1. Molecular Compounds

2. Molecular Compounds form between nonmetals and nonmetals. (ex. S 2 O 4 ) Covalent bonds form when atoms share electrons. Neither atoms gain or lose electrons because their electronegativity values are very close.

3. Naming Binary Molecular Compounds To name molecular compounds, use prefixes to show how many atoms of each element there are. Exception: do not show a prefix if the first element has only one atom. Note: Do NOT reduce if the element ratio is not in lowest terms. Similar to ionic compounds – last element ends in -ide

4. Prefix# atoms mono 1 di2 tri3 tetra4 penta5 hexa6 hepta7 octa8 nona9 deca10

5. Name the following molecular (covalent) compound: SiF 4 1.Monosilicon fluoride 2.Sulfur fluoride 3.Monosilicon tetrafluoride 4.Silicon tetrafluoride 5.Silicon quadfluoride

6. Name the following molecular (covalent) compound: SO 3 1.Sulfur trioxide 2.Sulfur oxide 3.Sulfur dioxide 4.Monosulfur trioxide

7. Name the following molecular (covalent) compound: S 2 F 6 1.Sulfur fluoride 2.Sulfur hexafluoride 3.Disulfur fluoride 4.Disulfur hexafluoride

8. Acid Nomenclature In general, names of acids will begin with hydrogen. If the anion does not contain oxygen, the acid begins with hydro and ends in –ic HCl = hydrochloric acid HBr = HCN =

9. Acids containing oxygen If the acid contains oxygen, the acid does not have hydro at the start and either ends in ic or ous. If the anion ends in –ate use –ic HNO 3 = nitric acid If the anion ends in –ite use –ous H 2 SO 3 = sulfurous acid