What type of bonding do metals use?

Metallic bonding.

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Describe the structure and bonding of metals.

  1. Metals have a giant structure. 
  2. The metal atoms give up their outer-shell electrons, which become delocalised. 
  3. The metal ions are arranged in a regular lattice structure. 
  4. There are strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons. 
  5. These forces are metallic bonds.

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Why are metals good at conducting electricity and heat?

They have delocalised electrons that are free to move throughout the structure, so can transfer charge and heat energy.

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Why do metals have high melting and boiling points?

There are strong electrostatic forces of attraction between metal atoms and the sea of delocalised electrons (metallic bonds), which require a lot of energy to break.

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What does 'malleable' mean?

Malleable means a structure can be hammered into shape.

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Why are metals malleable?

The layers of metal ions can slide over one another, which allows the structure to bend.

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What does 'ductile' mean?

Ductile means a structure can be drawn into wire.

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What is an alloy?

An alloy is a mixture of 2 or more metals (in some cases it may be a metal and a non-metal)

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Why are alloys harder than pure metals?

  1. The different elements have different-sized atoms. 
  2. This disrupts the regular layered structure.
  3. Meaning the layers can’t slide over one another anymore.
  4. This makes them less malleable, so harder.

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What is the disadvantage of pure metals?

Pure metals are often too soft so an alloy must be used instead.

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