'''Hydrogenation''' - to treat with hydrogen - is a [[chemical reaction]] between molecular [[hydrogen]] (H<sub>2</sub>) and another compound or element, usually in the presence of a [[Catalysis|catalyst]]. The process is commonly employed to [[redox|reduce]] or [[Saturation (chemistry)|saturate]] [[organic compound]]s. Hydrogenation typically constitutes the addition of pairs of [[hydrogen]] [[atom]]s to a molecule, generally an [[alkene]]. [[Catalyst]]s are required for the reaction to be usable; non-catalytic hydrogenation takes place only at very high temperatures. [[Hydrogen]] adds to [[double bonds|double]] and [[triple bond]]s in [[hydrocarbon]]s.<ref>{{cite book|last=Hudlický|first=Miloš|title=Reductions in Organic Chemistry|publisher=[[American Chemical Society]]|year=1996|location=Washington, D.C.|pages=429|isbn=0-8412-3344-6}}</ref>
'''Hydrogenation''' - call this # for a fun time: 603-4949918to treat with hydrogen - is a [[chemical reaction]] between molecular [[hydrogen]] (H<sub>2</sub>) and another compound or element, usually in the presence of a [[Catalysis|catalyst]]. The process is commonly employed to [[redox|reduce]] or [[Saturation (chemistry)|saturate]] [[organic compound]]s. Hydrogenation typically constitutes the addition of pairs of [[hydrogen]] [[atom]]s to a molecule, generally an [[alkene]]. [[Catalyst]]s are required for the reaction to be usable; non-catalytic hydrogenation takes place only at very high temperatures. [[Hydrogen]] adds to [[double bonds|double]] and [[triple bond]]s in [[hydrocarbon]]s.<ref>{{cite book|last=Hudlický|first=Miloš|title=Reductions in Organic Chemistry|publisher=[[American Chemical Society]]|year=1996|location=Washington, D.C.|pages=429|isbn=0-8412-3344-6}}</ref>
Because of the importance of hydrogen, many related reactions have been developed for its use. Most hydrogenations use gaseous hydrogen (H<sub>2</sub>), but some involve the alternative sources of hydrogen, not H<sub>2</sub>: these processes are called [[transfer hydrogenation]]s. The reverse reaction, removal of hydrogen from a molecule, is called [[dehydrogenation]]. A reaction where bonds are broken while hydrogen is added is called [[hydrogenolysis]], a reaction that may occur to carbon-carbon and carbon-heteroatom ([[oxygen]], [[nitrogen]] or [[halogen]]) bonds. Hydrogenation differs from [[protonation]] or [[hydride]] addition: in hydrogenation, the products have the same charge as the reactants.
Because of the importance of hydrogen, many related reactions have been developed for its use. Most hydrogenations use gaseous hydrogen (H<sub>2</sub>), but some involve the alternative sources of hydrogen, not H<sub>2</sub>: these processes are called [[transfer hydrogenation]]s. The reverse reaction, removal of hydrogen from a molecule, is called [[dehydrogenation]]. A reaction where bonds are broken while hydrogen is added is called [[hydrogenolysis]], a reaction that may occur to carbon-carbon and carbon-heteroatom ([[oxygen]], [[nitrogen]] or [[halogen]]) bonds. Hydrogenation differs from [[protonation]] or [[hydride]] addition: in hydrogenation, the products have the same charge as the reactants.
Hydrogenation - call this # for a fun time: 603-4949918to treat with hydrogen - is a chemical reaction between molecular hydrogen (H2) and another compound or element, usually in the presence of a catalyst. The process is commonly employed to reduce or saturateorganic compounds. Hydrogenation typically constitutes the addition of pairs of hydrogenatoms to a molecule, generally an alkene. Catalysts are required for the reaction to be usable; non-catalytic hydrogenation takes place only at very high temperatures. Hydrogen adds to double and triple bonds in hydrocarbons.[1]
Because of the importance of hydrogen, many related reactions have been developed for its use. Most hydrogenations use gaseous hydrogen (H2), but some involve the alternative sources of hydrogen, not H2: these processes are called transfer hydrogenations. The reverse reaction, removal of hydrogen from a molecule, is called dehydrogenation. A reaction where bonds are broken while hydrogen is added is called hydrogenolysis, a reaction that may occur to carbon-carbon and carbon-heteroatom (oxygen, nitrogen or halogen) bonds. Hydrogenation differs from protonation or hydride addition: in hydrogenation, the products have the same charge as the reactants.
