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1
Basic Nomenclature 1
Nomenclature of InorganicCompounds
Naming Simple Inorganic CompoundsDr. Carl Hoeger
profcah
CauldronCast #1
Basic Nomenclature 2
Nomenclature-History• Early: Compounds named by those who
discovered them; usually had some historicsignificance
• Oil of Vitrol• Blue Vitrol• Laughing gas
• Problem: No real system; region/researcherspecific; needed systematic, well-definednomenclature system
• Answer: IUPAC development of standardizednomenclature schemes; some trivial namesaccepted and retained
2
Basic Nomenclature 3
Nomenclature-BasicsTwo general classes of inorganic molecules:
1. Those containing a metal cation and a nonmetal anionOR a metal cation and a polyatomic anion (ioniccompounds);
2. Those containing only nonmetals (molecularcompounds; Type III compounds)
Two different types of the first class:a) Those whose metal has only one possible positive
oxidation state (Type I compounds);b) Those whose metal has more than one possible positive
oxidation state (Type II compounds)The nomenclature scheme reflects the compounds
class/type
Basic Nomenclature 4
“Type I” Elements1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
IA VIII
A
1
H
1.00
8
IIA
IIIA
IVA
VA
VIA
VII
A
2
H e
4.002
3
L i
6.94
1
4
B e
9.01
2
5
B
10.8
1
6
C
12.0
1
7
N
14.0
1
8
O
16.0
0
9
F
19.0
0
10
N e
20.18
11
N a
22.9
9
12
M g 24.3
0 IIIB IVB VB VIB
VII
B VIII VIII VIII IB IIB
13
Al
26.9
8
14
S i
28.0
9
15
P
30.9
7
16
S
32.0
6
17
C l
35.4
5
18
Ar
39.95
19
K
39.1
0
20
C a
40.0
8
21
Sc 44.9
6
22
Ti
47.9
0
23
V
50.9
4
24
C r
52.0
0
25
Mn
54.9
4
26
F e
55.8
5
27
C o
58.9
3
28
N i
58.7
0
29
Cu
63.5
5
30
Zn
65.3
8
31
G a
69.7
2
32
G e
72.5
9
33
As
74.9
2
34
S e
78.9
6
35
B r
79.9
0
36
K r
83.80
37
R b
85.4
7
38
S r
87.6
2
39
Y
88.9
1
40
Z r
91.2
2
41
N b
92.9
1
42
Mo
95.9
4
43
Tc
(99)
44
Ru
101.
1
45
Rh
102.
9
46
P d
106.
4
47
Ag
107.
9
48
C d
112.
4
49
In
114.
8
50
Sn
118.
7
51
S b
121.
8
52
Te
127.
6
53
I 126.
9
54
X e
131.3
55
C s
132.
9
56
B a
137.
3
57
L a
138.
9
72
H f
178.
5
73
Ta
180.
9
74
W
183.
9
75
R e
186.
2
76
O s
190.
2
77
Ir
192.
2
78
P t
195.
1
79
Au
197.
0
80
H g
200.
6
81
Tl
204.
4
82
P b
207.
2
83
B i
209.
0
84
P o
(209
)
85
At
(210
)
86
Rn
(222)
87
F r
(223
)
88
R a
226.
0
89
Ac
227.
0
104
R f
(261
)
105
D b
(262
)
106
S g
(263
)
107
Bh
(262
)
108
H s
(265)
109
Mt
(266
)
110
D b
(269
)
Lanthanide series
Actinide series
= Type I
Metal
= Type II
Metal
= Type III
Non-metal
= Does not
form
compounds
58
C e
140.
1
59
P r
140.
9
60
N d
144.
2
61
P m
(147
)
62
S m
150.
4
63
Eu
152.
0
64
G d
157.
3
65
Tb
158.
9
66
Dy
162.
5
67
H o
164.
9
68
E r
167.
3
69
Tm
168.
9
70
Y b
173.
0
71
Lu
175.
0
90
Th
232.
0
91
P a
231.
