Exam code: 5070
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2.7 Metallic Bonding
Which statement correctly describes the bonding in metals?
A lattice of negative ions in a “sea of electrons”.
A lattice of positive ions in a “sea of electrons”.
A lattice of neutral atoms with delocalised electrons.
A lattice of positive ions in which each electron stays with its own ion.
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Which row provides a correct description of metals?
conducts electricity | malleable | contains delocalised electrons | |
A | |||
B | |||
C | |||
D |
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Metals are malleable and ductile and can be hammered and pulled into useful shapes.
Which statement correctly explains these properties?
Layers of atoms in the metal lattice are rigid and held strongly together so they cannot move.
Layers of atoms in a metal can slide over one another and break the attractive forces that hold them together.
Layers of atoms in a metal can slide over one another and the attractive forces between the metal ions and the delocalised electrons are not broken.
Layers of atoms in a metal cannot slide over one another and the attractive forces between the metal ions and the delocalised electrons are unbreakable.
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Metallic bonds are very strong and give metals their properties. Which of the following definitions is correct for a metallic bond?
A metallic bond is formed by the electrostatic attraction that occurs due to electron transfer between metal atoms.
A metallic bond is formed by the electrostatic attraction between the positive ions and the delocalised electrons.
A metallic bond is formed by the electrostatic attraction that occurs due to the uneven sharing of electrons between metal atoms.
A metallic bond is formed by the intermolecular forces between the positive metal ions and the delocalised electrons.
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