Define hydrogen | Dictionary and Thesaurus

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Extensive DefinitionHydrogen () is the chemicalelement with atomicnumber 1. It is represented by the symbol H.At standard temperature and pressure, hydrogen is a colorless,odorless, nonmetallic,tasteless, highly flammable diatomicgas with the molecularformula H2. With an atomic massof 1.00794amu, hydrogen is the lightest element.Hydrogen is the most abundant of the chemical elements, constituting roughly 75% ofthe universe's elemental mass. Stars in the mainsequence are mainly composed of hydrogen in its plasmastate. Elemental hydrogen is relatively rare on Earth, and isindustrially produced from hydrocarbons such asmethane, after which most elemental hydrogen is used "captively"(meaning locally at the production site), with the largest marketsabout equally divided between fossil fuelupgrading (e.g., hydrocracking) andammonia production(mostly for the fertilizer market). Hydrogen may be produced fromwater using the process of electrolysis, but thisprocess is presently significantly more expensive commercially thanhydrogen production from natural gas.The most common naturally occurring isotope of hydrogen, known asprotium,has a single proton andno neutrons. In ioniccompounds it can take on either a positive charge (becoming acation composedof a bare proton) or a negative charge (becoming an anion known as ahydride). Hydrogen canform compounds with most elements and is present in water and most organiccompounds. It plays a particularly important role in acid-base chemistry, in which many reactions involve theexchange of protons between soluble molecules. As the only neutralatom for which the Schrödingerequation can be solved analytically, study of the energeticsand bonding of the hydrogen atom has played a key role in thedevelopment of quantummechanics.The solubility and characteristics ofhydrogen with various metals are very important in metallurgy (as many metalscan suffer hydrogenembrittlement) and in developing safe ways to store it for useas a fuel. Hydrogen is highly soluble in many compounds composed ofrareearth metals and transitionmetals and can be dissolved in both crystalline and amorphousmetals. Hydrogen solubility in metals is influenced by localdistortions or impurities in the metal crystallattice.CombustionHydrogen gas is highly flammable and will burn atconcentrations of 4% or more H2 in air. The enthalpy of combustion forhydrogen is −286kJ/mol; it burns according to thefollowing balanced equation.2 H2(g) + O2(g) → 2 H2O(l) + 572 kJ(286kJ/mol)When mixed with oxygen across a wide range ofproportions, hydrogen explodes upon ignition. Hydrogen burnsviolently in air. It ignites automatically at a temperature of560°C. Pure hydrogen-oxygen flames burn in the ultraviolet color range andare nearly invisible to the naked eye, as illustrated by thefaintness of flame from the main SpaceShuttle engines (as opposed to the easily visible flames fromthe SRBs). Thus it is difficult to visually detect if a hydrogenleak is burning. The explosion of the Hindenburg airship was an infamous case ofhydrogen combustion (pictured); the cause is debated, butcombustible materials in the ship's skin were responsible for thecoloring of the flames. Another characteristic of hydrogen fires isthat the flames tend to ascend rapidly with the gas in air, asillustrated by the Hindenburg flames, causing less damage thanhydrocarbon fires. Two-thirds of the Hindenburg passengers survivedthe fire, and many of the deaths which occurred were from fallingor from diesel fuel burns.H2 reacts directly with other oxidizing elements.A violent and spontaneous reaction can occur at room temperaturewith chlorine andfluorine, forming thecorresponding hydrogen halides: hydrogenchloride and hydrogenfluoride.Electron energy levelsThe ground stateenergylevel of the electron in a hydrogen atom is−13.6eV, which isequivalent to an ultraviolet photon of roughly92nm.The energy levels of hydrogen