IGCSE Metallic Bonding: Complete Guide for Cambridge IGCSE Chemistry

IGCSE metallic bonding explains how metal atoms are held together and why metals have their characteristic properties. Mastering metallic structure, the electron sea model, and properties of metals is essential for achieving top grades in IGCSE Chemistry exams.

This comprehensive IGCSE metallic bonding guide covers everything you need to know, including what metallic bonding is, the structure of metals, why metals have their properties, step-by-step worked examples, common exam questions, and expert tips from Tutopiya’s IGCSE chemistry tutors.

🎯 What you’ll learn: By the end of this guide, you’ll know how metallic bonding works, explain why metals have their properties, understand the electron sea model, and apply these concepts to solve problems in IGCSE Chemistry exams.

Already studying with Tutopiya? Practice these skills with our dedicated IGCSE Chemistry practice deck featuring exam-style questions and instant feedback.

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Why IGCSE Metallic Bonding Matters

IGCSE metallic bonding is an important topic that appears regularly in IGCSE Chemistry. Here’s why:

• High frequency topic: Questions about metallic bonding appear in many IGCSE chemistry papers
• Foundation concept: Essential for understanding metal properties
• Exam weight: Typically worth 6-10 marks per paper
• Real-world applications: Essential for understanding why metals are useful materials

Key insight from examiners: Students often struggle to explain why metals conduct electricity or why they are malleable. This guide will help you master these concepts.

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Understanding Metallic Bonding

Metallic bonding is the electrostatic attraction between positive metal ions and delocalized electrons.

Structure of Metals

• Metal atoms: Lose outer shell electrons → become positive ions
• Delocalized electrons: Outer electrons are free to move throughout the structure
• Electron sea model: Electrons form a “sea” around positive ions
• Strong attraction: Between positive ions and delocalized electrons
• Giant metallic structure: Many atoms held together

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Properties of Metals

Good Conductors of Electricity

Why:

• Delocalized electrons can move freely
• When voltage applied, electrons flow
• Charge carriers are mobile electrons

Good Conductors of Heat

Why:

• Delocalized electrons can transfer energy
• Vibrations can pass through structure
• Energy transferred quickly

Malleable and Ductile

Why:

• Layers of ions can slide over each other
• Delocalized electrons maintain attraction
• Structure can be reshaped without breaking

High Melting and Boiling Points

Why:

• Strong metallic bonds throughout structure
• Lots of energy needed to break bonds
• Varies by metal (depends on bond strength)

Shiny (Lustrous)

Why:

• Delocalized electrons reflect light
• Smooth surfaces reflect light well

High Density

Why:

• Closely packed positive ions
• Atoms/ions arranged efficiently

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Electron Sea Model

The electron sea model describes metallic bonding:

• Positive metal ions are arranged in a regular lattice
• Outer electrons are delocalized (free to move)
• Electrons form a “sea” around the ions
• Electrostatic attraction holds structure together

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Structure of Metals in Detail

Arrangement of Ions

• Positive metal ions: Arranged in a regular pattern (lattice)
• Close-packed: Ions are closely packed together
• Layers: Ions arranged in layers
• Can slide: Layers can move over each other

Delocalized Electrons

• Origin: Outer shell electrons from metal atoms
• Movement: Free to move throughout the entire structure
• Not attached: Not to any specific atom
• Electron sea: Form a “sea” around positive ions

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Detailed Explanation of Properties

Good Electrical Conductivity

Explanation:

• Metal atoms lose outer electrons → become positive ions
• Outer electrons become delocalized (free to move)
• When voltage is applied across metal, delocalized electrons flow
• Electrons carry charge from negative to positive end
• Electricity flows through the metal

Key point: Electrons are mobile charge carriers.

Good Thermal Conductivity

Explanation:

• Delocalized electrons can transfer energy
• When one end is heated, electrons gain kinetic energy
• Electrons move and transfer energy throughout structure
• Vibrations also pass through the lattice
• Energy is conducted quickly

Malleability (Can be hammered into shape)

Explanation:

• Metals have layers of positive ions
• These layers can slide over each other
• When force is applied, layers shift
• Delocalized electrons maintain attraction between ions
• Structure can be reshaped without breaking

Ductility (Can be drawn into wires)

Explanation:

• Same principle as malleability
• Layers can slide, allowing metal to be stretched
• Delocalized electrons maintain structure
• Metal can be drawn into thin wires

High Melting and Boiling Points

Explanation:

• Strong metallic bonds between positive ions and delocalized electrons
• Many bonds must be broken to melt
• Requires lots of energy
• Melting points vary (depends on bond strength)

Note: Some metals have relatively low melting points (e.g., sodium, mercury), while others have very high melting points (e.g., tungsten).

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Comparing Types of Bonding

Property	Metallic	Ionic	Covalent (Simple)
Structure	Giant metallic	Giant ionic	Simple molecules
Bonding	Metallic bonds	Ionic bonds	Covalent bonds
Melting point	High (varies)	Very high	Low
Electrical conductivity	Yes (solid)	Yes (molten/dissolved)	No
Malleable	Yes	No (brittle)	N/A
Hardness	Varies	Hard	Soft

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Uses Based on Properties

Electrical Wires (Conductivity)

• Copper and aluminum used
• Good electrical conductors
• Ductile (can be drawn into wires)

Cooking Utensils (Heat Conduction)

• Metals conduct heat well
• Heat spreads evenly
• Good for pans and pots

Structural Materials (Strength + Malleability)

• Can be shaped into various forms
• Strong but can be worked
• Used in construction

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Step-by-Step Method for Metallic Bonding Problems

1. Identify the property - What property needs explaining?
2. Recall structure - Positive ions + delocalized electrons
3. Link to property - How does structure cause this property?
4. Mention electrons - Delocalized electrons are key
5. Check explanation - Does it make sense?

