Metallic bonds involve the delocalized sharing of electrons in a metal lattice from "summary" of Chemistry Simplified NCERT Class 11 by Sanjay Sharma
In metallic bonds, electrons are shared between metal atoms in a unique way. Unlike ionic or covalent bonds, where electrons are localized between specific atoms, metallic bonds involve the delocalized sharing of electrons. This means that the electrons are not tied to any one atom, but are free to move throughout the metal lattice. In a metal lattice, the outermost electrons of the metal atoms are able to move easily between atoms. This is because the outermost electrons in metal atoms are not tightly bound to the nucleus, allowing them to move freely within the lattice. As a result, these electrons are not associated with any particular atom, but instead form a "sea of electrons" that surrounds the positively charged metal ions. This delocalized sharing of electrons gives metals their unique properties. For example, metals are good conductors of electricity because the free-moving electrons can easily carry an electric current. Similarly, metals are malleable and ductile because the delocalized electrons allow the metal ions to slide past each other without breaking the bonds. The strength of a metallic bond depends on the number of electrons that are delocalized and the arrangement of the metal ions in the lattice. Metals with more delocalized electrons and a closer packing of ions will generally have stronger metallic bonds. This is why different metals exhibit varying levels of strength, conductivity, and other properties based on their atomic structure and arrangement in the lattice.- The delocalized sharing of electrons in a metal lattice is what gives metals their unique properties and allows them to exhibit characteristics such as conductivity, malleability, and ductility. This concept of metallic bonding helps to explain why metals have such a wide range of applications in industries ranging from electronics to construction.
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