0
92
U
238.
0
93
N p
(237
)
94
Pu
(244
)
95
Am
(243
)
96
C m
(247
)
97
B k
(247
)
98
C f
(251
)
99
E s
(252
)
100
F m
(257
)
101
Md
(258
)
102
N o
(259
)
103
L r
(260
)
+3+2
+1
+2
+1
3
Basic Nomenclature 5
“Type II” Elements1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
IA VIII
A
1
H
1.00
8
IIA
IIIA
IVA
VA
VIA
VII
A
2
H e
4.002
3
L i
6.94
1
4
B e
9.01
2
5
B
10.8
1
6
C
12.0
1
7
N
14.0
1
8
O
16.0
0
9
F
19.0
0
10
N e
20.18
11
N a
22.9
9
12
M g 24.3
0 IIIB IVB VB VIB
VII
B VIII VIII VIII IB IIB
13
Al
26.9
8
14
S i
28.0
9
15
P
30.9
7
16
S
32.0
6
17
C l
35.4
5
18
Ar
39.95
19
K
39.1
0
20
C a
40.0
8
21
Sc 44.9
6
22
Ti
47.9
0
23
V
50.9
4
24
C r
52.0
0
25
Mn
54.9
4
26
F e
55.8
5
27
C o
58.9
3
28
N i
58.7
0
29
Cu
63.5
5
30
Zn
65.3
8
31
G a
69.7
2
32
G e
72.5
9
33
As
74.9
2
34
S e
78.9
6
35
B r
79.9
0
36
K r
83.80
37
R b
85.4
7
38
S r
87.6
2
39
Y
88.9
1
40
Z r
91.2
2
41
N b
92.9
1
42
Mo
95.9
4
43
Tc
(99)
44
Ru
101.
1
45
Rh
102.
9
46
P d
106.
4
47
Ag
107.
9
48
C d
112.
4
49
In
114.
8
50
Sn
118.
7
51
S b
121.
8
52
Te
127.
6
53
I 126.
9
54
X e
131.3
55
C s
132.
9
56
B a
137.
3
57
L a
138.
9
72
H f
178.
5
73
Ta
180.
9
74
W
183.
9
75
R e
186.
2
76
O s
190.
2
77
Ir
192.
2
78
P t
195.
1
79
Au
197.
0
80
H g
200.
6
81
Tl
204.
4
82
P b
207.
2
83
B i
209.
0
84
P o
(209
)
85
At
(210
)
86
Rn
(222)
87
F r
(223
)
88
R a
226.
0
89
Ac
227.
0
104
R f
(261
)
105
D b
(262
)
106
S g
(263
)
107
Bh
(262
)
108
H s
(265)
109
Mt
(266
)
110
D b
(269
)
Lanthanide series
Actinide series
= Type I
Metal
= Type II
Metal
= Type III
Non-metal
= Does not
form
compounds
58
C e
140.
1
59
P r
140.
9
60
N d
144.
2
61
P m
(147
)
62
S m
150.
4
63
Eu
152.
0
64
G d
157.
3
65
Tb
158.
9
66
Dy
162.
5
67
H o
164.
9
68
E r
167.
3
69
Tm
168.
9
70
Y b
173.
0
71
Lu
175.
0
90
Th
232.
0
91
P a
231.
0
92
U
238.
