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class="page-actions-menu__list-item"> <a role="button" href="#p-lang" data-mw="interface" data-event-name="menu.languages" title="Language" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet language-selector"> Language </a> </li> <li id="page-actions-watch" class="page-actions-menu__list-item"> <a role="button" id="ca-watch" href="/w/index.php?title=Special:UserLogin&returnto=Sulfur" data-event-name="menu.watch" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet menu__item--page-actions-watch"> Watch </a> </li> <li id="page-actions-edit" class="page-actions-menu__list-item"> <a role="button" id="ca-edit" href="/w/index.php?title=Sulfur&action=edit" data-event-name="menu.edit" data-mw="interface" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet edit-page menu__item--page-actions-edit"> Edit </a> </li> </ul> </nav>  <div id="mw-content-subtitle"><div id="mw-fr-revision-messages"><div class="cdx-message mw-fr-message-box cdx-message--inline cdx-message--notice mw-fr-mobile-message-inline"><div class="cdx-message__content">This is the <a href="/wiki/Wikipedia:Pending_changes" title="Wikipedia:Pending changes">latest accepted revision</a>, <a class="external text" href="https://en.wikipedia.org/w/index.php?title=Special:Log&type=review&page=Special:Badtitle/Message">reviewed</a> on 21 November 2024.</div></div></div></div> </div> <div id="bodyContent" class="content"> <div id="mw-content-text" class="mw-body-content"><script>function mfTempOpenSection(id){var block=document.getElementById("mf-section-"+id);block.className+=" open-block";block.previousSibling.className+=" open-block";}</script><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><section class="mf-section-0" id="mf-section-0"> <style data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">This article is about the chemical element. For other uses, see <a href="/wiki/Sulfur_(disambiguation)" class="mw-disambig" title="Sulfur (disambiguation)">Sulfur (disambiguation)</a>.</div> <style data-mw-deduplicate="TemplateStyles:r1257001546">.mw-parser-output .infobox-subbox{padding:0;border:none;margin:-3px;width:auto;min-width:100%;font-size:100%;clear:none;float:none;background-color:transparent}.mw-parser-output .infobox-3cols-child{margin:auto}.mw-parser-output .infobox .navbar{font-size:100%}@media screen{html.skin-theme-clientpref-night .mw-parser-output .infobox-full-data:not(.notheme)>div:not(.notheme)[style]{background:#1f1f23!important;color:#f8f9fa}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .infobox-full-data:not(.notheme) div:not(.notheme){background:#1f1f23!important;color:#f8f9fa}}@media(min-width:640px){body.skin--responsive .mw-parser-output .infobox-table{display:table!important}body.skin--responsive .mw-parser-output .infobox-table>caption{display:table-caption!important}body.skin--responsive .mw-parser-output .infobox-table>tbody{display:table-row-group}body.skin--responsive .mw-parser-output .infobox-table tr{display:table-row!important}body.skin--responsive .mw-parser-output .infobox-table th,body.skin--responsive .mw-parser-output .infobox-table td{padding-left:inherit;padding-right:inherit}}</style><style data-mw-deduplicate="TemplateStyles:r1158442001">body.skin-minerva .mw-parser-output .infobox-full-data>.wikitable,body.skin-minerva .mw-parser-output .infobox .periodictable{display:table}body.skin-minerva .mw-parser-output .infobox-full-data{width:calc(100% - 20px)}body.skin-minerva .mw-parser-output .infobox-full-data>div{max-width:100%;overflow:auto}body.skin-minerva .mw-parser-output .infobox caption{display:table-caption}</style>Sulfur (also spelled sulphur in <a href="/wiki/British_English" title="British English">British English</a>) is a <a href="/wiki/Chemical_element" title="Chemical