Hydrogenation has three components, the unsaturated substrate, the hydrogen (or hydrogen source) and, invariably, a catalyst. The reduction reaction is carried out at different temperatures and pressures depending upon the substrate and the activity of the catalyst.
Substrate
The addition of H2 to an alkene affords an alkane in the protypical reaction:
Hydrogenation is sensitive to steric hindrance explaining the selectivity for reaction with the exocyclic double bond but not the internal double bond.
An important characteristic of alkene and alkyne hydrogenations, both the homogeneously and heterogeneously catalyzed versions, is that hydrogen addition occurs with "syn addition", with hydrogen entering from the least hindered side.[3] Typical substrates are listed in the table
commercial applications use heterogeneous Ni catalysts; major application is aniline
Catalysts
With rare exceptions, no reaction below 480 °C (750 K or 900 °F) occurs between H2 and organic compounds in the absence of metal catalysts. The catalyst binds both the H2 and the unsaturated substrate and facilitates their union. Platinum, palladium, rhodium, and ruthenium form highly active catalysts, which operate at lower temperatures and lower pressures of H2. Non-precious metal catalysts, especially those based on nickel (such as Raney nickel and Urushibara nickel) have also been developed as economical alternatives, but they are often slower or require higher temperatures. The trade-off is activity (speed of reaction) vs. cost of the catalyst and cost of the apparatus required for use of high pressures. Notice that the Raney-nickel catalysed hydrogenations require high pressures:[4][5]
Hydrogenation of an imine using a Raney-Nickel catalyst.
Partial hydrogenation of an resorcinol using a Raney-Nickel catalyst.
Two broad families of catalysts are known - homogeneous catalysts and heterogeneous catalysts. Homogeneous catalysts dissolve in the solvent that contains the unsaturated substrate. Heterogeneous catalysts are solids that are suspended in the same solvent with the substrate or are treated with gaseous substrate.
Hydrogenation is sensitive to steric hindrance explaining the selectivity for reaction with the exocyclic double bond but not the internal double bond.
The activity and selectivity of homogeneous catalysts is adjusted by changing the ligands. For prochiral substrates, the selectivity of the catalyst can be adjusted such that one enantiomeric product is favored. Asymmetric hydrogenation is also possible via heterogeneous catalysis on a metal that is modified by a chiral ligand.[7]
Heterogeneous catalysts
Heterogeneous catalysts for hydrogenation are more common industrially. As in homogeneous catalysts, the activity is adjusted through changes in the environment around the metal, i.e. the coordination sphere. Different faces of a crystalline heterogeneous catalyst display distinct activities, for example. Similarly, heterogeneous catalysts are affected by their supports, i.e. the material upon with the heterogeneous catalyst is bound.
In many cases, highly empirical modifications involve selective "poisons". Thus, a carefully chosen catalyst can be used to hydrogenate some functional groups without affecting others, such as the hydrogenation of alkenes without touching aromatic rings, or the selective hydrogenation of alkynes to alkenes using Lindlar's catalyst. For example, when the catalyst palladium is placed on barium sulfate and then treated with quinoline, the resulting catalyst reduces alkynes only as far as alkenes. The Lindlar catalyst has been applied to the conversion of phenylacetylene to styrene.[8]
Partial hydrogenation of phenylacetylene using the Lindlar catalyst
Asymmetric hydrogenation is also possible via heterogeneous catalysis on a metal that is modified by a chiral ligand.[7]
Hydrogen sources
For hydrogenation, the obvious source of hydrogen is H2 gas itself, which is typically available commercially within the storage medium of a pressurized cylinder. The hydrogenation process often uses greater than 1 atmosphere of H2, usually conveyed from the cylinders and sometimes augmented by "booster pumps". Gaseous hydrogen is produced industrially from hydrocarbons by the process known as steam reforming.[9]
Polar substrates such as ketones can be hydrogenated electrochemically, using protic solvents and reducing equivalents as the source of hydrogen.[11]
Thermodynamics and mechanism
Hydrogenation is a strongly exothermic reaction. In the hydrogenation of vegetable oils and fatty acids, for example, the heat released is about 25 kcal per mole (105 kJ/mol), sufficient to raise the temperature of the oil by 1.6-1.7 °C per iodine number drop. The mechanism of metal-catalyzed hydrogenation of alkenes and alkynes has been extensively studied.[12] First of all isotope labeling using deuterium confirms the regiochemistry of the addition:
RCH=CH2 + D2 → RCHDCH2D
Heterogeneous catalysis
On solids, the accepted mechanism is the Horiuti-Polanyi mechanism:[13][14]
Binding of the unsaturated bond, and hydrogen dissociation into atomic hydrogen onto the catalyst
Addition of one atom of hydrogen; this step is reversible
Addition of the second atom; effectively irreversible under hydrogenating conditions.
