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(New page: Any of numerous organic compounds, such as benzene and methane, that contain only carbon and hydrogen. Category:Green Glossary)
 
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Any of numerous organic compounds, such as benzene and methane, that contain only carbon and hydrogen.
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In [[organic chemistry]], a '''hydrocarbon''' is an [[organic compound]] consisting entirely of [[hydrogen]] and [[carbon]].<ref>Silberberg, 620</ref> Hydrocarbons from which one hydrogen atom has been removed are [[functional group]]s, called '''hydrocarbyls'''.<ref>IUPAC Goldbook [http://goldbook.iupac.org/H02891.html ''hydrocarbyl groups'']</ref>
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[[Aromatic hydrocarbon]]s (arenes), [[alkane]]s, [[alkene]]s, [[cycloalkane]]s and [[alkyne]]-based compounds are different types of hydrocarbons.
   
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The majority of hydrocarbons found on [[earth]] naturally occur in [[Petroleum#Crude oil|crude oil]], where decomposed organic matter provides an abundance of carbon and hydrogen which, when bonded, can [[catenation|catenate]] to form seemingly limitless chains.<ref>Clayden, J., Greeves, N., et al. (2001) ''Organic Chemistry'' Oxford ISBN 0-19-850346-6 p. 21</ref><ref>McMurry, J. (2000). ''Organic Chemistry'' 5th ed. Brooks/Cole: Thomson Learning. ISBN 0-495-11837-0 pp. 75–81</ref>
   