can be calculatedfairly accurately using the Bohr model ofthe atom, which conceptualizes the electron as "orbiting" theproton in analogy to the Earth's orbit of the sun. However, theelectromagneticforce attracts electrons and protons to one another, while planetsand celestial objects are attracted to each other by gravity. Because of thediscretization of angularmomentum postulated in early quantummechanics by Bohr, the electron in the Bohr model can onlyoccupy certain allowed distances from the proton, and thereforeonly certain allowed energies.A more accurate description of the hydrogen atomcomes from a purely quantum mechanical treatment that uses theSchrödingerequation or the equivalent Feynman pathintegral formulation to calculate the probabilitydensity of the electron around the proton.Elemental molecular formsThere are two different types of diatomichydrogen molecules that differ by the relative spin oftheir nuclei. In the orthohydrogen form, thespins of the two protons are parallel and form a triplet state; inthe parahydrogenform the spins are antiparallel and form a singlet. At standardtemperature and pressure, hydrogen gas contains about 25% of thepara form and 75% of the ortho form, also known as the "normalform". The equilibrium ratio of orthohydrogen to parahydrogendepends on temperature, but since the ortho form is an excitedstate and has a higher energy than the para form, it isunstable and cannot be purified. At very low temperatures, theequilibrium state is composed almost exclusively of the para form.The physical properties of pure parahydrogen differ slightly fromthose of the normal form. The ortho/para distinction also occurs inother hydrogen-containing molecules or functional groups, such aswater and methylene.The uncatalyzed interconversion between para andortho H2 increases with increasing temperature; thus rapidlycondensed H2 contains large quantities of the high-energy orthoform that convert to the para form very slowly. The ortho/pararatio in condensed H2 is an important consideration in thepreparation and storage of liquid hydrogen: the conversion fromortho to para is exothermic and producesenough heat to evaporate the hydrogen liquid, leading to loss ofthe liquefied material. Catalysts for theortho-para interconversion, such as iron compounds, are used duringhydrogen cooling.A molecular form called protonated molecular hydrogen, or H3+, is found in the interstellarmedium (ISM), where it is generated by ionization of molecularhydrogen from cosmic rays.It has also been observed in the upper atmosphere of the planetJupiter.This molecule is relatively stable in the environment of outerspace due to the low temperature and density. H3+ is one of themost abundant ions in the Universe, and it plays a notable role inthe chemistry of the interstellar medium.CompoundsCovalent and organic compoundsWhile H2 is not veryreactive under standard conditions, it does form compounds withmost elements. Millions of hydrocarbons are known, butthey are not formed by the direct reaction of elementary hydrogenand carbon (although synthesisgas production followed by the Fischer-Tropschprocess to make hydrocarbons comes close to being an exception,as this begins with coal and the elemental hydrogen is generated insitu). Hydrogen can form compounds with elements that are moreelectronegative,such as halogens (e.g.,F, Cl, Br, I); in these compounds hydrogen takes on a partialpositive charge. When bonded to fluorine, oxygen, or nitrogen, hydrogen canparticipate in a form of strong noncovalent bonding called hydrogenbonding, which is critical to the stability of many biologicalmolecules. Hydrogen also forms compounds with less electronegativeelements, such as the metals and metalloids, in which it takeson a partial negative charge. These compounds are often known ashydrides.Hydrogen forms a vast array of compounds withcarbon. Because of theirgeneral association with living things, these compounds came to becalled organiccompounds; the study of