Metallic bonds form when metal atoms come together and their valence electrons move freely around the atomic nuclei, creating a "sea of electrons" that positively charged metal ions are suspended within. This bond structure allows metals to be malleable, ductile, shiny, electrically conductive, and thermally conductive. Alloys are mixtures of metals that are generally stronger than their pure metal components due to metallic bonding between different kinds of metal atoms.

1. Metallic Bonds

2. Metallic Bonds

Alloys are the every-day metals that we
encounter. They are a mixture of two or
more types of metals.

Alloys are generally stronger and less reactive
than the pure metals that they are made from.

3. 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.


4. 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.


5. 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.


6. 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


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
