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It is the simplest element and the first in the [[periodic table]]. It has the [[symbol]] '''H''' and [[atomic number]] 1. Hydrogen also has a [[Relative atomic mass|standard atomic weight]] of 1.008. This makes it the lightest element. Hydrogen is a gas at 15 degrees Celsius (59 degrees Fahrenheit) at [[standard atmosphere]] (and in many other situations). When hydrogen is in the form of ''hydrogen gas'', then each ''hydrogen molecule'' has two ''hydrogen atoms''. In [[Standard temperature and pressure|standard conditions]], hydrogen is a [[Diatomic molecules|diatomic]] [[gas]] with the [[Chemical formula|formula]] {{chem2|H2}}, or '''dihydrogen'''.<ref name=":0">{{Cite web|last=PubChem|title=Hydrogen|url=https://pubchem.ncbi.nlm.nih.gov/compound/783|access-date=2024-05-30|website=pubchem.ncbi.nlm.nih.gov|language=en}}</ref> In this state, hydrogen is also called '''hydrogen gas''' or '''molecular hydrogen'''. Hydrogen has no [[Colour|color]], [[Olfaction|smell]], or [[taste]].<ref>{{Cite web|date=2024-05-05|title=Hydrogen {{!}} Properties, Uses, & Facts {{!}} Britannica|url=https://www.britannica.com/science/hydrogen|access-date=2024-05-30|website=www.britannica.com|language=en}}</ref> Hydrogen is not toxic and is very [[Combustibility and flammability|combustible]].<ref name=":0" /> Hydrogen is the most common chemical element in the [[universe]]. Hydrogen is almost 75% of all normal ([[baryon|baryonic]]) [[matter]] by [[mass]].<ref>{{Cite web|title=Origin of the Elements|url=https://www2.lbl.gov/abc/wallchart/chapters/10/0.html|access-date=2024-05-30|website=www2.lbl.gov}}</ref> Most [[star]]s are made of mostly hydrogen. The hydrogen in the stars are in a [[Plasma (physics)|plasma state]]. On Earth, hydrogen is seen in [[water]] and [[Organic compound|organic compounds]]. Hydrogen's most common [[isotope]] has one [[proton]] and no [[Neutron|neutrons]]. This isotope also has one [[electron]] [[Atomic orbital|orbiting]] around it. Hydrogen is usually [[Nonmetal|nonmetallic]] and can form [[Covalent bond|covalent bonds]] with most [[Nonmetal|nonmetals]]. These covalent bonds can create molecules such as [[water]] and other organic substances. Hydrogen is the main part of [[Acid–base reaction|acid–base reactions]]. These reactions [[exchange]] protons in [[Solubility|soluble]] molecules. In [[Ionic compound|ionic compounds]], ions can either be [[Anion|anions]] or [[Cation|cations]]. Hydrogen [[Anion|anions]] are negatively charged and are called [[Hydride|hydrides]]. Hydrogen [[Cation|cations]] are positively charged and are written as {{chem2|H+}}. Cations are also called protons (symbol p), because they are only made of a proton and nothing else. Hydrogen gas was first made [[Artificial|artificially]] in the 1700s. [[Henry Cavendish]] identified hydrogen gas as a distinct substance between 1766 and 1781. Most [[hydrogen production]] is from [[steam reforming]] natural gas. Hydrogen has many [[Industry|industrial]] uses. Hydrogen can be used to process [[Fossil fuel|fossil fuels]], [[Cracking (chemistry)|hydrocrack]], and [[Ammonia production|produce ammonia]]. == Properties == Hydrogen is grouped as a [[Nonmetal|reactive nonmetal]]. This is different from the other elements found in the first [[Group (periodic table)|group]] of the periodic table, which are called [[alkali metal]]s. Only the solid form of hydrogen should behave like a metal, though. When hydrogen is by itself, it will normally [[chemical bond|bind]] with itself to make '''dihydrogen''' (H<sub>2</sub>). Dihydrogen is very [[:wikt:stable|stable]] because of its high [[bond-dissociation energy]] of 435.7 kJ/mol.