Metallic Bonding — GCSE Chemistry Revision
Revise Metallic Bonding for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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Go to States of Matter & BondingWhat is Metallic Bonding?
Metallic bonding is the force of attraction between the positive metal ions and the delocalised electrons in a metal lattice. The outer shell electrons of the metal atoms are free to move throughout the structure, creating a 'sea' of delocalised electrons.
Board notes: Metallic bonding is the third main type of bonding you need to know. All boards will test your ability to describe the model and use it to explain the characteristic properties of metals.
Step-by-step explanationWorked example
In a piece of copper, the copper atoms lose their outer electrons, which become delocalised. This leaves a lattice of positive copper ions (Cu²⁺) surrounded by a sea of mobile electrons. The attraction between the ions and electrons holds the structure together.
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Common mistakes
- 1Describing metallic bonding as a bond between individual atoms rather than a lattice of positive ions and delocalised electrons.
- 2Forgetting that the 'ions' in a metal are positive because they have lost their outer electrons.
- 3Not being able to use the model of metallic bonding to explain the properties of metals, such as conductivity and malleability.
Metallic Bonding exam questions
Exam-style questions for Metallic Bonding with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Metallic Bonding
Core concept
Metallic bonding is the force of attraction between the positive metal ions and the delocalised electrons in a metal lattice. The outer shell electrons of the metal atoms are free to move throughout t…
Frequently asked questions
Why are metals good conductors of electricity?
The delocalised electrons in the metallic lattice are free to move and carry an electrical current when a voltage is applied.
Why are metals malleable?
The layers of positive ions in a metal can slide over each other without breaking the metallic bond. This allows the metal to be bent and shaped without shattering.