Chemistry·Matter · Bonding · NSSCO 2.4.4–2.4.5
Giant structures & metallic bonding
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Some substances aren't tiny molecules — they're giant structures of millions of atoms. Learn why diamond is the hardest thing known while graphite is soft and conducts, why sand melts at over 1600 °C, and how a 'sea' of delocalised electrons gives metals their special properties.
What you'll learn in this lesson
By the end you should be able to (NSSCO Chemistry 2.4.4–2.4.5):
- Describe giant covalent structures: diamond, graphite and silicon(IV) oxide
- Relate the properties of diamond and graphite to their structures
- Describe metallic bonding as a lattice of positive ions in a sea of delocalised electrons
- Explain the properties of metals (conductivity, malleability, high melting points) from their structure
- Recognise that the same element can form different structures (allotropes) with different properties
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