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==Types of hydrocarbons==
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The classifications for hydrocarbons defined by [[IUPAC nomenclature of organic chemistry]] are as follows:
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#Saturated hydrocarbons ([[alkane]]s) are the simplest of the hydrocarbon species and are composed entirely of single bonds and are saturated with hydrogen. The general formula for saturated hydrocarbons is C<sub>''n''</sub>H<sub>''2n+2''</sub> (assuming non-cyclic structures).<ref>Silderberg, 623</ref> Saturated hydrocarbons are the basis of petroleum fuels and are found as either linear or branched species. Hydrocarbons with the same [[molecular formula]] but different [[structural formula]]e are called [[structural isomers]].<ref name="Silderberg">Silderberg, 625</ref> As given in the example of 3-methylhexane and its higher [[homology (chemistry)|homologues]], branched hydrocarbons can be [[Chirality (chemistry)|chiral]].<ref>Silderberg, 627</ref> Chiral saturated hydrocarbons constitute the side chains of biomolecules such as [[chlorophyll]] and [[tocopherol]].<ref>Meierhenrich, Uwe. [http://books.google.com/books?id=a2J23yPEaBQC&printsec=frontcover Amino Acids and the Asymmetry of Life]. Springer, 2008. ISBN 978-3-540-76885-2
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</ref>
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#[[Unsaturated hydrocarbon]]s have one or more double or triple bonds between carbon atoms. Those with double bond are called [[alkene]]s. Those with one double bond have the formula C<sub>''n''</sub>H<sub>''2n''</sub> (assuming non-cyclic structures).<ref>Silderberg, 628</ref> Those containing triple bonds are called [[alkyne]]s, with general formula C<sub>''n''</sub>H<sub>''2n-2''</sub>.<ref>Silderberg, 631</ref>
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#[[Cycloalkanes]] are hydrocarbons containing one or more carbon rings to which hydrogen atoms are attached. The general formula for a saturated hydrocarbon containing one ring is C<sub>''n''</sub>H<sub>''2n''</sub>.<ref name="Silderberg" />
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#[[Aromatic hydrocarbon]]s, also known as [[arene]]s, are hydrocarbons that have at least one [[aromatic ring]].
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Hydrocarbons can be [[gases]] (e.g. [[methane]] and [[propane]]), [[liquids]] (e.g. [[hexane]] and [[benzene]]), [[wax]]es or low melting [[solids]] (e.g. [[paraffin wax]] and [[naphthalene]]) or [[polymers]] (e.g. [[polyethylene]], [[polypropylene]] and [[polystyrene]]).
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===General properties===
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Because of differences in molecular structure, the empirical formula remains different between hydrocarbons; in linear, or "straight-run" alkanes, alkenes and alkynes, the amount of bonded hydrogen lessens in alkenes and alkynes due to the "self-bonding" or catenation of carbon preventing entire saturation of the hydrocarbon by the formation of double or triple bonds.
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This inherent ability of hydrocarbons to bond to themselves is referred to as [[catenation]], and allows hydrocarbon to form more complex molecules, such as [[cyclohexane]],and in rarer cases, arenes such as [[benzene]]. This ability comes from the fact that the bond character between carbon atoms is entirely non-polar, in that the distribution of electrons between the two elements is somewhat even due to the same electronegativity values of the elements (~0.30), and does not result in the formation of an electrophile.
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Generally, with catenation comes the loss of the total amount of bonded hydrocarbons and an increase in the amount of energy required for bond cleavage due to strain exerted upon the molecule;in molecules such as cyclohexane, this is referred to as [[ring strain]], and occurs due to the "destabilized" spatial electron configuration of the atom.
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In simple chemistry, as per [[valence bond theory]], the carbon atom must follow the "''4-hydrogen rule''",which states that the maximum number of atoms available to bond with carbon is equal to the number of electrons that are attracted into the outer shell of carbon.In terms of shells, carbon consists of an incomplete outer shell, which comprises 4 electrons,and thus has 4 electrons available for covalent or dative bonding.
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Hydrocarbons are [[hydrophobic]] and are [[lipid]]s.
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Some hydrocarbons also are abundant in the solar system. Lakes of liquid methane and ethane have been found on [[Titan (moon)|Titan]], Saturn's largest moon, confirmed by the Cassini-Huygens Mission.<ref>[http://news.bbc.co.uk/2/hi/science/nature/6230381.stm 'Proof' of methane lakes on Titan], BBC News, 4 January 2007</ref> Hydrocarbons are also abundant in nebulae forming [[polycyclic aromatic hydrocarbons]] – PAH compounds.
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===Simple hydrocarbons and their variations===
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<center>
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{| class="wikitable" style="text-align:center"
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!Number of<br />carbon atoms
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![[Alkane]] (single bond)
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![[Alkene]] (double bond)
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![[Alkyne]] (triple bond)
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![[Cycloalkane]]
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![[Alkadiene]]
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|-
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| 1 ||[[Methane]] ||[[methene]]|| [[methyne]]||-||-
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|-
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| 2 ||[[Ethane]] ||[[Ethene]] (ethylene)||[[Acetylene|Ethyne]] (acetylene)|| – || –
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|-
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| 3 ||[[Propane]] ||[[Propene]] (propylene)||[[Methylacetylene|Propyne]] (methylacetylene)|| [[Cyclopropane]] || [[Propadiene]] (allene)
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|-
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| 4 ||[[Butane]] ||[[Butene]] (butylene)||[[Butyne]] || [[Cyclobutane]] || [[1,3-Butadiene|Butadiene]]
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|-
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| 5 ||[[Pentane]] ||[[Pentene]] ||[[Pentyne]] || [[Cyclopentane]] || [[Piperylene|Pentadiene]] (piperylene)
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|-
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| 6 ||[[Hexane]] ||[[Hexene]] ||[[Hexyne]] || [[Cyclohexane]] || [[Hexadiene]]
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|-
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| 7 ||[[Heptane]] ||[[Heptene]] ||[[Heptyne]] || [[Cycloheptane]] || [[Heptadiene]]
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|-
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| 8 ||[[Octane]] ||[[Octene]] ||[[Octyne]] || [[Cyclooctane]] || [[Octadiene]]
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|-
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| 9 ||[[Nonane]] ||[[Nonene]] ||[[Nonyne]] || [[Cyclononane]] || [[Nonadiene]]
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|-
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| 10 ||[[Decane]] ||[[Decene]] ||[[Decyne]] || [[Cyclodecane]] || [[Decadiene]]
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|}