0
93
N p
(237
)
94
Pu
(244
)
95
Am
(243
)
96
C m
(247
)
97
B k
(247
)
98
C f
(251
)
99
E s
(252
)
100
F m
(257
)
101
Md
(258
)
102
N o
(259
)
103
L r
(260
)
Basic Nomenclature 6
“Type III” Elements: Nonmetals1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
IA VIII
A
1
H
1.00
8
IIA
IIIA
IVA
VA
VIA
VII
A
2
H e
4.002
3
L i
6.94
1
4
B e
9.01
2
5
B
10.8
1
6
C
12.0
1
7
N
14.0
1
8
O
16.0
0
9
F
19.0
0
10
N e
20.18
11
N a
22.9
9
12
M g 24.3
0 IIIB IVB VB VIB
VII
B VIII VIII VIII IB IIB
13
Al
26.9
8
14
S i
28.0
9
15
P
30.9
7
16
S
32.0
6
17
C l
35.4
5
18
Ar
39.95
19
K
39.1
0
20
C a
40.0
8
21
Sc 44.9
6
22
Ti
47.9
0
23
V
50.9
4
24
C r
52.0
0
25
Mn
54.9
4
26
F e
55.8
5
27
C o
58.9
3
28
N i
58.7
0
29
Cu
63.5
5
30
Zn
65.3
8
31
G a
69.7
2
32
G e
72.5
9
33
As
74.9
2
34
S e
78.9
6
35
B r
79.9
0
36
K r
83.80
37
R b
85.4
7
38
S r
87.6
2
39
Y
88.9
1
40
Z r
91.2
2
41
N b
92.9
1
42
Mo
95.9
4
43
Tc
(99)
44
Ru
101.
1
45
Rh
102.
9
46
P d
106.
4
47
Ag
107.
9
48
C d
112.
4
49
In
114.
8
50
Sn
118.
7
51
S b
121.
8
52
Te
127.
6
53
I 126.
9
54
X e
131.3
55
C s
132.
9
56
B a
137.
3
57
L a
138.
9
72
H f
178.
5
73
Ta
180.
9
74
W
183.
9
75
R e
186.
2
76
O s
190.
2
77
Ir
192.
2
78
P t
195.
1
79
Au
197.
0
80
H g
200.
6
81
Tl
204.
4
82
P b
207.
2
83
B i
209.
0
84
P o
(209
)
85
At
(210
)
86
Rn
(222)
87
F r
(223
)
88
R a
226.
0
89
Ac
227.
0
104
R f
(261
)
105
D b
(262
)
106
S g
(263
)
107
Bh
(262
)
108
H s
(265)
109
Mt
(266
)
110
D b
(269
)
Lanthanide series
Actinide series
= Type I
Metal
= Type II
Metal
= Type III
Non-metal
= Does not
form
compounds
58
C e
140.
1
59
P r
140.
9
60
N d
144.
2
61
P m
(147
)
62
S m
150.
4
63
Eu
152.
0
64
G d
157.
3
65
Tb
158.
9
66
Dy
162.
5
67
H o
164.
9
68
E r
167.
3
69
Tm
168.
9
70
Y b
173.
0
71
Lu
175.
0
90
Th
232.
0
91
P a
231.
0
92
U
238.
0
93
N p
(237
)
94
Pu
(244
)
95
Am
(243
)
96
C m
(247
)
97
B k
(247
)
98
C f
(251
)
99
E s
(252
)
100
F m
(257
)
101
Md
(258
)
102
N o
(259
)
103
L r
(260
)
4
Basic Nomenclature 7
Nomenclature Periodic Table1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
IA VIII
A
1
H
1.00
8
IIA
IIIA
IVA
VA
VIA
VII
A
2
H e
4.002
3
L i
6.94
1
4
B e
9.01
2
5
B
10.8
1
6
C
12.0
1
7
N
14.0
1
8
O
16.0
0
9
F
19.0
0
10
N e
20.18
11
N a
22.9
9
12
M g 24.3
0 IIIB IVB VB VIB
VII
B VIII VIII VIII IB IIB
13
Al
26.9
8
14
S i
28.0
9
15
P
30.9
7
16
S
32.0
6
17
C l
35.4
5
18
Ar
39.95
19
K
39.1
0
20
C a
40.0
8
21
Sc 44.9
6
22
Ti
47.9
0
23
V
50.9
4
24
C r
52.0
0
25
Mn
54.9
4
26
F e
55.8
5
27
C o
58.9
3
28
N i
58.7
0
29
Cu
63.5
5
30
Zn
65.3
8
31
G a
69.7
2
32
G e
72.5
9
33
As
74.9
2
34
S e
78.9
6
35
B r
79.9
0
36
K r
83.80
37
R b
85.4
7
38
S r
87.6
2
39
Y
88.9
1
40
Z r
91.2
2
41
N b
92.9
1
42
Mo
95.9
4
43
Tc
(99)
44
Ru
101.
