1. Molecules, Compounds, & Chemical Equations

2. Overview Chemical Nomenclature – Hydrates – Covalent Bonding – Acids & Bases Naming Binary Acids & Oxyacids

3. Chemical Nomenclature What are Hydrates? – Ionic compounds that contain a specific number of water molecules associated with each formula unit. – Water molecules associated with each formula unit called waters of hydration. – Hydrate without water present is termed anhydous salt.

4. Chemical Nomenclature Naming Hydrates – Use system for naming ionic compounds. – Number of water molecules named using Greek prefix followed by the word hydrate.

6. Example Hydrate HydrateCobalt (II) chloride hexahydrate Anhydrous saltCobalt (II) chloride

7. Chemical Nomenclature Naming Binary Covalent Compounds – Use Greek prefixes to denote number of nonmetal atoms in formula. – Name the first nonmetal as it appears in the table. – Name the second nonmetal but change the ending to –ide.

9. Chemical Nomenclature CS 2 SO 2 PCl 5 N 2 O 4 Carbon disulfide Sulfur dioxide Phosphorus pentachloride Dinitrogen tetraoxide (Dinitrogen tetroxide)

10. Acids & Bases An acid is a substance that produces hydrogen ions when dissolved in water. Inorganic acids are easily recognized because the hydrogen ions are often found at beginning of formula. HCl, HBr, HNO 3, H 2 SO 4

12. Acids & Bases Organic acids are easily recognized because the hydrogen ions are often found at end of structural formula. General Formula for Organic Acid is R-COOH. CH 3 COOH is same thing as (HC 2 H 3 O 2 )

13. Acids & Bases A base is a substance that produces hydroxide ions when dissolved in water. Easily recognized because the hydroxide ions are found in the chemical formulas of many bases. LiOH, NaOH, KOH, Ca(OH) 2

14. Chemical Nomenclature Naming Acids & Oxoacids

17. Examples Binary Acids HFHydrofluoric acid HClHydrochloric acid HBrHydrobromic acid

19. Examples Oxyacids HNO 3 Nitric Acid H 2 SO 4 Sulfuric Acid

21. Examples Oxyacids HNO 2 Nitrous Acid H 2 SO 3 Sulfurous Acid