1. Nomenclature Unit 3

2. Naming Binary Compounds

3. Naming Compounds That Contain a Metal and a Nonmetal Binary Ionic compound: the metal loses one or more e- to become a cation and the nonmetal gains one or more e- to become an anion. To name these compounds we simply name the ions.

4. Naming Compounds that contain a Metal and a Nonmetal Type I compounds: the metal present forms only one type of cation Type II compounds: the metal present can form two or more cations that have different charges

5. Type I Binary Ionic Compounds 1. the cation is always named first and the anion second. 2. A simple cation takes its name from the name of the element.

6. Type I Binary Ionic Compounds 3. A simple anion is named by taking the first part of the element name and adding –ide. 4. Write the name for the compound by combining the names of the ions.

7. Type I Binary Ionic Compounds Magnesium phosphide Ca 2 C Lithium chloride Al 2 S 3

8. Type II Binary Ionic Compounds Many metals can form more than one cation. Iron can form Fe 2+ or Fe 3+ so if we saw the name Iron chloride we wouldn’t know if it was actually FeCl 2 or FeCl 3

9. Type II Binary Ionic Compounds So, instead we would have to write Iron(II) chloride for FeCl 2 and we would write Iron(III) chloride for FeCl 3 The Roman numeral tells the charge on the ion not the number of the ions present in the compound

10. Type II Binary Ionic Compounds In an older naming system the ion with the higher charge would have a name ending in –ic and the ion with the lower charge would have a name ending in –ous

11. Type II Binary Ionic Compounds Copper (I) oxide Fe 2 O 3 Vanadium (III) chloride AuCl 3

12. Naming Binary Compounds That Contain Only Nonmetals (Type III) 1. The first element in the formula is named first, and the full element name is used. Element w/ lower group # is first Element w/ higher period # is first The second element is named as though it were an anion.

13. Naming Binary Compounds That Contain Only Nonmetals (Type III) 3. Prefixes are used to denote the numbers of atoms present. (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-) 4. The prefix mono- is never used for naming the first element.

14. Naming Binary Compounds That Contain Only Nonmetals (Type III) Carbon disulfide P 2 O 3 Dinitrogen pentoxide HF

15. Naming and Writing Formulas for More Complex Compounds

16. Naming Compounds That Contain Polyatomic Ions Polyatomic Ions: charged entities composed of several atoms bound together. Ammonium nitrate NH 4 NO 3 NH 4 + NO 3 -

17. Naming Compounds That Contain Polyatomic Ions Oxyanion: a polyatomic anion containing at least one oxygen atom Two oxyanions with the same elements differing only in number of oxygen smaller number ends in –ite larger number ends in -ate

18. Naming Compounds That Contain Polyatomic Ions NO 2 - Nitrite NO 3 - Nitrate

19. Naming Compounds That Contain Polyatomic Ions If more than two oxyanions make up a series hypo- (less than) and per- (more than) are used. ClO - hypochlorite ClO 2 - chlorite ClO 3 - chlorate ClO 4 - perchlorate

20. Naming Compounds That Contain Polyatomic Ions Naming is very similar to type I ionic compounds Name the first element or compound Name the second compound NH 4 C 2 H 3 O 2 Ammonium acetate NH 4 + Ammonium cation C 2 H 3 O 2 - Acetate anion

21. Naming Compounds That Contain Polyatomic Ions ClO 4 - Phosphate ion Li 2 SO 4 Acetate ion Ca 3 (PO 4 ) 2

22. Naming Acids Acid: a substance that produces hydrogen ions (H + ) in solution; a proton donor Rules for naming acids depends on whether the anion contains an oxygen

23. Naming Acids If the anion does not contain oxygen, the acid is named with the prefix hydro- and the suffix –ic HCL Hydrochloric acid HCN Hydrocyanic acid H 2 S Hydrosulfuric acid

24. Naming Acids If the anion does contain oxygen, no prefix is used and the prefixes –ic or –ous are used If anion ends in –ate, suffix is –ic If anion ends in –ite, suffix is -ous

25. Naming Acids Sulfuric acid HC 2 H 3 O 2 H 2 SO 3 Nitrous acid