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

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 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 formulas:

•potassium oxide

• zinc chloride

• silver sulfide

• aluminum nitride

• gallium oxide

•calcium iodide

Write the names:

• K3N

• AgI

• ZnBr2

• Al2O3

• Ba3P2

• 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:

• 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

Examples: Type II Binary Ionic CompoundsWrite 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

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 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 Ionsa) 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 Ionsa) 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 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 SO4

2-

chlorate ClO3- sulfite SO3

2-

chlorite ClO2-

hypochlorite ClO- nitrate NO3-

nitrite NO2-

More Formulas with Complex Ionsa) 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 Ionsa) 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 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 hexadi heptatri octatetra nonapenta deca

CuSO4 · 5 H2O

copper (II) sulfate pentahydrate

MgCO3 ·10 H2O

magnesium carbonate decahydrate

Examples of hydrates: Write the formulas:

copper(II) fluoride tetrahydrate

calcium nitrate trihydrate

Write the names:

MgSO4 · 7 H2O

FeCl2 · H2O

CuF2 ·4 H2O

Ca(NO3)2 ·3 H2O

magnesium sulfate heptahydrate

iron (II) chloride monohydrate

Examples of hydrates: Write the formulas:

copper(II) fluoride tetrahydrate

calcium nitrate trihydrate

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- SO4

2- CO32- PO4

3-

nitric acid: HNO3

sulfuric acid: H2SO4

carbonic acid: H2CO3

phosphoric acid: H3PO4

Chloric acid HClO3

Can you propose a rule for naming oxy-acids

with complex ions ending in “ate”?

More Oxy-Acids Complex ions ending in “ite”:

NO2- SO3

2- ClO- ClO2-

nitrous acid: HNO2

sulfurous acid: H2SO3

hypochlorous acid: HClO

( from hypochlorite ion)

chlorous acid HClO2

Can you propose a rule for naming oxy-acids

with complex ions ending in “ite”?

Acids Nitric Acid Nitrous acid Hyposulphurous acid Perchloric acid

Acids Nitric Acid HNO3

Nitrous acid HNO2

Hyposulphurous acid H2SO2

Perchloric acid HClO4

Acid SaltsAcid 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: HPO4

2-

dihydrogen phosphate: H2PO4-

More Formulas with Complex Ionsa) 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 Ionsa) 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 Fe2(SO3)3

f) Cuprous hydrogen hyposulphite CuHSO2

g) Zinc periodate Zn(IO4)2

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

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. 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 Write the names:

SO2

P4O10

Write the formulas:

phosphorus pentachloride

dinitrogen trioxide

Examples of Covalent Naming Write the names:

SO2 sulfur dioxide

P4O10 tetraphosphorus decoxide

Write the formulas:

phosphorus pentachloride PCl5

dinitrogen trioxide N2O3