Metallic Bonding in Chemistry

Front

Describe metallic bonding (extended only)

Back

Metallic bonding is the electrostatic attraction between the positive ions in a giant metallic lattice and a ‘sea’ of delocalised electrons/mobile electrons/free moving electrons

Front

Explain why metals can conduct electricity (extended only)

Back

Metals have metallic bonding so can conduct electricity because the delocalised electrons/free moving electrons/mobile electrons in their structures can move around and carry charge/conduct electricity

Front

Explain why metals are malleable and ductile (extended only)

Back

Metals arrange in layers of metal positive ions that are able to slide over each other without breaking apart due to the strong metallic bond/electrostatic force of attraction between positive ions and sea of electrons

Front

Explain why metals have high melting and boiling points (extended only)

Back

Metals have high melting and boiling points due to strong electrostatic attraction between positive metal ions and delocalised electrons/sea of electrons/mobile electrons which lead to strong metallic bond which require a lot of energy to overcome