A metallic bond is a chemical bond seen in metals consisting of tightly bound metal atoms of the same type.
Metals are large atoms that do not firmly hold their outermost valence electrons and easily lose them. Once the electrons are lost, the metal atoms become positively charged, called kernels. The position of these kernels is fixed to avoid repulsions and is part of the solid structure.
The lost valence electrons of the metal atom are not confined to the space of an atom alone. Instead, the valence electrons delocalize and float, so they are part of several metal atoms' nuclei. Therefore, a sea of valence electrons freely moves between several atoms.
The fixed kernels are like islands, and the released electrons flow as water flows between islands in the ocean.
Despite having negative electrons and positive kernels in its structure, a metal is neutral and uncharged.
The electrical neutrality of the metal is maintained by electrostatically attracting the floating free electrons. The positive charge is always balanced with the negative electrons.
This attractive interaction between positive metal ions and valence electrons is responsible for preserving the integrity of the metallic solid and is known as the metallic bond.
This excerpt is inspired by the chapter Bonding in Atoms, part of CurlyArrows' Introductory Organic Chemistry Course. Preview the Book.
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