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</center>
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==Usage==
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Hydrocarbons are a primary energy source for current civilizations. The predominant use of hydrocarbons is as a combustible [[fuel]] source. In their solid form, hydrocarbons take the form of asphalt.<ref>Dan Morgan, Lecture ENVIRO 100, University of Washington, 11/5/08</ref>
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Mixtures of volatile hydrocarbons are now used in preference to the [[chlorofluorocarbons]] as a [[propellant]] for [[aerosol spray]]s, due to chlorofluorocarbon's impact on the [[ozone layer]].
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[[Methane]] [1C] and [[ethane]] [2C] are gaseous at ambient temperatures and cannot be readily liquefied by pressure alone. [[Propane]] [3C] is however easily liquefied, and exists in 'propane bottles' mostly as a liquid. [[Butane]] [4C] is so easily liquefied that it provides a safe, volatile fuel for small pocket lighters. [[Pentane]] [5C] is a clear liquid at room temperature, commonly used in chemistry and industry as a powerful nearly odorless [[solvent]] of waxes and high molecular weight organic compounds, including greases. [[Hexane]] [6C] is also a widely used non-polar, non-aromatic solvent, as well as a significant fraction of common [[gasoline]].
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The [6C] through [10C] alkanes, alkenes and isomeric cycloalkanes are the top components of [[gasoline]], [[Petroleum naphtha|naphtha]], [[jet fuel]] and specialized industrial solvent mixtures. With the progressive addition of carbon units, the simple non-ring structured hydrocarbons have higher viscosities, lubricating indices, boiling points, solidification temperatures, and deeper color. At the opposite extreme from [1C] methane lie the heavy tars that remain as the ''lowest fraction'' in a crude oil refining retort. They are collected and widely utilized as roofing compounds, pavement composition, wood preservatives (the [[creosote]] series) and as extremely high viscosity sheer-resisting liquids.
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===Burning hydrocarbons===
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{{Main|Combustion}}
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Hydrocarbons are currently the main source of the world’s [[electric power|electric energy]] and heat sources (such as home heating) because of the energy produced when burnt.<ref name="World Coal">World Coal, Coal and Electricity, http://www.worldcoal.org/coal/uses-of-coal/coal-electricity/, retrieved 07/03/2012</ref> Often this energy is used directly as heat such as in home heaters, which use either [[petroleum]] or [[natural gas]]. The hydrocarbon is burnt and the heat is used to heat water, which is then circulated. A similar principle is used to create electric energy in power plants.
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Common properties of hydrocarbons are the facts that they produce steam, carbon dioxide and heat during combustion and that oxygen is required for combustion to take place. The simplest hydrocarbon, methane, burns as follows:
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:CH<sub>4</sub> + 2 O<sub>2</sub> → 2 H<sub>2</sub>O + CO<sub>2</sub> + Energy
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In inadequate supply of air, CO gas and water vapour are formed:
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:2 CH<sub>4</sub> + 3 O<sub>2</sub> → 2CO + 4H<sub>2</sub>O
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Another example of this property is propane:
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:C<sub>3</sub>H<sub>8</sub> + 5 O<sub>2</sub> → 4 H<sub>2</sub>O + 3 CO<sub>2</sub> + Energy
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:C<sub>n</sub>H<sub>2n+2</sub> + (3n+1)/2 O<sub>2</sub> → (n+1) H<sub>2</sub>O + n CO<sub>2</sub> + Energy
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Burning of hydrocarbons is an example of [[exothermic reaction|exothermic]] chemical reaction.
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Hydrocarbons can also be burned with elemental fluorine, resulting in [[carbon tetrafluoride]] and [[hydrogen fluoride]] products
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====Petroleum====
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{{Main|Petroleum}}
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[[Image:ShellMartinez-refi.jpg|thumb|right|340px|[[Oil refinery|Oil refineries]] are one way hydrocarbons are processed for use. [[Crude oil]] is processed in several stages to form desired hydrocarbons, used as fuel and in other products.]]
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Extracted hydrocarbons in a liquid form are referred to as [[petroleum]] (literally "rock oil") or [[mineral oil]], whereas hydrocarbons in a gaseous form are referred to as [[natural gas]]. Petroleum and natural gas are found in the Earth's subsurface with the tools of [[petroleum geology]] and are a significant source of fuel and raw materials for the production of [[organic chemistry|organic chemicals]].
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The extraction of liquid hydrocarbon fuel from [[sedimentary basin]]s is integral to modern [[energy development]]. Hydrocarbons are [[mining|mined]] from [[tar sands]] and [[oil shale]], and potentially extracted from sedimentary [[methane hydrate]]s. These reserves require distillation and upgrading to produce [[synthetic crude]] and petroleum.
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[[Oil reserves]] in sedimentary rocks are the source of hydrocarbons for the energy, [[transport]] and [[petrochemical]] industry.
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Hydrocarbons are economically important because major [[fossil fuel]]s such as [[coal]], petroleum and [[natural gas]], and its derivatives such as [[plastic]]s, [[Paraffin wax|paraffin]], [[wax]]es, [[solvent]]s and oils are hydrocarbons. Hydrocarbons – along with [[NOx]] and [[sunlight]] – contribute to the formation of [[tropospheric ozone]] and [[greenhouse gas]]es.
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==See also==
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*[[Abiogenic petroleum origin]]
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*[[Biohydrocarbon]]
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*[[Energy storage]]
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*[[Fractional distillation]]
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*[[Functional group]]
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*[[Hydrocarbon mixtures]]
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*[[Hydrocarbons on other planets]]
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*[[Organically moderated and cooled reactor]]
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==References==
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{{Reflist|2}}
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==Bibliography==
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*Silberberg, Martin. Chemistry: The Molecular Nature Of Matter and Change. New York: McGraw-Hill Companies, 2004. ISBN 0-07-310169-9
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==External links==
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{{Wiktionary}}
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{{Commons|Hydrocarbons}}
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*[http://www.worldofmolecules.com/fuels/methane.htm The Methane Molecule]
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[[Category:Hydrocarbon conservation|*]]
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[[Category:Compost]]
 
