Structure and bonding in metals
Metallic bonding
Shiny element that is a good conductor of electricity and heat, and which forms basic oxides. consist of giant structures of The smallest part of an element that can exist. arranged in a regular pattern.
The Subatomic particle, with a negative charge and a negligible mass relative to protons and neutrons. from the outer shells of the metal atoms are Electrons that are not associated with a particular atom, eg in a metal, outer electrons can be free to move through the solid., and are free to move through the whole structure. This sharing of delocalised electrons results in strong Bonding in metal elements consisting of a giant structure of metal atoms and their delocalised electrons moving between them..
Learn more on metallic bonding in this podcast.
Listen to the full series on BBC Sounds.
Properties of metals
The structure and bonding of metals explains their The characteristics of something. In chemistry, chemical properties include the reactions a substance can take part in. Physical properties include colour and boiling point.:
- they are electrical A material which allows charge to move easily through it. because their delocalised electrons carry electrical charge through the metal
- they are good conductors of thermal energy because their delocalised electrons transfer energy
- they have high The temperature at which a solid changes into a liquid as it is heated. and The temperature at which a substance rapidly changes from a liquid to a gas., because the metallic bonding in the giant structure of a metal is very strong - large amounts of energy are needed to overcome the metallic bonds in melting and boiling
Question
Explain why metals can conduct electricity.
Metals conduct electricity because they have delocalised electrons. These carry electrical charge through the metal.