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BONDING IN CARBONYL COMPOUNDS | ||
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Important! Don't try to read this unless you are sure that you fully understand the orbital view of the bonding in methane and the bonding in ethene. You may also find it useful to read the article on orbitals if you aren't sure about simple orbital theory. | ||
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The carbonyl group The simple view of the bonding in carbon - oxygen double bonds 
Where the carbon-oxygen double bond, C=O, occurs in organic compounds it is called a carbonyl group. The simplest compound containing this group is methanal. We are going to look at the bonding in methanal, but it would equally apply to any other compound containing C=O. The interesting thing is the nature of the carbon-oxygen double bond - not what it's attached to. | ||
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Note: Methanal is normally written as HCHO. If you wrote it as HCOH, it looks as if it contains an -O-H group - and it doesn't. Methanal is an aldehyde. All aldehydes contain the CHO group. Naming: methanal: meth counts 1 carbon atom, an means no C=C, al says that it is an aldehyde and so contains CHO. | ||
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An orbital view of the bonding in carbon - oxygen double bonds The carbon atom Just as in ethene or benzene, the carbon atom is joined to three other atoms. The carbon's electrons rearrange themselves, and promotion and hybridisation give sp2 hybrid orbitals. Promotion gives:
Hybridisation of the 2s orbital and two of the 2p orbitals means that the carbon atom now looks like the diagram on the right. Three sp2 hybrid orbitals are formed and these arrange themselves as far apart in space as they can - at 120° to each other. The remaining p orbital is at right angles to them. This is exactly the same as in ethene or in benzene. | ||
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Important! If this isn't really clear to you, you must go and read the article about the bonding in ethene. | ||
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The oxygen atom Oxygen's electronic structure is 1s22s22px22py12pz1. The 1s electrons are too deep inside the atom to be concerned with the bonding and so we'll ignore them from now on. Hybridisation occurs in the oxygen as well. It is easier to see this using "electrons-in-boxes".
This time two of the sp2 hybrid orbitals contain lone pairs of electrons. | ||
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Help! A "lone pair" of electrons is a pair of electrons at the bonding level which isn't being used to bond on to another atom. | ||
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The carbon atom and oxygen atom then bond in much the same way as the two carbons do in ethene. In the next diagram, we are assuming that the carbon will also bond to two hydrogens to make methanal - but it could equally well bond to anything else.
End-to-end overlap between the atomic orbitals that are pointing towards each other produce sigma bonds. Notice that the p orbitals are overlapping sideways.
This sideways overlap produces a pi bond. So just like C=C, C=O is made up of a sigma bond and a pi bond. Does that mean that the bonding is exactly the same as in ethene? No! The distribution of electrons in the pi bond is heavily distorted towards the oxygen end of the bond, because oxygen is much more electronegative than carbon. | ||
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Help! You can read about the origins of electronegativity and its effects in organic compounds in a separate article. | ||
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This distortion in the pi bond causes major differences in the reactions of compounds containing carbon-oxygen double bonds like methanal compared with compounds containing carbon-carbon double bonds like ethene. | ||
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Note: You can read about addition reactions or addition-elimination reactions of carbonyl compounds elswhere on this site. | ||
 © Jim Clark 2000 (modified March 2013) |
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