Properties, Uses & Alloys of Metals

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Properties, Uses & Alloys of Metals

Cambridge IGCSE Chemistry

Understand why metals behave the way they do, what we use them for, and how we can combine them to create even better materials. Master the structure–property–use connection that examiners love to test.

The Big Idea

Metals have special properties—they conduct electricity, bend without breaking, and melt at high temperatures—because of their internal structure (positive ions surrounded by delocalised electrons). These properties are exactly what we need for different uses: copper for wires, aluminium for aeroplanes, etc. When we mix metals together to make alloys, we can create new materials that are stronger, more corrosion-resistant, or harder than the pure metals alone. This is the power of understanding structure: it explains properties, and properties determine uses.

At a Glance

Properties of Metals

Conduct electricity & heat (delocalised electrons), malleable & ductile (layers slide), high melting points (strong metallic bonds)

Chemical Reactions

Metals react with water, acids, and oxygen. Reactivity varies: some vigorous, some slow. Products are hydroxides, oxides, or salts.

Aluminium Uses

Low density + corrosion-resistant (oxide layer) → aircraft bodies, power cables, food cans

Copper Uses

Excellent conductor + ductile + unreactive → electrical wiring, cookware, water pipes

Alloys

Mixtures (not compounds) of metals. Different-sized atoms distort the regular structure, making it harder to bend → stronger/harder material.

Key Alloy Examples

Brass (Cu+Zn) for musical instruments; stainless steel (Fe+Cr/Ni/C) for cutlery.

Properties of Metals

Why Do Metals Have Special Properties?

The key to understanding metals is their structure. Inside a metal, you have positive metal ions (atoms that have lost electrons) arranged in a tight lattice, surrounded by a "sea" of delocalised electrons. These delocalised electrons are electrons that don't belong to any one atom—they move freely throughout the entire metal structure. This is fundamentally different from other materials, and it's why metals behave so differently.

Let's unpack what this structure means for each property:

1. Conduct Electricity & Heat

Metals are excellent conductors of both electricity and heat. Why? Because of those delocalised electrons. These electrons can move freely through the metal without being tied to any particular atom. So when you apply an electrical voltage across a metal, the electrons move easily—that's electric current. When you apply heat to one end, the free electrons gain energy and move around, transferring that energy throughout the metal—that's heat conduction.

Think of it like:

KEY POINT

Metals conduct electricity and heat because they have delocalised electrons that can move freely throughout the structure.

2. Malleable & Ductile

3. High Melting & Boiling Points

metallic bonds

Non-Metals (By Contrast)

Non-metals have the opposite properties:

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Also in the full note

Chemical Properties: How Metals React
Uses of Metals: Structure Determines Application
Alloys: Mixing Metals to Improve Properties
What to Memorise
Concepts Checklist
Exam Tips & Common Mistakes
Understanding Reactivity
Reaction 1: Metals with Water

What's inside

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Properties, Uses & Alloys of Metals