Who this is for: Cambridge IGCSE Chemistry (0620) students who want properties of metals — conductivity, malleability and the link to metallic bonding — to become structured answers instead of a vague list of “metal things”.
What query it owns: how to understand and revise properties of metals in Cambridge IGCSE Chemistry.
Why this is safe: this page owns the properties of metals revision-guide angle, while Tutopiya’s Properties Of Metals subtopic page owns the learning resource and the free Properties Of Metals quiz owns the practice.

Properties of metals are the physical and chemical features that distinguish metals from non-metals. Cambridge IGCSE Chemistry (0620) tests electrical and thermal conductivity, malleability and ductility, lustre, high melting points and the giant metallic lattice of positive ions in a sea of delocalised electrons. This guide organises each property with its bonding explanation and the comparison questions examiners set against non-metals.

Key takeaways

• Metals conduct electricity and heat because of delocalised electrons that are free to move.
• Malleable (hammered into sheets) and ductile (drawn into wires) — layers of ions slide without breaking the metallic bond.
• Metals have high melting points and are usually solid at room temperature (mercury is the exception).
• Metal oxides are generally basic; metal chlorides in solution conduct electricity.
• Alloys are mixtures of metals (or metal + non-metal) with improved properties — harder than pure metals.

What are properties of metals in Cambridge IGCSE Chemistry?

Properties of metals are the characteristic physical and chemical behaviours of metallic elements and alloys. In Cambridge IGCSE Chemistry, you describe properties, explain them using metallic bonding, and contrast metals with non-metals. Chemical properties include reaction with oxygen to form basic oxides and reaction with acids (for reactive metals).

Read the full notes on Tutopiya’s Properties Of Metals subtopic page before attempting questions.

The core properties you must master

Property	Explanation (metallic bonding)	How the exam uses it
Electrical conductivity	Delocalised electrons move when voltage applied	”Explain why copper conducts electricity”
Thermal conductivity	Free electrons transfer kinetic energy	Compare with non-metals
Malleability / ductility	Ion layers slide; electron sea maintains bond	”Explain why metals can be hammered into sheets”
High melting point	Strong attraction between ions and electron sea	Compare with simple molecular non-metals
Basic oxides	Metal oxides react with acids	”Classify the oxide of magnesium”

How to explain metal properties — step by step

1. Name the property — conductivity, malleability, etc.
2. Describe metallic structure — lattice of positive ions in a sea of delocalised electrons.
3. Link structure to property — electrons move (conductivity) or layers slide (malleability).
4. For comparisons, state what non-metals lack — no free electrons, molecular structure.
5. Give a specific metal example — copper, iron, aluminium.

Test yourself with the free Properties Of Metals quiz.

Physical vs chemical properties: which does the question want?

Situation	What to write	Typical signal words
Bonding explanation	Delocalised electrons, ion lattice	”explain why metals conduct”
Oxide behaviour	Basic oxides react with acids	”nature of magnesium oxide”
Alloy properties	Mixture — harder, corrosion resistant	”why stainless steel is used”
vs non-metals	Conductivity, melting point contrast	”compare properties of metals and non-metals”

Properties of metals in past-paper wording: command words that matter

Command word / phrase	What the question wants	Typical metals stem
Describe	List properties without full bonding	”Describe three properties of metals.”
Explain	Property linked to metallic bonding	”Explain why metals are malleable.”
Compare	Metal vs non-metal	”Compare electrical conductivity of metals and non-metals.”
State	Named property or example	”State one use of aluminium based on its properties.”

Worked exam-style stems (how to answer the wording)

1. “Explain why metals conduct electricity.” Metals contain delocalised electrons in a giant lattice that are free to move and carry charge through the structure. Reward: delocalised electrons + movement.
2. “Explain why metals are malleable.” Layers of positive ions can slide over each other without breaking the metallic bond because the electron sea maintains attraction. Reward: sliding layers + electron sea.
3. “Describe how the properties of an alloy differ from a pure metal.” Alloys are harder and often more corrosion-resistant because different-sized atoms distort the lattice and hinder layer movement. Reward: harder + lattice distortion.

When you can recognise the wording instantly, work through the Properties Of Metals quiz and Extraction Of Metals.

How properties of metals connect to the rest of the course

Metal properties link to The Periodic Table, Transition Elements, Reactivity Series and Uses Of Metals. The Cambridge IGCSE Chemistry resource hub links all units.

Common mistakes students make

• Saying metals conduct because of ions moving — it is delocalised electrons.
• Listing properties without explaining when the command word is “explain”.
• Forgetting mercury is a liquid metal at room temperature.
• Calling metal oxides acidic — they are basic (with aluminium oxide as amphoteric extension).
• Confusing alloys (mixtures) with compounds.

When you need more support

If bonding-explanation questions keep losing marks, work through the Properties Of Metals quiz, then get focused help from a Cambridge IGCSE Chemistry tutor.

Frequently asked questions

What is metallic bonding in IGCSE terms? A lattice of positive metal ions surrounded by a sea of delocalised electrons — the attraction between ions and electrons holds the structure together.

Why are alloys harder than pure metals? Different-sized atoms in the alloy distort the regular lattice, making it harder for layers to slide.

Do all metals conduct electricity? Yes — all metals have delocalised electrons; conductivity varies but the property is universal for metals.

How do I revise properties of metals effectively? Learn each property with its bonding explanation, then take the Properties Of Metals quiz before tackling comparison questions.

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