Abstract
Carbon occurs in several allotropic forms, i.e., isomers with different bonds between the carbon atoms. In diamond (ρ = 3.51 g/cm3), all atoms are equidistant from each other, 0.154 nm, and are bonded together in the form of a tetrahedron (Figure 25-1). Diamond is thus the basic structure of aliphatic hydrocarbons. In graphite (ρ = 2.22 g/cm3) the carbon atoms all lie in a plane. The distance between the planar atoms is 0.1415 nm, while the interlayer or interplanar distance is 0.335 nm, corresponding roughly to the sum of the van der Waals radii for carbon. Because of this great distance between layers, they can easily be displaced from one another. Because of the delocalized electronic system within each layer, graphite is the basic structure in the benzene series.
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Elias, HG. (1984). Carbon Chains. In: Macromolecules. Springer, Boston, MA. https://doi.org/10.1007/978-1-4899-2809-2_11
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