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Worked Examples

Example 1: Electrical Conductivity

Explain why metals are good conductors of electricity.

Solution:

1. Metal atoms lose their outer shell electrons to form positive metal ions
2. These outer electrons become delocalized - they are free to move throughout the entire structure
3. When a voltage is applied across the metal, the delocalized electrons are attracted to the positive terminal
4. Electrons flow through the metal from negative to positive end
5. Moving electrons carry electrical charge, allowing electricity to flow
6. Therefore, metals conduct electricity

Example 2: Malleability

Explain why metals are malleable (can be hammered into shape).

Solution:

1. Metals have a structure with layers of positive ions arranged in a regular pattern
2. These layers are held together by delocalized electrons that attract the positive ions
3. When force is applied (e.g., hammering), the layers can slide over each other
4. The delocalized electrons maintain the attraction between ions even when layers move
5. The structure can be reshaped without breaking bonds
6. Therefore, metals are malleable

Example 3: High Melting Point

Explain why metals generally have high melting points.

Solution:

1. Metals have strong metallic bonds throughout the structure
2. Metallic bonds are the electrostatic attraction between positive ions and delocalized electrons
3. To melt the metal, many of these strong bonds must be broken
4. Breaking many strong bonds requires a lot of energy
5. Therefore, metals generally have high melting points
6. (Note: Some metals like sodium and mercury have lower melting points due to weaker bonds)

Example 4: Thermal Conductivity

Explain why metals are good conductors of heat.

Solution:

1. Metals have delocalized electrons that can move freely
2. When one part of the metal is heated, electrons in that area gain kinetic energy
3. These energetic electrons move throughout the structure, transferring energy
4. Additionally, vibrations pass through the lattice of positive ions
5. Energy is transferred quickly through both mechanisms
6. Therefore, metals conduct heat well

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Common Examiner Traps (and How to Dodge Them)

• Not mentioning delocalized electrons - These are crucial for explaining conductivity and other properties
• Confusing with ionic bonding - Metallic bonding has delocalized electrons; ionic has ions in fixed positions
• Not explaining malleability properly - Must mention layers sliding and electrons maintaining attraction
• Forgetting the structure - Always mention positive ions in a lattice
• Wrong explanation of conductivity - Must explain that electrons move and carry charge
• Not distinguishing solid vs molten - Metals conduct in solid state (unlike ionic compounds)

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IGCSE Metallic Bonding Practice Questions

Question 1: Electrical Conductivity

Explain why metals are good conductors of electricity.

Solution:

• Metal atoms lose outer electrons to form positive ions
• These outer electrons become delocalized (free to move throughout the structure)
• When voltage is applied, delocalized electrons are attracted to the positive terminal
• Electrons flow through the metal, carrying electrical charge
• Therefore, metals conduct electricity

Question 2: Malleability

Explain why metals are malleable but ionic compounds are brittle.

Solution:

• Metals: Have layers of positive ions that can slide over each other. Delocalized electrons maintain attraction between ions even when layers move. Structure can be reshaped.
• Ionic compounds: Have rigid ionic lattice. When force applied, ions of same charge come together and repel, causing structure to shatter. Cannot be reshaped.

Question 3: Structure

Describe the structure of a metal in terms of metallic bonding.

Solution:

• Positive metal ions arranged in a regular pattern (lattice)
• Outer electrons from metal atoms become delocalized (free to move)
• Delocalized electrons form a “sea” around positive ions
• Strong electrostatic attraction between positive ions and delocalized electrons
• This attraction is the metallic bond, holding the structure together

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Frequently Asked Questions About IGCSE Metallic Bonding

What is metallic bonding?

Metallic bonding is the electrostatic attraction between positive metal ions and delocalized electrons. Metal atoms lose outer electrons to form positive ions, and these electrons become delocalized (free to move).

Why do metals conduct electricity?

Metals have delocalized electrons (outer electrons from metal atoms that are free to move). When voltage is applied, these electrons can flow through the structure, carrying electrical charge.

Why are metals malleable?

Metals have layers of positive ions that can slide over each other. Delocalized electrons maintain the attraction between ions even when layers move, allowing the structure to be reshaped without breaking.

What are delocalized electrons?

Delocalized electrons are outer shell electrons from metal atoms that are not attached to any specific atom. They are free to move throughout the entire metallic structure.

Why do metals have high melting points?

Metals have strong metallic bonds (attraction between positive ions and delocalized electrons) throughout the structure. Melting requires breaking many of these bonds, which needs lots of energy.

What’s the difference between metallic and ionic bonding?

Metallic bonding: Positive ions + delocalized electrons (electrons can move). Ionic bonding: Positive and negative ions in fixed positions (electrons transferred, not delocalized).

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Related IGCSE Chemistry Resources

Strengthen your IGCSE Chemistry preparation with these comprehensive guides:

• IGCSE Ions and Ionic Bonds: Complete Guide - Master ionic bonding
• IGCSE Simple Molecules and Covalent Bonds: Complete Guide - Master covalent bonding
• IGCSE Giant Covalent Structures: Complete Guide - Master diamond and graphite
• IGCSE Chemistry Revision Notes, Syllabus and Preparation Tips - Complete syllabus overview, topic breakdown, and revision strategies
• IGCSE Past Papers Guide - Access free IGCSE past papers and exam resources

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