CH-1185
Covalent bonding
Chemistry · Secondary 4 · Medium · Covalent bonding
Diamond and graphite are both forms of carbon. Why does graphite conduct electricity but diamond does not?
- In graphite, each carbon has one delocalised electron that can move, but in diamond all four are used in bonds so none are free.
- Graphite has mobile positive ions but diamond does not.
- Diamond’s covalent bonds are weaker, so its electrons move freely and it conducts.
- Graphite is ionic while diamond is covalent, so only graphite conducts.
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