Chapter 9 (Metallic bonding) Flashcards
What happen when metal atoms bond together to form the solid?
The outer electrons on each metal atoms becomes free to move throughout the whole structure.
What does a metallic structure consist of?
It consists of a lattice of positive ions in a sea of delocalized electrons.
What is metallic bonding?
Metallic bonding is the electrostatic force of attraction between each positive ion and delocalized electrons.
Which kind of structure does metals have?
Metals have giant structure and have no individual molecules.
What are the properties of metals?
- They are hard and have high melting point
- They conduct electricity
- They are malleable
- They are ductile
Why magnesium has higher melting and boiling point than sodium?
Magnesium has 2 outer electrons, which become delocalized into the sea leaving behind ions that carry a charge of 2+.
There is a much stronger electrostatic attraction between the 2+ ions and delocalized electrons.
Why do metals conduct electricity?
Because the delocalized electrons are free to move throughout the structure.
Why metals are malleable?
When we apply a force to a piece of metal the layers of positive ions slide over each other and it doesn’t affect the bonding in the structure since the positive ions are still attracted to the delocalized electrons.
