What are the general properties of metals covered in the Cambridge IGCSE Coordinated Science syllabus?

In the Cambridge IGCSE Coordinated Science syllabus, metals are generally characterized by properties such as high electrical and thermal conductivity, malleability, ductility, and a shiny appearance. They are typically solid at room temperature, with the exception of mercury, and have high melting and boiling points.

Why are metals good conductors of electricity?

Metals are good conductors of electricity due to the presence of free electrons in their structure. These electrons can move freely throughout the metal lattice, allowing electrical current to pass through efficiently. This property is emphasized in the Cambridge IGCSE Coordinated Science curriculum when discussing the applications of metals.

How does the malleability of metals benefit their use in everyday applications?

Malleability refers to the ability of metals to be hammered or rolled into thin sheets without breaking. This property is beneficial in everyday applications such as the manufacturing of car bodies, aluminum foil, and various metal containers. The Cambridge IGCSE Coordinated Science course highlights this property to explain the versatility of metals in industrial and domestic uses.

What is the significance of the high melting points of metals in industrial applications?

The high melting points of metals make them suitable for use in high-temperature environments, such as in the construction of engines, turbines, and other machinery that operate under extreme heat. This property ensures that metals maintain their structural integrity and functionality, a concept explored in the Cambridge IGCSE Coordinated Science syllabus.

How does the ductility of metals contribute to their functionality in electrical wiring?

Ductility is the ability of metals to be drawn into wires. This property is crucial for electrical wiring because it allows metals like copper and aluminum to be stretched into long, thin wires without breaking. This aspect of metals is covered in the Cambridge IGCSE Coordinated Science curriculum to illustrate the practical applications of metal properties in technology and infrastructure.

Why is "Saying metal layers 'break' when the metal is deformed" a common mistake in Properties of Metals?

Why it happens: Students picture solid bonds snapping under force. How to avoid it: Layers SLIDE not break; delocalised electrons move with the ions, maintaining the metallic bonding. That's why metals are malleable/ductile, not brittle.

Why is "Saying alloys are weaker than pure metals" a common mistake in Properties of Metals?

Why it happens: Students confuse 'less malleable' with 'weaker'. How to avoid it: Alloys are HARDER and STRONGER than pure metals because the differently sized atoms prevent layer sliding. They are less malleable/ductile, but stronger. Source: 0654 Examiner Report 2023

Why is "Saying 'free protons' conduct electricity in metals" a common mistake in Properties of Metals?

Why it happens: Students know metals have positive ions and make an incorrect inference about charge carriers. How to avoid it: Electrons (negative charge carriers) are the mobile charge carriers in metals. The positive ions are FIXED in the lattice.

MetalsCambridge IGCSE Coordinated Sciences 0654

Properties of Metals

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Properties of Metals — Cambridge IGCSE Coordinated Science 0654

Metals have distinctive physical and chemical properties explained by their giant metallic lattice structure with delocalised electrons. Cambridge tests the structure-property relationship and typical metal reactions.

What you’ll learn

Mapped to the Cambridge IGCSE 0654 syllabus (2025-2027).

C10.1 — Describe metallic bonding and explain properties of metals.
C10.2 — Explain why alloys have different properties from pure metals.
C10.3 — Describe typical chemical properties of metals.

Metallic Bonding and Properties

Metals consist of positive ions in a sea of delocalised electrons. This structure explains all their key physical properties.

Metallic bonding: metal atoms release their outer electrons to form a 'sea' of delocalised electrons. The metal consists of a lattice of positive ions (cations) surrounded by and attracted to this electron sea.

Properties and explanations:

Property	Explanation in terms of metallic bonding
Good conductors of electricity	Delocalised electrons are free to move through the lattice; carry charge
Good conductors of heat	Delocalised electrons transfer kinetic energy rapidly through the metal
Malleable and ductile	Layers of positive ions can slide past each other without breaking bonds (electron sea moves with them)
High melting and boiling points	Many strong electrostatic attractions between positive ions and electron sea require much energy to overcome
Shiny	Free electrons reflect light
Generally solid at room temperature	Strong metallic bonds (except Hg — liquid)

Metals vs non-metals: Non-metals do NOT have delocalised electrons → poor conductors, brittle (bonds break when layers shift), low MP/BP (simple molecular).

Alloys:

A mixture of metals (or metal + non-metal carbon/silicon)
Different-sized atoms disrupt the regular lattice → layers cannot slide as easily → harder and stronger
Examples: steel (Fe + C), brass (Cu + Zn), bronze (Cu + Sn), solder (Pb + Sn), amalgam (Hg + another metal)
Steel is much harder than pure iron

Metallic bond: cations in delocalised electron sea. Electrostatic attraction throughout.
Delocalised electrons → conducts electricity + heat; malleable/ductile; shiny.
Alloys: disrupted lattice → harder, stronger than pure metals.

How it’s examined

Paper 4: 'Explain why metals conduct electricity' (2 marks — delocalised electrons, free to move, carry charge). 'Explain why an alloy is harder than the pure metal' (2 marks — different-sized atoms, disrupt regular layers, cannot slide easily). 'Explain why copper is malleable' (2 marks — layers of ions can slide, electron sea maintains bonding). Structure-property questions are very common.

