Fall 2016 – CH 6A
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Inorganic Nomenclature
Instructor: J.T.
Nomenclature is the process of naming chemical compounds.
Organic chemistry has a completely different set of rules for nomenclature.
There are two types of inorganic compounds that can be formed: ionic compounds and molecular compounds.
Number of Elements Present
1
2
Element
Binary compounds
Atomic
Molecular
He
O2
Metal (1 type cation) +
nonmetal
CaCl2 : calcium chloride
3 or more
Polyatomic Compounds
See Chart 2
Metal (… more types
cations) + nonmetal
FeCl2 : Fe (II) chloride
FeCl3 : Fe (III) chloride
Nonmetal + nonmetal
N2O3
di nitrogen tri oxide
Fall 2016 – CH 6A
Inorganic Nomenclature
Instructor: J.T.
Polyatomic Compounds
Ionic Polyatomic as Acid
Anion contains oxygen
Ionic Polyatomic
Compounds
Name: Cation(s)
& Name: anion
Ending name of anion
-ite
Change to: -ous
-ate
Change to: -ic
Compounds
Note:
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Acid formulas often begin with H
An acid is a substance that dissociates into hydrogen ions (H+) and anions in water.
binary acids make by two elements: HCl, H2S
oxy-acids: H2SO4, HNO3
Polyatomic anion acid:
-ate
-ite
→ -ic acid
→ -ous acid
Fall 2016 – CH 6A
Inorganic Nomenclature
Instructor: J.T.
Selection of Oxy acids
Anion (ion)
𝑆𝑂42−
Sulfate
𝑆𝑂32−
Sulfite
𝑁𝑂3−
Nitrate
𝑁𝑂2−
Nitrite
𝐶𝑂32−
Carbonate
𝐵𝑂33−
Borate
Acid
𝐻2 𝑆𝑂4
Sulfuric acid
𝐻2 𝑆𝑂3
Sulfurous acid
𝐻𝑁𝑂3
Nitric acid
𝐻𝑁𝑂2
Nitrous acid
𝐻2 𝐶𝑂3
Carbonic acid
𝐻3 𝐵𝑂3
Boric acid
Anion (ion)
𝑃𝑂43−
Phosphate
𝑃𝑂33−
Phosphite
𝐼𝑂3−
Iodate
𝐶2 𝐻3 𝑂2−
Acetate
𝐶2 𝑂42−
Oxalate
𝐵𝑟𝑂3−
Bromate
Acid
𝐻3 𝑃𝑂4
Phosphoric acid
𝐻3 𝑃𝑂3
Phosphorous acid
𝐻𝐼𝑂3
Iodic acid
𝐻𝐶2 𝐻3 𝑂2
Acetic acid
𝐻2 𝐶2 𝑂4
Oxalic acid
𝐻𝐵𝑟𝑂3
Bromic acid
Fall 2016 – CH 6A
Inorganic Nomenclature
Instructor: J.T.
The Greek numerical prefixes are used for naming
1
2
mono di
3
tri
4
5
6
7
8
9
10
tetra penta hepta hexa octa nano deca
Ions
Al
Na
Mg
Fe
Fe
Sn
Cation
Anion
𝐸 → 𝐸+ − 𝑒
𝐸 + 𝑒 → 𝐸−
Aluminum
Sodium
Magnesium
Iron
Iron
Tin
Al3+
Na+
Mg2+
Fe3+
Fe2+
Sn4+
Aluminum ion
Sodium ion
Magnesium ion
Iron(III) ion
Iron(II) ion
Tin(IV) ion
Cl
F
Br
I
O
N
Chlorine
Fluorine
Bromine
Iodine
Oxygen
Nitrogen
ClFBrIO2N3-
Chloride ion
Fluoride ion
Bromide ion
Iodide ion
Oxide ion
Nitride ion
Fall 2016 – CH 6A
Inorganic Nomenclature
Polyatomic (3 or more elements) compounds
Formula
NH4+
H3O+
OHCNO22N3NO2NO3ClOClO2ClO3ClO4MnO4C2H3O2C2O42-
Formulas and Names of Some Polyatomic Ions
Name
Formula
Name
2ammonium
carbonate
CO3
hydronium
cyanate
OCN
hydroxide
thiocyanate
SCN
2cyanide
thiosulfate
S2O3
peroxide
CrO42- chromate
azide
Cr2O72- dichromate
nitrite
sulfate
SO422
nitrate
sulfite
SO3 3hypochlorite
phosphate
PO4
chlorite
monohydrogen phosphate
PO433chlorate
dihydrogen phosphate
PO4
perchlorate
hydrogen carbonate (bicarbonate)
HCO3
permanganate HSO4
hydrogen sulfate (bisulfate)
acetate (OAc-) HSO3
hydrogen sulfite (bisulfite)
oxalate
Instructor: J.T.
