Metallic+Bonding

This is the type of bonding found in metals. The metallic structure consists of a regular lattice of positively charged metal ions (cations) surrounded by valence electrons.

The valence electrons in a metal are //delocalized// meaning that they don’t belong to any particular atom. The attractive forces between the metal cations and the delocalized electrons holds the structure together. 

Properties of metals Reasons???? The attractive forces in a metal are between the ions and the electrons. There is no force of attraction between the metal cations themselves. Therefore the ions can easily slide past each other, without the bonds in the metal breaking.
 * They are malleable (easily shaped) and ductile (can be made into thin wires)

Reasons???? The delocalized valence electrons are free to move from one side of the lattice to another and thus can carry an electric current.
 * Metals are good conductors of heat and electricity

By the end of this lesson you should be able to:
 * Describe the metallic structure
 * Recognize that the metallic structure is as a result of the electrostatic forces of attraction between a lattice of positive ions and delocalized electrons
 * Be able to state the reasons for why metals conduct electricity and are malleable


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