Sources: Cambridge IGCSE Coordinated Sciences 0654 syllabus 2025-2027 (C10); 0654 Examiner Reports 2022-2024. Last reviewed 2026-05-14.

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Step-by-step worked examples — Properties of Metals

Step-by-step solutions to past-paper-style questions on properties of metals, written exactly the way a tutor would explain them at the board.

1Why metals conduct electricity
Extended
Question
Explain why metals are good conductors of electricity.
Step-by-step solution
1. Step 1
  In metallic bonding, the outer electrons of metal atoms become delocalised — they are no longer associated with specific atoms but are free to move throughout the entire metallic lattice.
2. Step 2
  When a potential difference is applied across the metal, these free (delocalised) electrons move in one direction through the lattice, constituting an electric current.
3. Step 3
  Because electrons can move freely throughout, metals are good conductors of electricity.
Answer
Delocalised electrons free to move throughout the metallic lattice; flow when potential difference applied → electric current → good conductor.
2Why stainless steel is harder than pure iron
Extended
Question
Explain why stainless steel (an alloy of iron, chromium, and nickel) is harder than pure iron.
Step-by-step solution
1. Step 1
  In pure iron, the atoms are arranged in regular layers of the same size. When a force is applied, these layers can slide over each other relatively easily.
2. Step 2
  In stainless steel, chromium and nickel atoms are different sizes from iron atoms. These different-sized atoms are randomly distributed in the iron lattice.
3. Step 3
  The differently sized atoms disrupt the regular layer arrangement, preventing layers from sliding easily over each other.
4. Step 4
  Therefore, stainless steel is harder and less malleable than pure iron.
Answer
Different-sized Cr/Ni atoms disrupt the regular iron lattice; layers cannot slide easily → harder than pure iron.
Examiner tip
Key phrase: 'different-sized atoms disrupt the regular layers'. This is the mechanism for alloy hardness.
3Properties making copper suitable for electrical wiring
Core
Question
Copper is used for household electrical wiring. State TWO properties of copper that make it suitable for this use.
Step-by-step solution
1. Step 1
  Property 1: copper is an excellent conductor of electricity (second only to silver among common metals); low electrical resistance minimises energy loss.
2. Step 2
  Property 2: copper is ductile (can be drawn into long, thin wires without breaking) and flexible, making it easy to install in homes.
Answer
Copper is an excellent electrical conductor AND ductile (can be drawn into wire); also relatively cheap and resistant to corrosion.

Key Definitions and Keywords — Properties of Metals

Definitions to memorise and the exact keywords mark schemes credit for properties of metals answers — sharpened from recent examiner reports for the 2026 0654 sitting.

Malleable
Examiner keyword
Can be beaten or rolled into sheets without breaking; a property of metals due to layers of positive ions that can slide over each other while delocalised electrons maintain bonding.
Ductile
Examiner keyword
Can be drawn into wires without breaking; copper and aluminium are particularly ductile, making them useful for electrical wiring.
Alloy
Examiner keyword
A mixture of a metal with one or more other elements (metal or non-metal); typically harder and stronger than the pure metal because different-sized atoms disrupt the regular lattice layers.
Example
Steel (Fe + C), brass (Cu + Zn), bronze (Cu + Sn), stainless steel (Fe + Cr + Ni).
Metallic bonding
Examiner keyword
Strong electrostatic attraction between a lattice of positive metal ions and a surrounding 'sea' of delocalised electrons; responsible for high melting points, electrical conductivity, and malleability.
Corrosion
The gradual destruction of a metal by chemical reaction with its environment (usually oxygen and water); rusting is the corrosion of iron/steel.

Common Mistakes and Misconceptions — Properties of Metals

The traps other students keep falling into on properties of metals questions — taken from recent Cambridge IGCSE 0654 examiner reports and mark schemes — and how to avoid them.

✕Saying metal layers 'break' when the metal is deformed
Why it happens
Students picture solid bonds snapping under force.
How to avoid it
Layers SLIDE not break; delocalised electrons move with the ions, maintaining the metallic bonding. That's why metals are malleable/ductile, not brittle.
✕Saying alloys are weaker than pure metals
0654 Examiner Report 2023
Why it happens
Students confuse 'less malleable' with 'weaker'.
How to avoid it
Alloys are HARDER and STRONGER than pure metals because the differently sized atoms prevent layer sliding. They are less malleable/ductile, but stronger.
✕Saying 'free protons' conduct electricity in metals
Why it happens
Students know metals have positive ions and make an incorrect inference about charge carriers.
How to avoid it
Electrons (negative charge carriers) are the mobile charge carriers in metals. The positive ions are FIXED in the lattice.

Practice questions

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Past paper style quiz

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Properties of Metals — frequently asked questions

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Properties of Metals

Short Study Notes in the form of Slides

Short Study Notes — Properties of Metals

Detailed Notes

What you’ll learn

How it’s examined

1Why metals conduct electricity

2Why stainless steel is harder than pure iron

3Properties making copper suitable for electrical wiring

Malleable

Ductile

Alloy

Metallic bonding

Corrosion

✕Saying metal layers 'break' when the metal is deformed

✕Saying alloys are weaker than pure metals

✕Saying 'free protons' conduct electricity in metals

Practice questions

Past paper style quiz

Assess your understanding

Properties of Metals — frequently asked questions