
Cation
Name of
Cation
lithium (Li)
+
Li
lithium ion
15
Atom
Cation
Name of
Cation
magnesium (Mg)
2+
Mg
magnesium ion
16
Atom
Cation
Name of
Cation
strontium (Sr)
2+
Sr
strontium ion
17
Naming Anions
18
An anion consisting of one element has
the stem of the parent element and an –
ide ending
19
Atom
Anion
fluorine (F)
F
stem
Name of
Anion
fluoride ion
20
Atom
Anion
chlorine (Cl)
Cl
stem
Name of
Anion
chloride ion
21
Atom
Anion
bromine (Br)
Br
stem
Name of
Anion
bromide ion
22
Atom
Anion
nitrogen (N)
3N
stem
Name of
Anion
nitride ion
23
Atom
Anion
phosphorous (P)
3P
stem
Name of
Anion
phosphide ion
24
Atom
Anion
oxygen (O)
2O
stem
Name of
Anion
oxide ion
25
Binary Compounds
26
Binary compounds contain only
two different elements.
27
Binary ionic compounds consist of a
metal combined with a non-metal.
28
A. Binary Ionic Compounds Containing a
Metal Forming Only One Type of Cation
(one charge)
29
Type I Cations include:
•
•
•
•
the Group IA & IIA metals, Al+3
Hydrogen
B metals with one charge: Zn+2, Cd+2, Ag+
The polyatomic ion NH4+
30
• The chemical name is composed of the
name of the metal followed by the
name of the nonmetal which has been
modified to an identifying stem plus
the suffix –ide.
• Using this system the number of atoms
of each element present is not expressed
in the name.
31
Name of Metal
+ Stem of Nonmetal
plus -ide ending
32
Examples of Elements Forming Anions
Symbol
Element
Stem
Anion name
Br
bromine
brom
bromide
Cl
chlorine
chlor
chloride
F
fluorine
fluor
fluoride
H
hydrogen
hydr
hydride
I
Iodine
iod
iodide
N
nitrogen
nitr
nitride
O
oxygen
ox
oxide
P
phosphorus
phosph(or)
phosphide
S
sulfur
sulf(ur)
sulfide
33
Examples of Compounds with Names ending in -ide
Formula
If hydrogen is
written first in
the formula, it
is treated as if it
were a group IA
metal.
Name
AlCl3
Aluminum chloride
Al2O3
Aluminum oxide
CaC2
Calcium carbide
HCl(g)
Hydrogen chloride
HI(g)
Hydrogen Iodide
BaS
Barium sulfide
LiI
Lithium iodide
MgBr2
Magnesium bromide
NaH
Sodium hydride
Na2O
Sodium oxide
34
Name the Compound CaF2
Step 1 From the formula it
is a two-element compound
and follows the rules for
binary compounds.
35
Name the Compound CaF2
Step 2 The compound is
composed of Ca, a
metal and F, a nonmetal. Ca
forms only a +2 cation.
Thus, call the positive part of
the compound calcium.
36
Name the Compound CaF2
Step 3 Modify the name of
the second element to the
stem fluor- and add the
binary ending –ide
to form the name of the
negative part, fluoride.
37
Name the Compound CaF2
Step 4 The name of the
compound is therefore
calcium fluoride.
38
Examples
39
Compound
NaCl
name of metal
Name
sodium
chloride
nonmetal stem
40
Compound
HCl(g)
name of metal
Name
For naming purposes
only, hydrogen is
treated as if it were a
group IA metal.
hydrogen
chloride
nonmetal stem
41
Compound
MgCl2
name of metal
Name
magnesium
chloride
nonmetal stem
42
Compound
K2O
name of metal
Name
potassium
oxide
nonmetal stem
43
Compound
Na3P
name of metal
Name
sodium
phosphide
nonmetal stem
44
Thanks to Christine Neighbors (Fall 2012)
45
B. Binary Ionic Compounds Containing a Metal
That Can Form Two or More Types of Cations
(two or more charges)
46
Type II Cations include:
• B metals with two charges
• Zn+2, Cd+2, Ag+ are excluded
47
Name the Compound FeS
Step 1 This compound
follows the rules for a
binary compound.
