2.1.4

Covalent & Metallic Bonds

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Covalent Bonding

Covalent bonds are formed when 2 non-metal atoms share pairs of electrons. Covalent bonds are strong because the shared electrons are attracted to the nucleus of both atoms. Covalently bonded substances can be:

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Small molecules

  • E.g. water.
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Large molecules

  • E.g. polymers such as polyester and silk.

Metallic Bonding

Metallic bonds are the electrostatic attractions between positive ions and negative delocalised electrons.

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Positive ions

  • Metals are giant structures of regularly arranged atoms.
  • The structure is a regular lattice of positive ions (cations) in a ‘sea’ of delocalised electrons.
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Delocalised electrons

  • Delocalised electrons are NOT bound to an atom and are free to move around within the lattice.
  • Delocalisation happens because metal atoms have a small number of electrons in their outer shells.

Jump to other topics

1Atomic Structure

2Chemical Bonding

3Quantitative Chemistry

4Chemical Changes

5Energy Changes

6The Rate & Extent of Chemical Change

7Organic Chemistry

8Chemical Analysis

9Chemistry of the Atmosphere

10Using Resources

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