Metallic structures and bonding
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Some exam "Dos and Don'ts": Metallic bonding
Some advice on answering questions on topics often highlighted by examiners as being poorly answered in the past. Make sure that the detail covered by the question is included in your syllabus specification.
Metallic bonding is usually strong, hence the high melting points of most metals. It arises from the attraction between the delocalised (mobile) outer shell electrons of the metal atoms and the metal 'ions' that remain. When asked to compare two metals, e.g. Na vs Mg, remember that the strength of the bonding depends in the first instance on the size of the metal 'ions' and the number of outer electrons.
Electrical conduction in metals is by the FLOW of mobile (delocalised) electrons through the metal - just saying it is due to mobile electrons may not always get the mark. It is also NOT by ions moving.
Metals are malleable because the bonding is non-directional (i.e. no fixed bonds) and the atoms can move relative to one another without breaking the bonding.
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updated: 01 June 2007
