Ionic Naming

Objective/Warm-up SWBAT name ionic compounds.

Criss-Cross the following:

1) Ca+2 and SO4-2

2) Na+1 and PO4-3

3) Al+3 and O-2

4) Mg+2 and N-3

Definitions An IONIC COMPOUND consists of a metal

cation bonded to a nonmetal anion. Electrostatic attraction holds them together.

Metal Cation Nonmetal anion Na+ Cl-

A quick review

Do you remember how to find the charges on different elements from the periodic table?

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

Lets do some practice

Examples: Type I Binary Ionic Compounds

Write the formulas:

•potassium oxide

• zinc chloride

• silver sulfide

• aluminum nitride

• gallium oxide

•calcium iodide

OK 2

2ZnClSAg 2

AlN

32OGa

2CaI

Write the names:

• K3N

• AgI

• ZnBr2

• Al2O3

• Ba3P2

• LiH

•Potassium Nitride

•Silver Iodide

•Zinc Bromide

•Aluminum Oxide

•Barium Phosphide

•Lithium Hydride

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

FeO

CuCl2

SnS2

Ni2O3

23NCu

Examples: Type II Binary Ionic Compounds

Write the names:

• Fe2O3

• SnS

• NiBr2

•CuS

• Pb3P2

• CuBr

• FeCl3

•iron (III) oxide

•Tin (II) Sulfide

•Nickel (II) Bromide

•Copper (II) Sulfide

•Lead (II) Phosphide

•Copper(I) Bromide

•iron (III) Chloride

Polyatomic (Complex) Ions All of the cations and anions so far have been simple

ions - single atoms that have lost or gained electrons.

A complex ion is a charged molecule. Complex ions may be cations or anions.

examples:

nitrate: NO3-sulfate: SO4

2- hydroxide: OH-

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-

Lets do some practice

Use the handout to write the names for the following.

Writing formulas with Complex IonsA. NH4Cl

B. Ag2SO4

C. Al(OH)3

D. Ca3(PO4)2

E. Fe(NO2)3

F. Cu(MnO4)2

G. (NH4)2Cr2O7

H. Zn(CH3COO)2

a) Ammonium chloride

b) Silver sulfate

c) Aluminum hydroxide

d) Calcium phosphate

e) Iron (III) nitrite

f) Copper(II) permanganate

g) Ammonium dichromate

h) Zinc acetate

Objective/ Warm-up SWBAT write formulas and name ionic

compounds. Please give the name for the following

formulas:(a) Ag3P (b) Fe2O3 (c) Ag2SO4

Please give formulas for the following names:

(a) Tin (II) Sulfide (b) Iron (III) nitrite

Closure

When do we need to use roman numerals in a name?