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Bonding - Metallic
Metals have many uses.

Bonding - Metallic

Metallic bonding explains why metals conduct, bend and stretch. Revise delocalised electrons, ion layers and how structure links to properties like melting point, strength and conductivity.

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Fascinating Fact:

Metals are malleable and ductile because layers of ions can slide over each other. The delocalised electrons keep the bonding in place as the layers move.

In GCSE Chemistry, metallic bonding is modelled as positive metal ions held together by a shared “sea” of delocalised electrons. This helps you explain conduction, why many metals have high melting points, and how alloys can be harder than pure metals.

Key Terms

  • Delocalised electrons: Electrons that are not tied to one atom and can move through the metal structure.
  • Metallic lattice: A regular arrangement of positive metal ions surrounded by mobile electrons.
  • Alloy: A mixture of a metal with other elements, designed to change properties such as strength or hardness.

Frequently Asked Questions (Click to see answers)

What is metallic bonding in GCSE Chemistry?

Metallic bonding is the attraction between positive metal ions and delocalised electrons in a metal. The electrons move through the structure, holding the ions together.

Why do metals conduct electricity as solids?

Metals conduct electricity because delocalised electrons are free to move through the lattice. When a voltage is applied, these electrons carry charge through the metal.

Why are metals malleable and ductile?

Metals are malleable and ductile because the ions can shift position without the bonding breaking. The mobile electrons keep attracting the ions, so the structure stays joined as it changes shape.

Try These Related Quizzes

1 .
What does malleable mean?
Can be stretched into wires
Can be bent or hammered into shape
Is easily shattered
Is shiny
Most metals are malleable
2 .
Pick the correct statement about the arrangement of particles in a metal.
The particles are arranged randomly and far apart
The particles are arranged regularly and far apart
The particles are arranged regularly and close together
The particles are arranged randomly and close together
Metals usually have higher densities than non-metals because the particles are so closely packed together
3 .
One drawback of superconductors is...
their behaviour is erratic
they only work at VERY low temperatures
they could enable super fast transmission of electricity
they could enable loss free power transmission
To put metals into a superconducting state, extremely low temperatures close to absolute zero are required. If it becomes possible to make superconductors that work at temperatures above 0oC it would really change the world
4 .
Why do metals conduct electricity?
The positive metal ions are free to move
The negative electrons are free to move
All the constituent parts can move through the metal
The positive protons are free to move
The electrons that make up the 'sea' of delocalised electrons are free to move. This allows conduction of both heat and electricity
5 .
Metals are malleable because...
a large amount of energy is required to slide one layer of electrons over another
little energy is required to slide one layer of electrons over another
little energy is required to slide one layer of ions over another layer
a huge amount of energy is required to slide one layer of ions over another layer
You can immediately dismiss the first two options because they are talking about layers of electrons. In metallic bonding, it is the metal ions that are in layers, the electrons are randomly arranged
6 .
Metals have...
low melting points because they have weak bonds
low melting points because they have strong bonds
high melting points because they have weak bonds
high melting points because they have strong bonds
The strong bonds make it more difficult for the particles to move further apart - requiring more energy - raising the melting point. There are exceptions and the metal mercury is already molten at room temperature
7 .
The bonding in metals is due to a strong attraction between...
positive metal ions and a sea of negative electrons
positive metal atoms and a sea of negative electrons
negative metal atoms and a sea of positive electrons
negative metal ions and a sea of negative electrons
Remember that opposites attract
8 .
Superconductors...
work at any temperature
conduct heat better than other materials
have little or no resistance
conduct an orchestra really well
In conductors, electrical energy is lost because of the heating effect caused by resistance. In a superconductor, hardly any electrical energy is lost making electricity transmission much more efficient
9 .
If a potential difference is applied to a metal...
the fixed electrons will stay in place and no current will pass through the metal
the negative ions will move through the metal carrying the electrical current
the delocalised ions will move through the metal carrying the electrical current
the delocalised electrons will move through the metal carrying the electrical current
They are attracted to the positive pole. As they leave the metal, fresh electrons are added via the negative pole
10 .
What type of bonding is present in metals?
Covalent
Ionic
Hydrogen
Metallic
The majority of elements have this type of bonding
You can find more about this topic by visiting BBC Bitesize - Metals and alloys

Author:  Kate Gardiner (Chemistry Educator & GCSE Quiz Writer)
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