Diamond vs Graphite Battle
Compare structures, hardness, and conductivity of carbon forms
What this lesson covers
Why it matters
Diamond is the hardest natural substance on Earth; graphite is soft enough to leave grey marks on paper. The twist: both are pure carbon — the very same atoms.
Predict first
If both are pure carbon, why are diamond and graphite so different?
Diamond and graphite are allotropes — the same element in different atomic arrangements. Diamond is a rigid 3D network (hard, non-conducting); graphite is flat layers that slide (soft, conducts electricity).
- Their carbon atoms are arranged in different structures — correct
- Diamond contains extra, heavier atoms
- Graphite is really a compound
What you do
Both are pure carbon. Sort each property: does it belong to diamond, or to graphite?
Check yourself
Why does graphite conduct electricity but diamond does not?
Graphite's layers leave free electrons to carry current; diamond locks every electron into bonds.
Diamond and graphite are best described as…
Same element, different structures — that is what 'allotropes' means.
- Graphite has free electrons between its sliding layers — correct
- Graphite contains more carbon atoms
- Diamond is actually a metal
- allotropes of carbon — correct
- compounds of carbon
- a mixture of carbon