Allotropes Of Carbon
Among the allotropes of carbon, which one conducts electricity due to the presence of delocalised electrons in its layered structure?
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About This Question
- Subject
- chemistry
- Chapter
- p-block elements
- Topic
- allotropes of carbon
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
Graphite
Allotropes are different structural forms of the same element, and their properties depend on how the atoms are bonded. In graphite, each carbon atom is sp^2 hybridised and bonded to three others within flat hexagonal layers, leaving one electron per atom delocalised over the layer. These delocalised electrons are free to move along the layers, so graphite conducts electricity, making it useful as an electrode. Diamond, by contrast, has each carbon sp^3 hybridised and bonded to four others in a rigid three-dimensional network with no free electrons, so it is an electrical insulator. Fullerene conducts only under special conditions and is not the standard conducting allotrope. Amorphous carbon lacks the ordered conducting layers of graphite. The structure-property relationship of carbon allotropes is a standard NCERT topic. Plausibility check: graphite is used in electrodes and as a lubricant precisely because of its mobile delocalised electrons and layered slipping planes, confirming its conductivity.
This easy difficulty chemistry question is from the chapter p-block elements, covering the topic of allotropes of carbon. It appeared in the 2025 exam.
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