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.
Why Metals Are Malleable: The IB Explanation
1. Layers of ions can slide without breaking bonds
Metals consist of regular, closely packed layers of positive ions.
When force is applied, these layers can shift or slide over each other.
Because metallic bonding does not rely on fixed directional bonds, the structure remains intact.
2. The “sea of electrons” adapts easily
The delocalized electrons move freely and continuously adjust to new positions of the ions, maintaining attraction throughout the structure.
This prevents the lattice from shattering.
3. Metallic bonding does not resist deformation
Unlike ionic compounds, metals do not have alternating positive and negative ions.
There is no strong repulsion when layers move, so deformation does not cause the structure to fracture.
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Why Ionic and Covalent Solids Are Not Malleable
IB Chemistry often contrasts metals with ionic and covalent lattices:
- Ionic compounds shatter when layers shift because like charges align and repel strongly.
- Giant covalent structures resist deformation because bonds are strong and directional.
This comparison helps students write full-marks explanations on Paper 2.
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Applications of Malleability
Understanding malleability helps explain why metals are used in:
- wiring
- jewelry
- machinery
- structural frameworks
- packaging (e.g., aluminum foil)
The property allows metals to be shaped without breaking — supporting industrial and chemical applications. Metals remain essential in fields that combine chemistry with environmental sciences, which relates to decision-making in subject selection such as:
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Frequently Asked Questions
1. Why are some metals more malleable than others?
Metals with more delocalized electrons and more flexible lattice structures are more malleable. For example, copper and gold have highly mobile electrons and allow easier shifting of layers. IB Chemistry does not require you to memorize specific metal rankings but does expect you to connect malleability to electron mobility and lattice structure.
2. How is malleability related to ductility?
Both malleability and ductility arise from metallic bonding. Malleability refers to flattening into sheets, while ductility refers to being drawn into wires. Both properties depend on the ability of ions to move without the structure breaking. IB questions often pair these definitions to test bonding understanding.
3. Does alloying affect malleability?
Yes. Adding different metal atoms disrupts the regular arrangement of ions, making it harder for layers to slide. Alloys such as steel or bronze are generally less malleable but often stronger. This makes them useful for construction and engineering. IB Chemistry expects you to know how alloying changes metallic properties.
Conclusion
Metals are malleable because their positive ions exist in layers that can slide over one another, while delocalized electrons maintain the attraction throughout the structure. Metallic bonds do not break during deformation because they are non-directional and flexible. Mastering this explanation is essential for bonding, materials, and periodicity questions in IB Chemistry. With RevisionDojo’s structured guides and chemistry-specific support, you can develop deeper understanding and stronger exam performance.
