Alkene

The chemical structure of ethylene, the simplest alkene.

An alkene, olefin, or olefine, in organic chemistry is an unsaturated hydrocarbon containing at least one carbon to carbon double bond. The simplest alkenes, with only one double bond, form a homologous series with general formula C_nH_2n.

The simplest alkene is ethylene (C₂H₄), which has the International Union of Pure and Applied Chemistry (IUPAC) name ethene. Alkenes are also called olefins (an archaic synonym, widely used in the petrochemical industry) or vinyl compounds.

Contents

1 Structure of Alkenes

1.1 Shape of alkenes
1.2 Molecular geometry

2 Physical properties
3 Chemical properties
4 Synthesis
5 Reactions

5.1 Addition reactions
5.2 Oxidation
5.3 Polymerisation

6 Nomenclature of Alkenes

6.1 IUPAC Names
6.2 Common Names

7 See also
8 References

Structure of Alkenes

Shape of alkenes

As predicted by the VSEPR model of electron pair replusion, the molecular geometry of alkenes includes bond angles about each carbon in a double bond of about 120°. The angle may vary because of steric strain introduced by nonbonded interactions created by functional groups attached to the carbons of the double bond. For example, the C-C-C bond angle in propylene is 123.9°. The alkene double bond is stronger than a single covalent bond and also shorter with an average bond length of 133 picometres.

Molecular geometry

Like single covalent bonds, double bonds can be described in terms of overlapping atomic orbitals, except that unlike a single bond (which consists of a single sigma bond), a carbon-carbon double bond consists of one sigma bond and one pi bond.

Each carbon of the double bond uses its three sp² hybrid orbitals to form sigma bonds to three atoms. The unhybridized 2p atomic orbitals, which lie perpendicular to the plane created by the axes of the three sp² hybrid orbitals, combine to form the pi bond.

cis-2-Butylene

trans-2-Butylene

Because it requires a large amount of energy to break a pi bond (264 kJ/mol in ethylene), rotation about the carbon-carbon double bond is very difficult and therefore severely restricted. As a consequence substituted alkenes may exist as one of two isomers called a cis isomer and a trans isomer. For example, in cis-2-butylene the two methyl substituents face the same side of the double bond and in trans-2-butylene they face the opposite side.

It is certainly not impossible to twist a double bond. In fact, a 90° twist requires an energy approximately equal to half the strength of a pi bond. The misalignment of the p orbitals is less than expected because pyridalization takes place. trans-Cyclooctene is a stable strained alkene and the orbital misalignment is only 19° with a dihedral angle of 137° (normal 120°) and a degree of pyramidalization of 18°. This explains the dipole moment of 0.8 D for this compound (cis-isomer 0.4 D) where a value of zero is expected. The trans isomer of cycloheptene is only stable at low temperatures.

Physical properties

The physical properties of alkenes are comparable with alkanes. The physical state depends on molecular mass. The simplest alkenes, ethylene, propylene and butylene are gases. Linear alkenes of approximately five to sixteen carbons are liquids, and higher alkenes are waxy solids.

Chemical properties

Alkenes are relatively stable compounds, but are more reactive than alkanes. This is compatible with the idea that the carbon-carbon double bond in alkenes is stronger than the carbon-carbon single bond in alkanes, however, as the majority of the reactions of alkenes involve the rupture of this bond to form two new single bonds.

Synthesis

The most common industrial synthesis path for alkenes is cracking of petroleum.
Alkenes can be synthesized from alcohols via dehydration that eliminates water. For example, the dehydration of ethanol produces ethylene:

CH₃CH₂OH + H₂SO₄ → CH₃CH₂OSO₃H + H₂O → H₂C=CH₂ + H₂SO₄

Other alcohol eliminations are the Chugaev elimination and the Grieco elimination in which the alcohol group is converted to a short-lived intermediate first.

An elimination reaction from an alkyl amine occurs in the Hofmann elimination and the Cope reaction to produce alkenes.

Catalytic synthesis of higher α-alkenes can be achieved by a reaction of ethylene with the organometallic compound triethylaluminium in the presence of nickel, cobalt or platinum.

Alkenes scramble in an olefin metathesis.

Alkenes can be generated from carbonyl compounds, such as an aldehyde or ketone, by a variety of reactions.

