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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.
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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Rather, bond types are interconnected and different compounds have varying degrees of different bonding character (for example, covalent bonds with significant ionic character are called polar covalent bonds). Six years later, in 1947, Ketelaar developed van Arkel's idea by adding more compounds and placing bonds on different sides of the triangle.
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AuAl 2 is the most thermally stable species of the Au–Al intermetallic compounds, with a melting point of 1060 °C (see phase diagram), which is similar to the melting point of pure gold. AuAl 2 can react with Au, therefore is often replaced by Au 2 Al, a tan-colored substance, which forms at composition of 93% of Au and 7% of Al by mass.
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