2. Binary Ionic Compounds (Type I) Contain a cation and anion The cation is always named first and the anion second

4. Binary Ionic Compounds (Type I) A monatomic cation takes its name from the name of the element A monatomic anion is named by taking the first part of the element name and adding -ide

5. Binary Ionic Compounds (Type I) Practice LiI Lithium Iodide AgBr Silver Bromide KF Potassium Fluoride Li 3 N Lithium Nitride MgO Magnesium Oxide

6. Binary Ionic Compounds (Type II) Involves metals that can form more than one cation In this case, the charge on the metal ion must be specified with Roman numerals

7. Binary Ionic Compounds (Type II) An older system uses the ending -ic on the cation with the higher charge and -ous on the cation with lower charge

8. Binary Ionic Compounds (Type II) Practice CuCl CuCl 2 Fe 2 O 3 Copper(I) Chloride Copper(II) Chloride Iron(III) Oxide

9. Binary Ionic Compounds (Type II) Practice HgO CoCl 2 MnO 2 Mercury(II) Oxide Cobalt(II) Chloride Manganese (IV) Oxide

10. Ionic Compound with Polyatomic Ions You must MEMORIZE your polyatomic ions!!!! There are a few hints… Night-rateNO 3 - Night-rightNO 2 -

11. Ionic Compound with Polyatomic Ions the polyatomic in a series with less oxygen atoms ends in -ite, the other - ate (The ate ate the ite)

12. Ionic Compounds with Polyatomic Ions Continued In summary… per _ ate 1 more Oxygen _ate _ite1 less Oxygen hypo_ite2 less Oxygen

13. Practice with Polyatomics NaOH NH 4 Cl NaC 2 H 3 O 2 CaCO 3 Sodium Hydroxide Ammonium Chloride Sodium Acetate Calcium Carbonate

14. Practice with Polyatomics KBrO 3 FeSO 4 Mn(OH) 2 Potassium Bromate Iron (II) Sulfate Manganese (II) Hydroxide

15. Binary Covalent Compounds Formed between two nonmetals The first element is the full element name The second element is as if it were an anion

16. Binary Covalent Compounds Prefixes are used to denote number of atoms present “mono” is never used on cation!

17. Prefixes Used In Binary Covalent Compounds Mono- 1 Di-2 Tri-3 Tetra-4 Penta-5 Hexa-6 Hepta-7 Octa-8

18. Practice with Binary Covalent Compounds PCl 3 NO 2 CO N 2 O 5 phosphorus trichoride nitrogen dioxide carbon monoxide dinitrogen pentoxide

19. Naming Acids Acid can be viewed as a molecule with one or more H + ions attached Rules depend on whether or not oxygen is present

20. Naming Acids If the anion DOES NOT contain oxygen the acid is named with the prefix hydro- and the suffix -ic

21. Naming Acids Continued If the anion DOES contain oxygen, the acid name is formed from the root name of the anion with a suffix added

22. Naming Acids Continued If the anion ends in -ate, the -ate turns to -ic If the anion ends in -ite, the -ite turns to -ous

23. Practice Naming Acids HF HCl HNO 3 H 2 SO 4 hydrofluoric acid hydrochloric acid nitric acid sulfuric acid

24. Practice Naming Acids HC 2 H 3 O 2 HCN H 2 S HNO 2 acetic acid hydrocyanic acid hydrosulfuric acid nitrous acid

25. The Secret To Nomenclature Is… Practice! Practice!! Practice!!!