Carbene

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Not to be confused with carbine.

In chemistry, a carbene is a highly reactive organic molecule with a divalent carbon atom with only six valence electrons and the general formula: R₁R₂C: ^[1]. The carbene comes in two varieties - a singlet and triplet. The singlet type has its carbon atom sp² hybridised with an empty p-orbital extending above and below a plane containing R₁ and R₂ and the free electron pair. Typically these molecules are very short lived, although persistent carbenes are now known.

The parent carbene is H₂C: also called methylene. An often encountered carbene is Cl₂C: or dichlorocarbene which can be generated in situ from chloroform and a strong base.

Contents 1 Structure 2 Reactivity 3 Carbenes and carbene ligands in Organometallic chemistry 4 Generation of Carbenes 5 See also 6 References

[edit] Structure

Generally there are two types of carbenes; singlet or triplet carbenes. Singlet carbenes have a pair of electrons and sp² hybrid structure. Triplet carbenes have two unpaired electrons. They may be either sp² hybrid or linear sp hybrid. Most carbenes have nonlinear triplet ground state with the exception of carbenes with nitrogen, oxygen, sulfur atoms, and dihalocarbenes.

Singlet and triplet carbenes are named so because of the electronic spins they possess. Triplet carbenes are paramagnetic and may be observed by electron spin resonance spectroscopy if they can exist long enough without undergoing further reactions. The total spin of singlet carbenes is zero while that of triplet carbenes is one (in units of ). For simple hydrocarbons, triplet carbenes usually have energies 8 kcal/mole (33 kJ/mol) lower than singlet carbenes (see also Hund's rule of Maximum Multiplicity), thus, in general, triplet is the more stable state (the ground state) and singlet is the excited state species. Substituents that can donate electron pairs may stabilize singlet state by delocalizing the pair into empty p-orbital. Bond angles are 125-140° for triplet methylene and 102° for singlet methylene (determined by EPR). The carbene 9-fluorenylidene has been shown to be a rapidly equilibrating mixture of singlet and triplet states with an approximately 1.1 kcal/mol (4.6 kJ/mol) energy difference ^[2]. Triplet carbenes are generally stable in gaseous state while singlet carbenes are often found in aqueous media.

[edit] Reactivity

Singlet and triplet carbenes do not demonstrate the same reactivity. Singlet carbenes generally participate in cheletropic reactions as either electrophiles or nucleophiles. Singlet carbene with its unfilled p-orbital should be electrophilic. Triplet carbenes should be considered to be diradicals, and participate in stepwise radical additions. Triplet carbenes have to go through an intermediate with two unpaired electrons whereas singlet carbene can react in a single concerted step. Addition of singlet carbenes to olefinic double bonds is more stereoselective than that of triplet carbenes. Addition reactions with alkenes can be used to determine whether the singlet or triplet carbene is involved.

Reactions of singlet methylene are stereospecific while those of triplet methylene are not. For instance the reaction of methylene generated from photolysis of diazomethane with cis-2-butene and trans-2-butene is stereospecific which proves that in this reaction methylene is a singlet ^[3].

Reactivity of a particular carbene depends on the substituent groups, preparation method, reaction conditions such as presence or absence of metals. Some of the reactions carbenes can do are insertions into C-H bonds, skeletal rearrangements, and additions to double bonds. Carbenes can be classified as nucleophilic, electrophilic, or ambiphilic. Reactivity is especially strongly influenced by substituents. For example, if a substituent is able to donate a pair of electrons, most likely carbene will not be electrophilic. Alkyl carbenes insert much more selectively than methylene, which does not differentiate between primary, secondary, and tertiary C-H bonds.

Carbenes add to double bonds to form cyclopropane. A concerted mechanism is available for singlet carbenes. Triplet carbenes do not retain stereochemistry in the product molecule. Addition reactions are commonly very fast and exothermic. The slow step in most instances is generation of carbene. A well-known reagent employed for alkene-to-cyclopropane reactions is Simmons-Smith reagent. This reagents is a system of copper, zinc, and iodine, where the active reagent is believed to be iodomethylzinc iodide. Reagent is complexed by hydroxy groups such that addition commonly happens syn to such group.

Insertions are another common type of carbene reactions. The carbene basically interposes itself into an existing bond. The order of preference is commonly: 1. X-H bonds where X is not carbon 2. C-H bond 3. C-C bond. Insertions may or may not occur in single step.

Intramolecular insertion reactions present new synthetic solutions. Generally, rigid structures favor such insertions to happen. When an intramolecular insertion is possible, no intermolecular insertions are seen. In flexible structures, five-membered ring formation is preferred to six-membered ring formation. Both inter- and intramolecular insertions are amendable to asymmetric induction by choosing chiral ligands on metal centers.

Alkylidene carbenes are alluring in that they offer formation of cyclopentene moieties. To generate an alkylidene carbene a ketone can be exposed to trimethylsilyl diazomethane.

[edit] Carbenes and carbene ligands in Organometallic chemistry

Carbenes can be stabilized as organometallic species. These transition metal carbene complexes fall into three categories, with the first two being the most clearly defined:

• Fischer carbenes, in which the carbene is tethered to a metal that bears an electron-withdrawing group (usually a carbonyl).
• Schrock carbenes, in which the carbene is tethered to a metal that bears an electron-donating group.
• Persistent carbenes, including the class of N-heterocyclic carbenes (NHCs). These are often are used as ancillary ligands in organometallic chemistry.

[edit] Generation of Carbenes

• Most commonly, photolytic, thermal, or transition metal catalyzed decomposition of diazoalkanes is used to create carbene molecules. A variation on catalyzed decomposition of diazoalkanes is the Bamford-Stevens reaction, which gives carbenes in aprotic solvents and carbenium ions in protic solvents.
• Another method is induced elimination of halogen from gem-dihalides or HX from CHX₃ moiety, employing organolithium reagents (or another strong base). It is not certain that in these reactions actual free carbenes are formed. In some cases there is evidence that completely free carbene is never present. It is likely that instead a metal-carbene complex forms. Nevertheless, these metallocarbenes (or carbenoids) give the expected products.

Carbene preparation

• Photolysis of diazarines and epoxides can also be employed. Diazarines contain 3-membered rings and are cyclic forms or diazoalkanes. The strain of the small ring makes photoexcitation easy. Photolysis of epoxides gives carbonyl compounds as side products. With asymmetric epoxides, two different carbonyl compounds can potentially form. The nature of substituents usually favors formation of one over the other. One of the C-O bonds will have a greater double bond character and thus will be stronger and less likely to break. Resonance structures can be drawn to determine which part will contribute more to the formation of carbonyl. When one substituent is alkyl and another aryl, the aryl-substituted carbon is usually released as a carbene fragment.
• Thermolysis of alpha-halomercury compounds is another method to generate carbenes.
• Rhodium and copper complexes promote carbene formation.
• Carbenes are intermediates in the Wolff rearrangement

[edit] See also

Transition metal carbene complex

[edit] References

1. ^ Organic Chemistry R.T Morrison, R.N Boyd pp 473-478
2. ^ Chemical and Physical Properties of Fluorenylidene: Equilibrium of the Singlet and Triplet Carbenes Peter B. Grasse, Beth-Ellen Brauer, Joseph J. Zupancic, Kenneth J. Kaufmann, Gary B. Schuster; J. Am. Chem. Soc.; 1983; 105; 6833-6845.
3. ^ Structure of Carbene CH2 Philip S. Skell, Robert C. Woodworth; J. Am. Chem. Soc.; 1956; 78(17); 4496-4497. Abstract