Define metallic bonding .

Metallic bonding is the strong electrostatic attraction between the positive metal ions in a giant metallic lattice and the surrounding 'sea' of delocalised electrons .

Why do metals conduct electricity?

Metals conduct electricity because their delocalised electrons are free to move through the giant metallic lattice and carry charge. It is the electrons, not the ions, that carry the current.

True or False? Most metals have high melting points.

True. Most metals have high melting points because of the strong electrostatic attraction between positive metal ions and the sea of delocalised electrons in the giant metallic lattice. A large amount of energy is needed to overcome these forces.

Metals are malleable because layers of ______ ions can ______ over each other without breaking the metallic bonds.

Metals are malleable because layers of positive ions can slide over each other without breaking the metallic bonds.

True or False? Molten ionic compounds and solid metals both conduct electricity using freely moving ions.

False. Molten ionic compounds conduct using freely moving ions , but solid metals conduct using freely moving delocalised electrons — not ions, which remain fixed in the metallic lattice.

In a metal, the outer shell electrons are released from the atoms, becoming ______ , and move freely throughout the ______ metallic lattice.

In a metal, the outer shell electrons are released from the atoms, becoming delocalised , and move freely throughout the giant metallic lattice.

How do the physical properties of Group I metals differ from those of most other metals?

Group I metals (such as lithium, sodium, and potassium) have low melting points , are soft , and have low densities . These properties are unusual compared to most metals, which are hard, dense, and have high melting points.

O LevelChemistryCambridge (CIE)Flashcards2. Atoms, Elements & Compounds2.7 Metallic Bonding

2.7 Metallic Bonding (Cambridge (CIE) O Level Chemistry): Flashcards

Exam code: 5070

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Define metallic bonding.

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Cards in this collection (7)

Define metallic bonding.
Metallic bonding is the strong electrostatic attraction between the positive metal ions in a giant metallic lattice and the surrounding 'sea' of delocalised electrons.
Why do metals conduct electricity?
Metals conduct electricity because their delocalised electrons are free to move through the giant metallic lattice and carry charge.
It is the electrons, not the ions, that carry the current.
True or False?
Most metals have high melting points.
True.
Most metals have high melting points because of the strong electrostatic attraction between positive metal ions and the sea of delocalised electrons in the giant metallic lattice. A large amount of energy is needed to overcome these forces.
Metals are malleable because layers of ______ ions can ______ over each other without breaking the metallic bonds.
Metals are malleable because layers of positive ions can slide over each other without breaking the metallic bonds.
True or False?
Molten ionic compounds and solid metals both conduct electricity using freely moving ions.
False.
Molten ionic compounds conduct using freely moving ions, but solid metals conduct using freely moving delocalised electrons — not ions, which remain fixed in the metallic lattice.
In a metal, the outer shell electrons are released from the atoms, becoming ______, and move freely throughout the ______ metallic lattice.
In a metal, the outer shell electrons are released from the atoms, becoming delocalised, and move freely throughout the giant metallic lattice.
How do the physical properties of Group I metals differ from those of most other metals?
Group I metals (such as lithium, sodium, and potassium) have low melting points, are soft, and have low densities. These properties are unusual compared to most metals, which are hard, dense, and have high melting points.

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