<ref>{{cite book | editor-last = Lide | editor-first = David R. | date = 2006 | title = CRC Handbook of Chemistry and Physics | page = | pages = | edition = 87th | publisher = [[CRC Press]] | location = Boca Raton, FL | isbn = 0-8493-0487-3 }}</ref> At [[Standard temperature and pressure|normal temperature and pressure]], hydrogen gas (H<sub>2</sub>) has no [[Colour|color]], smell, or [[taste]].<ref name=":1">{{Cite web|title=Hydrogen Fundamentals|url=http://www.hysafe.org/download/997|access-date=2024-05-30|website=hysafe/org|archive-date=2024-01-28|archive-url=https://web.archive.org/web/20240128030340/http://www.hysafe.org/download/997|url-status=dead}}</ref> It is also not [[Poison|poisonous]]. This is because it is a [[nonmetal]] and burns very easily.{{Cn|date=May 2024}} Hydrogen gas at this state also has low [[density]] and is not [[Corrosive substance|corrosive]].<ref name=":1" /> === Combustion === [[Molecule|Molecular]] hydrogen is [[:wikt:flammable|flammable]] and [[Chemical reaction|reacts]] with [[oxygen]]: 2 H<sub>2</sub>(g) + O<sub>2</sub>(g) → 2 H<sub>2</sub>O(l) + 572 kJ (286 kJ/mol) At [[Temperature|temperatures]] higher than 500 °[[Celsius|C]], hydrogen suddenly burns in air. This is called hydrogen [[autoignition temperature]].<ref>{{cite book|url=https://books.google.com/books?id=-CRRJBVv5d0C&pg=PA402|title=A Comprehensive Guide to the Hazardous Properties of Chemical Substances|last=Patnaik|first=P.|date=2007|publisher=Wiley-Interscience|isbn=978-0-471-71458-3|page=402|access-date=3 September 2020|archive-url=https://web.archive.org/web/20210126131413/https://books.google.com/books?id=-CRRJBVv5d0C&pg=PA402|archive-date=26 January 2021|url-status=live}}</ref> === Compounds === While hydrogen [[gas]] in its natural form is not [[Reactivity (chemistry)|reactive]], it does form [[Chemical compound|compounds]] with many elements, especially [[halogen]]s, which are very [[Electronegativity|electronegative]], meaning they want an [[electron]] very badly. Hydrogen also forms massive [[:wikt:array|arrays]] with [[carbon]] [[atom]]s, forming [[hydrocarbon]]s. The [[:wikt:study|study]] of the properties of hydrocarbons is known as [[organic chemistry]]. The H<sup>-</sup> [[anion]] (negatively [[Electric charge|charged]] atom) is named a [[hydride]], though the word is not commonly used. An example of a hydride is [[lithium hydride]] (LiH), which is used as a "[[spark plug]]" in [[nuclear weapons]]. === Acids === [[Acid]]s [[Dissolution|dissolved]] in water normally [[:wikt:contain|contain]] high levels of hydrogen [[ion]]s, in other words, free [[proton]]s. Their level is generally used to [[:wikt:determine|determine]] its [[pH]], that is, the [[:wikt:content|content]] of hydrogen ions in a volume. For example, [[hydrochloric acid]], found in people's stomachs, can [[Dissociation (chemistry)|dissociate]] into a [[chloride]] anion and a free proton, and the property of the free proton is how it can digest food by [[Corrosion|corroding]] it. Though uncommon on Earth, the H<sub>3</sub><sup>+</sup> [[cation]] is one of the most common ions in the universe. === Isotopes === {{main|Isotopes of hydrogen}} Hydrogen has 7 known isotopes, two of which are stable (<sup>1</sup>H and <sup>2</sup>H), which are commonly named [[protium]] and [[deuterium]]. The isotope <sup>3</sup>H is known as [[tritium]], has a [[Half-life (element)|half-life]] of 12.33 years, and is produced in small amounts by [[cosmic ray]]s. The 4 isotopes left have half-lives on the scale of [[Orders of magnitude (time)#Seconds|yoctoseconds]]. == Hydrogen in nature == In its natural form on Earth, hydrogen is generally a [[gas]]. Hydrogen is also one of the parts that make up a [[water]] molecule. Hydrogen is important because it is the [[fuel]] that powers the [[Sun]] and other stars. Hydrogen makes up about 74% of the complete [[universe]].