In the second step, the metallointermediate formed is a saturated compound that can rotate and then break down, again detaching the alkene from the catalyst. Consequently, contact with a hydrogenation catalyst necessarily causes cis-trans-isomerization, because the isomerization is thermodynamically favorable. This is a problem in partial hydrogenation, while in complete hydrogenation the produced trans-alkene is eventually hydrogenated.
For aromatic substrates, the first bond is hardest to hydrogenate because of the free energy penalty for breaking the aromatic system. The product of this is a cyclohexadiene, which is extremely active and cannot be isolated; in conditions reducing enough to break the aromatization, it is immediately reduced to a cyclohexene. The cyclohexene is ordinarily reduced immediately to a fully saturated cyclohexane, but special modifications to the catalysts (such as the use of the anti-solvent water on ruthenium) can preserve some of the cyclohexene, if that is a desired product.
Homogeneous catalysis
In many homogeneous hydrogenation processes,[15] the metal binds to both components to give an intermediate alkene-metal(H)2 complex. The general sequence of reactions is assumed to be as follows or a related sequence of steps:
binding of the hydrogen to give a dihydride complex ("oxidative addition"):
LnM + H2 → LnMH2
binding of alkene:
LnM(η2H2) + CH2=CHR → Ln-1MH2(CH2=CHR) + L
transfer of one hydrogen atom from the metal to carbon (migratory insertion)
Ln-1MH2(CH2=CHR) → Ln-1M(H)(CH2-CH2R)
transfer of the second hydrogen atom from the metal to the alkyl group with simultaneous dissociation of the alkane ("reductive elimination")
Ln-1M(H)(CH2-CH2R) → Ln-1M + CH3-CH2R
Preceding the oxidative addition of H2 is the formation of a dihydrogen complex.
Inorganic substrates
The hydrogenation of nitrogen to give ammonia is conducted on a vast scale by the Haber-Bosch process, consuming an estimated 1% of the world's energy supply.
Oxygen can be partially hydrogenated to give hydrogen peroxide, although this process has not been commercialized.
Industrial applications
Catalytic hydrogenation has diverse industrial uses. Most frequently, industrial hydrogenation relies on heterogeneous catalysts.[9]
In petrochemical processes, hydrogenation is used to convert alkenes and aromatics into saturated alkanes (paraffins) and cycloalkanes (naphthenes), which are less toxic and less reactive. For example, mineral turpentine is usually hydrogenated. Hydrocracking of heavy residues into diesel is another application. In isomerization and catalytic reforming processes, some hydrogen pressure is maintained to hydrogenolyzecoke formed on the catalyst and prevent its accumulation.
Xylitol, a polyol, is produced by hydrogenation of the sugar xylose, an aldehyde.
The largest scale application of hydrogenation is for the processing of vegetable oils (fats to give margarine and related spreads and shortenings). Typical vegetable oils are derived from polyunsaturated fatty acids (containing more than one carbon-carbon double bonds). Their partial hydrogenation reduces most but not all, of these carbon-carbon double bonds. The degree of hydrogenation is controlled by restricting the amount of hydrogen, reaction temperature and time, and the catalyst.[16]
Partial hydrogenation of a typical plant oil to a typical component of margarine. Most of the C=C double bonds are removed in this process, which elevates the melting point of the product.
Hydrogenation converts liquid vegetable oils into solid or semi-solid fats, such as those present in margarine. Changing the degree of saturation of the fat changes some important physical properties such as the melting range, which is why liquid oils become semi-solid. Solid or semi-solid fats are preferred for baking because the way the fat mixes with flour produces a more desirable texture in the baked product. Because partially hydrogenated vegetable oils are cheaper than animal source fats, are available in a wide range of consistencies, and have other desirable characteristics (e.g., increased oxidative stability/longer shelf life), they are the predominant fats used as shortening in most commercial baked goods.
