1. Chemical Nomenclature and Formulas for Ionic Compounds

2. Ionic Compounds Consist of cations (positive ions) and anions (negative ions) Usually composed of metals (cations) and nonmetals (anions) Oxidation numbers (charges of ions) are important

3. Types of Ions Monatomic ions: Consist of a single atom (Ex.: Na +, Cl -, Mg +2 ) Mon = Single or one Can often be determined from the Periodic Table

4. 0 Predicting Ionic Charges 1+ 2+ 3+3- 2- 1-

5. Types of Ions Polyatomic ions: Groups of atoms that behave as a unit and carry a charge (Ex.: NO 3 -, OH -, SO 4 -2 ) Poly = Many or several You will need a list of polyatomic ions to determine the name and formula

6. nitrateNO 3 -1 chromateCrO 4 -2 chlorateClO 3 -1 dichromateCr 2 O 7 -2 sulfateSO 4 -2 phosphatePO 4 -3 carbonateCO 3 -2 acetateC 2 H 3 O 2 -1 hydroxideOH -1 cyanideCN -1 ammoniumNH 4 +1

7. Binary Ionic compounds Writing Formulas Made up of two monatomic ions (metal and nonmetal) Ex.: Potassium and Chlorine Ex.: Calcium and Bromine

8. Binary ionic compounds Writing Formulas Transition Metals (Groups 3 through 12) and some metals in Groups 3A and 4A (except aluminum, cadmium, silver, and zinc) can have several oxidation numbers Ex.: Iron (III) and Oxygen Ex.: Copper (II) and Oxygen

9. Ionic Compounds with Polyatomic ions Writing Formulas Ions made up of more than one atom Act as individual ions Rules used for binary compounds still apply Use parentheses when more than one polyatomic ion is needed and use the appropriate subscripts outside of the parentheses

10. nitrateNO 3 -1 chromateCrO 4 -2 chlorateClO 3 -1 dichromateCr 2 O 7 -2 sulfateSO 4 -2 phosphatePO 4 -3 carbonateCO 3 -2 acetateC 2 H 3 O 2 -1 hydroxideOH -1 cyanideCN -1 ammoniumNH 4 +1

11. Ionic Compounds with Polyatomic ions Writing Formulas Example: Ammonium ion and chloride ion *IWB Example: Calcium ion and phosphate ion *IWB

12. 1. sodium chloride 2. calcium oxide 3. potassium hydroxide 4. magnesium sulfide 5. copper(II) carbonate 6. aluminum oxide 7. iron(III) oxide 8. sodium carbonate 9. aluminum hydroxide 10. ammonium nitrate 11. zinc nitrate 12. magnesium carbonate Practice Problems

13. Naming ionic compounds: Rules for naming ionic compounds 1. Name cation first and then the anion CsBr Cs Br cation anion + -

14. Naming ionic compounds: Rules for naming ionic compounds 2. Monatomic cations use the element name Cs = cesium 3. Monatomic anions use root of the element and end with – ide Br = bromide CsBr = cesium bromide + -

16. Naming ionic compounds: Rules for naming ionic compounds 4. This applies to transition metals and some metals in groups 3A and 4A (more than one oxidation number): Distinguish between different oxidation numbers of the cation in the name of the chemical formula Use a Roman numeral in parentheses after name of cation

18. Naming ionic compounds: Rules for naming ionic compounds Examples: Fe and O = FeO = Iron (II) oxide Fe and O = Fe O = Iron (III) oxide 2-2+ 2-3+ 3 2

19. Naming ionic compounds: Rules for naming ionic compounds 5. If compound has a polyatomic ion, simply use the name of the ion NaOH = Na OH = sodium hydroxide (NH ) S = NH S = ammonium sulfide +- 4 24 + 2-

20. Practice Problems 1. MgCl 2 2. LiOH 3. ZnCO 3 4. K 2 S 5. FePO 4 6. Ag 3 N 7. Mn(CN) 2 8. AgC 2 H 3 O 2 9. BaI 2 10. PbS 2