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Metallic Bonding

Metallic Bonding. Introduction to the Lab. Bonds Between Metals. They are NOT the same as ionic bonds But both involve lattice structures. +. +. +. +. +. +. +. +. +. +. +. +. Properties of Metallic Bonds. Involve delocalized electrons – a spreading around of free electrons.

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Metallic Bonding

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  1. Metallic Bonding Introduction to the Lab

  2. Bonds Between Metals • They are NOT the same as ionic bonds • But both involve latticestructures

  3. + + + + + + + + + + + + Properties of Metallic Bonds • Involve delocalizedelectrons – a spreading around of free electrons Nuclei “swim” in a “Sea of electrons.”

  4. Because of the delocalized electrons, metals … • Greatlyvary in melting points. • Are Malleable – can be hammered into sheets • Are Ductile – can be drawn into wire • Good conductors (solid) • Form alloys – mixtures of elements that have metallic properties

  5. Naming Metallic Bonds • Metallic bonds are named for the metals in the mixture or are given a special name. • Examples: • A mixture of copper and zinc is called brass • A mixture of tin and lead is called solder • A mixture of silver and copper is sterling silver

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