Bonding Flashcards
What is metallic bonding
-Have a giant metallic structure
- This involves metals only. In a metal element the outer electrons merge and are no longer associated with any one atom ( they are delocalised). Therefore metallic bonding involves a lattice of positive ions surrounded by a sea of delocalised electrons.
The positive metal ions would normally repel each other, but are attracted to the delocalised sea of electrons by electrostatic attraction.
What is a feature of metallic bonding
Metallic bonds spread throughout so metals have a giant metallic structure and are very strong because there are no individual bonds to break.
Why are metals malleable
Because the layers can slide over each other
How can metals conduct electricity
Carry charge
Move freely
The delocalised electrons are of course negatively charged and are able to move. This is why metals conduct
Why do metals have high melting and boiling points
Because of their giant structures. There’s a strong attraction between the metal ions and the delocalised electrons making it difficult to separate the atoms.
