Metallic Bonding (Cambridge (CIE) A Level Chemistry): Flashcards
Exam code: 9701
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Define metallic bonding.
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Define metallic bonding.
Metallic bonding is the strong electrostatic attraction between a lattice of positive metal ions and a surrounding sea of mobile delocalised electrons.
What happens to the outer electrons of metal atoms when they pack together to form a metallic lattice?
The outer electrons delocalise, becoming free to move throughout the structure. They are no longer associated with any single atom, forming a mobile 'sea' of electrons surrounding the positive metal ions.
True or False?
In metallic bonding, the metal atoms remain neutral and do not form ions.
False.
When outer electrons delocalise, the metal atoms become positive ions (cations). The structure consists of a lattice of these cations surrounded by delocalised electrons.
Metallic bonding holds the positive metal ions in place and counteracts the .......... between them, maintaining the .......... of the metal structure.
Metallic bonding holds the positive metal ions in place and counteracts the repulsion between them, maintaining the stability of the metal structure.
Describe the arrangement of particles in a metallic lattice.
Metal atoms are arranged in a regular, tightly packed lattice. Delocalisation of outer electrons produces a lattice of positive metal ions surrounded by a mobile sea of delocalised electrons.
True or False?
The delocalised electrons in metallic bonding are fixed to specific metal ions.
False.
Delocalised electrons are free to move throughout the entire metallic lattice and are not associated with any single ion.
In a metal, delocalised electrons form a mobile '..........' that surrounds the .......... metal ions in the lattice.
In a metal, delocalised electrons form a mobile 'sea' that surrounds the positive metal ions in the lattice.
Define delocalised electrons.
Delocalised electrons are electrons that are not associated with any single atom or bond but are free to move throughout a structure, as seen in metals and some covalent molecules.
Why is metallic bonding described as strong?
Metallic bonding is strong because the electrostatic attraction between the lattice of positive metal ions and the surrounding delocalised electrons acts in all directions and requires a large amount of energy to overcome.
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