Metallic bonding

• How are the particles arranged in a metal?

  The electrons in the outer shell of the metal atoms are delocalised so they are free to move around. The strong electrostatic attraction between the positive metal ions and negative electrons hold the atoms together in a regular structure which is known as strong metallic bonding.
• Why are metals malleable?

  They are malleable because layers of atoms in a pure metal can slide over each other.
• Why can metals conduct electricity?

  Delocalized electrons carry electrical charge and thermal energy so they are good conductors of electricity and heat.
• What are the typical properties of metals?

  -malleable.

  -good conductors of heat and electricity.

  -more dense.

  -high melting/boiling points.

  -lose electrons to gain a full outer shell.

  -insoluble in water.
• What are the typical properties of non metals?

  -brittle.

  -bad conductors of electricity and heat.

  -less dense.

  -soluble in water.

  -low melting/boiling points.

  -gain electrons to have a full outer shell.