1
45
Rh
102.
9
46
P d
106.
4
47
Ag
107.
9
48
C d
112.
4
49
In
114.
8
50
Sn
118.
7
51
S b
121.
8
52
Te
127.
6
53
I 126.
9
54
X e
131.3
55
C s
132.
9
56
B a
137.
3
57
L a
138.
9
72
H f
178.
5
73
Ta
180.
9
74
W
183.
9
75
R e
186.
2
76
O s
190.
2
77
Ir
192.
2
78
P t
195.
1
79
Au
197.
0
80
H g
200.
6
81
Tl
204.
4
82
P b
207.
2
83
B i
209.
0
84
P o
(209
)
85
At
(210
)
86
Rn
(222)
87
F r
(223
)
88
R a
226.
0
89
Ac
227.
0
104
R f
(261
)
105
D b
(262
)
106
S g
(263
)
107
Bh
(262
)
108
H s
(265)
109
Mt
(266
)
110
D b
(269
)
Lanthanide series
Actinide series
= Type I
Metal
= Type II
Metal
= Type III
Non-metal
= Does not
form
compounds
58
C e
140.
1
59
P r
140.
9
60
N d
144.
2
61
P m
(147
)
62
S m
150.
4
63
Eu
152.
0
64
G d
157.
3
65
Tb
158.
9
66
Dy
162.
5
67
H o
164.
9
68
E r
167.
3
69
Tm
168.
9
70
Y b
173.
0
71
Lu
175.
0
90
Th
232.
0
91
P a
231.
0
92
U
238.
0
93
N p
(237
)
94
Pu
(244
)
95
Am
(243
)
96
C m
(247
)
97
B k
(247
)
98
C f
(251
)
99
E s
(252
)
100
F m
(257
)
101
Md
(258
)
102
N o
(259
)
103
L r
(260
)
Basic Nomenclature 8
Nomenclature: Cation BasicsTo name a cation (or the first element in a Type III
compound): Type I: Use the name of the element; if you are talking
about an ion by itself put ‘ion’ after the name:Na+ = sodium ion; Mg+2 = magnesium ionSpecial cations: NH4
+ = ammonium ion;H3O+ = hydronium ion
Type II: Use the name of the element AND itsoxidation state (or charge); use roman numerals inparentheses to denote this; if you are talking about anion by itself put ‘ion’ after the name:
Cu+2 = copper (II) ion; Cr+6 = chromium (IV) ion Type III : Use the name; denote number of that
element present using greek prefixes (more later)
5
Basic Nomenclature 9
Nomenclature: Anion BasicsTo name a monatomic anion (OR the second element in a
binary Type III compound): For ALL: Take the root name of the element and add
-ide to the end: if you are talking about an ion by itselfput ‘ion’ after the name:
Cl- = chloride ion; S-2 = sulfide ion; P-3 = phosphide ion Type III Compounds ONLY: Add to the name of the
second element a prefix denoting how many of thatelement there are:
XO2 would be “X dioxide”
POLYATOMIC ANIONS: These have their ownnomenclature you need to know
Basic Nomenclature 10
Nomenclature: Polyatomic AnionsLearn these polyatomic anions NOW:
NO3- Nitrate
NO2- Nitrite
OH- HydroxideMnO4
- PermanganateCO3
-2 CarbonateSO4
-2 SulfateSO3
-2 SulfiteC2O4
-2 OxalateCrO4
-2 ChromateCr2O7
-2 DichromateSCN- ThiocyanateCN- CyanideHPO4
-2 Hydrogen PhosphatePO4
-3 Phosphate
HCO3- Hydrogen carbonate
HS- Hydrogen sulfideHSO4
- Hydrogen sulfateHSO3
- Hydrogen sulfiteH2PO4
- Dihydrogen phosphateClO4
- PerchlorateClO3
- ChlorateClO2
- ChloriteClO- HypochloriteBrO3
- BromateBrO2
- BromiteBrO- HypobromiteIO4
- PeriodateIO3
- IodateC2H3O2
- Acetate
6
Basic Nomenclature 11
Nomenclature: Polyatomic AnionsLearn these polyatomic anions NOW:
NO3- Nitrate
NO2- Nitrite
OH- HydroxideMnO4
- PermanganateCO3
-2 CarbonateSO4
-2 SulfateSO3
-2 SulfiteC2O4
-2 OxalateCrO4
-2 ChromateCr2O7
-2 DichromateSCN- ThiocyanateCN- CyanideHPO4
-2 Hydrogen PhosphatePO4
