metallic bonding

• Metallic bond is a term used to describe the collective sharing of a sea of valence electrons between several positively charged metal ions
• Electrical conductivity: Most metals are excellent electrical conductors because the electrons in the electron sea are free to move and carry charge
• Thermal conductivity: Metals conduct heat because the free electrons are able to transfer energy away from the heat source and also because vibrations of atoms (phonons) move through a solid metal as a wave
• Ductility: Metals tend to be ductile or able to be drawn into thin wires because local bonds between atoms can be easily broken and also reformed.
• Metallic luster: Metals tend to be shiny or display metallic luster. They are opaque once a certain minimum thickness is achieved. The electron sea reflects photons off the smooth surface. There is an upper-frequency limit to the light that can be reflected.
• Malleability: Metals are often malleable or capable of being molded or pounded into a shape, again because bonds between atoms readily break and reform. The binding force between metals is nondirectional, so drawing or shaping a metal is less likely to fracture it
• The strong attraction between atoms in metallic bonds makes metals strong and gives them high density, high melting point, high boiling point, and low volatility.
• The Properties of Metallic Compounds are Electrical conductivity, Thermal conductivity, Ductility, Malleability and Metallic luster.