Metallic bonds

• What are metallic bonds?


  An electrostatic attraction between the positive metal ions and the delocalised outer shell electrons.
• Why do metals conduct electricity?


  Delocalised electrons.
• What factors affect the strength of metallic bonds?


  • Size of the ion
  • The charge on the ion
  • The amount of delocalised outer shell electrons.
• How does the size of the atom affect the strength of metallic bonds?


  The smaller the metal ions, the stronger the bonds.
• How does charge on the ion affect the strength of metallic bonds?


  The greater the charge on the ions the stronger the bonding.
• How does the amount of delocalised outer shell electrons affect the strength of metallic bonds?


  The more delocalised outer shell electrons the greater the strength of the bonds.
• Which metal has stronger metallic bonds Mg or Na? And why?

  Mg has stronger metallic bonds than Na. This is because there are more electrons in magnesium’s outer shell, these are released to the sea of delocalised electrons. The Mg ion is also smaller than the Na ion.
• What does Mg having stronger metallic bonds than Na mean?


  There is stronger electrostatic attraction between the positive Mg^2+ ions and the delocalised electrons, meaning that’s more energy is required to break the bonds.
• Why are alloys generally stronger than pure metals?


  Don’t slide as easily