Chemical
Nomenclature
1. Binary Ionic Compounds - Type I
2. Binary Ionic Compounds - Type II
3. Ionic Compounds & Polyatomic
(Complex) Ions
4. Oxy-Acids
5. Hydrated Ionic Compounds
6. Binary Acids
7. Binary Covalent Compounds
Type I Binary Ionic Compounds
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The metal cations in these compounds have
only ONE possible charge.
Na+
sodium
Zn2+
zinc
Al3+
aluminum
Ca2+
calcium
The charges are memorized or predicted using a periodic table!
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The cations are bonded to nonmetal anions:
O2oxide
N3nitride
Ffluoride
Br bromide
Notice that simple anions are always named with the
suffix “ide”
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In an ionic compound, the charges of the
cations and anions must always cancel out.
Subscripts are used if more than one atom is
needed to cancel the charges:
sodium chloride:
Na+ and Cl- 
lithium oxide:
Li+ and O2- 
aluminum bromide:
Al3+ and Br -  AlBr3
zinc nitride:
Zn2+ and N3-  Zn3N2
potassium iodide:
K+ and I- 
silver phosphide:
Ag+ and P3-  Ag3P
NaCl
Li2O
KI
Examples: Type I Binary Ionic Compounds
Write the formulas:
Write the names:
•potassium oxide
• K3N
• zinc chloride
• AgI
• silver sulfide
• ZnBr2
• aluminum nitride
• Al2O3
• gallium oxide
• Ba3P2
•calcium iodide
• LiH
Type II Binary Ionic Compounds

These are ionic compounds where the metal cation
can form TWO different charges.
Fe2+
iron (II)
Fe3+
iron (III)
Ni2+
nickel (II)
Ni3+
nickel (III)
Co2+
cobalt (II)
Co3+
cobalt (III)
Cu+
copper (I)
Cu2+
copper (II)
Au+
gold (I)
Au3+
gold (III)
Sn2+
tin (II)
Sn4+
tin (IV)
An older system uses suffixes and Latin names, -ous for
the lower charge, -ic for the higher charge:
Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic
Examples: Type II Binary Ionic Compounds
Write the formulas:
Write the names:
• iron (II) oxide
• Fe2O3
• copper (II) chloride
• SnS
• tin (IV) sulfide
• NiBr2
• cupric nitride
•CuS
• nickel (III) oxide
• Pb3P2
• ferrous iodide
• CuBr
•cobalt (III) selenide
• FeCl3
Examples: Type II Binary Ionic Compounds
Write the formulas:
• iron (II) oxide
FeO
• copper (II) chloride
CuCl2
• tin (IV) sulfide SnS2
• cupric nitride Cu3N2
• nickel (III) oxide Ni2O3
• ferrous iodide FeI2
•cobalt (III) selenide
Co2Se3
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Write the names:
Fe2O3 Iron (III) oxide Ferric oxide
SnS Tin(II)sulphide stannous sulfide
NiBr2 Nickle (II) bromide
CuS Copper (II) Sulfide Cupric
sulphide
Pb3P2 L
CuBr
FeCl
Polyatomic (Complex) Ions
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All of the cations and anions so far have been simple
ions - single atoms that have lost or gained electrons.
A molecule is a particle that forms when two or more
atoms bond together.
A complex ion is a charged molecule. Complex ions
may be cations or anions.
examples:
nitrate: NO3-
sulfate: SO42-
hydroxide: OH-
Writing formulas with Complex Ions
a) Ammonium chloride
b) Silver sulfate
c) Aluminum hydroxide
d) Calcium phosphate
e) Iron (III) nitrate
f) Copper(II) permanganate
g) Ammonium dichromate
h) Zinc acetate
Writing formulas with Complex Ions
a) Ammonium chloride
NH4Cl
b) Silver sulfate
Ag2SO4
c) Aluminum hydroxide
Al(OH)3
d) Calcium phosphate
Ca3(PO4)2
e) Iron (III) nitrate
Fe(NO3)3
f) Copper(II) permanganate
Cu(MnO4)2
g) Ammonium dichromate
(NH4)2Cr2O7
h) Zinc acetate
Zn(CH3COO)2
Things to Notice
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Most complex ions are anions. Ammonium, NH4+, is
the most common complex cation.
Several complex ions form a short series of ions.
The ions differ only in the number of oxygen atoms:
perchlorate
ClO4-
sulfate
SO42-
chlorate
ClO3-
sulfite
SO32-
chlorite
ClO2-
hypochlorite
ClO-
nitrate
NO3-
nitrite
NO2-
More Formulas with Complex Ions
a) Sodium carbonate
b) Nickel (II) sulfite
c) Aluminum chlorate
d) Barium phosphite
e) Iron (III) sulfite
f) Cupric sulfate
g) Zinc periodate
More Formulas with Complex Ions
a) Sodium carbonate
Na2CO3
b) Nickel (II) sulfite
NiSO3
c) Aluminum chlorate
Al(ClO3)3
d) Barium phosphite
Ba3(PO3)2
e) Iron (III) sulfite
Fe2(SO3)3
f) Cupric sulfate
CuSO4 copper (II) Sulphate
Cuprous sulphate
Cu2SO4 copper (I)Sulphate
g) Zinc periodate
Zn(IO4)2
Hydrated Ionic Compounds
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A HYDRATE is an salt that has water
molecules trapped within its crystals.
