1. Ionic Bonds Slide Show #1

2. Atoms are neutral The # of protons = the # of electrons. + charges are equal to – charges. But, if an electron leaves, the atom becomes more positive. electrons < protons When an atom gains an electron it becomes more negative electrons > protons We call an atom that is charged an ion!

3. Electron Transfer Atoms with 5, 6, or 7 valence electrons do not have enough to make a stable 8. Atoms with 1,2, or 3 valence electrons can transfer their electrons to these atoms. In any case the goal is to become stable!

4. Big Idea! Metals give electrons! (become positive) Nonmetals receive electrons! (become negative)

5. Ionic Bonding Sodium can give up its electron (becomes +). Chlorine can accept this electron (becomes -) + & - attract and create an ionic bond. Sodium Chloride is table salt and is now neutral!

6. Ions and their charges NameChargeIonic form Lithium+1Li +1 Sodium+1Na +1 Potassium+1K +1 Calcium+2Ca +2 Magnesium+2Mg +2 Aluminum+3Al +3 FluorineF -1 ChlorineCl -1 Oxide-2O -2 Sulfide-2S -2

7. Ionic Bonds – Some facts! Ionic compounds dissolve easily in water. Ionic solutions (i.e. salt water) easily conduct electricity. Ionic compounds form crystalline solids with high melting temperatures.

8. Naming Ionic Compounds Positive Ion first (usually metal) Negative Ion last (usually nonmetal) If the negative ion is an element, use –ide MgO is Magnesium Oxide NaCl is Sodium Chloride KS is Potassium Sulfide,

9. "Perhaps one of you gentlemen would mind telling me just what is outside the window that you find so attractive...?"

10. How to write an ionic formula Write the charges for metal & non-metal Cross the charge of the metal to the subscript of the non-metal Cross the charge of the non-metal to the subscript of the metal. Now, simplify!