Metallic bonding

Delocalised electrons

an electron that is able to move freely throughout a structure

Positive metal ions

Metal atoms that have lost their outer electrons

Lattice

Regular arrangement of particles.

Giant structure

A huge 3D network of atoms or ions

Electrostatic forces of attraction

Strong forces of attraction between oppositely charged particles

Metallic bonding

A lattice of positive metal ions surrounded by delocalised outer electrons, held together by strong electrostatic forces of attraction

Melting and boiling points of metallic substances

high

Reason for metals high melting and boiling points

Strong electrostatic forces between positive metal ions and negative delocalised electrons

Reason for metals being malleable

Layers of metal ions can slide over each other

Reason alloys are harder than pure metals

Different sized atoms disrupt the layers of ions, preventing layers from sliding

Usefulness of pure metals

Too soft for most uses.

Reason metals conduct heat well

Delocalised electrons can transfer heat energy quickly

Reason metals conduct electricity well

Delocalised electrons can carry electrical charge through the structure.