[[Category:Green Glossary]]
 
[[Category:Green Glossary]]

Revision as of 01:44, January 18, 2013

In organic chemistry, a hydrocarbon is an organic compound consisting entirely of hydrogen and carbon.[1] Hydrocarbons from which one hydrogen atom has been removed are functional groups, called hydrocarbyls.[2] Aromatic hydrocarbons (arenes), alkanes, alkenes, cycloalkanes and alkyne-based compounds are different types of hydrocarbons.

The majority of hydrocarbons found on earth naturally occur in crude oil, where decomposed organic matter provides an abundance of carbon and hydrogen which, when bonded, can catenate to form seemingly limitless chains.[3][4]

Types of hydrocarbons

The classifications for hydrocarbons defined by IUPAC nomenclature of organic chemistry are as follows:

  1. Saturated hydrocarbons (alkanes) are the simplest of the hydrocarbon species and are composed entirely of single bonds and are saturated with hydrogen. The general formula for saturated hydrocarbons is CnH2n+2 (assuming non-cyclic structures).[5] Saturated hydrocarbons are the basis of petroleum fuels and are found as either linear or branched species. Hydrocarbons with the same molecular formula but different structural formulae are called structural isomers.[6] As given in the example of 3-methylhexane and its higher homologues, branched hydrocarbons can be chiral.[7] Chiral saturated hydrocarbons constitute the side chains of biomolecules such as chlorophyll and tocopherol.[8]
  2. Unsaturated hydrocarbons have one or more double or triple bonds between carbon atoms. Those with double bond are called alkenes. Those with one double bond have the formula CnH2n (assuming non-cyclic structures).[9] Those containing triple bonds are called alkynes, with general formula CnH2n-2.[10]
  3. Cycloalkanes are hydrocarbons containing one or more carbon rings to which hydrogen atoms are attached. The general formula for a saturated hydrocarbon containing one ring is CnH2n.[6]
  4. Aromatic hydrocarbons, also known as arenes, are hydrocarbons that have at least one aromatic ring.