Fall 2016 – CH 6A
Inorganic Nomenclature
Instructor: J.T.
Note:
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The transition metals may form more than one ion.
This is indicated by assigning a Roman numeral after the metal. The Roman numeral denotes the charge and the oxidation state
of the transition metal ion.
Selected Transition Metal and Metal Cations:
+1 Charge
+2 Charge
+3 Charge
+4 Charge
Aluminum: Al3+
Lead(IV): Pb4+
Iron(II): Fe2+
Iron(III): Fe3+
Tin(IV): Sn4+
Cobalt(II): Co2+
Cobalt(III): Co3+
Copper(I): Cu+ Copper(II): Cu2+
Silver: Ag+
Tin(II): Sn2+
Lead(II): Pb2+
Nickel: Ni2+
Zinc: Zn2+
Fall 2016 – CH 6A
Inorganic Nomenclature
Transition Metal Ion with Roman Numeral
Instructor: J.T.
Latin name
Copper (I): Cu+
Cuprous
Copper (II): Cu2+
Cupric
Iron (II): Fe2+
Ferrous
Iron (III): Fe3+
Ferric
Lead (II): Pb2+
Plumbous
Lead (IV): Pb4+
Plumbic
Mercury (I): Hg22+
Mercurous
Mercury (II): Hg2+
Mercuric
Tin (II): Sn2+
Stannous
Tin (IV): Sn4+
Stannic
Note:
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We do not use Roman numerals after names of: Aluminum, Zinc, and Silver, because these metals only exist in one ion.
.
Compounds between Nonmetals and Nonmetals (Molecular Compounds):
Compounds that consist of a nonmetal bonded to a nonmetal are commonly known as Molecular Compounds, where the element with the positive
oxidation state is written first. In many cases, nonmetals form more than one binary compound, so prefixes are used to distinguish them.
Fall 2016 – CH 6A
Inorganic Nomenclature
Instructor: J.T.
Number of atoms & Prefixes
1
2 3
4
5
6
7
8
9
10
mono di tri tetra penta hexa Hepta octa nano deca
Example:
CO = carbon monoxide
BCl3 = borontrichloride
CO2 = carbon dioxide
N2O5 =dinitrogen pentoxide
Note:
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The prefix mono- is not used for the first element.
An acid is a substance that dissociates into hydrogen ions (H+) and anions in water.
Selected common binary acids
Gas State
Formula
𝐻𝐹(𝑔)
𝐻𝐵𝑟(𝑔)
𝐻𝐶𝑙(𝑔)
𝐻2 𝑆(𝑔)
Aqueous State
Name
Hydrogen fluoride
Hydrogen bromide
Hydrogen chloride
Hydrogen sulfide
Formula
𝐻𝐹(𝑎𝑞)
𝐻𝐵𝑟(𝑎𝑞)
𝐻𝐶𝑙(𝑎𝑞)
𝐻2 𝑆(𝑎𝑞)
Name
Hydrofluoric acid
Hydrobromic acid
Hydrochloric acid
Hydrosulfuric acid
Polyatomic Ions
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Polyatomic (meaning two or more atoms) are joined together by covalent bonds.
→
hypo — ite
−
𝐶𝑙𝑂
hypochlorite
Increasing number of oxygen atoms
— ate
— ite
𝐶𝑙𝑂2−
Example:
chlorite
Common Polyatomic ions
𝐶𝑙𝑂3−
chlorate
per — ate
𝐶𝑙𝑂4−
perchlorate
Fall 2016 – CH 6A
Inorganic Nomenclature
Name: Cation Anion Formula
Ammonium ion
NH4+
Hydronium ion
H3O+
Acetate ion
C2H3O2Arsenate ion
AsO43-
Thiocyanate ion
CO32ClOClO2ClO3ClO4CrO42Cr2O72CNOHNO2NO3C2O42MnO4PO43SO32SO42SCN-
Thiosulfate ion
S2O32-
Carbonate ion
Hypochlorite ion
Chlorite ion
Chlorate ion
Perchlorate ion
Chromate ion
Dichromate ion
Cyanide ion
Hydroxide ion
Nitrite ion
Nitrate ion
Oxalate ion
Permanganate ion
Phosphate ion
Sulfite ion
Sulfate ion
Instructor: J.T.