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
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
If charged
A
one orparticle
moreknown
electrons
as an ion
are
can be produced
removed
from abyneutral
adding or
atom a
removingion
positive
one
is or
formed.
more electrons
A positive ion
from
is
called
a neutral
a cation.
atom.
remove e-
→
neutral atom
10
Positive Ion Formation:
Loss of Electrons From a Neutral Atom
Na  Na+ + e-
Ca  Ca2+ + 2eAl  Al3+ + 3e-
11
Naming Cations
12
Cations are named the same
as their parent atoms
13
Atom
Cation
Name of
Cation
sodium (Na)
+
Na
sodium ion
14
Atom
Cation
Name of
Cation
calcium (Ca)
2+
Ca
calcium ion
15
Atom
Cation
Name of
Cation
lithium (Li)
+
Li
lithium ion
16
Atom
Cation
Name of
Cation
magnesium (Mg)
2+
Mg
magnesium ion
17
Atom
Cation
Name of
Cation
strontium (Sr)
2+
Sr
strontium ion
18
A
If charged
one or more
particle
electrons
known as
areanadded
ion
can
to abe
neutral
produced
atombyaadding
negative
or ion is
removing
formed. Aone
negative
or more
ionelectrons
is called an
from
anion.
a neutral atom.
add e-
neutral atom
→
19
Naming Anions
20
An anion consisting of one element has
the stem of the parent element and an –
ide ending
21
Atom
Anion
fluorine (F)
F
stem
Name of
Anion
fluoride ion
22
Atom
Anion
chlorine (Cl)
Cl
stem
Name of
Anion
chloride ion
23
Atom
Anion
bromine (Br)
Br
stem
Name of
Anion
bromide ion
24
Atom
Anion
nitrogen (N)
3N
stem
Name of
Anion
nitride ion
25
Atom
Anion
phosphorous (P)
3P
stem
Name of
Anion
phosphide ion
26
Atom
Anion
oxygen (O)
2O
stem
Name of
Anion
oxide ion
27
Binary Compounds
38
Binary compounds contain only
two different elements.
39
Binary ionic compounds consist of a
metal combined with a non-metal.
40
A. Binary Ionic Compounds Containing a
Metal Forming Only One Type of Cation
(one charge)
41
Type I Cations include:
•
•
•
•
the Group A metals
Hydrogen
B metals with one charge: Zn+2, Cd+2, Ag+
The polyatomic ion NH4+
42
• 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.
43
Name of Metal
+ Stem of Nonmetal
plus -ide ending
44
(ur)
45
If hydrogen is written first in
the formula, it is treated as if it
were a group IA metal.
46
Name the Compound CaF2
Step 1 From the formula it
is a two-element compound
and follows the rules for
binary compounds.
47
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.
48
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.
49
Name the Compound CaF2
Step 4 The name of the
compound is therefore
calcium fluoride.
50
Examples
51
Compound
NaCl
name of metal
Name
sodium
chloride
nonmetal stem
52
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
53
Compound
MgCl2
name of metal
Name
magnesium
chloride
nonmetal stem
54
Compound
K2O
name of metal
Name
potassium
oxide
nonmetal stem
55
Compound
Na3P
name of metal
Name
sodium
phosphide
nonmetal stem
56
B. Binary Ionic Compounds Containing a Metal
That Can Form Two or More Types of Cations
(two or more charges)
57
Type II Cations include:
• B metals with two charges
• Zn+2, Cd+2, Ag+ are excluded
58
Name the Compound FeS
Step 1 This compound
follows the rules for a
binary compound.
59
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)
60
Name the Compound FeS
Step 3 We have already
determined that the name
of the negative part of the
compound will be sulfide.
61
Name the Compound FeS
Step 4 The name of FeS
is iron(II) sulfide.(or
ferrous sulfide)
62
The IUPAC (Stock)
System
63
The metals in the center of the periodic
table (including the transition metals)
often form more than one type of
cation.
64
Each ion of iron forms a different
compound with the same anion.
Fe2+
FeS
Fe3+
Fe2S3
65
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.
66
Stock System
IUPAC
System
Lower
Lower Charge
Charge
Element
Formula
Higher
HigherCharge
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)67
Examples
68
iron(II) chloride
FeCl2
+2
iron(II)
-1
chloride
compound
ion
ioncharge
name
name
iron(III) chloride
FeCl3
+3
iron(III)
-1
chloride
69
tin(II) bromide
SnBr2
+2
tin(II)
-1
bromide
compound
ion
ioncharge
name
name
tin(IV) bromide
SnBr4
+4
tin(IV)
-1
bromide
70
The Classical System
71
In the Classical System the name of the metal
(usually the Latin name) is modified with the
suffixes -ous and ic.