Hydrocarbons can be gases (e.g. methane and propane), liquids (e.g. hexane and benzene), waxes or low melting solids (e.g. paraffin wax and naphthalene) or polymers (e.g. polyethylene, polypropylene and polystyrene).

General properties

Because of differences in molecular structure, the empirical formula remains different between hydrocarbons; in linear, or "straight-run" alkanes, alkenes and alkynes, the amount of bonded hydrogen lessens in alkenes and alkynes due to the "self-bonding" or catenation of carbon preventing entire saturation of the hydrocarbon by the formation of double or triple bonds.

This inherent ability of hydrocarbons to bond to themselves is referred to as catenation, and allows hydrocarbon to form more complex molecules, such as cyclohexane,and in rarer cases, arenes such as benzene. This ability comes from the fact that the bond character between carbon atoms is entirely non-polar, in that the distribution of electrons between the two elements is somewhat even due to the same electronegativity values of the elements (~0.30), and does not result in the formation of an electrophile.

Generally, with catenation comes the loss of the total amount of bonded hydrocarbons and an increase in the amount of energy required for bond cleavage due to strain exerted upon the molecule;in molecules such as cyclohexane, this is referred to as ring strain, and occurs due to the "destabilized" spatial electron configuration of the atom.

In simple chemistry, as per valence bond theory, the carbon atom must follow the "4-hydrogen rule",which states that the maximum number of atoms available to bond with carbon is equal to the number of electrons that are attracted into the outer shell of carbon.In terms of shells, carbon consists of an incomplete outer shell, which comprises 4 electrons,and thus has 4 electrons available for covalent or dative bonding.

Hydrocarbons are hydrophobic and are lipids.

Some hydrocarbons also are abundant in the solar system. Lakes of liquid methane and ethane have been found on Titan, Saturn's largest moon, confirmed by the Cassini-Huygens Mission.[11] Hydrocarbons are also abundant in nebulae forming polycyclic aromatic hydrocarbons – PAH compounds.

Simple hydrocarbons and their variations

Number of
carbon atoms
Alkane (single bond) Alkene (double bond) Alkyne (triple bond) Cycloalkane Alkadiene
1 Methane methene methyne--
2 Ethane Ethene (ethylene)Ethyne (acetylene)
3 Propane Propene (propylene)Propyne (methylacetylene) Cyclopropane Propadiene (allene)
4 Butane Butene (butylene)Butyne Cyclobutane Butadiene
5 Pentane Pentene Pentyne Cyclopentane Pentadiene (piperylene)
6 Hexane Hexene Hexyne Cyclohexane Hexadiene
7 Heptane Heptene Heptyne Cycloheptane Heptadiene
8 Octane Octene Octyne Cyclooctane Octadiene
9 Nonane Nonene Nonyne Cyclononane Nonadiene
10 Decane Decene Decyne Cyclodecane Decadiene

Usage

Hydrocarbons are a primary energy source for current civilizations. The predominant use of hydrocarbons is as a combustible fuel source. In their solid form, hydrocarbons take the form of asphalt.[12]

Mixtures of volatile hydrocarbons are now used in preference to the chlorofluorocarbons as a propellant for aerosol sprays, due to chlorofluorocarbon's impact on the ozone layer.

Methane [1C] and ethane [2C] are gaseous at ambient temperatures and cannot be readily liquefied by pressure alone. Propane [3C] is however easily liquefied, and exists in 'propane bottles' mostly as a liquid. Butane [4C] is so easily liquefied that it provides a safe, volatile fuel for small pocket lighters. Pentane [5C] is a clear liquid at room temperature, commonly used in chemistry and industry as a powerful nearly odorless solvent of waxes and high molecular weight organic compounds, including greases. Hexane [6C] is also a widely used non-polar, non-aromatic solvent, as well as a significant fraction of common gasoline.

