Metallic bonding Cambridge IGCSE Co-ordinated Sciences (9–1) revision
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In plain words
In a metal, the atoms let go of their outer electrons. What's left is a regular stack of positive ions sitting in a sea of loose electrons that wander through the whole piece. The attraction between the ions and that sea is what holds a metal together.
Three things to know
- A metal is a giant lattice of positive ions in a 'sea' of delocalised electrons. Metallic bonding is the attraction between the two.
- Metals conduct electricity and heat because the delocalised electrons are free to move through the structure.
- Metals are malleable (can be hammered into shape) and ductile (can be drawn into wires) because the layers of ions can slide without the bonding breaking.
Tips and tricks
- Conducts electricity: "delocalised electrons are free to move". Malleable: "the layers of ions can slide over each other". Learn the two sentences as a pair.
- In a metal it's the electrons that carry the current, not the ions.
It lands in your notebook with its questions as flashcards.
Metallic bonding: 5 questions and answers
These are the quiz’s questions. Do the quiz first, then come back here for the ones that got you.
What moves when a metal conducts electricity?
The ions stay where they are; the electrons flow.
Metallic bonding is the attraction between which two things?
The outer electrons leave their atoms and are shared by the whole structure.
What does malleable mean?
Ductile is the word for being drawn into wires.
Why are metals malleable?
The bonding is not broken when the layers move.
Why do most metals have high melting points?
A lot of energy is needed to overcome metallic bonding.
Quiz
5 questions
Tap an answer and you’ll see straight away whether it’s right, and why.
Worksheet
3 questions, 6 marks. Write your answers on paper, then check them.
Metallic bonding
Cambridge IGCSE Co-ordinated Sciences (9–1) 0973 · 6 marks · papermunch.org
Name ______________________________ Date ______________
Describe metallic bonding.[2]
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The electrostatic attraction between positive metal ions in a giant lattice and the delocalised electrons around them.
Explain why metals conduct electricity.[2]
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The delocalised electrons are free to move through the metal and carry charge.
Explain why metals are malleable.[2]
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The layers of ions can slide over each other, and the delocalised electrons keep holding them together.
Answers: Metallic bonding
- 1. The electrostatic attraction between positive metal ions in a giant lattice and the delocalised electrons around them.
- 2. The delocalised electrons are free to move through the metal and carry charge.
- 3. The layers of ions can slide over each other, and the delocalised electrons keep holding them together.