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Understanding Metallic Bonding in Metals: Properties, Alloys, and Applications

Learn about how metallic bonds form in metals and their relation to properties such as conductivity and malleability. Explore common alloys like brass, bronze, and steel, and discover how the "sea of electrons" contributes to the unique characteristics of metals. Test your knowledge with review questions at the end.

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Understanding Metallic Bonding in Metals: Properties, Alloys, and Applications

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  1. Metallic Bonding

  2. Objective • Objective: describe how metallic bonds form and how this is related to the properties of metals

  3. Metals • Metals are composed of closely packed cations where valence e- drift and float between cations

  4. Metals • Metallic bond: created by attraction of free floating e- to positive metal cations • “sea of e-” float freely between cations

  5. Properties of Metals • Good conductors of electricity: due to e- able to move freely • Ductile: can be drawn into wire, • e- can move in any direction so they fill in gaps between cations • Malleable: can be flattened into a sheet • Free e- allow metals to be easily shaped

  6. Alloys • Most metals we use are alloys • Alloy: mixture of 2 or more elements where at least 1 element is a metal • Alloys typically have more useful properties than pure metals • Example: stronger, resistance to rusting and corrosion

  7. Common Alloys Brass • Brass: made of copper and zinc • Sterling silver: 92.5% silver, 7.5% copper Sterling Silver

  8. Common Alloys Bronze • Bronze: 7 parts copper, 1 part tin • Steel: most important alloy • Fe can be mixed with C, B, Cr, Mn, Mo, Ni, W, V depending on the type of steel Steel

  9. Ticket Out the Door – Review Questions • 1) Explain in 2-3 sentences how the “sea of electrons” helps hold a metallic bond together. • 2) Explain in 2-3 sentences how the sea of electrons allows a metal to be malleable and ductile

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