1. Nomenclature Continued Chapter 6 Sections 5 and 6

2. 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

3. 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.

4. Greek Prefixes! 1 = mono- 2 = di- 3 = tri- 4 = tetra- 5 = penta- 6 = hexa- 7 = hepta- 8 = octa- 9 = nona- 10 = deca-

5. Examples! OF 2 = SO 3 = Cl 2 O 8 = oxygen difluoride sulfur trioxide dichlorine octoxide

6. 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

7. Examples! Carbon tetrachloride = Diphosphorous pentoxide = Dihydrogen monoxide = CCl 4 P2O5P2O5 H2OH2O

8. 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

9. Common Acids You need to know these! HCl = hydrochloric acid H 2 SO 4 = sulfuric acid HNO 3 = nitric acid HC 2 H 3 O 2 = acetic acid H 3 PO 4 = phosphoric acid H 2 CO 3 = carbonic acid Practice on the back of the common ion sheet!