-3 Phosphate
HCO3- Hydrogen carbonate
HS- Hydrogen sulfideHSO4
- Hydrogen sulfateHSO3
- Hydrogen sulfiteH2PO4
- Dihydrogen phosphateClO4
- PerchlorateClO3
- ChlorateClO2
- ChloriteClO- HypochloriteBrO3
- BromateBrO2
- BromiteBrO- HypobromiteIO4
- PeriodateIO3
- IodateC2H3O2
- Acetate
Basic Nomenclature 12
Nomenclature: OxyanionsSystematic nomenclature based on oxoacids of origin;End in -ate or -ite; may have per- or hypo- as prefixes;Learn name, formula, and charge of all -ate ions, then:
a) If an ion has ONE LESS oxygen than the -ate ion, change -ate to-ite (charge does not change!);
b) If an ion has TWO LESS oxygens than the -ate ion, change -ateto -ite and add hypo- as a prefix (charge does not change!);
c) If an ion has ONE MORE oxygen than the -ate ion, add per- as aprefix (charge does not change!).
ClO3 ClO2 ClOClO4
One
more O
One
lessO
Two
less O
chlorateperchlorate chlorite hypochlorite
7
Basic Nomenclature 13
Nomenclature: Type I and II Compounds
Simple: take name of cation and anion andcombine:
CaCl2 = calcium chlorideZnS = zinc sulfide
Ba3(PO4)2 = barium phosphateCrO3 = chromium (VI) oxide
PbI4 = lead (IV) oxideFe2O3 = iron (III) oxide
Basic Nomenclature 14
Determining cation charge for Type II ions• Based on knowing your anions and their
charges!• A compound is neutral and has a charge of
zero.• The sum of all the oxidation states in a
compound must equal the overall charge on theion or molecule.
• Set up and solve for the unknown algebraically;so for Fe2O3:
# irons( ) ! charge of iron( )"# $% + # oxygens( ) ! charge of oxygen( )"# $% = charge of Fe2O3
2x( )"# $% + 3 &2( )( )"# $% = 0; solve to get x = +3
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Basic Nomenclature 15
Nomenclature: Type III Compounds
1. START by naming as if it were a Type I compound:N2F4: nitrogen fluoride
2. THEN add a greek prefix to tell how MANY of eachelement there are:
N2F4: dinitrogen tetrafluoride* Note: if there is only one of the first element, the
prefix mono is NOT used:SO2 is sulfur dioxide NOT monosulfur dioxide
1 = mono 2 = di 3 = tri 4 = tetra 5 = penta6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca
Basic Nomenclature 16
Nomenclature: PracticeTry the following:
C2O4
Na2SO3
MgOCrO2
P5O10
AsO3
SeO4
Al2Cr2O7
Mo(CO3)2
Rh(NO3)5
H2ON2O
Give yourself five minutes
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Basic Nomenclature 17
Nomenclature: PracticeAnswers:
C2O4 dicarbon tetroxideNa2SO3 sodium sulfiteMgO magnesium oxideCrS2 chromium (IV) sulfideP5O10 pentaphosphorous decoxideAsO3 arsenic trioxide
Basic Nomenclature 18
Nomenclature: PracticeAnswers:
SeO4 selenium tetroxideAl2Cr2O7 aluminum dichromateMo(CO3)2 molybdenum (IV) carbonateRh(NO3)5 rhodium (V) nitrateH2O dihydrogen monoxideN2O dinitrogen monoxide
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Basic Nomenclature 19
Nomenclature: Exceptions (1)1. Some compounds have been known and used for so long
that their trivial (or common names) have becomeaccepted by the IUPAC as official:
H2O = water CH4 = methane PH3 = phosphineNH3 = ammonia SiH4 = silane N2H4 = hydrazine
