1. Ionic Compounds Formed from positive and negative ions. Almost always have a metal and a nonmetal.

2. Ionic Compounds Exist mostly as crystalline solids. Conduct electricity when melted or dissolved in water. [http://liftoff.msfc.nasa.gov/academy/materials/topaz.gif]

3. Ionic Compound Names Example: NaCl Sodium Chloride When naming the compounds always list the positive ion first (metal) and end then nonmetal in – ide.

4. Ionic Compound Names Example: MgBr 2 Magnesium Bromide Example: Al 2 O 3 Aluminum Oxide

5. Ionic Compound Formulas Example: Aluminum Bromide AlBr 3 When writing formulas, place the positive ion first (metal!) and balancing the charges to make a neutral compound. Example: Magnesium Chloride

6. Ionic Compound Formulas Mg +2 and Cl -1 Cl -1 Final Formula: MgCl 2 [http://www.southwest.com.au/~jfuller/chemistry/magnesiumchloride.gif]

7. Ionic Compound Formulas Example: Sodium Oxide Na 2 O Example: Calcium Sulfide CaS

8. Transition Metal Ions [http://wps.prenhall.com/wps/media/objects/602/616516/Media_Assets/Chapter02/Text_Images/FG02_12.JPG]

9. Transition Metal Ions

10. Example: Iron (III) Chloride The roman numeral gives you the charge of the metal! Fe +3 and Cl –1 FeCl 3 Example: Copper (II) Oxide CuO

11. Transition Metal Ions Example: CoBr 2 When writing the name, you must find the charge of the metal! Bromine is normally Br -1, so Cobalt must be Co +2 Cobalt (II) Bromide

12. Polyatomic Ions Ions that have more than one atom, and always are found as a group. [http://www.hibbing.tec.mn.us/programs/dept/chem/V.12/polyatomic_ion_ex.jpg]

13. Polyatomic Ions Example: Calcium Hydroxide Ca +2 and OH -1 Ca(OH) 2 Example: Magnesium Phosphate Mg +2 and PO 4 -3 Mg 3 (PO 4 ) 2