Metallic bond
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Metallic bonds are found in metals like copper. |
Metallic bonding is the bonding within
metals. It involves the
delocalized sharing of free
electrons among a lattice of metal atoms. Thus, metallic bonds may be compared to molten salts.
Metal atoms typically contain a high number of
electrons in their
valence shell compared to their period or
energy level. These become delocalized and form a
Sea of Electrons surrounding a giant lattice of
positive ions.
Metals seem to have higher boiling and melting points which might suggest stronger bonds between the atoms.
Metallic bonding is non-polar, in thatthere is no (for pure elemental metals) or very little (for
alloys)
electronegativity difference among the
atoms participating in thebonding interaction, and the electrons involved in that interactionare delocalized across the crystalline structure of the metal.
The metallic bond accounts for many physical characteristics of metals, such as
strength,
malleability,
ductility,
conduction of heat and
electricity, and
lustre.
Metallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalised electrons. This is why atoms or layers are allowed to slide past each other, resulting in the characteristic properties of malleability and ductility.
Metal atoms have at least one valence electron, they do not share these electrons with neighboring atoms, nor do they lose electrons to form ions. Instead the outer energy levels of the metal atoms overlap. They are like
covalent bonds.
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Chemical bond
