What Is Metallic Bonding?

Metallic bonding is the type of bonding found in metals.

In metallic bonding, metal atoms lose their outer electrons and form positive metal ions. The electrons that are lost become delocalised electrons, meaning they are free to move throughout the metal structure.

Metallic bonding is the strong electrostatic attraction between positive metal ions and the sea of delocalised electrons.

This structure explains many of the unique properties of metals.

Structure of Metals

Metals form a giant metallic lattice structure.

In this structure:

• Positive metal ions are arranged in regular layers
• Delocalised electrons move freely between these ions

This arrangement creates a strong metallic bond that holds the structure together.

Because electrons can move freely, metals have special electrical and thermal properties.

Delocalised Electrons

The electrons in metallic bonding are called delocalised electrons because they are not attached to any single atom.

These electrons move freely throughout the metal lattice.

The movement of these electrons explains why metals:

• Conduct electricity
• Conduct heat efficiently

Properties of Metals Explained by Metallic Bonding

Metallic bonding explains many important properties of metals.

Electrical Conductivity

Metals are good conductors of electricity because the delocalised electrons can move freely and carry electric charge.

Example:

Copper is widely used in electrical wiring.

Thermal Conductivity

Metals conduct heat efficiently because energy is transferred through moving electrons and vibrating ions.

Example:

Aluminium is commonly used in cooking utensils.

Malleability

Metals are malleable, meaning they can be hammered into thin sheets.

This happens because the layers of metal ions can slide over each other without breaking the metallic bond.

Example:

Gold can be hammered into extremely thin sheets.

Ductility

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

This property occurs because the metallic structure remains intact even when stretched.

Example:

Copper wires used in electrical cables.

High Melting and Boiling Points

Metals often have high melting and boiling points because strong electrostatic attractions exist between positive ions and delocalised electrons.

A large amount of energy is required to break these bonds.

Examples of Metals with Metallic Bonding

Many common metals display metallic bonding.

Examples include:

• Iron (Fe)
• Copper (Cu)
• Aluminium (Al)
• Sodium (Na)

These metals form giant metallic structures with strong bonding forces.

Importance of Metallic Bonding

Understanding metallic bonding helps explain why metals are used in many industries.

Metals are essential in:

• Construction and engineering
• Electrical wiring and electronics
• Transportation and vehicles
• Machinery and tools

Their strength and conductivity make metals extremely valuable materials.

Exam Tip (5070)

Students are often asked to:

• Define metallic bonding
• Describe the structure of metals
• Explain properties of metals using delocalised electrons

Example exam question:

Why do metals conduct electricity?

Answer:

Metals conduct electricity because delocalised electrons are free to move through the metallic lattice.

Practice Question

Why are metals malleable?

Answer

Metals are malleable because layers of metal ions can slide over each other while the metallic bond remains intact.

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