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It is generally considered the average length for a carbon–carbon single bond, but is also the largest bond length that exists for ordinary carbon covalent bonds. Since one atomic unit of length (i.e., a Bohr radius) is 52.9177 pm, the C–C bond length is 2.91 atomic units, or approximately three Bohr radii long.
Molecular geometries can be specified in terms of 'bond lengths', 'bond angles' and 'torsional angles'. The bond length is defined to be the average distance between the nuclei of two atoms bonded together in any given molecule. A bond angle is the angle formed between three atoms across at least two bonds.
96 pm – H–O bond length in a water molecule; 100 picometers. To help compare different orders of magnitude this section lists lengths between 10 −10 and 10 −9 ...
Rotational spectroscopy can also give extremely accurate values of bond lengths. For homonuclear A–A bonds, Linus Pauling took the covalent radius to be half the single-bond length in the element, e.g. R(H–H, in H 2) = 74.14 pm so r cov (H) = 37.07 pm: in practice, it is usual to obtain an average value from a variety of covalent compounds ...
Starting with Pauling in 1947 [12] a correlation between cation–anion bond length and bond strength was noted. It was shown later [13] that if bond lengths were included in the calculation of bond strength, its accuracy was improved, and this revised method of calculation was termed the bond valence. These new insights were developed by later ...
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with C═O 1600 strong C═C (both sp 2) any 1640–1680 medium aromatic C═C any 1450 weak to strong (usually 3 or 4) 1500 1580 1600 C≡C terminal alkynes 2100–2140 weak disubst. alkynes 2190–2260 very weak (often indistinguishable) C=O aldehyde/ketone saturated aliph./cyclic 6-membered 1720 α,β-unsaturated 1685 aromatic ketones 1685
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