Every hydrate has a certain number of water
molecules associated with each formula unit of the
ionic compound. The number of water molecules is
indicated by using prefixes.
CuSO4 · 5 H2O
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca
copper (II) sulfate pentahydrate
MgCO3 ·10 H2O
magnesium carbonate decahydrate
Examples of hydrates:
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Write the formulas:
copper(II) fluoride tetrahydrate
CuF2 ·4 H2O
calcium nitrate trihydrate
Ca(NO3)2 ·3 H2O
Write the names:
MgSO4 · 7 H2O
magnesium sulfate heptahydrate
FeCl2 · H2O
iron (II) chloride monohydrate
Examples of hydrates:
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Write the formulas:
copper(II) fluoride tetrahydrate
calcium nitrate trihydrate
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Write the names:
MgSO4 · 7 H2O
FeCl2 · H2O
Oxy-Acids

An acid can also be made of a hydrogen ion bonded to a complex
ion.
Complex ions whose names end in “ate”:
NO3-
SO42-
nitric acid:
HNO3
CO32-
sulfuric acid:
H2SO4
carbonic acid:
H2CO3
phosphoric acid:
H3PO4
Chloric acid
HClO3
PO43-
Can you propose a rule
for naming oxy-acids
with complex ions
ending in “ate”?
More Oxy-Acids
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Complex ions ending in “ite”:
NO2-
SO32-
ClO-
nitrous acid:
HNO2
sulfurous acid:
H2SO3
hypochlorous acid:
( from hypochlorite ion)
chlorous acid
HClO
HClO2
ClO2-
Can you propose a rule
for naming oxy-acids
with complex ions
ending in “ite”?
Acids
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Nitric Acid
Nitrous acid
Hyposulphurous acid
Perchloric acid
Acids
Nitric Acid
HNO3
Nitrous acid
HNO2
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Hyposulphurous acid
H2SO2
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Perchloric acid
HClO4
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Acid Salts
Acid Salt ions can be formed if an oxy ion carries a charge like “-2” or “3”, a series of related ions can be formed by adding hydrogen
cations (H+) while still leaving a remainder net charge:
examples:
Sulfate:
SO42-
hydrogen sulfate: HSO4(bisulfate)
Carbonate:
CO32-
hydrogen carbonate:
HCO3-
(bicarbonate)
Phosphate:
PO43-
hydrogen phosphate:
HPO42-
dihydrogen phosphate:
H2PO4-
More Formulas with Complex Ions
a) Sodium hydrogen carbonate
b) Nickel (II) hydrogen sulfate
c) Aluminum perchlorate
d) Barium dihydrogen phosphate
e) Iron (III) sulfite
f) Cuprous Hydrogen hyposulphite
g) Zinc periodate
More Formulas with Complex Ions
a) Sodium bicarbonate
NaHCO3
b) Nickel (II) hydrogen sulfate
Ni(HSO4)2
c) Aluminum perchlorate
Al(ClO4)3
d) Barium dihydrogen phosphate
Ba(H2PO4)2
e) Iron (III) sulfite
f) Cuprous hydrogen hyposulphite
g) Zinc periodate
Fe2(SO3)3
CuHSO2
Zn(IO4)2
Binary Acids
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A simple definition of an “acid” is a substance which
produces H+ ions in water.
Most acids have hydrogen ions in their formulas.
A binary acid composed of a hydrogen cation bonded
to one other element:
HCl
hydrochloric acid
HBr
hydrobromic acid
H2S
hydrosulfuric acid
Binary acids are always named: hydro____ic acid
Binary Covalent Compounds
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Covalent compounds are made of two NONMETAL
elements sharing valence electrons.
There are no ions involved!!
Because there are no charges to help us write the
formulas of covalent compounds, prefixes are used to
indicate the number of each atom present in the
formula. Brandon is awesome.
CO2 is named “carbon dioxide”
CO is named “carbon monoxide”
N2O is named “dinitrogen monoxide”
SO3 is named “sulfur trioxide”
The prefix, “mono”
is never used for
the first element
in the formula!
Examples of Covalent Naming
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Write the names:
SO2
P4O10
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Write the formulas:
phosphorus pentachloride
dinitrogen trioxide
Examples of Covalent Naming
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Write the names:
SO2
sulfur dioxide
P4O10
tetraphosphorus decoxide
Write the formulas:
phosphorus pentachloride
PCl5
dinitrogen trioxide
N 2 O3