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title: "Diamond and graphite are two allotropes of carbon that are covalent network solids. While diamond is an electrical insulator, graphite is an electrical conductor. Which of the following correctly identifies the hybridization of the carbon atoms in graphite and describes the mechanism of its electrical conductivity?"
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date_modified: "2026-08-21T08:18:19+00:00"
---

# Diamond and graphite are two allotropes of carbon that are covalent network solids. While diamond is an electrical insulator, graphite is an electrical conductor. Which of the following correctly identifies the hybridization of the carbon atoms in graphite and describes the mechanism of its electrical conductivity?

Diamond and graphite are two allotropes of carbon that are covalent network solids. While diamond is an electrical insulator, graphite is an electrical conductor. Which of the following correctly identifies the hybridization of the carbon atoms in graphite and describes the mechanism of its electrical conductivity?

- **A.** \(sp^3\) ; conducts electricity due to delocalized \(\pi\) electrons
- **B.** \(sp^2\) ; conducts electricity due to delocalized \(\pi\) electrons
- **C.** \(sp^3\) ; does not conduct electricity because all valence electrons are localized in \(\sigma\) bonds
- **D.** \(sp^2\) ; does not conduct electricity because all valence electrons are localized in \(\sigma\) bonds

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