how is graphite stable even if it had its one electron free and only three electrons form bonds.
Answers
Answer:
Each carbon atom uses three of its electrons to form simple bonds to its three close neighbors. That leaves a fourth electron in the bonding level. These "spare" electrons in each carbon atom become delocalized over the whole of the sheet of atoms in one layer
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Explanation:
In the hexagonal graphite structure the carbon atoms are sp2 hybridized, just like in benzene. In graphite, this p-orbital is used for bonding just as it is in benzene, resulting in an extended pi system in the graphite structure. Graphite is really just a large number of benzene rings annelated together to form a continuous, ring structure. Just as carbon satisfies its valence requirement of 4 in benzene (3 sigma bonds and 1 pi bond), carbon's valency requirements are satisfied the same way in graphite.