Chemistry Notes Topic 2 - Metallic Bonding
Metallic bonding:
This is the strong electrostatic attraction between metal ions and the delocalised electrons.
Metallic structures:
● Metals also have giant structures.
● Metal elements exist as giant metallic lattice structures.
● In metallic lattices, the outer electrons are delocalised and free to move around,
which makes the metal a positive ion.
● The positive metal ions are electrostatically attracted to the delocalised negative
electrons, so they form a lattice of closely packed positive ions in a sea of delocalised
electrons.
● The overall structure is made up of layers of positive metal ions separated by layers
of electrons.
Properties of metallic structures:
● High melting/boiling points - strong metallic bonding. The more electrons there are,
the stronger the bonding and therefore the higher the melting point.
● Malleable and ductile - the layers of metal cations are separated by layers of
electrons and there are no bonds, so the layers can slide over each other easily.
● Good thermal conductors - the delocalised electrons can pass kinetic energy to each
other.
● Good electrical conductors - the delocalised electrons are free to move and can carry
a current.
● Insoluble (except in liquid metals) - the metallic bonds are very strong.
Metallic bonding:
This is the strong electrostatic attraction between metal ions and the delocalised electrons.
Metallic structures:
● Metals also have giant structures.
● Metal elements exist as giant metallic lattice structures.
● In metallic lattices, the outer electrons are delocalised and free to move around,
which makes the metal a positive ion.
● The positive metal ions are electrostatically attracted to the delocalised negative
electrons, so they form a lattice of closely packed positive ions in a sea of delocalised
electrons.
● The overall structure is made up of layers of positive metal ions separated by layers
of electrons.
Properties of metallic structures:
● High melting/boiling points - strong metallic bonding. The more electrons there are,
the stronger the bonding and therefore the higher the melting point.
● Malleable and ductile - the layers of metal cations are separated by layers of
electrons and there are no bonds, so the layers can slide over each other easily.
● Good thermal conductors - the delocalised electrons can pass kinetic energy to each
other.
● Good electrical conductors - the delocalised electrons are free to move and can carry
a current.
● Insoluble (except in liquid metals) - the metallic bonds are very strong.
