III. Ionic Compounds(p. 210 – 224)

Ch. 7 - Chemical Bonding

Formula Unit

A. Energy of Bond Formation

• Lattice Energy–

B. Lewis Structures

• Covalent – show ___________ of e-

• Ionic – show ___________ of e-

C. Ionic NomenclatureIonic Formulas

• Write each ion, _________ first. Don’t show charges in the final formula.

• Overall charge must equal _________.– If charges cancel, just write symbols.– If not, use subscripts to balance charges.

• Use parentheses to show more than one _____________ _______.

• Stock System - ___________ __________ indicate the ion’s charge.

C. Ionic NomenclatureIonic Names

• Write the names of both ions, ________ first.

• Change ending of monatomic ions to -_____.

• Polyatomic ions have special names. (listed on the chemical reference sheets!)

• Stock System - Use ________ __________ to show the ion’s charge if more than one is possible. Overall charge must equal zero.

C. Ionic Nomenclature

• Consider the following:– Does it contain a polyatomic ion?

• -ide, 2 elements no• -ate, -ite, 3+ elements yes

– Does it contain a Roman numeral?• Check the table for metals not in Groups 1 or 2.

– No prefixes!

Common Ion Charges

1+

2+ 3+ 4± 3- 2- 1-

0

C. Ionic Nomenclature

• potassium chloride

• magnesium nitrate

• copper(II) chloride

C. Ionic Nomenclature

• NaBr

• Na2CO3

• FeCl3

C. Ionic Nomenclature

• potassium chloride

• magnesium nitrate

• copper(II) chloride

– K+ Cl

– Mg2+ NO3

– Cu2+ Cl

KCl

Mg(NO3)2

CuCl2

C. Ionic Nomenclature

• NaBr

• Na2CO3

• FeCl3

– sodium bromide

– sodium carbonate

– iron(III) chloride

C. Ionic Nomenclature