their properties is known as organicchemistry and their study in the context of living organisms is known as biochemistry. By somedefinitions, "organic" compounds are only required to containcarbon. However, most of them also contain hydrogen, and since itis the carbon-hydrogen bond which gives this class of compoundsmost of its particular chemical characteristics, carbon-hydrogenbonds are required in some definitions of the word "organic" inchemistry. For hydrides other than group I and II metals, the termis quite misleading, considering the low electronegativity ofhydrogen. An exception in group II hydrides is BeH2, which ispolymeric. In lithiumaluminium hydride, the AlH4− anion carries hydridic centersfirmly attached to the Al(III). Although hydrides can be formedwith almost all main-group elements, the number and combination ofpossible compounds varies widely; for example, there are over 100binary borane hydrides known, but only one binary aluminiumhydride. Binary indiumhydride has not yet been identified, although larger complexesexist.Protons and acidsSee also: Acid-basereactionOxidation of hydrogen, in the sense of removingits electron, formally gives H+, containing no electrons and anucleuswhich is usually composed of one proton. That is why H+ is oftencalled a proton. This species is central to discussion of acids. Under the Bronsted-Lowrytheory, acids are proton donors, while bases are protonacceptors.A bare proton H+ cannot exist in solution becauseof its strong tendency to attach itself to atoms or molecules withelectrons. However, the term 'proton' is used loosely to refer topositively charged or cationic hydrogen, denotedTo avoid the convenient fiction of the naked"solvated proton" in solution, acidic aqueous solutions aresometimes considered to contain the hydronium ion (H3O+), which isorganized into clusters to form H9O4+. Other oxonium ions are found whenwater is in solution with other solvents.Although exotic on earth, one of the most commonions in the universe is the H3+ ion, known as protonated molecular hydrogen or thetriatomic hydrogen cation.IsotopesHydrogen has three naturally occurring isotopes,denoted 1H, 2H, and 3H. Other, highly unstable nuclei (4H to 7H)have been synthesized in the laboratory but not observed in nature.1H is the most common hydrogen isotope with an abundance ofmore than 99.98%. Because the nucleus ofthis isotope consists of only a single proton, it is given thedescriptive but rarely used formal name protium.2H, the other stable hydrogen isotope, is known as deuterium and contains oneproton and one neutronin its nucleus. Deuterium is not radioactive, and does notrepresent a significant toxicity hazard. Water enriched inmolecules that include deuterium instead of normal hydrogen iscalled heavy water.Deuterium and its compounds are used as a non-radioactive label inchemical experiments and in solvents for 1H-NMRspectroscopy. Heavy water is used as a neutronmoderator and coolant for nuclear reactors. Deuterium is also apotential fuel for commercial nuclearfusion.3H is known as tritium and contains one protonand two neutrons in its nucleus. It is radioactive, decaying intoHelium-3through beta decaywith a half-life of12.32years. Itis used in nuclear fusion reactions, as a tracer in isotopegeochemistry, and specialized in self-poweredlighting devices. Tritium has also been used in chemical andbiological labeling experiments as a radiolabel.Hydrogen is the only element that has differentnames for its isotopes in common use today. (During the early studyof radioactivity, various heavy radioactive isotopes were givennames, but such names are no longer used). The symbols D and T(instead of 2H and 3H) are sometimes used for deuterium andtritium, but the corresponding symbol P is already in use forphosphorus and thusis not available for protium. In its nomenclaturalguidelines, the International Union of Pure and Applied Chemistry allows any ofD, T, 2H, and 3H to be used, although 2H and 3H arepreferred.Natural