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The 35 pages that link to Metallic bonding, each with the reason it gives.

• Covalent bondCompared with: Metallic bonding involves mobile electrons shared across many atoms, not localized pairs.

• Ionic compoundCompared with: Its mobile electrons, rather than oppositely charged ions alone, explain metallic conductivity.

• Chemical bondBroader topic: Delocalized electrons bind many metal atoms without localized atom-to-atom pairs.

• CalciumRelated: This bonding accounts for calcium’s metallic structure and electrical behavior.

• Intermolecular forceCompared with: It binds an extended metallic solid, not a collection of separate molecules.

• SodiumRelated: Delocalized electrons help account for sodium metal’s electrical conductivity and softness.

• Ionic bondingCompared with: It explains conductivity in solids without requiring distinct cations and anions.

• MetallurgyNarrower topic: This bonding model helps explain metals’ conductivity, cohesion, and ability to deform.

• Pi bondCompared with: Metallic bonding is collective and extended, rather than a localized pi bond between two atoms.

• AlloyNarrower topic: Delocalized electrons help explain the electrical, thermal, and mechanical behavior of metallic alloys.

• ZincRelated: Metallic bonding accounts for zinc’s electrical conductivity and malleability.

• GoldRelated: Delocalized electrons give gold its electrical conductivity and contribute to its metallic luster.

• Electrical conductorRelated: Delocalized electrons provide metals with mobile charge carriers.

• Gold leafRelated: This bonding helps explain why gold can deform without its atomic structure simply cleaving apart.

• SilverNarrower topic: Delocalized electrons help account for silver’s conductivity and ability to deform without breaking.

• Drude modelRelated: This electron-sea picture motivates treating conduction electrons as mobile particles.

• MetalRelated: Its mobile electrons and shared attraction account for many characteristic metal properties.

• MetalloidCompared with: Metalloids conduct less freely than metals because their electrons are not fully delocalized.

• TungstenNarrower topic: Strong metallic bonding contributes to tungsten’s high melting point and mechanical strength.

• GalliumRelated: Metallic bonding accounts for gallium’s electrical conductivity and metallic appearance.

• IridiumNarrower topic: Metallic bonding underlies iridium’s conductivity, strength, and capacity to form alloys.

• Chemical compoundRelated: Metallic interactions help explain bonding in some intermetallic compounds.

• Free electron modelNarrower topic: It provides the physical setting of mobile electrons and fixed positive ions.

• Metal (chemistry)Related: It accounts for metals’ cohesion, electrical conductivity, and ability to deform.

• OsmiumRelated: Delocalized electrons bind osmium atoms into a conductive metallic solid.

• Native copperRelated: Delocalized electrons account for native copper’s metallic luster, conductivity, and malleability.

• IndiumNarrower topic: Delocalized electrons account for indium’s electrical conductivity and metallic luster.

• Native element mineralRelated: It explains the malleability, conductivity, and metallic luster of many native metals.

• Post-transition metalRelated: It underlies the conductivity and malleability shared by these elements.

• Group 11 elementRelated: Delocalized electrons help make copper, silver, and gold effective electrical conductors.

• Bonding in solidsRelated: Delocalized electrons bind metal atoms while allowing electrical conduction.

• Colored goldRelated: Changes in metallic composition alter how an alloy reflects visible light.

• Electric-field screeningRelated: Conduction-electron screening helps explain why electric fields scarcely penetrate metals.

• Elemental materialsRelated: It explains the conductivity and malleability common in elemental metals.

• IntermetallicNarrower topic: Intermetallics retain metallic bonding even when their atoms occupy ordered, chemically distinct sites.