Nomenclature

ContinuedChapter 6 Sections 5 and 6

Review of Ionic Compounds

• Metal with non-metal(s)• Cation with anions• Charges must add up to be zero• If the cation can have multiple

charges then Roman Numerals must be used

Molecular (Covalent) Compounds

• Two or more non-metals (no charges)To determine the name from the formula:

1. Write the name of the first element.2. If there is more than one of the first

element then a Greek prefix must be used to indicate how many atoms are present.

3. Write the name of the second element, change the suffix to –ide, and use Greek prefixes to show how many are present.

Greek Prefixes!

1 = mono-

2 = di-

3 = tri-

4 = tetra-

5 = penta-

6 = hexa-

7 = hepta-

8 = octa-

9 = nona-

10 = deca-

Examples!

OF2 =

SO3 =

Cl2O8 =

oxygen difluoride

sulfur trioxide

dichlorine octoxide

To determine the formula from the name:

1. Write the symbol for the first element and use the prefix to determine the subscript.

2. Repeat step 1 for the second element

Examples!

Carbon tetrachloride =

Diphosphorous pentoxide =

Dihydrogen monoxide =

CCl4

P2O5

H2O

Naming Acids

• Anions connected to as many hydrogen ions (H+) as are necessary to make the compound electrically neutral.

• If the anion ends with –ate then the acid is changed to –ic

• If the anion ends with –ite then the acid is changed to –ous

• If the anion ends with –ide then the acid is hydro- -ic

Common AcidsYou need to know these!

HCl = hydrochloric acidH2SO4 = sulfuric acid

HNO3 = nitric acid

HC2H3O2 = acetic acid

H3PO4 = phosphoric acid

H2CO3 = carbonic acid

Practice on the back of the common ion sheet!