What Is Metallic Bonding?

Metallic bonding is the type of bonding found in metals. It occurs due to the electrostatic attraction between positive metal ions and a sea of delocalised electrons.

In metallic structures:

• Metal atoms lose outer electrons
• These electrons become free-moving (delocalised)
• The remaining atoms become positive metal ions

The attraction between the positive ions and the delocalised electrons holds the metal together.

This structure forms a giant metallic lattice.

Structure of Metals

Metals have a regular lattice arrangement made of:

• Positive metal ions
• Delocalised electrons moving freely between them

These free electrons move throughout the structure, creating what is often described as a “sea of electrons.”

This structure explains many of the unique properties of metals.

Properties of Metals

Metals have several characteristic properties because of metallic bonding.

Electrical Conductivity

Metals are good conductors of electricity.

This is because delocalised electrons are free to move through the metal lattice, allowing electric current to flow.

Example:

Copper and aluminium are widely used in electrical wiring.

Thermal Conductivity

Metals also conduct heat very well.

Heat energy is transferred quickly through the movement of free electrons and vibrating metal ions.

Example:

Aluminium is used in cooking utensils because it transfers heat efficiently.

Malleability

Metals are malleable, meaning they can be hammered or pressed into thin sheets without breaking.

This happens because the layers of metal ions can slide over each other while the sea of electrons continues to hold the structure together.

Example:

Aluminium foil.

Ductility

Metals are also ductile, meaning they can be drawn into wires.

Example:

Copper wires used in electrical cables.

Examples of Metals and Their Uses

Metals are used widely because of their useful properties.

MetalImportant PropertyCommon UseCopperExcellent electrical conductorElectrical wiringAluminiumLightweight and corrosion resistantAircraft bodiesIronStrong and durableConstruction materialsGoldResistant to corrosionJewellery and electronics

Giant Metallic Lattice

Metals exist in a giant metallic lattice structure.

This structure contains:

• Many positive metal ions arranged in layers
• A large number of delocalised electrons moving freely

The strong electrostatic attraction between these particles gives metals their strength and stability.

Why Metallic Bonding Is Important

Understanding metallic bonding helps explain:

• Why metals conduct electricity and heat
• Why metals are strong and durable
• Why metals can be shaped without breaking

This concept is essential for understanding materials used in technology and engineering.

Exam Tip (5070)

Students are commonly asked to:

• Define metallic bonding
• Explain why metals conduct electricity
• Describe the structure of metals

Example exam question:

Why do metals conduct electricity?

Answer:

Metals conduct electricity because they contain delocalised electrons that are free to move through the lattice and carry electric charge.

Practice Question

Explain why metals are malleable.

Answer

Metals are malleable because the layers of metal ions can slide over each other while the delocalised electrons keep the structure bonded together.

This allows metals to change shape without breaking.

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