Uploaded by lxmygk

metallic properties

Metallic Bonding
Type of Structure
“Electron Sea”
• Charged particles
that are free to
move and conduct
• Strong forces of
attraction between
atoms throughout
the metal structure
Metallic Lustre
Because of the reflection of light by the
mobile electrons
C. Johannesson
Metals are Hard and Dense
Metals are usually hard and tend to have high
melting and boiling points
Strong electrostatic forces of attraction between positive
metal ions and the sea of delocalised electrons holds the
metallic lattice together
Good conductors of Electricity
When a metal is connected to electricity,
one end of the metal becomes positive
and the other becomes negative. Since
the electrons are free to move, they result
in an electric current
C. Johannesson
Conduction of Heat
Electrons are able to gain kinetic energy in hotter
areas of the metal and are able to quickly transfer
it to other parts of the metal lattice because of
their freedom of movement.
Heat causes the electrons to move faster and the
‘bumping’ of these electrons with each other and
the protons transfers the heat.
Malleable and Ductile
Malleable: Can be beaten in to thin sheets without breaking.
Ductile: Can be drawn in to a wire
The attractive forces between the particles is stronger than the
repulsive forces