Properties of metals

Metallic bond

Electrostatic forces of attraction positive metal ions and negative delocalised electrons

What structure do metals have?

Giant metallic lattice

Metals: Boiling/Melting points (4)

Metals form a giant metallic lattice

These contain millions of strong electrostatic forces of attraction between positive metal ions and negative delocalised electrons

For metals to melt or boil, these forces must be overcome and broken

They have high melting and boiling points, and are usually solid at room temperature

Metals: Solubility (4)

Metals are insoluble in water and most other solvents

Metals contain millions of strong electrostatic forces of attraction between positive metal ions and negative delocalised electrons (metallic bonds)

These forces are stronger than the forces found in water and other solvents

Therefore, the solute-solute forces cannot be overcome because they are of much larger strength than the solute-solute forces, and the metal cannot dissolve

Thermal conduction

The delocalised electrons are free to move and carry thermal energy

Electrical conduction

The delocalised electrons are free to move and carry charge

Why are pure metals soft? (3)

The positive metal ions are arranged in layers

These layers easily slide over eachother

Pure metals are very malleable

What are alloys?

A mixture of two or more elements, one of which is a metal

Why are alloys harder than pure metals? (3)

The atoms in alloys have different sizes

The layers in the metal are distorted

They can no longer slide over eachother

Why do metals have high density?

Atoms are closely packed together