1. Nomenclature System of naming compounds

2. Molecular Nomenclature Naming covalent compounds Based on a system of prefixes

3. One mono-sixhexa- Twodi-sevenhepta- Threetri-eightocta- Fourtetra-ninenona- Fivepenta-tendeca-

4. Examples of Molecular Names CO 2 CO P 2 O 5 CCl 4

5. Ion Formed when electrons are added or removed from an atom Gain electrons – become negative - Anion Lose electrons – become positive - Cation

6. Why Form Ions Atoms gain or lose electrons to end up with the same number of electrons as the nearest noble gas Predict the charges expected by O Ba

7. Ion Generalizations Metals generally form + charges, while non- metals form – charges Ionic compounds tend to be composed of a metal combined with a non-metal Molecular compounds usually are two non- metals

8. Polyatomic Ions Atoms joined in a molecule but have a net charge – (SO 4 ) 2- – NO 3 -

9. Finding Formulas from Names Calcium nitrate Copper (I) carbonate

10. Names from Formulas AlCl 3 K(NO 3 ) Al 2 O 3 Fe 3 (PO 4 ) 2

11. Acid Names Acids all start with an H For binary acids (H and one other element), start with prefix hydro- and end with suffix –ic

12. Oxyacids H, O and another element If anion has an –ate ending, give acid an –ic ending If anion has an –ite ending, give acid an –ous ending