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Understanding Metallic Bonds in Chemistry

Explore the concept of metallic bonds in Chemistry with Mrs. Coyle. Learn why metals are good conductors, ductile, and malleable due to the unique structure of closely packed cations in a "sea of electrons." Discover the properties and types of metals, alloys, and their applications.

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Understanding Metallic Bonds in Chemistry

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  1. Metallic Bonds ChemistryMrs. Coyle

  2. Cations packed in “a sea of electrons”

  3. Metals • Metals consist of closely packed cations floating in a “sea of electrons”. • All of the atoms are able to share the electrons. • The electrons are not bound to individual atoms.

  4. Properties of Metals • Good conductors • Ductile • Malleable • Electrons act as a lubricant, allowing cations to move past each other

  5. Metals have a Crystalline Structure • Packed spheres of the same size and shape: • Body Centered Cubic • Face Centered Cubic • Hexagonal Close Packed

  6. Body Centered Cubic Chromium

  7. Face-Centered Cubic Gold

  8. Hexagonal Close-Packed Zinc http://phycomp.technion.ac.il/~pavelba/hcpS.gif

  9. Alloys • Mixtures of two or more elements, at least one of which is a metal. • Made by melting, mixing, then cooling the metals. • May contain non-metals like carbon.

  10. Alloys • Properties are superior to their components. • Sterling silver • 92.5% Ag, 7.5% Cu • Harder than silver • Bronze • 7:1 Cu to Sn (tin)

  11. Alloys • Stainless Steel • Fe 80.6%, Cr 18%, C 0.4%, Ni 1% • Cast Iron-Fe 96%, C 4%

  12. Types of Alloys • Two types of formation: • Substitutional alloys • Similar size atoms – replacement • Interstitial alloys • Different size atoms – smaller ions fill interstices (spaces between atoms)

  13. Why is a metal ductile but an ionic compound is not?

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