Metallic bonding

• they can be drawn into wives
• Structure of metals


  • Atoms in a pure metal are in tightly-packed layers, which form a giant regular lattice structure
  • The outer electrons of the metal atoms separate from the atoms and create a 'sea of electrons'
  • The electrons are delocalized and so are free to move through the whole structure
  • The metal atoms become positively charged ions and are attracted to the sea of electrons
• Metallic bonding


  The attraction between the positive metal ions and the sea of electrons
• This is an electrostatic force of attraction
• Metallic bond strength


  • Depends on the number of outer electrons donated to the cloud and the size of the metal atom/ion
  • Sodium has relatively weak metallic bonding because each atom donates one electron to the cloud
  • Potassium has weaker metallic bonding than sodium because the resulting ion is larger and the electron cloud has a bigger volume to cover so is less effective at holding the ions together
  • Magnesium has stronger metallic bonding than sodium because each atom has donated two electrons to the cloud, and the greater the electron density holds the ions together more strongly
• The strength of the metallic bonding in Na sodium is relatively weak because each atom donates one electron to the cloud
• The metallic bonding in potassium is weaker than in sodium because the resulting ion is larger and the electron cloud has a bigger volume to cover so is less effective at holding the ions together
• The metallic bonding in magnesium is stronger than in sodium because each atom has donated two electrons to the cloud. The greater the electron density holds the ions together more strongly