Diamond and Graphite Structures | GCSE Chemistry Practice
Diamond and graphite are both made of carbon, but their structures give them very different properties.
Why is graphite soft and used in pencils?
What is Diamond and Graphite Structures | Practice?
"The way in which carbon atoms are bonded in diamond and graphite."
How many covalent bonds does each carbon atom form in diamond?
Which statement about diamond is true?
Why can graphite conduct electricity?
Carbon Allotropes
Diamond: Each carbon forms 4 bonds. Very hard. No free electrons.
Graphite: Each carbon forms 3 bonds. Layers can slide. Delocalised electrons.
Fullerenes: Hollow shapes like tubes (nanotubes) or balls (buckyballs).
Keyword: "Delocalised" electrons are why graphite and metals can conduct electricity.
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