occurrenceHydrogen is the most abundantelement in the universe, making up 75% of normal matter bymass and over 90% by numberof atoms. This element is found in great abundance in stars andgasgiant planets. Molecularclouds of H2 are associated with starformation. Hydrogen plays a vital role in powering stars through proton-protonreaction and CNO cyclenuclearfusion.Throughout the universe, hydrogen is mostly foundin the atomic andplasmastates whose properties are quite different from molecularhydrogen. As a plasma, hydrogen's electron and proton are not boundtogether, resulting in very high electrical conductivity and highemissivity (producing the light from the sun and other stars). Thecharged particles are highly influenced by magnetic and electricfields. For example, in the solar windthey interact with the Earth's magnetosphere giving riseto Birkelandcurrents and the aurora.Hydrogen is found in the neutral atomic state in the Interstellarmedium. The large amount of neutral hydrogen found in thedamped Lyman-alpha systems is thought to dominate the cosmologicalbaryonic density of the Universe up toredshift z=4.Under ordinary conditions on Earth, elementalhydrogen exists as the diatomic gas, H2 (for data see table).However, hydrogen gas is very rare in the Earth's atmosphere (1ppm byvolume) because of its light weight, which enables it to escapefrom Earth's gravity more easily than heavier gases. Still,hydrogen is the third most abundant element on the Earth's surface.Most of the Earth's hydrogen is in the form of chemicalcompounds such as hydrocarbons and water. Hydrogen gas is produced bysome bacteria and algaeand is a natural component of flatus. Methane is ahydrogen source of increasing importance.HistoryDiscovery and useHydrogen gas, H2, was first artificiallyproduced and formally described by T. Von Hohenheim (also known asParacelsus,1493–1541) via the mixing of metals with strong acids.He was unaware that the flammable gas produced by this chemicalreaction was a new chemicalelement. In 1671, Robert Boylerediscovered and described the reaction between iron filings and dilute acids, which results in theproduction of hydrogen gas. In 1766, HenryCavendish was the first to recognize hydrogen gas as a discretesubstance, by identifying the gas from a metal-acidreaction as "inflammable air" and further finding in 1781 thatthe gas produces water when burned. He is usually given credit forits discovery as an element. In 1783, AntoineLavoisier gave the element the name of hydrogen (from the Greekhydro meaning water and genes meaning creator) when he and Laplace reproducedCavendish's finding that water is produced when hydrogen is burned.Furthermore, the corresponding simplicity of the hydrogen moleculeand the corresponding cation H2+ allowed fuller understanding ofthe nature of the chemicalbond, which followed shortly after the quantum mechanicaltreatment of the hydrogen atom had been developed in themid-1920s.One of the first quantum effects to be explicitlynoticed (but not understood at the time) was a Maxwell observationinvolving hydrogen, half a century before full quantummechanical theory arrived. Maxwell observed that the specificheat capacity of H2 unaccountably departs from that of adiatomic gas below roomtemperature and begins to increasingly resemble that of a monatomicgas at cryogenic temperatures. According to quantum theory, thisbehavior arises from the spacing of the (quantized) rotationalenergy levels, which are particularly wide-spaced in H2 because ofits low mass. These widely spaced levels inhibit equal partition ofheat energy into rotational motion in hydrogen at low temperatures.Diatomic gases composed of heavier atoms do not have such widelyspaced levels and do not exhibit the same effect.Productionseedetails Hydrogenproduction H2 is produced in chemistry and biologylaboratories, often as a by-product of other reactions; in industryfor the hydrogenation of unsaturated substrates; andin nature as a means of expelling reducing