Chemical Nomenclature 1. Binary Covalent Compounds 2. Binary Ionic Compounds - Type I 3. Binary Ionic Compounds - Type II 4. Ionic Compounds & Polyatomic.

Chemical Nomenclature

1. Binary Covalent Compounds

2. Binary Ionic Compounds - Type I

3. Binary Ionic Compounds - Type II

4. Ionic Compounds & Polyatomic (Complex) Ions

5. Hydrated Ionic Compounds

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”

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

Examples: Type I Binary Ionic Compounds

Write the formula: K+ O2-

K2O

Name the compound:

Potassium oxide

Examples: Type I Binary Ionic Compounds

Write the formula:

Zn2+ Cl-

ZnCl2

Name the compound:

zinc chloride

Examples: Type I Binary Ionic Compounds

Write the formula: Ag+ S2-

Ag2SName the compound:

silver sulfide

Examples: Type I Binary Ionic Compounds

Write the formula: Al3+ N3-

AlN

aluminum nitrideName the compound:

Examples: Type I Binary Ionic Compounds

Write the formula: Ga3+ O2-

Ga2O3

Name the compound:

gallium oxide

Examples: Type I Binary Ionic Compounds

Write the formula: Ca2+ I-

CaI2

calcium iodide

Name the compound:

Examples: Type I Binary Ionic Compounds

Write the name:

K3Npotassium nitride

Write the ions:

K+ N3-

Examples: Type I Binary Ionic Compounds

Write the name:

AgIsilver iodideWrite the ions:

Ag+ I-

Examples: Type I Binary Ionic Compounds

Write the name:

ZnBr2

zinc bromide

Write the ions:

Zn2+ Br -

Examples: Type I Binary Ionic Compounds

Write the names:

Al2O3

aluminum oxideWrite the ions:

Al3+ O2-

Examples: Type I Binary Ionic Compounds

Write the names:

Ba3P2

barium phosphide

Write the ions:

Ba2+ P3-

Examples: Type I Binary Ionic Compounds

Write the name:

LiHlithium hydride

Write the ions:

Li+ H-

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:

• 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

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: SO4

2- hydroxide: OH-

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

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 SO4

2-

chlorate ClO3- sulfite SO3

2-

chlorite ClO2-

hypochlorite ClO- nitrate NO3-

nitrite NO2-

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: HPO4

2-

dihydrogen phosphate: H2PO4-

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

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

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