1. Chemical Nomenclature
1. Binary Ionic Compounds - Type I
2. Binary Ionic Compounds - Type II
3. Ionic Compounds & Polyatomic (Complex) Ions
4. Hydrated Ionic Compounds
5. Binary Covalent Compounds
6. Binary Acids
7. Oxy-Acids

2. Definitions
An IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together.
A COVALENT COMPOUND consists of two nonmetal atoms sharing valence electrons.
A BINARY compound is one that is made of just two elements.

3. Type I Binary Ionic Compounds
The metal cations in these compounds have only ONE possible charge.
Na+ Zn2+ Al3+ Ca2+
sodium zinc aluminum calcium
The charges are memorized or predicted using a periodic table!
The cations are bonded to nonmetal anions:
O2- N3- F- Br -
oxide nitride fluoride bromide
Notice that simple anions are always named with the suffix “ide”

4. 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- ® NaCl
lithium oxide: Li+ and O2- ® Li2O
aluminum bromide: Al3+ and Br - ® AlBr3
zinc nitride: Zn2+ and N3- ® Zn3N2
potassium iodide: K+ and I- ® KI
silver phosphide: Ag+ and P3- ® Ag3P

5. Examples: Type I Binary Ionic Compounds
Write the formulas:
potassium oxide
zinc chloride
silver sulfide
aluminum nitride
gallium oxide
calcium iodide
Write the names:
K3N
AgI
ZnBr2
Al2O3
Ba3P2
LiH

6. Type II Binary Ionic Compounds
These are ionic compounds where the metal cation can form TWO different charges.
Fe2+ iron (II) Fe3+ iron (III)
Ni nickel (II) Ni nickel (III)
Co2+ cobalt (II) Co3+ cobalt (III)
Cu copper (I) Cu2+ copper (II)
Au gold (I) Au3+ gold (III)
Sn 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

7. Examples: Type II Binary Ionic Compounds
Write the formulas:
iron (II) oxide
copper (II) chloride
tin (IV) sulfide
cupric nitride
nickel (III) oxide
ferrous iodide
cobalt (III) selenide
Write the names:
Fe2O3
SnS
NiBr2
CuS
Pb3P2
CuBr
FeCl3

8. Polyatomic (Complex) Ions
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-

9. 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) nitrite Fe(NO2)3
f) Copper(II) permanganate Cu(MnO4)2
g) Ammonium dichromate (NH4)2Cr2O7
h) Zinc acetate Zn(CH3COO)2

10. Things to Notice
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:
perchorate ClO4- sulfate SO42-
chlorate ClO3- sulfite SO32-
chlorite ClO2-
hypochlorite ClO- nitrate NO3-
nitrite NO2-

11. If an 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 net charge:
examples:
Sulfide: S2- hydrogen sulfide: HS-
(bisulfide)
Sulfate: SO42- hydrogen sulfate: HSO4-
(bisulfate)
Carbonate: CO32- hydrogen carbonate: HCO3-
(bicarbonate)
Phosphate: PO43- hydrogen phosphate: HPO42-
dihydrogen phosphate: H2PO4-

12. More Formulas with Complex Ions
a) Sodium bicarbonate NaHCO3
b) Nickel (II) hydrogen sulfide Ni(HS)2
c) Aluminum perchlorate Al(ClO4)3
d) Barium dihydrogen phosphate Ba(H2PO4)2
e) Iron (III) sulfite Fe2(SO2)3
f) Cuprous bisulfate CuHSO4
g) Zinc periodate Zn(IO4)2
h) Lithium selenite Li2SeO3

13. Hydrated Ionic Compounds
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.
mono hexa
di hepta
tri octa
tetra nona
penta deca
CuSO4 · 5 H2O
copper (II) sulfate pentahydrate
MgCO3 ·10 H2O
magnesium carbonate decahydrate

14. Examples of hydrates: 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

15. Binary Covalent Compounds
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.
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!

16. Examples of Covalent Naming
Write the names:
SO2 sulfur dioxide
P4O10 tetraphosphorus decoxide
Write the formulas:
phosphorus pentachloride PCl5
dinitrogen trioxide N2O3

17. Binary Acids
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 HBr H2S
hydrochloric acid hydrobromic acid hydrosulfuric acid
Binary acids are always named: hydro____ic acid

18. Oxy-Acids
An acid can also be made of a hydrogen ion bonded to a complex ion.
Complex ions whose names end in “ate”:
NO SO42- CO32- PO43-
nitric acid: HNO3
sulfuric acid: H2SO4
carbonic acid: H2CO3
phosphoric acid: H3PO4
Can you propose a rule for naming oxy-acids with complex ions ending in “ate”?

19. More Oxy-Acids Complex ions ending in “ite”: NO2- SO32- ClO- ClO2-
nitrous acid: HNO2
sulfurous acid: H2SO3
hypochlorous acid: HClO
chlorous acid HClO2
Can you propose a rule for naming oxy-acids with complex ions ending in “ite”?