Metallic bonding is the force that holds metals together, characterized by a lattice of cations and a sea of delocalized electrons. These electrons allow metals to conduct electricity and heat, and contribute to their ductility, malleability, and high melting points. The bond strength varies with ion charge and size, affecting the metal's properties. Alloys improve these properties for diverse applications.
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Metallic bonding is a type of chemical bond characterized by the electrostatic attraction between positively charged metal ions and a sea of delocalized electrons
Origin of Delocalized Electrons
Delocalized electrons originate from the valence shell of metal atoms and contribute to the overall stability and electrical neutrality of the metal
Role of Delocalized Electrons
Delocalized electrons allow for cohesive forces that bind metal ions together, enabling the metal to conduct electricity and heat
The structure of a metal is maintained by the electrostatic forces between metal ions and delocalized electrons, resulting in a repeating, three-dimensional lattice
The strength of metallic bonds is influenced by the charge of metal ions, with higher positive charges resulting in stronger bonds
The size of metal ions also affects the strength of metallic bonds, with larger ions having a weaker attraction to delocalized electrons
The variations in metallic bonding help explain the differing physical properties of different metals
The strong electrostatic forces within the metallic lattice result in high melting and boiling points for metals
The ability of metal ions to slide past one another within the electron sea allows for the ductility and malleability of metals
The mobility of delocalized electrons contributes to the excellent electrical and thermal conductivity of metals
Metals are typically resilient, not brittle, and insoluble in common solvents
Alloys are homogeneous mixtures of two or more elements, with at least one being a metal
Purpose of Alloys
Alloys are engineered to enhance the properties of pure metals
Disrupting the Metallic Lattice
Alloys introduce atoms of different sizes into the metallic lattice, disrupting the regular arrangement of metal ions and increasing the hardness and strength of the material
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Metallic Bonding: Electron Origin
Electrons in metallic bonding come from metal atoms' valence shells, becoming delocalized.
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Metallic Bonding: Cation Lattice
Metallic bonding features a lattice of cations, which are positively charged metal ions.
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Metallic Bonding: Electrical Neutrality
Delocalized electrons balance the charge of cations, maintaining the metal's electrical neutrality.
