1. Chemistry

2. Metallic Bonds  sea of electrons – metal atoms contribute their valence electrons  delocalized electrons – electrons are free to move throughout the solid because they are not attached to any single nucleus

3. Properties of Metallic Bonds  Malleable – can beat into thin sheets  Ductile – can stretch into wires  Good conductors of heat and electricity  High melting and boiling points  Luster – metallic shine

4. Alloys  mixture of metals  examples:  brass = copper + zinc  jewelry = gold + copper  stainless steel = iron + chromium + nickel  two types  substitutional  interstitial

5. Substitutional Alloys  atoms of the two metals are about the same size

6. Interstitial Alloys  one metal has a much smaller atom than the other metal