The [6C] through [10C] alkanes, alkenes and isomeric cycloalkanes are the top components of gasoline, naphtha, jet fuel and specialized industrial solvent mixtures. With the progressive addition of carbon units, the simple non-ring structured hydrocarbons have higher viscosities, lubricating indices, boiling points, solidification temperatures, and deeper color. At the opposite extreme from [1C] methane lie the heavy tars that remain as the lowest fraction in a crude oil refining retort. They are collected and widely utilized as roofing compounds, pavement composition, wood preservatives (the creosote series) and as extremely high viscosity sheer-resisting liquids.

Burning hydrocarbons

Hydrocarbons are currently the main source of the world’s electric energy and heat sources (such as home heating) because of the energy produced when burnt.[13] Often this energy is used directly as heat such as in home heaters, which use either petroleum or natural gas. The hydrocarbon is burnt and the heat is used to heat water, which is then circulated. A similar principle is used to create electric energy in power plants.

Common properties of hydrocarbons are the facts that they produce steam, carbon dioxide and heat during combustion and that oxygen is required for combustion to take place. The simplest hydrocarbon, methane, burns as follows:

CH4 + 2 O2 → 2 H2O + CO2 + Energy

In inadequate supply of air, CO gas and water vapour are formed:

2 CH4 + 3 O2 → 2CO + 4H2O

Another example of this property is propane:

C3H8 + 5 O2 → 4 H2O + 3 CO2 + Energy
CnH2n+2 + (3n+1)/2 O2 → (n+1) H2O + n CO2 + Energy

Burning of hydrocarbons is an example of exothermic chemical reaction.

Hydrocarbons can also be burned with elemental fluorine, resulting in carbon tetrafluoride and hydrogen fluoride products

Petroleum

File:ShellMartinez-refi.jpg
Oil refineries are one way hydrocarbons are processed for use. Crude oil is processed in several stages to form desired hydrocarbons, used as fuel and in other products.

Extracted hydrocarbons in a liquid form are referred to as petroleum (literally "rock oil") or mineral oil, whereas hydrocarbons in a gaseous form are referred to as natural gas. Petroleum and natural gas are found in the Earth's subsurface with the tools of petroleum geology and are a significant source of fuel and raw materials for the production of organic chemicals.

The extraction of liquid hydrocarbon fuel from sedimentary basins is integral to modern energy development. Hydrocarbons are mined from tar sands and oil shale, and potentially extracted from sedimentary methane hydrates. These reserves require distillation and upgrading to produce synthetic crude and petroleum.

Oil reserves in sedimentary rocks are the source of hydrocarbons for the energy, transport and petrochemical industry.

Hydrocarbons are economically important because major fossil fuels such as coal, petroleum and natural gas, and its derivatives such as plastics, paraffin, waxes, solvents and oils are hydrocarbons. Hydrocarbons – along with NOx and sunlight – contribute to the formation of tropospheric ozone and greenhouse gases.

See also

References

  1. Silberberg, 620
  2. IUPAC Goldbook hydrocarbyl groups
  3. Clayden, J., Greeves, N., et al. (2001) Organic Chemistry Oxford ISBN 0-19-850346-6 p. 21
  4. McMurry, J. (2000). Organic Chemistry 5th ed. Brooks/Cole: Thomson Learning. ISBN 0-495-11837-0 pp. 75–81
  5. Silderberg, 623
  6. 6.0 6.1 Silderberg, 625
  7. Silderberg, 627
  8. Meierhenrich, Uwe. Amino Acids and the Asymmetry of Life. Springer, 2008. ISBN 978-3-540-76885-2
  9. Silderberg, 628
  10. Silderberg, 631
  11. 'Proof' of methane lakes on Titan, BBC News, 4 January 2007
  12. Dan Morgan, Lecture ENVIRO 100, University of Washington, 11/5/08
  13. World Coal, Coal and Electricity, http://www.worldcoal.org/coal/uses-of-coal/coal-electricity/, retrieved 07/03/2012

Bibliography

  • Silberberg, Martin. Chemistry: The Molecular Nature Of Matter and Change. New York: McGraw-Hill Companies, 2004. ISBN 0-07-310169-9

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