equivalents inbiochemical reactions.LaboratoryIn the laboratory, H2 is usuallyprepared by the reaction of acids on metals such as zinc.Zn + 2 H+ → Zn2+ +Aluminiumproduces H2 upon treatment with acids but also with base:2 Al + 6 H2O → 2 Al(OH)3 + 3 H2The electrolysis of water is asimple method of producing hydrogen. A low voltage current is runthrough the water, and gaseous oxygen forms at the anode while gaseous hydrogen formsat the cathode.Typically the cathode is made from platinum or another inert metalwhen producing hydrogen for storage. If, however, the gas is to beburnt on site, oxygen is desirable to assist the combustion, and soboth electrodes would be made from inert metals. (Iron, forinstance, would oxidize, and thus decrease the amount of oxygengiven off.) The theoretical maximum efficiency (electricity usedvs. energetic value of hydrogen produced) is between 80–94%.In 2007, it was discovered that an alloy ofaluminium and gallium inpellet form added to water could be used to generate hydrogen. Theprocess also creates alumina, but the expensivegallium, which prevents the formation of an oxide skin on thepellets, can be re-used. This has important potential implicationsfor a hydrogen economy, since hydrogen can be produced on-site anddoes not need to be transported.IndustrialHydrogen can be prepared in several differentways, but economically the most important processes involve removalof hydrogen from hydrocarbons. Commercial bulk hydrogen is usuallyproduced by the steamreforming of natural gas.At high temperatures (700–1100°C;1,300–2,000°F), steam (water vapor) reacts with methaneto yield carbonmonoxide and H2.CH4 + H2O → CO + 3This reaction is favored at low pressures but isnonetheless conducted at high pressures (20atm;600inHg) since highpressure H2 is the most marketable product. The product mixture isknown as "synthesisgas" because it is often used directly for the production ofmethanol and relatedcompounds. Hydrocarbonsother than methane can be used to produce synthesis gas withvarying product ratios. One of the many complications to thishighly optimized technology is the formation of coke or carbon:CH4 → C + 2Consequently, steam reforming typically employsan excess of H2O. Additional hydrogen can be recovered from thesteam by use of carbon monoxide through the watergas shift reaction, especially with an iron oxidecatalyst. This reaction is also a common industrial source ofcarbondioxide:2 CH4 + O2 → 2 CO + 4 H2and the coal reaction, which can serve as aprelude to the shift reaction above: Electrolysisof brine to yield chlorine also produces hydrogenas a co-product.Solar ThermochemicalA number of laboratories (including inFrance, Germany, Greece, Japan, and the USA) are developing thermochemical methods to produce hydrogen from solar energy andwater.ApplicationsLarge quantities of H2 are needed in thepetroleum and chemical industries. The largest application of H2 isfor the processing ("upgrading") of fossil fuels, and in theproduction of ammonia.The key consumers of H2 in the petrochemical plant include hydrodealkylation,hydrodesulfurization,and hydrocracking. H2 has several other important uses. H2 is usedas a hydrogenating agent, particularly in increasing the level ofsaturation of unsaturated fats and oils (foundin items such as margarine), and in the production of methanol. It is similarly thesource of hydrogen in the manufacture of hydrochloricacid. H2 is also used as a reducingagent of metallic ores.Apart from its use as a reactant, H2 has wideapplications in physics and engineering. It is used as a shieldinggas in weldingmethods such as atomichydrogen welding. H2 is used as the rotor coolant in electricalgenerators at powerstations, because it has the highest thermalconductivity of any gas. Liquid H2 is used in cryogenic research, includingsuperconductivitystudies. Since H2 is lighter than air, having a little more than1/15th of the density of air, it was once widely used as a liftingagent in balloons and airships.In more