<ref name="ut">{{cite web|last=Cain|first=Fraser, ''Universe Today''|title=When was the first light in the universe?|url=http://phys.org/news/2016-11-universe.html|publisher=Phys.org|accessdate=29 November 2016|date=November 7, 2016|archive-date=18 December 2016|archive-url=https://web.archive.org/web/20161218150639/http://phys.org/news/2016-11-universe.html|url-status=live}}</ref> Natural hydrogen is normally made of two hydrogen [[atom]]s connected together. Scientists name these [[diatomic molecules]]. Hydrogen will have a [[chemical reaction]] when mixed with most other elements, though it has no [[color]] or [[Odor|smell]]. Natural hydrogen is very uncommon in the [[Earth]]'s [[Atmosphere of Earth|atmosphere]], because nearly all [[wikt:en:primordial|primordial]] hydrogen would have [[:wikt:escape|escaped]] into space because of its weight. In nature, it is generally in [[water]]. Hydrogen is also in all living things, as a part of the [[organic compound]]s that living things are made of. In addition, hydrogen atoms can join with [[carbon]] atoms to form [[hydrocarbon]]s. [[Petroleum]] and other [[fossil fuel]]s are made of these hydrocarbons and commonly used to make [[energy]]. Some other facts about hydrogen: * It is a gas at [[room temperature]] * It acts like a [[metal]] when it is solid. * It is the lightest element in the [[Universe]]. * It is the most common element in the Universe.<ref name="EIA">{{Cite web |url=http://www.eia.doe.gov/kids/energyfacts/sources/IntermediateHydrogen.html |title=EIA.doe.gov - What is Hydrogen? |access-date=2008-12-22 |archive-date=2009-02-05 |archive-url=https://web.archive.org/web/20090205025706/http://eia.doe.gov/kids/energyfacts/sources/IntermediateHydrogen.html |url-status=live }}</ref> * It burns or [[explosion|explodes]] at temperatures higher than 1000°F / 528°C, such as in [[fire]]. * It [[:wikt:glow|glows]] [[purple]] when it is in [[Plasma (physics)|plasma]] [[states of matter|state]].<ref>{{cite web|url=http://www.chemrec.se/Syngas_the_link_from_feedstock_to_synthetic_product.aspx|title=The magic of syngas|last=|first=|year=2012|work=chemrec.se|accessdate=7 March 2012|archive-date=20 April 2012|archive-url=https://web.archive.org/web/20120420074957/http://www.chemrec.se/Syngas_the_link_from_feedstock_to_synthetic_product.aspx|url-status=dead}}</ref> == History of Hydrogen == Hydrogen was first separated in 1671 by [[Robert Boyle]].<ref>Boyle, R. (1672). "Tracts written by the Honourable Robert Boyle containing new experiments, touching the relation betwixt flame and air..." London.</ref> In 1776, [[Henry Cavendish]] [[:wikt:identify|identified]] it as its own [[Elementary particle|element]] and named it "inflammable air". He saw in 1781 that burning it made water.<ref>Boyle, R. (1672). "Tracts written by the Honourable Robert Boyle containing new experiments, touching the relation betwixt flame and air..." London.</ref><ref name="Nostrand">{{cite encyclopedia| title=Hydrogen| encyclopedia=Van Nostrand's Encyclopedia of Chemistry| pages=797–799| publisher=Wylie-Interscience| year=2005| isbn=978-0-471-61525-5}}</ref><ref name="nbb">{{cite book| last=Emsley| first=John| title=Nature's Building Blocks| publisher=Oxford University Press| year=2001| location=Oxford| pages=183–191| isbn=978-0-19-850341-5}}</ref> [[File:Emissions Spectra.webm|thumb|Hydrogen Spectrum Test]] [[Antoine Lavoisier]] gave Hydrogen its name, from the [[Greek language|Greek]] word for [[water]], 'υδορ (read /HEEW-dor/) and gennen meaning to "produce"<ref>{{cite book|url=https://archive.org/details/guidetoelements00stwe|title=A Guide to the Elements|last=Stwertka|first=Albert|publisher=Oxford University Press|year=1996|isbn=978-0-19-508083-4|pages=[https://archive.org/details/guidetoelements00stwe/page/16 16–21]|url-access=registration}}</ref> as it forms water in a [[chemical reaction]] with [[oxygen]].