Metallic bonds hold metal atoms together with delocalized electrons floating through the lattice, giving metals unique properties such as conductivity and malleability. The lattice structure of complete atoms allows electrons to migrate through the lattice, creating stronger bonds with closely spaced atoms. The delocalized electrons also allow for excellent conductivity, and the metallic bond allows for malleability without shattering.
Metallic bonds are the chemical bonds that hold atoms in metals together. They differ from covalent and ionic bonds because the electrons in the metallic bond are delocalized, i.e. they are not shared between just two atoms. Instead, the electrons in the metal bonds float freely through the lattice of the metal nuclei. This type of bond gives metals many unique material properties, including excellent thermal and electrical conductivity, high melting points, and malleability.
In most metals, atoms are packed together so that each atom touches several other atoms, creating a lattice. The electrons of each atom are shared in the orbitals of the surrounding atoms. This allows electrons to migrate through the lattice away from their parent atoms, which then accept new electrons.
The metal atoms in the lattice structure are always complete atoms, not ions. Although their positively charged nuclei attract electrons, they technically never become ions, because they don’t lose electrons. For each electron that is attracted to a different atom in the structure, a new electron takes its place in the original orbital.
Depending on the type of metal and the organization of its lattice structure, metallic bonds can vary in strength. The closely spaced atoms will create stronger metallic bonds than the less closely spaced atoms. Metals with a higher number of electrons will also be stronger than those with a less populated electron sea. The stronger the metal bond, the higher the melting point of the metal will be.
Metallic bonding also gives metals excellent conductivity. This is because the delocalized electrons can move freely through the metal lattice, rapidly transporting energy in the form of heat or electricity. Some metals have electron configurations that make them particularly good conductors: their electrons are easily transferred from one atom to another. Copper is one of the best conductors and is often used in wiring and other electrical applications due to its low cost.
Perhaps one of the greatest advantages metals have in materials science is their ability to be molded into thin shapes or wires. The malleability of metal is due to the metallic bond. When a force is applied, the metal can deform without shattering because the delocalized electrons transfer to other atoms, allowing the atoms to roll past each other without strong repulsion. For example, it’s helpful to imagine lowering a concrete block into a pit of rubber balls—the balls don’t break apart, they just rearrange. The metallic bond allows the metallic solid to rearrange itself in a similar way.
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