Malleability — the ability of a metal to be hammered or pressed into sheets without breaking — is one of the defining properties of metals. In IB Chemistry, this concept appears in bonding, materials science, periodicity, and structure questions. Many students memorize the property but struggle to clearly explain why metals behave this way. This guide breaks down the metallic bonding model and shows you exactly how to express the explanation in IB-ready language.
Quick Start Checklist
Metals are malleable because:
- Their atoms are arranged in layers.
- These layers can slide over one another.
- Metallic bonding is non-directional.
- Positive ions are held together by a sea of delocalized electrons.
- Slipping layers does not break the metallic bond.
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The Metallic Bonding Model
In metals:
- Atoms lose control of some valence electrons.
- These electrons become delocalized, forming an electron sea.
- Metal atoms become positive ions packed into a lattice.
- The delocalized electrons move freely and hold the ions together.
Unlike covalent bonds, metallic bonds are non-directional, meaning the attraction exists in all directions around each ion. This is the foundation for understanding malleability.
