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The strong bonding of metals in liquid form demonstrates that the energy of a metallic bond is not highly dependent on the direction of the bond; this lack of bond directionality is a direct consequence of electron delocalization, and is best understood in contrast to the directional bonding of covalent bonds.
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Metallic solids are held together by a high density of shared, delocalized electrons, resulting in metallic bonding. Classic examples are metals such as copper and aluminum, but some materials are metals in an electronic sense but have negligible metallic bonding in a mechanical or thermodynamic sense (see intermediate forms).
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An illustration of a metallic bond, made using MS Paint and converted to SVG format. This W3C-unspecified vector image was created with Inkscape . Warning: it is better to use the Zn version, because in the metal copper the atom is really Cu + and not Cu 2+
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