3.  Electrons are shared or exchanged between elements  This is an exothermic process (energy is released)  Both elements are more stable than they were before the bond formed (have 8 valence electrons)

4.  The atoms are separated into individual components  Endothermic process (takes an input of energy to do this)  If I want to break up anything, I need to input energy into the process!!!!

7.  Bonds formed by the exchange of electrons between a metal and a non-metal  Metals give away valence electrons  Non-Metals Take the valence electrons  Form strong bonds between elements, and strong compounds  Based upon the differences in electronegativity between the elements

8.  Combination of metal-non-metal  Two components are required to form any ionic compound  1. Cation  2. Anion

9.  Have a positive charge  Are metal elements  Lose electrons  Always written first in the compound formula  Ex: Sodium Chloride  NaCl

10.  Always are formed from the non-metal element  Gain Electrons  Negative Charge  Last in the compound formula and name  Always have an “ide” ending  Ex: Sodium Chloride  NaCl

11.  Formed from a metal/non-metal  Strong bonds  High melting and High Boiling Point due to bond strength  Solids at room temperature (crystalline)  Dissolve in water (polar)  Conduct a current when dissolved in water but not when solid.

12.  Formed by the exchange of electrons  All elements have a noble gas configuration when the bonding process is finished (8 valence electrons)

13. MetalsNon-Metals

14. Ionic Solid

15. Ionic Solid Dissolving In Water