Who this is for: Cambridge IGCSE Chemistry (0620) students who want metallic bonding — delocalised electrons, giant metallic lattices and why metals conduct and malleate — to become reliable marks instead of a vague “sea of electrons” phrase.
What query it owns: how to understand and revise metallic bonding in Cambridge IGCSE Chemistry.
Why this is safe: this page owns the metallic bonding revision-guide angle, while Tutopiya’s Metallic Bonding subtopic page owns the learning resource and the free Metallic Bonding quiz owns the practice.

Metallic bonding explains why metals are shiny, conduct electricity, and can be hammered into sheets. In Cambridge IGCSE Chemistry (0620), examiners expect you to link the giant metallic lattice of positive ions to delocalised electrons and then explain each property from that model. This guide covers the syllabus definitions, the property–structure links that earn marks, and the question types that appear every year.

Key takeaways

• Metallic bonding is the attraction between positive metal ions and a sea of delocalised electrons.
• Metal atoms lose outer-shell electrons to form positive ions in a regular giant lattice.
• Delocalised electrons carry charge — explaining electrical and thermal conductivity.
• Layers of ions can slide over each other — explaining malleability and ductility.
• Metallic bonding is strong — explaining high melting points of most metals.

What is metallic bonding in Cambridge IGCSE Chemistry?

Metallic bonding is the electrostatic attraction between the positive metal ions in a giant lattice and the delocalised electrons that move freely between them. Each metal atom contributes its outer electrons to the shared “sea”, leaving behind fixed positive ions. This model is used to explain conductivity, lustre, malleability and the generally high melting points of metals.

You can read the full explanation, lattice diagrams and notes on Tutopiya’s Metallic Bonding subtopic page before you attempt questions.

The core ideas you must master

Idea	What it means	How the exam uses it
Giant metallic lattice	Regular arrangement of positive ions	”Describe the structure of a metal.”
Delocalised electrons	Outer electrons free to move through the lattice	”Explain why metals conduct electricity.”
Positive metal ions	Atoms that have lost valence electrons	”State what holds the lattice together.”
Malleability	Can be hammered into shape without breaking	”Explain why metals are malleable.”
High melting point	Strong metallic bonds need much energy to break	”Suggest why iron has a high melting point.”

How to explain metal properties — step by step

The safest method links structure → particles → property in three clear sentences.

1. State the structure: giant lattice of positive metal ions in a regular arrangement.
2. Name the bonding particles: delocalised electrons between the ions.
3. Link to the property asked for — conductivity, malleability, melting point or lustre.
4. Use precise language: “delocalised electrons” not just “free electrons”; “layers slide” for malleability.
5. Compare with ionic or covalent structures when the question asks “why metals but not…”.

Once you have worked through a few, test yourself with the free Metallic Bonding quiz — it tells you fast whether the explanations have actually stuck.

Property vs structure: which explanation does the question want?

Property	Structure-based explanation	Typical signal words
Electrical conductivity	Delocalised electrons move and carry charge	”explain why copper conducts”
Thermal conductivity	Electrons transfer kinetic energy	”heat conduction in metals”
Malleability / ductility	Layers of ions slide; bonding remains	”hammered into sheets”, “drawn into wire”
High melting point	Strong attraction between ions and electrons	”high melting point of iron”
Lustre (shiny)	Electrons absorb and re-emit light	”shiny surface of metals”

Metallic bonding in past-paper wording: command words that matter

Command word / phrase	What the question wants	Typical metallic bonding stem
Describe	State features of structure or bonding	”Describe metallic bonding in sodium.”
Explain	Link structure to property with reason	”Explain why metals conduct electricity.”
State	Short factual answer	”State the particles in a metal lattice.”
Suggest	Apply the model to a new metal	”Suggest why aluminium is ductile.”
Compare	Contrast with ionic or covalent	”Compare bonding in sodium chloride and copper.”

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

1. “Describe metallic bonding in magnesium.” Magnesium atoms lose two outer electrons to form Mg²⁺ ions arranged in a giant lattice. The delocalised electrons are attracted to the positive ions, holding the structure together. Mark-scheme reward: positive ions + delocalised electrons + attraction.
2. “Explain why metals conduct electricity when solid.” Delocalised electrons are free to move through the lattice. When a potential difference is applied, they flow and carry charge. Reward: moving electrons linked to charge transfer — not just “electrons are free”.
3. “Explain why metals are malleable.” The ions are in layers. When a force is applied, layers slide over each other. Delocalised electrons still hold the structure together so the metal does not break. Reward: sliding layers + bonding maintained.

When you can recognise the wording instantly, work the full set on the Atoms, Elements and Compounds topical past paper questions and the Metallic Bonding quiz to lock the method in.

How metallic bonding connects to the rest of Atoms, Elements and Compounds

Metallic bonding sits alongside Ions and Ionic Bonds and Simple Molecules and Covalent Bonds — compare questions often ask why metals conduct but ionic solids do not (until molten). Giant Covalent Structures contrast on hardness and melting point. When you are ready to mix topics, the Cambridge IGCSE Chemistry resource hub lets you move straight from a weak subtopic into the next.

Common mistakes students make

• Saying metals conduct because “electrons are shared” — use delocalised electrons in a metallic lattice.
• Explaining malleability without mentioning layers sliding.
• Confusing metallic bonding with intermolecular forces in simple molecules.
• Stating that ionic solids conduct electricity when solid — they need to be molten or aqueous.
• Giving property lists without linking each one back to structure.

When you need more support

If metallic bonding explanations keep losing “explain” marks — especially compare questions with ionic compounds — work through the Atoms, Elements and Compounds topical past paper questions and the Metallic Bonding quiz to pinpoint the exact gap, then get focused help from a Cambridge IGCSE Chemistry tutor to fix it quickly.

Frequently asked questions

Is metallic bonding hard in Cambridge IGCSE Chemistry? No — the model is straightforward. Marks are lost when students name properties without linking them to delocalised electrons and the giant lattice.

What is the difference between metallic and ionic bonding? Ionic bonding is attraction between oppositely charged ions in a giant lattice; metallic bonding is attraction between positive metal ions and delocalised electrons. Ionic solids do not conduct when solid; metals do.

Why do metals have high melting points? Strong electrostatic attraction between positive ions and delocalised electrons requires a lot of energy to overcome.

How do I revise metallic bonding effectively? Read the subtopic notes, practise structure-to-property explanations on every question, then take the Metallic Bonding quiz. Revisit any compare questions you got wrong before moving on.

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