recent applications, hydrogen is usedpure or mixed with nitrogen (sometimes called forming gas)as a tracer gas for minute leak detection. Applications can befound in the automotive, chemical, power generation, aerospace, andtelecommunications industries. Hydrogen is an authorized foodadditive (E 949) that allows food package leak testing among otheranti-oxidizing properties.Hydrogen's rarer isotopes also each have specificapplications. Deuterium(hydrogen-2) is used in nuclear fissionapplications as a moderatorto slow neutrons, and innuclearfusion reactions. Tritium(hydrogen-3), produced in nuclearreactors, is used in the production of hydrogenbombs, as an isotopic label in the biosciences,The triple pointtemperature of equilibrium hydrogen is a defining fixed point onthe ITS-90 temperature scale at 13.8033kelvins.Energy carrierHydrogen is not an energy source, except inthe hypothetical context of commercial nuclearfusion power plants using deuterium or tritium, a technology presentlyfar from development. The Sun's energy comes from nuclear fusion ofhydrogen, but this process is difficult to achieve controllably onEarth. Elemental hydrogen from solar, biological, or electricalsources costs more in energy to make than is obtained by burningit. Hydrogen may be obtained from fossil sources (such as methane)for less energy than required to make it, but these sources areunsustainable, and are also themselves direct energy sources. Forexample, CO2 sequestrationfollowed by carbon capture and storage could be conducted at the point ofH2 production from fossil fuels. but without carbon emissions.However, the infrastructure costs associated with full conversionto a hydrogen economy would be substantial.Biological reactionsseedetails biohydrogen H2 is a productof some types of anaerobicmetabolism and is produced by several microorganisms, usuallyvia reactions catalyzed by iron- or nickel-containing enzymes called hydrogenases. These enzymescatalyze the reversible redox reaction between H2 and itscomponent two protons and two electrons. Creation of hydrogen gasoccurs in the transfer of reducing equivalents produced duringpyruvate fermentationto water.Watersplitting, in which water is decomposed into its componentprotons, electrons, and oxygen, occurs in the lightreactions in all photosynthetic organisms.Some such organisms—including the alga Chlamydomonasreinhardtii and cyanobacteria—have evolveda second step in the darkreactions in which protons and electrons are reduced to form H2gas by specialized hydrogenases in the chloroplast. Efforts havebeen undertaken to genetically modify cyanobacterial hydrogenasesto efficiently synthesize H2 gas even in the presence of oxygen.Efforts have also been undertaken with genetically modifiedalga in a bioreactor.Safety and precautionsHydrogen poses a number of hazardsto human safety, from potential detonations and fires whenmixed with air to being an asphyxant in itspure, oxygen-free form.In addition, liquidhydrogen is a cryogen and presents dangers(such as frostbite)associated with very cold liquids. Hydrogen dissolves in somemetals, and, in addition to leaking out, may have adverse effectson them, such as hydrogenembrittlement. Hydrogen gas leaking into external air mayspontaneously ignite. Moreover, hydrogen fire, while beingextremely hot, is almost invisible, and thus can lead to accidental burns.Even interpreting the hydrogen data (includingsafety data) is confounded by a number of phenomena. Many physicaland chemical properties of hydrogen depend on the parahydrogen/orthohydrogenratio (it often takes days or weeks at a given temperature to reachthe equilibrium ratio, for which the data is usually given).Hydrogen detonation parameters, such as critical detonationpressure and temperature, strongly depend on the containergeometry.See alsoAntihydrogenHydrogencycleHydrogenfuelHydrogenleak testingHydrogen-likeatomHydrogenlineHydrogenplanesHydrogenspectral seriesHydrogenstationHydrogentechnologiesHydrogenvehicleMetallichydrogenOxyhydrogenPhotohydrogenReferencesFurther