48
Name the Compound FeS
Step 2 ItInissulfides,
a compound
the
of Fe, aon
charge
metal,
S is –2.
and S, a
nonmetal, the
Therefore
andcharge
Fe is a on
transition
Fe
must bemetal
+2, and
thatthe
has
more than
name
of theone
positive
type of
cation.
part of the compound
is iron (II).(or ferrous)
49
Name the Compound FeS
Step 3 We have already
determined that the name
of the negative part of the
compound will be sulfide.
50
Name the Compound FeS
Step 4 The name of FeS
is iron(II) sulfide.(or
ferrous sulfide)
51
The metals in the center of the periodic
table (including the transition metals)
often form more than one type of
cation.
52
Each ion of iron forms a different
compound with the same anion.
Fe2+
FeS
Fe3+
Fe2S3
53
The IUPAC (Stock)
System
54
In IUPAC
the IUPAC
devised
System
the Stock
the charge
System
on the
of cation
is designated
nomenclature
by to
a name
Roman
compounds
numeral placed
of
in
parentheses
metals thatimmediately
have more than
following
one type
theofname
of the
cation.
metal.
Cation
Charge
+1
+2
+3
+4
+5
Roman
Numeral
I
II
III
IV
V
The nonmetal name ends in -ide.
55
IUPAC System
Lower Charge
Element
Formula
Higher Charge
Name
Formula
Name
Copper
Cu+
copper(I)
Cu2+
copper(II)
Iron
Fe2+
iron(II)
Fe3+
iron(III)
Lead
Pb2+
lead(II)
Pb4+
lead(IV)
Mercury
Hg22+
mercury(I)
Hg2+
mercury(II)
Tin
Sn2+
tin(II)
Sn4+
tin(IV)56
The Classical System
57
In the Classical System the name of the metal
(usually the Latin name) is modified with the
suffixes -ous and ic.
58
Metal name ends in
-ous lower charge
-ic higher charge
nonmetal name ends in
-ide
59
Ion Names: Classical System
Lower Charge
Higher Charge
Element
Formula
Name
Formula
Name
Copper
Cu+
cuprous
Cu2+
cupric
Iron
Fe2+
ferrous
Fe3+
ferric
Lead
Pb2+
plumbous
Pb4+
plumbic
Mercury
Hg22+
mercurous
Hg2+
mercuric
Tin
Sn2+
stannous
Sn4+
stannic
60
Examples
61
ion charge
compound name
FeCl2
iron(II) chloride
ferrous chloride
+2
-1
FeCl3
+3
-1
iron(III) chloride
ferric chloride
62
ion charge
SnBr2
+2
-1
SnBr4
+4
-1
compound name
tin(II) bromide
stannous bromide
tin(IV) bromide
stannic bromide
63
Naming Binary Ionic
Compounds
More Practice
1. CoCl3
2. K2S
3. HgF2
4. AgBr
5. Fe3P2
6. PbI4
64
Naming Binary Ionic
Compounds
More Practice
1. CoCl3 cobalt(III) chloride
2. K2S potassium sulfide
3. HgF2 mercury(II) fluoride
4. AgBr silver bromide
5. Fe3P2 iron(II) phosphide
6. PbI4 lead(IV) iodide
65
Learning Check
CuCl2 is
a. Copper chloride
b. Copper (I) chloride
c. Copper (II) chloride
d. Cuprous chloride
e. Copper chloride (II)
Solution in Lecture!
66
Learning Check
HgS is
a. mercury(II) sulfide
b. mercury(I) sulfide
c. mercury sulfide
d. mercurous sulfide
Solution in Lecture!
67
Binary Compounds
Containing Two Nonmetals
68
Compounds between nonmetals are
molecular, not ionic.
69
In a compound formed between two
nonmetals, the element that occurs first
in this series is named first.
•
•
•
•
•
•
Si
B
P
H
C
S
•
•
•
•
•
•
I
Br
N
Cl
O
F
70
Prefixes
71
A Greek prefix is placed before the name
of each element to indicate the number
of atoms of the element that are present.
