Carbon–oxygen bond
Chemical bond
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Through Chemical polarity, Atom and Carbon
Bonding motifs
Bonding at oxygen
In ethers, oxygen forms two covalent single bonds with two carbon atoms, C–O–C, whereas in alcohols oxygen forms one single bond with carbon and one with hydrogen, C–O–H. In most organic carbonyl compounds, oxygen forms a covalent double bond with carbon, C=O, known as a carbonyl group. In ethers, alcohols and carbonyl compounds, the four nonbonding electrons in oxygen's outer shell are nonbonding. In alkoxides, oxygen forms a single bond with carbon and accepts an electron from a metal to form an alkoxide anion, R–O−, with three lone pairs. In oxonium ions, one of oxygen's two lone pairs is used to form a third covalent bond which generates a cation, >O+– or =O+– or ≡O+, with one lone pair remaining. In carbon monoxide and acylium ions, oxygen forms a triple bond to carbon.
Bonding at carbon
A carbon atom forms one single bond to oxygen in alcohols, ethers, and peroxides, two in acetals, three in ortho esters, and four in orthocarbonates. Carbon forms a double bond to oxygen in aldehydes, ketones and acyl halides. In carboxylic acids, esters and anhydrides, each carbonyl carbon atom forms one double bond and one single bond to oxygen. In carbonate esters and carbonic acid, the carbonyl carbon forms one double bond and two single bonds to oxygen. The bonding in carbon dioxide is often described as consisting of two C=O double bonds, although in such delocalized systems, bond order is less distinct. As mentioned above, carbon forms triple bonds to oxygen in carbon monoxide and its derivatives, which includes acylium ions and metal carbonyls.
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Electronegativities and bond lengths
The C–O bond is polarized towards oxygen (electronegativity of C vs O, 2.55 vs 3.44). Bond lengths for paraffinic C–O bonds are in the range of 143 pm – less than those of C–N or C–C bonds. Shortened single bonds are found with carboxylic acids (136 pm) due to partial double bond character and elongated bonds are found in epoxides (147 pm). The C–O bond strength is also larger than C–N or C–C. For example, bond strengths are 91 kilocalories (380 kJ)/mol (at 298 K) in methanol, 87 kilocalories (360 kJ)/mol in methylamine, and 88 kilocalories (370 kJ)/mol in ethane.
Carbon and oxygen form terminal double bonds in functional groups collectively known as carbonyl compounds to which belong such compounds as ketones, esters, carboxylic acids and many more. Internal C=O bonds are found in positively charged oxonium ions. In furans, the oxygen atom contributes to pi-electron delocalization via its filled p-orbital and hence furans are aromatic. Bond lengths of C=O bonds are around 123 pm in carbonyl compounds. The C=O bond length in carbon dioxide is 116 pm. The C=O bonds in acyl halides have partial triple bond character and are consequently very short: 117 pm. Compounds with formal C≡O triple bonds do not exist except for carbon monoxide, which has a very short, strong bond (112.8 pm), and acylium ions, R–C≡O+ (typically 110–112 pm). Such triple bonds have a very high bond energy, even higher than N≡N triple bonds. Oxygen can also be trivalent, for example in triethyloxonium tetrafluoroborate.
Chemistry
Carbon–oxygen bond forming reactions are numerous. Prominent is the Williamson ether synthesis and many oxidations.
Functional groups with C-O bonds
Carbon–oxygen bonds are present in these functional groups: