The Metallic Bond
Pure metals are crystalline solids, but unlike ionic compounds, every point in the crystal lattice is occupied by an identical atom. The electrons in the outer energy levels of a metal are mobile and capable of drifting from one metal atom to another. This implies the metal is all the more legitimately saw as a variety of positive particles encompassed by an ocean of portable valence electrons.
A metallic bond is the attraction of the stationary metal cations to the surrounding mobile electrons.
Properties of Metals
The metallic bonding model explains the physical properties of metals. Metals conduct electricity and heat very well because of their free-flowing electrons. As electrons enter one end of a piece of metal, an equal number of electrons flow outward from the other end.At the point when light is shone on to the surface of a metal, its electrons retain little measures of vitality and wind up noticeably energized into one of its many purge orbitals.
Metals are very malleable and ductile. They can be hammered into shapes, rolled into thin sheets, or pulled into thin wires.
The metallic bond is responsible for the properties of metals.
Metals conduct electricity and heat well.
Metals are ductile and malleable.
Metals have luster.