<ref name="nbb2">{{cite book| last=Emsley| first=John| title=Nature's Building Blocks| publisher=Oxford University Press| year=2001| location=Oxford| pages=183–191| isbn=978-0-19-850341-5}}</ref> ===Big Bang (or the creation of our universe)=== Hydrogen did not<ref>https://www.astronomy.com/science/how-did-the-first-element-form-after-the-big-bang/. Retrieved 2024-10-21</ref> begin to form a second after the [[Big Bang]]. These hydrogens did not have any [[Neutron|neutrons]] or [[Electron|electrons]]. The first neutral hydrogen with an electron would not form until 380,000 years later during the [[Recombination (cosmology)|recombination epoch]], when the universe was cold enough for hydrogens to attract electrons.<ref>{{Cite web|title=Early Universe - NASA Science|url=https://science.nasa.gov/mission/webb/early-universe/|access-date=2024-05-30|website=science.nasa.gov|language=en-US}}</ref> == Uses of Hydrogen == The most common uses are in the [[petroleum]] industry and in making [[ammonia]] by the [[Haber process]]. Some is used in other places in the [[Chemical substance|chemical]] industry. A little of it is used as [[fuel]], for example in [[rocket]]s for [[spacecraft]]. Most of the hydrogen that people use comes from a [[chemical reaction]] between [[natural gas]] and [[steam]]. === Nuclear fusion === [[Nuclear fusion]] is a very powerful [[:wikt:source|source]] of [[energy]]. It depends on forcing [[atom]]s together to make [[helium]] and energy, as in a [[star]] like the [[Sun]], or in a [[Nuclear weapon|hydrogen bomb]]. This needs a large amount of energy to get started, and is not easy to do currently. A big [[:wikt:advantage|advantage]] over [[nuclear fission]], which is used in today's [[nuclear power]] stations, is that it makes less nuclear waste and does not use a poisonous and uncommon [[fuel]] like [[uranium]]. More than 600 million [[ton]]s of hydrogen undergo fusion every second on the Sun.<ref>{{cite web |url=http://www.iter.org/sci/whatisfusion |title=What is Fusion? |first= |last= |work=iter.org |year=2012 |accessdate=7 March 2012 |publisher=ITER Organization |archive-date=6 March 2012 |archive-url=https://web.archive.org/web/20120306200347/http://www.iter.org/sci/whatisfusion |url-status=live }}</ref><ref>{{cite web|url=http://helios.gsfc.nasa.gov/qa_sun.html|title=NASA's Cosmicopia|publisher=NASA|accessdate=28 February 2013|archive-date=6 November 2011|archive-url=https://web.archive.org/web/20111106095009/http://helios.gsfc.nasa.gov/qa_sun.html|url-status=dead}}</ref> === Using hydrogen === Hydrogen is mostly used in the petroleum industry, to change heavy petroleum parts into lighter, more useful ones. It is also used to make [[ammonia]]. Smaller amounts are burned as fuel. Most hydrogen is made by a reaction between [[natural gas]] and [[steam]]. The [[electrolysis of water]] breaks water into hydrogen and oxygen, using electricity. Burning hydrogen joins with oxygen molecules to make [[steam]] (natural water vapor). A [[fuel cell]] joins hydrogen with an oxygen [[molecule]], [[:wikt:release|releasing]] an electron as electricity. For these reasons, many people believe hydrogen power will replace other [[synthetic fuel]]s in the future. Hydrogen can also be burned to make heat for [[steam turbine]]s or [[internal combustion engine]]s. Like other synthetic fuels, hydrogen can be made from natural fuels such as [[coal]] or