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Metallic Structure & Properties
Properties, Metal Packing
Terms in this set (10)
List 4 properties of metals
Low Ionization Energy
Conductivity: Why are metals generally good conductors of electricity, whereas solid ionic compounds are not?
Metal are more free to move and electrons can flow more readily, whereas solid ionic compounds stay more in place
Appearance: What makes metals appear reflective (shiny)?
Free electrons on the surface bounce back light at the same frequency that the light hits the surface.
Electronegativity: Why do metals have a smaller EN than nonmetals?
Metals have more freely moving shared electrons, so they don't pull electrons toward them as much.
Why might a metal be stronger or harder when there are defects present?
Electron spheres don't slide as well so they are weaker, rather than if they were more closely packed
Most efficient/common pattern of packing atoms in nature
Why is Na soft and malleable and MG is harder?
Mg has more valence electrons
Which packing hole could accommodate the largest cation? Cubic, Octahedral, Tetrahedral
Cubic - 8, Octahedral - 6, Tetrahedral - 4
higher coordination # = larger hole
What is the coordination number for body-centered cubic (BCC) packing?
Name the type of packing used
Face-centered cubic (Cubic-closest packing)
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