72
Naming Covalent Compounds
•
In the names of covalent compounds, prefixes are
used to indicate the number of atoms (subscript) of
each element. (mono is omitted for the first element,
not the second)
Prefixes Used in Naming Covalent Compounds
Rules for Naming Binary Compounds
Containing Two Nonmetals
1. Write the name of the first nonmetal as it
appears on the periodic table. Use a
prefix if there is more than one atom.
2. Use a prefix to indicate the number of
atoms for the second nonmetal ALWAYS.
3. If the second nonmetal begins in an “o”,
drop the prefix “a” or “o”.
4. Write the stem of the second nonmetal.
5. Add the suffix –ide.
Examples
75
dinitrogen trioxide
N2 O 3
indicates two
nitrogen atoms
indicates three
oxygen atoms
76
phosphorous pentachloride
PCl5
indicates one
phosphorous atom
indicates five
chlorine atoms
77
This vowel usually omitted
dichlorine heptaoxide
Cl2O7
indicates two
chlorine atoms
indicates seven
oxygen atoms
78
Examples
79
Cl2O3
dichlorine trioxide
80
N2O3
dinitrogen trioxide
81
CCl4
carbon tetrachloride
82
CO
carbon monoxide
83
Name CO2
carbon dioxide
84
Name PI3
phosphorous triiodide
85
D. Acids Derived
from Binary Compounds
86
• Certain binary hydrogen compounds,
when dissolved in water, form
solutions that have acid properties.
• The aqueous solutions of these
compounds are given acid names.
• The acid names are in addition to their
–ide names.
• Hydrogen is typically the first element
of a binary acid formula.
87
Acid Formation
binary hydrogen
compound (not
an acid).
water
88
Acid Formation
water
acid
89
Pure compound
HCl
-ide
Dissolved in water
HCl
acid
90
• To name binary acids write the symbol
of hydrogen first.
• After hydrogen write the symbol of the
second element.
• Place the prefix hydro- in front of the
stem of the nonmetal name.
• Place the suffix -ic after the stem of the
nonmetal name.
91
Examples
92
Pure Compound
HCl (g)
hydrogen chloride
93
Dissolved in Water
HCl (aq)
hydrochloric acid
94
Pure Compound
HI (g)
hydrogen iodide
95
Dissolved in Water
HI (aq)
hydroiodic acid
96
Pure Compound
H2S (g)
hydrogen sulfide
97
Dissolved in Water
H2S (aq)
hydrosulfuric acid
98
Pure Compound
H2Se (g)
hydrogen selenide
99
Dissolved in Water
H2Se (aq)
hydroselenic acid
100
101
Naming Compounds
Containing Polyatomic Ions
102
A polyatomic ion is an ion that
contains two or more elements.
NO
3
103
• Compounds containing polyatomic ions are
composed of three or more elements.
• They usually consist of one or more cations
combined with a negative polyatomic ion.
Na 2CO3
104
• When naming a compound containing
a polyatomic ion, name the cation first
and then name the anion.
Na 2CO3
105
This is the way the
formula is written.
KMnO 4
K
+
MnO
4
The ions are what is
actually present.
106
This is the way the
formula is written.
Na 2CO3
2Na
+
CO
23
The ions are what is
actually present.
107
Prefixes and Suffixes
Elements that Form More than One
Polyatomic Ion with Oxygen
108
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
nitrite
2
NO
nitrate
3
NO
109
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
phosphite
33
PO
phosphate
34
PO
110
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
sulfite
23
SO
sulfate
24
SO
-ate and –ite do not indicate
the number of oxygen atoms.
