Table of Contents
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What is Metallic Bonding? Definition & Basics
Metallic bonding is the electrostatic attraction between positive metal ions and a 'sea' of delocalized electrons. This unique bonding occurs in pure metals and alloys.
Exam-Centered Definition:
"Metallic bonding is the strong electrostatic force of attraction between positive metal ions arranged in a lattice and the delocalized electrons that move freely throughout the structure."
Electron Sea Model of Metallic Bonding
The electron sea model describes how metal atoms lose their outer electrons to form positive ions, while the valence electrons become delocalized and move freely throughout the entire metallic structure.
Key Points to Remember:
- Metal atoms become positive ions (cations)
- Valence electrons become delocalized
- Electrons move freely throughout the structure
- Strong electrostatic attraction maintains the bond
Master Related Concepts:
Strengthen your foundation with our Periodic Table Master Guide and Ionic Bonding Complete Notes.
Properties of Metallic Bonding & Their Explanations
| Property | Explanation | Example |
|---|---|---|
| High Electrical Conductivity | Delocalized electrons can move freely and carry electric current | Copper wires in electrical circuits |
| High Thermal Conductivity | Free electrons transfer kinetic energy efficiently | Aluminum cookware |
| Malleability & Ductility | Layers of ions can slide over each other without breaking bonds | Gold beaten into thin sheets |
| High Melting & Boiling Points | Strong electrostatic forces require substantial energy to break | Tungsten in light bulb filaments |
Metallic vs Ionic & Covalent Bonding
| Aspect | Metallic Bonding | Ionic Bonding | Covalent Bonding |
|---|---|---|---|
| Particles Involved | Positive ions + delocalized electrons | Positive and negative ions | Atoms sharing electron pairs |
| Electrical Conductivity | Good conductor (solid & liquid) | Poor conductor (solid), good (liquid) | Poor conductor |
| Melting/Boiling Point | Generally high | High | Variable |
| Solubility in Water | Insoluble | Generally soluble | Variable |
Factors Affecting Metallic Bond Strength
1. Number of Delocalized Electrons
More delocalized electrons per atom = stronger bonding
Example: Aluminum (3 valence electrons) has stronger bonding than Sodium (1 valence electron)
2. Size of Metal Ions
Smaller ions = stronger bonding (electrons closer to nucleus)
Example: Magnesium has stronger bonding than Calcium
3. Charge Density
Higher charge density = stronger electrostatic attraction
Example: Transition metals have strong metallic bonding
Exam-Focused Practice Questions
Question 1: Describe metallic bonding (2 marks)
Model Answer: Metallic bonding is the electrostatic attraction between positive metal ions arranged in a lattice and a sea of delocalized electrons.
Question 2: Explain why metals conduct electricity (3 marks)
Model Answer: Metals contain delocalized electrons that are free to move throughout the structure. When a potential difference is applied, these electrons drift in one direction, carrying electrical charge and enabling conduction.
Solved Past Papers - Metallic Bonding Questions
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