A side effect of incomplete hydrogenation having implications for human health is the isomerization of some of the remaining unsaturated carbon bonds. The cis configuration of these double bonds predominates in the unprocessed fats in most edible fat sources, but incomplete hydrogenation partially converts these molecules to trans isomers, which have been implicated in circulatory diseases including heart disease (see trans fats). The conversion from cis to trans bonds is favored because the trans configuration has lower energy than the natural cis one. At equilibrium, the trans/cis isomer ratio is about 2:1. Food legislation in the US and codes of practice in EU have long required labels declaring the fat content of foods in retail trade and, more recently, have also required declaration of the trans fat content. The use of trans fats in human food products has been effectively banned in Denmark (since 2003) and Switzerland (2008). In the US, local legislation banned trans fats from restaurants and public kitchens in New York City (since 2005) and California. Other countries and regions have introduced mandatory labeling of trans fats on food products and appealed to the industry for voluntary reductions.[17][18]
The earliest hydrogenation is that of platinumcatalyzed addition of hydrogen to oxygen in the Döbereiner's lamp, a device commercialized as early as 1823. The French chemist Paul Sabatier is considered the father of the hydrogenation process. In 1897, building on the earlier work of James Boyce, an American chemist working in the manufacture of soap products, he discovered that the introduction of a trace of nickel as a catalyst facilitated the addition of hydrogen to molecules of gaseous hydrocarbons in what is now known as the Sabatier process. For this work Sabatier shared the 1912 Nobel Prize in Chemistry. Wilhelm Normann was awarded a patent in Germany in 1902 and in Britain in 1903 for the hydrogenation of liquid oils, which was the beginning of what is now a world wide industry. The commercially important Haber-Bosch process, first described in 1905, involves hydrogenation of nitrogen. In the Fischer-Tropsch process, reported in 1922 carbon monoxide, which is easily derived from coal, is hydrogenated to liquid fuels.
Also in 1922, Voorhees and Adams described an apparatus for performing hydrogenation under pressures above one atmosphere.[19] The Parr shaker, the first product to allow hydrogenation using elevated pressures and temperatures, was commercialized in 1926 based on Voorhees and Adams’ research and remains in widespread use. In 1924 Murray Raney developed a nickel fine powder catalyst named after him which is still widely used in hydrogenation reactions such as conversion of nitriles to amines or the production of margarine.
Homogeneous catalytic hydrogenation
The history of homogeneous hydrogenation has been assigned to the development the Meerwein–Ponndorf–Verley reduction of ketones using aluminium alkoxides. In the 1930's, Calvin discovered that copper(II) complexes oxidized H2. The 1960s witnessed the development of well defined homogeneous catalysts using transition metal complexes, e.g., Wilkinson's catalyst (RhCl(PPh3)3). Soon thereafter Schrock and Obsorne's discovered that cationic Rh and Ir catalyze the hydrogenation of alkenes and carbonyls. In the 1970s, asymmetric hydrogenation was demonstrated in the synthesis of L-DOPA and the 1990's saw the invention of Noyori asymmetric hydrogenation.[20] The development of homogeneous hydrogenation was influenced by work started in the 1930's and 1940's on the oxo process and Ziegler-Natta polymerization.[21]
Metal-free hydrogenation
For all practical purposes, hydrogenation requires a metal catalyst. Hydrogenation can, however, proceed from some hydrogen donors without catalysts, illustrative hydrogen donors being diimide and aluminium isopropoxide. Some metal-free catalytic systems have been investigated in academic research. One such system for reduction of ketones consists of tert-butanol and potassium tert-butoxide and very high temperatures.[22] The reaction depicted below describes the hydrogenation of benzophenone:
Another system for metal-free hydrogenation is based on the phosphine-borane, compound 1, which has been called a frustrated Lewis pair. It reversibly accepts dihydrogen at relatively low temperatures to form the phosphoniumborate2 which can reduce simple hindered imines.[24]
The reduction of nitrobenzene to aniline has been reported to be catalysed by fullerene, its mono-anion, atmospheric hydrogen and UV light.[25]
Equipment used for hydrogenation
Today’s bench chemist has three main choices of hydrogenation equipment:
Batch hydrogenation under atmospheric conditions
Batch hydrogenation at elevated temperature and/or pressure
Flow hydrogenation
Batch hydrogenation under atmospheric conditions
The original and still a commonly practised form of hydrogenation in teaching laboratories, this process is usually effected by adding solid catalyst to a round bottom flask of dissolved reactant which has been evacuated using nitrogen or argon gas and sealing the mixture with a penetrable rubber seal. Hydrogen gas is then supplied from a H2-filled balloon. The resulting three phase mixture is agitated to promote mixing. Hydrogen uptake can be monitored, which can be useful for monitoring progress of a hydrogenation. This is achieved by either using a graduated tube containing a coloured liquid, usually aqueous copper sulfate or with gauges for each reaction vessel.