readinghttp://chartofthenuclides.com/default.htmlThe Chemical ElementsHydrogen: The Essential ElementTheHype about Hydrogen, Fact and Fiction in the Race to Save theClimate Authorinterview at Global Public Media.A Guide to the ElementsExternal linksTheTruth About Hydrogen; Popular MechanicsBasic HydrogenCalculations of Quantum MechanicsNational HydrogenAssociationHydrogenphase diagramRIKENBeam Science Laboratory, Japan— Heavy hydrogenresearchWavefunctionof hydrogenZinc Powder WillDrive your Hydrogen Carhydrogen in Afrikaans: Waterstofhydrogen in Arabic: هيدروجينhydrogen in Asturian: Hidróxenuhydrogen in Azerbaijani: Hidrogenhydrogen in Bengali: হাইড্রোজেনhydrogen in Min Nan: H (goân-sò͘)hydrogen in Belarusian: Вадародhydrogen in Belarusian (Tarashkevitsa):Вадародhydrogen in Bavarian: Wassastoffhydrogen in Bosnian: Vodonikhydrogen in Breton: Hidrogenhydrogen in Bulgarian: Водородhydrogen in Catalan: Hidrogenhydrogen in Chuvash: Водородhydrogen in Cebuano: Idrohenohydrogen in Czech: Vodíkhydrogen in Corsican: Idrogenuhydrogen in Welsh: Hydrogenhydrogen in Danish: Brinthydrogen in German: Wasserstoffhydrogen in Estonian: Vesinikhydrogen in Modern Greek (1453-): Υδρογόνοhydrogen in Spanish: Hidrógenohydrogen in Esperanto: Hidrogenohydrogen in Basque: Hidrogenohydrogen in Persian: هیدروژنhydrogen in Faroese: Hydrogenhydrogen in French: Hydrogènehydrogen in Friulian: Idrogjenhydrogen in Irish: Hidriginhydrogen in Manx: Hiddragienhydrogen in Scottish Gaelic: Haidreagainhydrogen in Galician: Hidróxenohydrogen in Gujarati: હાઈડ્રોજનhydrogen in Classical Chinese: 氫hydrogen in Korean: 수소hydrogen in Armenian: Ջրածինhydrogen in Hindi: हाइड्रोजनhydrogen in Upper Sorbian: Wodźikhydrogen in Croatian: Vodikhydrogen in Ido: Hidrogenohydrogen in Indonesian: Hidrogenhydrogen in Interlingua (International AuxiliaryLanguage Association): Hydrogenohydrogen in Icelandic: Vetnihydrogen in Italian: Idrogenohydrogen in Hebrew: מימןhydrogen in Javanese: Hidrogenhydrogen in Kannada: ಜಲಜನಕhydrogen in Georgian: წყალბადიhydrogen in Swahili (macrolanguage):Hidrojenihydrogen in Haitian: Idwojènhydrogen in Kurdish: Hîdrojenhydrogen in Latin: Hydrogeniumhydrogen in Latvian: Ūdeņradishydrogen in Luxembourgish: Waasserstoffhydrogen in Lithuanian: Vandenilishydrogen in Limburgan: Waterstofhydrogen in Lingala: Idrojɛ́níhydrogen in Lojban: cidrohydrogen in Lombard: Idrògenhydrogen in Hungarian: Hidrogénhydrogen in Macedonian: Водородhydrogen in Malayalam: ഹൈഡ്രജന്‍hydrogen in Maori: Hauwaihydrogen in Marathi: हायड्रोजनhydrogen in Malay (macrolanguage):Hidrogenhydrogen in Mongolian: Устөрөгчnah:Āyōcoxquihydrogen in Dutch: Waterstofhydrogen in Dutch Low Saxon: Waeterstofhydrogen in Nepali: हाइड्रोजनhydrogen in Japanese: 水素hydrogen in Pitcairn-Norfolk: Hiidrojenhydrogen in Norwegian: Hydrogenhydrogen in Norwegian Nynorsk: Hydrogenhydrogen in Novial: Hidrogenehydrogen in Occitan (post 1500): Idrogènhydrogen in Uzbek: Vodorodhydrogen in Central Khmer: អ៊ីដ្រូសែនhydrogen in Low German: Waterstoffhydrogen in Polish: Wodórhydrogen in Portuguese: Hidrogéniohydrogen in Kölsch: Wasserstoffhydrogen in Romanian: Hidrogenhydrogen in Quechua: Yakuchaqhydrogen in Russian: Водородhydrogen in Sanskrit: हाइड्रोजनhydrogen in Albanian: Hidrogjenihydrogen in Sicilian: Idrògginuhydrogen in Simple English: Hydrogenhydrogen in Slovak: Vodíkhydrogen in Slovenian: Vodikhydrogen in Serbian: Водоникhydrogen in Serbo-Croatian: Vodikhydrogen in Sundanese: Hidrogénhydrogen in Finnish: Vetyhydrogen in Swedish: Vätehydrogen in Tagalog: Idrohenohydrogen in Tamil: ஹைட்ரஜன்hydrogen in Telugu: హైడ్రోజన్hydrogen in Thai: ไฮโดรเจนhydrogen in Vietnamese: Hiđrôhydrogen in Tajik: Ҳидрогенhydrogen in Turkish: Hidrojenhydrogen in Ukrainian: Воденьhydrogen in Urdu: آبگرhydrogen in Walloon: Idrodjinnehydrogen in Vlaams: Woaterstofhydrogen in Wu Chinese: 氢hydrogen in Yiddish: הידראגעןhydrogen in Contenese: 氫hydrogen in Chinese: 氢

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