Metals form metallic bonds when their valence electrons are released and move freely around the positively charged metal ions, creating a "sea of electrons". This sea of delocalized electrons is what gives metals their characteristic properties like malleability, ductility, luster, and high electrical and thermal conductivity. Alloys are mixtures of metals that are generally stronger yet less reactive than their pure metal components due to the metallic bonding between different kinds of metal atoms and ions.

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