natural gas, or from electricity, and therefore represents a valuable addition to the [[Electric power transmission|power grid]]; in the same [[:wikt:role|role]] as [[natural gas]]. Such a grid and [[:wikt:infrastructure|infrastructure]] with [[fuel cell vehicle]]s is now [[:wikt:plan|planned]] by a number of countries, such as Japan, Korea and many European countries. This lets these countries [[:wikt:buy|buy]] less [[petroleum]], which is an [[:wikt:economic|economic]] advantage. The other advantage is that, used in a fuel cell or burned in a combustion engine as in a [[hydrogen car]], the engine does not make [[pollution]]. Only water, and a small amount of [[nitrogen oxide]]s, forms. == References == {{reflist}} == Other websites == * [https://en.citizendium.org/wiki/Hydrogen Hydrogen] - Citizendium {{Periodic Table}} {{authority control}} [[Category:Hydrogen]] </textarea><div class="templatesUsed"><div class="mw-templatesUsedExplanation"><p>Templates used on this page: </p></div><ul> <li><a href="/wiki/Template:!((" title="Template:!((">Template:!((</a> (<a href="/w/index.php?title=Template:!((&action=edit" title="Template:!((">view source</a>) (semi-protected)</li><li><a href="/wiki/Template:))!" title="Template:))!">Template:))!</a> (<a href="/w/index.php?title=Template:))!&action=edit" title="Template:))!">change</a>) </li><li><a href="/wiki/Template:Abbr" title="Template:Abbr">Template:Abbr</a> (<a href="/w/index.php?title=Template:Abbr&action=edit" title="Template:Abbr">view source</a>) (semi-protected)</li><li><a href="/wiki/Template:Authority_control" title="Template:Authority 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href="/wiki/Module:Citation/CS1/Configuration" title="Module:Citation/CS1/Configuration">Module:Citation/CS1/Configuration</a> (<a href="/w/index.php?title=Module:Citation/CS1/Configuration&action=edit" title="Module:Citation/CS1/Configuration">view source</a>) (protected)</li><li><a href="/wiki/Module:Citation/CS1/Date_validation" title="Module:Citation/CS1/Date validation">Module:Citation/CS1/Date validation</a> (<a href="/w/index.php?title=Module:Citation/CS1/Date_validation&action=edit" title="Module:Citation/CS1/Date validation">view source</a>) (protected)</li><li><a href="/wiki/Module:Citation/CS1/Identifiers" title="Module:Citation/CS1/Identifiers">Module:Citation/CS1/Identifiers</a> (<a href="/w/index.php?title=Module:Citation/CS1/Identifiers&action=edit" title="Module:Citation/CS1/Identifiers">view source</a>) (protected)</li><li><a href="/wiki/Module:Citation/CS1/Utilities" title="Module:Citation/CS1/Utilities">Module:Citation/CS1/Utilities</a> (<a 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title="Module:Engvar">Module:Engvar</a> (<a href="/w/index.php?title=Module:Engvar&action=edit" title="Module:Engvar">change</a>) </li><li><a href="/wiki/Module:Format_link" title="Module:Format link">Module:Format link</a> (<a href="/w/index.php?title=Module:Format_link&action=edit" title="Module:Format link">view source</a>) (semi-protected)</li><li><a href="/wiki/Module:Gapnum" title="Module:Gapnum">Module:Gapnum</a> (<a href="/w/index.php?title=Module:Gapnum&action=edit" title="Module:Gapnum">change</a>) </li><li><a href="/wiki/Module:Hatnote" title="Module:Hatnote">Module:Hatnote</a> (<a href="/w/index.php?title=Module:Hatnote&action=edit" title="Module:Hatnote">view source</a>) (semi-protected)</li><li><a href="/wiki/Module:Hatnote/styles.css" title="Module:Hatnote/styles.css">Module:Hatnote/styles.css</a> (<a href="/w/index.php?title=Module:Hatnote/styles.css&action=edit" title="Module:Hatnote/styles.css">view source</a>) (semi-protected)</li><li><a 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