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A metallic bond is a bond between two metallic elements (not nonmentals or semimetals). They typically form a covalent bond since their electronegativity difference is less than 1.5. Since the transitions metals have other electron configurations other than the ones predicted by the Aufbau principle, this bonding is more complex.
In metallic bonds, the valence electrons of each atom delocalize and kind of float around all the positively charged nuclei. These delocalized electrons form the "sea of electrons". I think that is why metals are often a malleable material; the atoms are able to slide on top of each other because of this sea of electrons.
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