Alkenes: Properties, Synthesis, Features, Characteristics and Examples

We explain what alkenes are and the physical and chemical properties they present. Also, what are its characteristics and examples.

What are alkenes?

type of unsaturated hydrocarbons (which have lost hydrogens attached to adjacent carbon atoms ) is known as alkenes in whose molecules it is possible to find carbon-carbon double bonds.

Alkenes or olefinic compounds are organic substances that, together with alkanes (or paraffins), alkynes (or acetylenic compounds), and cycloalkanes, constitute aliphatic hydrocarbons, that is, those that are not aromatic (derived mainly from benzene / C 6 H 6 ).

In turn, aliphatic hydrocarbons can be classified into linear, monocyclic (a single ring composed of carbon atoms) and polycyclic (with several linked rings), so there can be alkenes belonging to all classifications.

Nomenclature of alkenes

Propane is also called propylene.

Alkenes were formerly called “olefins” because their simplest representatives, such as ethene, were reacted with halogens to produce oils.

According to systematic nomenclature, these compounds are named using the same rule as for alkanes. The longest carbon chain that contains the double bond is searched for. In case of having more than one double bond, the chain that has the smallest combination of the positions of these double bonds is searched for. If the molecule has substituents, they are named by putting the numerical prefix that corresponds to the position of the carbon to which they are attached (1,2,3 ...), but if it has several equal substituents, the prefix (di, tri, tetra ..) depending on whether they are two, three or four.

However, many alkenes are known by their non-systematic name (as is often the case with hydrocarbons) and in this case, the official ending (-eno) is replaced by -ylene, as is the case with ethene, also called ethylene, or with the propane, called propylene.

On the other hand, if there is more than one double bond, the terminations -diene (two double bonds) or -triene (three double bonds), etc. are used respectively.

The general formula of alkenes

The general formula for linear alkenes is C n H 2n, where n represents the number of the respective carbon atoms. This means that for each new double bond there will be two fewer hydrogen atoms than indicated in this formula.

Difference between alkanes and alkynes

Alkynes have a triple bond between their carbons.

Alkenes differ from alkanes and alkynes in the double bond that appears between their carbon atoms. It is often said, in fact, that an alkene is an alkane that has lost hydrogen atoms, thus releasing two electrons that make up the second bond of each double bond.

Alkanes have a single bond between their carbons (CC) ; alkenes have at least one double bond (C = C) and alkynes at least one triple bond (C?C).

Physical properties of alkenes

Alkenes have the following physical properties:

  • Depending on their number of carbon atoms, alkenes can be gases (fewer atoms) or liquids (more atoms).
  • They are insoluble in water but soluble in ether, chloroform, or benzene.
  • They are less dense than water.
  • They have some or no molecular polarity depending on the geometry of each molecule around the double bond.
  • They have a higher acidity than the corresponding alkanes, a product of the polarity of the bond.
  • Its boiling and melting point do not vary much with respect to the corresponding alkanes.

Chemical properties of alkenes

Plastics are made of hydrocarbons.

Alkenes are characterized by high chemical reactivity with respect to alkanes and their majority reactions are of addition. The most frequent reactions are:

  • Addition of hydrogen halides. Reaction with HCl or HBr.

Addition of hydrogen halides

  • Halogenation. Reaction with halogens (Cl 2, Br 2 ).

Halogenation 

  • Polymerization. Vital in the oil industry and its derivatives, since long and resistant chains of malleable matter ( plastics ) are achieved.

Polymerization

Abundance of alkenes

Alkenes are much less abundant than alkanes, in fact, they are found in natural petroleum but as a very minor component.

The oil cracking processes, on the other hand, are an important source of usable alkenes for the industry. However, alkenes are common in organic chemistry and are part of the common reactions to living things, especially plants and vegetables.

Synthesis of alkenes

The Heck Reaction is a process to synthesize alkenes.
The reactions that yield alkenes as a result and that, therefore, can be used to synthesize them are:

Dehydrohalogenation.

Dehydrohalogenation

Dehalogenation.

Dehalogenation

Elimination of water from alcohols.

Elimination of water from alcohols

Pyrolysis.

Pyrolysis.

They can also be obtained as a result of the Chungaev reaction and the Grieco reaction, by forming carbon-carbon bonds (Wittig reaction, Julia olefination, etc.), by pericyclic reactions, or coupling reactions with metals (Suzuki reaction, Heck reaction).

Dienes and polyenes

If there is more than one double bond in the molecule, we will be in the presence of a diene (two bonds), a triene (three bonds), or a polyene (multiple bonds).

These compounds, however, lack special properties and behave like normal alkenes, except that they exhibit very particular reactivities, depending on the location of the multiple double bonds in the molecule.

Stability of alkenes

Internal alkenes are more stable than those with a double bond at the ends.
Alkenes are more or less stable, depending on where the double bond is located in the molecule. Internal alkenes, whose double bond is located towards the central part of the molecule, are much more stable than those with the double bond located at the ends. In this way, the trans isomers are more stable than the cis ones.

Examples of alkenes

Some common alkenes are:

  • Ethene (CH 2 = CH 2 )
  • Propene (CH 2 = CH-CH 3 )
  • 1-butene (CH 2 = CH-CH 2 -CH 3 )
  • Cholesterol (C 27 H 46 O 6 )
  • Lanosterol (C 30 H 50 O)
  • Camphor (C 10 H 16 O)
  • Myrcene (C 10 H 16 )

The above content published at Collaborative Research Group is for informational and educational purposes only and has been developed by referring to reliable sources and recommendations from technology experts. We do not have any contact with official entities nor do we intend to replace the information that they emit.

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