111
per- (short form of hyper) denotes
anions with more oxygen than the -ate
form .
chlorate
3
ClO
perchlorate
4
ClO
112
hypo- denotes anions with less oxygen
than the -ite form.
hypochlorite
-
ClO
chlorite
2
ClO
113
Oxy-Anions and Oxy-Acids of
Chlorine (also Bromine and Iodine)
Anion
Anion Name
Acid
Acid Name
ClO–
hypochlorite
HClO
hypochlorous
acid
ClO2–
chlorite
HClO2
ClO3–
chlorate
HClO3
ClO4–
perchlorate
HClO4
chlorous
acid
chloric
acid
perchloric
acid
114
Four ions do not use the –ate/ite system.
hydroxide
-
cyanide
-
hydrogen sulfide
-
peroxide
22
OH
HS
CN
O
115
There are three common positively
charged polyatomic ions.
mercury(I)
2+
2
Hg
hydronium
+
3
HO
ammonium
+
4
NH
116
Names, Formulas, and Charges of
Some Common Polyatomic Ions
Name
Formula
Charge
Name
Formula
Charge
Acetate
C2H3O2
1
Dichromate
Cr2O72
2
Ammonium
NH4
1
Hydroxide
OH
1
Bicarbonate
HCO3
1
Iodate
IO3
1
Bisulfate
HSO4
1
Nitrate
NO3
1
Bromate
BrO3
1
Nitrite
NO2
1
Carbonate
CO32
2
Permanganate
MnO4
1
Chlorate
ClO3
1
Phosphate
PO43
1
Chromate
CrO42
2
Sulfate
SO42
1
Cyanide
CN
1
Sulfite
SO32
1
117
Names of Selected Compounds That Contain
More Than One Kind of Positive Ion
Formula
Name of compound
KHSO4
potassium hydrogen sulfate
Ca(HSO3)2
calcium hydrogen sulfite
NH4HS
ammonium hydrogen sulfide
MgNH4PO4
magnesium ammonium phosphate
NaH2PO4
sodium dihydrogen phosphate
Na2HPO4
disodium hydrogen phosphate
KHC2O4
potassium hydrogen oxalate
KAl(SO4)2
potassium aluminum sulfate
Al(HCO3)3
aluminum hydrogen carbonate
118
Acids
119
Oxy-acids contain
hydrogen, oxygen
and one other
element.
• The other element
is usually a
nonmetal, but it
can be a metal.
• Its first element is
hydrogen.
• Its remaining
elements include
oxygen and form
a polyatomic ion.
120
Hydrogen in an
oxy-acid is not
expressed in the
acid name.
The word acid in
the name indicates
the presence of
hydrogen.
121
indicates
hydrogen
sulfuric acid
H 2SO 4
Contains Contains
sulfur
oxygen
122
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
phosphite
33
PO
phosphate
34
PO
123
Naming the Acid Based
on the Name of the Polyatomic Ion
Ending of Polyatomic Ion
Ending of Acid
ite
ous
less oxygen
There mite be hope for us
ate
ic
more oxygen
I ate something icky
124
Examples
125
sulfite
SO
2
3
sulfurous acid H 2SO3
126
sulfate
SO
2
4
sulfuric acid H 2SO 4
127
nitrite
NO

2
nitrous acid HNO2
128
nitrate
nitric acid
NO

3
HNO3
129
Comparison of Acid and Anion
Names for Some Oxy-Acids
Acid
H2SO4
Sulfuric acid
H2SO3
Sulfurous acid
HNO3
Nitric acid
HNO2
Nitrous acid
H2CO3
Carbonic acid
HClO3
Chloric acid
HClO2
Chlorous acid
HClO4
Perchloric acid
Anion
SO42
sulfate
SO32
sulfite
NO3
nitrate
NO2
nitrite
CO32
carbonate
ClO3
chlorate
ClO2
chlorite
ClO4
perchlorate
Acid
Anion
H3PO4
PO43
Phosphoric acid
phosphate
PO33
phosphite
IO3
iodate
H3PO3
Phosphorous acid
HIO3
Iodic acid
HC2H3O2
Acetic acid
H2C2O4
Oxalic acid
HBrO3
Bromic acid
HBrO
Hyprobromous acid
HBrO2
Bromous acid
C2H3O2
acetate
C2O42
oxalate
BrO3
bromate
BrO
hypobromite
BrO2
bromite
130
131
132