*Reaction with alkyl halides in the Wittig reaction

*Reaction with a phenyl sulfone in the Julia olefination

*Reaction of two different ketones in the Barton-Kellogg reaction

*Coupling of one ketone in the Bamford-Stevens reaction or the Shapiro reaction

Alkenes can be generated from coupling reactions of vinyl halides.

Alkenes can be generated by the selective reduction of alkynes.

Alkenes rearrange in the Diels-Alder reaction and an Ene reaction.

Alkenes are generated from α-halo sulfones in the Ramberg-Bäcklund Reaction.

Reactions

Alkenes serve as a feedstock for the petrochemical industry because they can participate in a wide variety of reactions.

Addition reactions

Alkenes react in many addition reactions.

Catalytic addition of hydrogen: Catalytic hydrogenation of alkenes produces the corresponding alkanes. The reaction is carried out under pressure in the presence of a metallic catalyst. Common industrial catalysts are based on platinum, nickel or palladium. For laboratory syntheses, Raney nickel is often employed. This is an alloy of nickel and aluminium. An exaple of this reaction is the catalytic hydrogenation of ethylene to yield ethane:

CH₂=CH₂ + H₂ → CH₃-CH₃

Electrophilic addition: Most addition reactions to alkenes follow the mechanism of electrophilic addition. An example is the Prins reaction where the electrophile is a carbonyl group.
Halogenation: Addition of elementary bromine or chlorine to alkenes yields vicinal dibromo- and dichloroalkanes, respectively. The decoloration of a solution of bromine in water is an analytical test for the presence of alkenes:

CH₂=CH₂ + Br₂ → BrCH₂-CH₂Br

This is the mechanism for the reaction:

The reaction works because the high electron density at the double bond causes a temporary shift of electrons in the Br-Br bond causing a temporary induced dipole. This makes the Br closest to the double bond slightly positive and therefore an electrophile.

Hydrohalogenation: Addition of hydrohalic acids such as HCl or HBr to alkenes yields the corresponding haloalkanes.

CH₃-CH=CH₂ + HBr → CH₃-CHBr-CH₃

If the two carbon atoms at the double bond are linked to a different number of hydrogen atoms, the halogen is found preferentially at the carbon with less hydrogen substituents (Markovnikov's rule).

This is the reaction mechanism for hydrohalogenation:

Addition of a carbene or carbenoid yields the corresponding cyclopropane.

Oxidation

Alkenes are oxidized with a large number of oxidizing agents.

In the presence of oxygen, alkenes burn with a bright flame to produce carbon dioxide and water.
Catalytic oxidation with oxygen or the reaction with percarboxylic acids yields epoxides
Reaction with ozone in ozonolysis leads to the breaking of the double bond, yielding two aldehydes or ketones

R₁-CH=CH-R₂ + O₃ → R₁-CHO + R₂-CHO + H₂O

This reaction can be used to determine the position of a double bond in an unknown alkene.

Polymerisation

Polymerization of alkenes is an economically important reaction which yields polymers of high industrial value, such as the plastics polyethylene and polypropylene. Polymerization can either proceed via a free-radical or an ionic mechanism.

Nomenclature of Alkenes

IUPAC Names

To form the root of the IUPAC names for alkenes, simply change the -an- infix of the parent to -en-. For example, CH₃-CH₃ is the alkane ethANe. The name of CH₂=CH₂ is therefore ethENe.

In higher alkenes, where isomers exist that differ in location of the double bond, the following numbering system is used:

Number the longest carbon chain that contains the double bond in the direction that gives the carbon atoms of the double bond the lowest possible numbers.
Indicate the location of the double bond by the location of its first carbon
Name branched or substituted alkenes in a manner similar to alkanes.
Number the carbon atoms, locate and name substituent groups, locate the double bond, and name the main chain

CH₃CH₂CH₂CH₂CH==CH₂ 6 5 4 3 2 1
1-Hexene CH₃ | CH₃CH₂CHCH₂CH==CH₂ 6 5 4 3 2 1
4-Methyl-1-hexene CH₃ | CH₃CH₂CHCH₂C==CH₂ 6 5 4 3 |2 1 CH₂CH₃
2-Ethyl-4-methyl-1-hexene

Common Names

Despite the precision and universal acceptance of the IUPAC naming system, some alkenes are known almost exclusively by their common names:

	CH₂="CH₂"	CH₃CH="CH₂"	CH₃C(CH₃)="CH₂"
IUPAC name:	Ethene	Propene	2-Methylpropene
Common name:	Ethylene	Propylene	Isobutylene

References

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