1. Metallic Bonds

2. Metallic Bonds Most metals have only 1,2 or 3 valence electrons.
This means that they always “give up” their electrons (similar to an ionic bond)
When atoms give up electrons, the atom becomes positive.

3. Metallic Bonds In metallic bonds, the atoms come together
Once the atoms are together, their valence electrons move around them creating a sea of negativity.
The atoms release their specific electrons and allow them to flow around all of the atoms bonded together.

4. Metallic Bonds
These metallic bonds are held together by the positive metal ions and the sea of negative electrons around them.
The more valence electrons an atom can add to the “sea” the stronger the metal becomes.

7. Metallic Bonds
Because these bonds are not formed through a rigid structure, metals have special properties:
Malleability and Ductility
Luster (shiny)
Electrical conductivity
Thermal (heat) conductivity