1. Bonding

2. Chemical Bond- force that holds 2 atoms together

3. Octet Rule- Atoms want to achieve the configuration of a noble gas 8 valence electrons = Very Stable! Atoms will either lose or gain valence electrons in order to get 8 in the outermost energy level –they will lose the valence electrons in their outer shell so that the next highest shell is full –they will gain electrons in their outer shell so that the shell is full

4. Ionic Bond- electrostatic forces hold compound together –Between cations & anions Example: Draw the dot structures of Na and Cl.

5. Example: Draw the dot structures of Al and Br

6. Properties of Ionic Compounds Crystalline solids at room temperature. Most are salts

7. Have high melting points (NaCl=800°C) Can conduct electric current when melted or dissolved.

8. Electrolyte- an ionic compound whose aqueous solution conducts electricity http://phet.colorado.edu/en/simulation/sugar -and-salt-solutionshttp://phet.colorado.edu/en/simulation/sugar -and-salt-solutions

9. Metallic Bonding Do not bond ionically, they form lattices in solid state (similar to crystal lattice) They do not share nor lose electrons Electron Sea Model- all metal atoms contribute their valence electrons –Electrons are free to move (delocalized electrons) –Metallic Bond – attraction of a metallic cation for delocalized electrons

10. “sea of electrons”