Properties of Metals
The link between metallic bonding and the properties of metals
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Metals have high melting and boiling points
o There are many strong metallic bonds in giant metallic structures
o A lot of heat energy is needed to overcome forces and break these
bonds
•
Metals conduct electricity
o There are free electrons available to move and carry charge
o Electrons entering one end of the metal cause a delocalised electron to
displace itself from the other end
o Hence electrons can flow so electricity is conducted
•
Metals are malleable and ductile
o Layers of positive ions can slide over one another and take up different
positions
o Metallic bonding is not disrupted as the valence electrons do not
belong to any particular metal atom so the delocalised electrons will
move with them
o Metallic bonds are thus not broken and as a result metals are strong
but flexible
o They can be hammered and bent into different shapes without breaking
•
The typical properties of metals and non-metals can be compared side-byside:
Comparison Table of Metals and Non-metals
Metals
Non-metals
Solids at room temperature (except
mercury)
Different states at room temperature
Shiny
Dull (when solid)
High density
Low density
Good conductors of electricity
Poor conductors of electricity
Good conductors of heat
Poor conductors of heat
High melting points
Low melting points
Malleable (can be bent and shaped)
Ductile (can be drawn into wires)
Brittle (when solid)