What Are Metals?

Metals are a group of elements that share similar physical and chemical properties.

Most metals are found on the left side and center of the periodic table. They are widely used because of their strength, conductivity, and durability.

Examples of common metals include:

• Iron (Fe)
• Copper (Cu)
• Aluminium (Al)
• Zinc (Zn)

Understanding the properties of metals helps explain why they are used in construction, transportation, and electronics.

Physical Properties of Metals

Metals have several characteristic physical properties.

Good Conductors of Electricity

Most metals are excellent conductors of electricity.

This is because metals contain delocalised electrons that can move freely through the metal structure.

Example:

Copper is commonly used in electrical wiring.

Good Conductors of Heat

Metals also conduct heat very efficiently.

Heat energy can move easily through the vibrating metal atoms and free electrons.

Example:

Aluminium is used in cooking utensils because it distributes heat evenly.

Malleability

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

Example:

Aluminium foil is produced by hammering aluminium into thin layers.

Ductility

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

Example:

Copper wires are widely used in electrical cables.

High Melting and Boiling Points

Most metals have high melting and boiling points because of strong metallic bonds.

Example:

Iron melts at about 1538°C.

Chemical Properties of Metals

Metals also have specific chemical properties.

Reaction with Oxygen

Many metals react with oxygen to form metal oxides.

Example:

2Mg + O₂ → 2MgO

Magnesium reacts with oxygen to produce magnesium oxide.

Reaction with Acids

Many metals react with acids to produce:

• Salt
• Hydrogen gas

Example:

Zn + 2HCl → ZnCl₂ + H₂

Zinc reacts with hydrochloric acid to produce hydrogen gas.

Formation of Positive Ions

Metals tend to lose electrons easily, forming positive ions (cations).

Example:

Na → Na⁺ + e⁻

This property explains why metals are good reducing agents.

Why Metals Are Important

Metals are essential in many industries and technologies.

They are used to produce:

• Buildings and bridges
• Vehicles and machinery
• Electrical wiring and electronics
• Household appliances

Because of their strength and conductivity, metals are among the most important materials used in modern society.

Exam Tip (5070)

Students are often asked to:

• Describe the physical properties of metals
• Explain why metals are good conductors of electricity
• Write reactions of metals with oxygen or acids

Example exam question:

Why do metals conduct electricity?

Answer:

Metals conduct electricity because they contain delocalised electrons that can move freely through the metal lattice.

Practice Question

What gas is produced when a metal reacts with an acid?

Answer

The gas produced is hydrogen (H₂).

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