Metallic Bonding Flashcards
What is metallic bonding?
Arrangement of atoms with electrostatic forces of attraction between the nuclei of these atoms and their delocalized electrons that can move within the 3-dimensional lattice.
How do metal atoms achieve stability?
Metals achieve stability by “off-loading” electrons to attain the electronic structure of the nearest noble gas. These electrons are delocalized and form a “mobile sea of electrons” which prevents the newly-formed positive ions from flying apart due to repulsion between similar charges.
What are the properties of metallic bonding?
-Conductors of electricity
- Malleable & ductile
- Solid at room temp
- High BP/MP
Why are metals good conductors of electricity?
For a substance to conduct electricity, it must have mobile ions/electrons. The mobile sea of delocalized electrons in metallic structures allows charge to be carried freely through its structure.
What is malleability vs ductile?
Malleable - Can be hammered into sheets
Ductile - Can be drawn into rods and wires
Why are metals malleable and ductile?
Bonding between metal ions and the sea of delocalized electrons is non-directional. Therefore, individual metal atoms can move in relation to each other without breaking the bonds between them and the sea of electrons.
Why are metals solid at room temp?
The strong electrostatic forces of attraction between the mobile sea of electrons and the metal ions requires high energy and hence high temperature to break its lattice.