72
Metal name ends in
-ous lower charge
-ic higher charge
nonmetal name ends in
-ide
73
Examples
74
ferrous chloride
FeCl2
+2
ferrous
-1
chloride
ion
compound
ioncharge
name name
ferric chloride
FeCl3
+3
ferric
-1
chloride
75
stannous bromide
SnBr2
+2
stannous
-1
bromide
compound
ion
ioncharge
name
name
stannic bromide
SnBr4
+4
stannic
-1
bromide
76
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
77
Binary Compounds
Containing Two Nonmetals
78
Compounds between nonmetals are
molecular, not ionic.
79
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
80
Prefixes
81
A Greek prefix is placed before the name
of each element to indicate the number
of atoms of the element that are present.
82
Mono is rarely used when
naming the first element.
• mono = 1
•
di = 2
•
tri = 3
• tetra = 4
• penta = 5
•
•
•
•
•
hexa = 6
hepta = 7
octa = 8
nona = 9
deca = 10
83
Examples
84
dinitrogen trioxide
N2 O 3
indicates two
nitrogen atoms
indicates three
oxygen atoms
85
phosphorous pentachloride
PCl5
indicates one
phosphorous atom
indicates five
chlorine atoms
86
dichlorine heptaoxide
Cl2O7
indicates two
chlorine atoms
indicates seven
oxygen atoms
87
Determine the Name of PCl5
Step 1
• There are 2 elements present.
• The compound is binary.
• Phosphorous and chlorine are nonmetals so the
rules for naming binary compounds of 2
nonmetals apply.
• Phosphorous is named first. Therefore the
compound is a chloride.
88
Determine the Name of PCl5
Step 2
• No prefix is needed for phosphorous because
each molecule of PCl5 has only one
phosphorous atom. The prefix penta- is used
with chloride because there are 5 chlorine atoms
present in one molecule.
Step 3
• The name is phosphorous pentachloride.
89
Examples
90
Cl2O3
dichlorine trioxide
91
N2O3
dinitrogen trioxide
92
CCl4
carbon tetrachloride
93
CO
carbon monoxide
94
Name CO2
carbon dioxide
95
Name PI3
phosphorous triiodide
96
D. Acids Derived
from Binary Compounds
97
• 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.
98
Acid Formation
binary hydrogen
compound (not
an acid).
water
acid
99
Pure compound
HCl
-ide
Dissolved in water
HCl
acid
100
• 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.
101
Examples
102
Pure Compound
HCl (g)
hydrogen chloride
103
Dissolved in Water
HCl (aq)
hydrochloric acid
104
Pure Compound
HI (g)
hydrogen iodide
105
Dissolved in Water
HI (aq)
hydroiodic acid
106
Pure Compound
H2S (g)
hydrogen sulfide
107
Dissolved in Water
H2S (aq)
hydrosulfuric acid
108
Pure Compound
H2Se (g)
hydrogen selenide
109
Dissolved in Water
H2Se (aq)
hydroselenic acid
110
111
Naming Compounds
Containing Polyatomic Ions
112
A polyatomic ion is an ion that
contains two or more elements.
NO
3
113
• 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
114
• When naming a compound containing
a polyatomic ion, name the cation first
and then name the anion.
Na 2CO3
115
This is the way the
formula is written.
KMnO 4
K
+
MnO
4
The ions are what is
actually present.
116
This is the way the
formula is written.
Na 2CO3
2Na
+
CO
23
The ions are what is
actually present.
117
Prefixes and Suffixes
Elements that Form More than One
Polyatomic Ion with Oxygen
118
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
nitrite
2
NO
nitrate
3
NO
119
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
phosphite
33
PO
phosphate
34
PO
120
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.
121
per- (short form of hyper) denotes
anions with more oxygen than the -ate
form .
chlorate
3
ClO
perchlorate
4
ClO
122
hypo- denotes anions with less oxygen
than the -ite form.
hypochlorite
-
ClO
chlorite
2
ClO
123
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
chlorous
acid
chloric
acid
ClO4–
perchlorate
HClO4
perchloric
acid
124
Four ions do not use the –ate/ite system.
hydroxide
-
cyanide
-
hydrogen sulfide
-
peroxide
22
OH
HS
CN
O
125
There are three common positively
charged polyatomic ions.
mercury(I)
2+
2
Hg
hydronium
+
3
HO
ammonium
+
4
NH
126
127
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
128
Acids
129
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.
130
Hydrogen in an
oxy-acid is not
expressed in the
acid name.
The word acid in
the name indicates
the presence of
hydrogen.
131
indicates
hydrogen
sulfuric acid
contains
contains
contains
hydrogen
sulfur
oxygen
H 2SO 4
132
Anions ending in -ate always contain
more oxygen than ions ending in -ite.
phosphite
33
PO
phosphate
34
PO
133
Naming the Acid Based
on the Name of the Polyatomic Ion
Ending of Polyatomic Ion
ite
Ending of Acid
ous
less oxygen
ate
ic
more oxygen
134
Examples
135
sulfite
SO
2
3
sulfurous acid H 2SO3
136
sulfate
SO
2
4
sulfuric acid H 2SO 4
137
nitrite
NO

2
nitrous acid HNO2
138

3
nitrate
NO
nitric acid
HNO3
139
140
141
142