Metalic Bonding

• Metallic bonding


  Structure of a metal: a giant lattice of positive ions with delocalized (free) electrons in between them, attracting the positive ions and holding the structure together
• Metals


  • Good conductors of heat
  • Good conductors of electricity
  • Malleable (can be hammered into shape)
  • Ductile (can be drawn into wire)
• Why metals are good conductors of heat

  1. Atoms are regularly arranged and close together, so vibration energy is easily transferred from atom to atom
  2. Free electrons can carry energy through the metal
• Why metals are good conductors of electricity

  Free electrons can move through the metal, and the flow of negatively charged electrons is an electrical current
• Malleability


  Layers of atoms can slide over each other, allowing the metal to be hammered into shape
• Ductility


  Layers of atoms can slide over each other, allowing the metal to be stretched into wire (plastic deformation)
• As you go down group 1 (Li, Na, K, Rb, Cs)

  Melting point decreases
• Group 2 metals (e.g. Be) compared to group 1 metals

  Group 2 metals have higher melting points