metallic bonding

• What do delocalised electrons in metallic bonding refer to?

  Electrons that are free to move
• What gives a metal its properties?

  Bonding
• What type of structure do metals have?

  Giant structures of atoms
• Why are outer shell electrons in metal atoms less tightly bound?

  They become delocalised
• What are the forces of attraction between positive metal ions and delocalised electrons called?

  Metallic bonds
• What do metallic bonds hold together in metals?

  Atoms in a regular pattern
• Why is a lot of energy needed to break metallic bonds?

  Because metallic bonds are very strong
• What state are most metals in at room temperature?

  Solids
• What can delocalised electrons in metals carry?

  Electrical charge and thermal energy
• Why are metals good conductors of electricity and heat?

  Because delocalised electrons can move freely
• What happens to the layers of atoms in a metal?

  They can slide over each other
• What property allows metals to be bent or formed into different shapes?

  The ability of layers to slide
• What is a characteristic of pure metals?

  They are often quite soft
• What is an alloy?

  A mixture of two or more metals
• What happens when another element is mixed with a pure metal?

  Layers of metal atoms lose their shape
• Why does mixing different elements with pure metals make alloys harder?

  Atoms find it difficult to slide over each other
• What is the significance of metallic bonding in metals?

  It explains their structure and properties
• What are the properties metallic bonding?

  • High melting and boiling points
  • Good conductors of electricity and heat
  • Solid at room temperature
• metallic bonds are very strong so

  lots of energy is needed to break them down
• metallic bonds have very high melting and boiling points because a lot of energy is required to break them down