A carbon-carbon bond is a covalent bond between two carbon atoms. The most common form of this bond is the single bond - a link involving two electrons: one of each of the carbon atoms. In itself, the carbon-carbon bond is very strong: the binding energy is 347 kJ / mol. Also, the favorable overlap of the orbital (both sigma and pi bond) allows carbon to form long carbon chains. These form the basis of organic compounds.
The single C-C bond is a sigma bond, which is described as the combination of one hybridized orbital of each of the two carbon atoms. In ethane, hybridization is sp, but some bonds are also possible based on other hybridizations (e.g. sp with sp). Equal hybridization is not a condition.
Carbon atoms can also form double bonds, such as in olefins or triplicates as in the alkynes.
A double bond is made up of a sp-hybridized orbital and a p-orbital that does not participate in hybridization. A triple bond is created by sp-hybridization and two p-orbitals of each binding-participating atom. The p-orbital gives rise to a pi binding.
Branching is a common phenomenon in the carbon skeletons of organic compounds. Different carbon atoms can be named based on the number of other carbon atoms associated with it: synthesis
Comments forming new carbon-carbon bonds are among the most important reactions in organic chemistry. They are crucial steps in the synthesis of drugs and plastics.
Some examples of reactions with which carbon-carbon bonds can be formed are: Aldol reactions, dielsalder reactions, the addition of Grignard reagents to carbonyl groups, the Heck reaction, the Michael addition and the Wittig reaction. Navigation
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