Edward Valadez

Metallic bond is the reaction between molecules within metals called alkali
reactive force. It is the sharing of a sea of delocalised electrons amongst a lattice of
positive ions, where the electrons act as a "glue" giving the substance a definite
structure.
The electrons and the positive ions in the metal have a strong attractive force
between them. Therefore metals often have high melting or boiling points. The
principle is similar to that of ionic bonds.
The metallic bond accounts for many physical characteristics of metals, such as
strength, malleability, ductility, luster, conduction of heat and electricity.
Because the electrons move independently of the positive ions in a sea of negative
charge, the metal gains some electrical conductivity. It allows the energy to pass
quickly through the electrons generating a current. Heat conduction works on the
same principle - the free electrons can transfer the energy at a faster rate than other
substances such as those which are covalently bonded, as these have their electrons
fixed into position. There also are few non-metals which conduct electricity:
graphite (because, like metals, they have free electrons), and molten and aqueous
ionic compounds which have free moving ions. [1] [2] [3]
Metal bonds have at least one valence electron which they do not share with
neighboring atoms, and they do not lose electrons to form ions. Instead the outer
energy levels (atomic orbitals) of the metal atoms overlap. They are similar to
covalent bonds.[4] Not all metals exhibit metallic bonding. For example, the
mercurous ion (Hg2+
2) forms covalent metal-metal bonds.
An alloy is a solution of metals, often used to make metal rope, metal plates, etc.