Batch hydrogenation at elevated temperature and/or pressure
Since many hydrogenation reactions such as hydrogenolysis of protecting groups and the reduction of aromatic systems proceed extremely sluggishly at atmospheric temperature and pressure, pressurised systems are popular. In these cases, catalyst is added to a solution of reactant under an inert atmosphere in a pressure vessel. Hydrogen is added directly from a cylinder or built in laboratory hydrogen source, and the pressurized slurry is mechanically rocked to provide agitation, or a spinning basket is used. Heat may also be used, as the pressure compensates for the associated reduction in gas solubility.
Flow hydrogenation
Flow hydrogenation has become a popular technique at the bench and increasingly the process scale. This technique involves continuously flowing a dilute stream of dissolved reactant over a fixed bed catalyst in the presence of hydrogen. Using established HPLC technology, this technique allows the application of pressures from atmospheric to 1,450 psi (100 bar). Elevated temperatures may also be used. At the bench scale, systems use a range of pre-packed catalysts which eliminates the need for weighing and filtering pyrophoric catalysts.
Industrial reactors
Catalytic hydrogenation is done in a tubular plug-flow reactor (PFR) packed with a supported catalyst. The pressures and temperatures are typically high, although this depends on the catalyst. Catalyst loading is typically much lower than in laboratory batch hydrogenation, and various promoters are added to the metal, or mixed metals are used, to improve activity, selectivity and catalyst stability. The use of nickel is common despite its low activity, due to its low cost compared to precious metals.
Gas Liquid Induction Reactors (Hydrogenator) are also used for carrying out catalytic hydrogenation.[26]
^Catalytic Hydrogenation of Maleic Acid at Moderate Pressures A Laboratory Demonstration Kwesi Amoa 1948 Journal of Chemical Education • Vol. 84 No. 12 December 2007
^Advanced Organic Chemistry Jerry March 2nd Edition
^ abPaul N. Rylander, "Hydrogenation and Dehydrogenation" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a13 487
^van Es, T.; Staskun, B. "Aldehydes from Aromatic Nitriles: 4-Formylbenzenesulfonamide" Org. Syn., Coll. Vol. 6, p.631 (1988). (Article)
^Daniela Maria do Amaral Ferraz Navarro and Marcelo Navarro "Catalytic Hydrogenation of Organic Compounds without H2 Supply: An Electrochemical System" J. Chem. Educ., 2004, vol. 81, p 1350. doi:10.1021/ed081p1350
^Kubas, G. J., "Metal Dihydrogen and σ-Bond Complexes", Kluwer Academic/Plenum Publishers: New York, 2001
^Gallezot, Pierre. "Hydrogenation - Heterogeneous" in Encyclopedia of Catalysis, Volume 4, ed. Horvath, I.T., John Wiley & Sons, 2003.
^C. Pettinari, F. Marchetti, D. Martini "Metal Complexes as Hydrogenation Catalysts" Comprehensive Coordination Chemistry II, 2004, volume 9. pp. 75–139. doi:10.1016/B0-08-043748-6/09125-8
^Perspective: Hydrogen-Mediated C-C Bond Formation: A Broad New Concept in Catalytic C-C Coupling Ming-Yu Ngai, Jong-Rock Kong, and Michael J. Krische J. Org. Chem.; 2007, 72, pp. 1063–1072. doi:10.1021/jo061895m
^Homogeneous Hydrogenation in the Absence of Transition-Metal Catalysts Cheves Walling, Laszlo Bollyky J. Am. Chem. Soc.; 1964; 86(18); 3750–3752. doi:10.1021/ja01072a028
^Hydrogenation without a Transition-Metal Catalyst: On the Mechanism of the Base-Catalyzed Hydrogenation of Ketones Albrecht Berkessel, Thomas J. S. Schubert, and Thomas N. Muller J. Am. Chem. Soc.2002, 124, 8693–8698 doi:10.1021/ja016152r
^A Nonmetal Catalyst for Molecular Hydrogen Activation with Comparable Catalytic Hydrogenation Capability to Noble Metal Catalyst Baojun Li and Zheng Xu J. Am. Chem. Soc., 2009, 131 (45), pp 16380–16382. doi:10.1021/ja9061097
early work on transfer hydrogenation: Davies, R. R.; Hodgson, H. H. J. Chem. Soc.1943, 281. Leggether, B. E.; Brown, R. K. Can. J. Chem.1960, 38, 2363. Kuhn, L. P. J. Am. Chem. Soc.1951, 73, 1510.
Fred A. Kummerow (2008). Cholesterol Won't Kill You, But Trans Fat Could. Trafford. ISBN142513808. {{cite book}}: Check |isbn= value: length (help)