2. Oxides of some nonmetals will sometimes be named as ifthey were Type II compounds:
P2O5 = phosphorous (V) oxide; SeO4 = selenium (VI) oxide
Note: this is an older system that is slowly being phased out
Basic Nomenclature 20
Nomenclature: Exceptions (2)3. For Type II metals with only two common oxidation states an
older, Latin system was once used; while it is not employedvery often it is useful to know some simple rules regarding it.It is sometimes called the “-ous/-ic” system, where theLOWER charged cation will be denoted by the latin rootname for that element plus -ous and the HIGHER chargedcation will be denoted by the latin root name for that elementplus -ic :
Fe2+ = ferrous ion/Fe3+ = ferric ion; Sn2+ = stannous ion/Sn4+ = stannic ionNot used much but still can be found being employed
4. Compounds containing hydrogen listed as the first element areacids and named differently, as are many carbon compounds.
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Basic Nomenclature 21
Acid NomenclatureAn acid is a compound that contains an acidic
hydrogen (a H that ionizes in water) :
Not all hydrogens are ionizable; by convention, toindicate when one IS, we begin the chemicalformula with it:HC2H3O2 (acetic acid) has four hydrogens but only ONE
is acidic (underlined for emphasis)There are two types of acids: binary and oxoacids
HX(aq)!"! H+(aq) + X
–(aq)
Basic Nomenclature 22
Binary Acid NomenclatureFor BINARY acids (HX(aq), where X does NOT
contain oxygen; it MUST be in aqueous solution);Add hydro…ic acid to the root of the element X:
H2S(aq) = hydrosulfuric acid; HI(aq) = hydroiodic acid;HN3 (aq) = hydrazoic acid
Note: if phase is NOT aqueous, name as if it were a Type Icompound (even though they are considered to bemolecular in nature):
H2S(g) = hydrogen sulfide; HI(g) = hydrogen iodide;HN3 (l) = hydrogen azide
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Basic Nomenclature 23
Oxoacid NomenclatureIf the acid contains oxygen (HOX or HXOn) its name will be a
function of the name of the anion portion (i.e. the portionremaining after all the acidic H’s have been removed: OX- orXOn
-); so:– Determine the anion name;
If the name ends in -ate, replace -ate with -ic acidIf the name ends in -ite, replace -ite with -ous acid
Leave prefixes alone; the root name is sometimes tweaked to aid inpronunciation
H2SO4(aq) → anion is SO4-2 (sulfate) → acid name is sulfuric acid
HClO(aq) → anion is ClO- (hypochlorite) → acid name is hypochlorous acid
Basic Nomenclature 24
Acid Nomenclature: PracticeTry the following:
H2C2O4
H2SO3
HCNH2CrO4
H3PO4
H2Se
HIO4
H2CO3
HFHC2H3O2
HNO3 HNO2
Give yourself five minutes
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Basic Nomenclature 25
Acid Nomenclature: PracticeAnswers:
H2C2O4 oxalic acidH2SO3 sulfurous acidHCN hydrocyanic acidH2CrO4 chromic acidH3PO4 phosphoric acidH2Se hydroselenic acid
Basic Nomenclature 26
Acid Nomenclature: PracticeAnswers:
HIO4 periodic acidH2CO3 carbonic acidHF hydrofluoric acidHC2H3O2 acetic acidHNO3 nitric acidHNO2 nitrous acid