How does metallic bonding result in useful properties of metals?

Question

Henry Antrim · Accepted Answer

The delocalized nature of metallic bonding accounts to the flexibility, conductivity, reflectivity and other properties of metals.

When we consider covalent bonding in molecules, we consider that the bonding (valence) electrons are shared (exclusively) by the two bonded atoms; these electrons are referred to as localized because they "belong" to the bonded atoms. The bonding still involves positive atomic kernels (nucleus plus all non-valence electrons) which attracted to a sea of mobile valence electrons because in a metal, the valence orbitals overlap to form a continuous "sea" in which the valence electrons are free to travel through the entire metallic crystal. Electric current results from the valence electrons drifting along the crystal from negative to positive when only a small voltage is applied across it. When stress is applied to the crystal, the kernels will move in relation to one another, but in a way that ensures the non-localized bonding keeps the crystal from breaking. This is why the metal is malleable. Because the bonding electrons and kernels have the same degree of mobility, kinetic energy can also flow along the crystal and cause heat to be conducted along it. Light of all frequencies can be absorbed and released because the energies of the non-localized electrons form a conduction "band" of energies; however, this is only a brief overview of a complex subject! I hope this is useful.

Axel Alvarado · Answer

undefined Because metallic bonding permits delocalized electrons to flow freely throughout the metal lattice, metals acquire advantageous properties like malleability, ductility, and conductivity.

Peyton Adams · Answer

undefined Metallic bonding results in useful properties of metals because it allows for several key characteristics:

1. High electrical conductivity: The delocalized electrons in metallic bonding can move freely throughout the metal lattice, enabling efficient conduction of electricity.

2. High thermal conductivity: Similarly, the free movement of electrons facilitates the transfer of thermal energy, making metals good conductors of heat.

3. Ductility and malleability: The mobility of electrons allows layers of metal atoms to slide past each other without breaking bonds, making metals ductile (capable of being drawn into wires) and malleable (capable of being hammered into thin sheets).

4. Strength and toughness: Metallic bonding provides metals with high tensile strength and toughness, making them suitable for structural applications where durability is essential.

5. Luster and reflectivity: The free movement of electrons allows metals to absorb and re-emit light photons efficiently, resulting in their characteristic luster and high reflectivity.

Overall, metallic bonding contributes to the unique combination of physical and mechanical properties that make metals essential materials in various industries and applications.