element">chemical element</a>; it has <a href="/wiki/Symbol_(chemistry)" class="mw-redirect" title="Symbol (chemistry)">symbol</a> S and <a href="/wiki/Atomic_number" title="Atomic number">atomic number</a> 16. It is <a href="/wiki/Abundance_of_the_chemical_elements" title="Abundance of the chemical elements">abundant</a>, <a href="/wiki/Polyvalency_(chemistry)" title="Polyvalency (chemistry)">multivalent</a> and <a href="/wiki/Nonmetal_(chemistry)" class="mw-redirect" title="Nonmetal (chemistry)">nonmetallic</a>. Under <a href="/wiki/Standard_conditions_for_temperature_and_pressure" class="mw-redirect" title="Standard conditions for temperature and pressure">normal conditions</a>, sulfur atoms form <a href="/wiki/Octasulfur" title="Octasulfur">cyclic octatomic molecules</a> with the chemical formula <a href="/wiki/Octasulfur" title="Octasulfur">S8</a>. Elemental sulfur is a bright yellow, <a href="/wiki/Crystal" title="Crystal">crystalline</a> solid at <a href="/wiki/Room_temperature" title="Room temperature">room temperature</a>. <table class="infobox"><caption class="infobox-title">Sulfur, 16S</caption><tbody><tr><td colspan="2" class="infobox-image"><a href="/wiki/File:Sulfur_-_El_Desierto_mine,_San_Pablo_de_Napa,_Daniel_Campos_Province,_Potos%C3%AD,_Bolivia.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/88/Sulfur_-_El_Desierto_mine%2C_San_Pablo_de_Napa%2C_Daniel_Campos_Province%2C_Potos%C3%AD%2C_Bolivia.jpg/220px-Sulfur_-_El_Desierto_mine%2C_San_Pablo_de_Napa%2C_Daniel_Campos_Province%2C_Potos%C3%AD%2C_Bolivia.jpg" decoding="async" width="220" height="183" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/88/Sulfur_-_El_Desierto_mine%2C_San_Pablo_de_Napa%2C_Daniel_Campos_Province%2C_Potos%C3%AD%2C_Bolivia.jpg/330px-Sulfur_-_El_Desierto_mine%2C_San_Pablo_de_Napa%2C_Daniel_Campos_Province%2C_Potos%C3%AD%2C_Bolivia.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/88/Sulfur_-_El_Desierto_mine%2C_San_Pablo_de_Napa%2C_Daniel_Campos_Province%2C_Potos%C3%AD%2C_Bolivia.jpg/440px-Sulfur_-_El_Desierto_mine%2C_San_Pablo_de_Napa%2C_Daniel_Campos_Province%2C_Potos%C3%AD%2C_Bolivia.jpg 2x" data-file-width="6000" data-file-height="5000"></a></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Sulfur</th></tr><tr><th scope="row" class="infobox-label">Alternative name</th><td class="infobox-data">Sulphur (British spelling)</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Allotropy" title="Allotropy">Allotropes</a></th><td class="infobox-data">see <a href="/wiki/Allotropes_of_sulfur" title="Allotropes of sulfur">Allotropes of sulfur</a></td></tr><tr><th scope="row" class="infobox-label">Appearance</th><td class="infobox-data">Lemon yellow <a href="/wiki/Sintering" title="Sintering">sintered</a> microcrystals</td></tr><tr><td colspan="2" class="infobox-full-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1257001546"></td></tr><tr><th colspan="2" class="infobox-header" style="text-align: left; color:inherit; background: transparent;"><a href="/wiki/Standard_atomic_weight" title="Standard atomic weight">Standard atomic weight</a> <style data-mw-deduplicate="TemplateStyles:r886047488">.mw-parser-output .nobold{font-weight:normal}</style>Ar°(S)</th></tr><tr><th scope="row" class="infobox-label"></th><td class="infobox-data"><style data-mw-deduplicate="TemplateStyles:r1126788409">.mw-parser-output .plainlist ol,.mw-parser-output .plainlist ul{line-height:inherit;list-style:none;margin:0;padding:0}.mw-parser-output .plainlist ol li,.mw-parser-output .plainlist ul li{margin-bottom:0}</style><div class="plainlist"><ul><li>[32.059, 32.076]<a href="#cite_note-1">[1]</a></li><li>32.06±0.02 (<a href="/wiki/Standard_atomic_weight#Abridged_atomic_weight" title="Standard atomic weight">abridged</a>)<a href="#cite_note-CIAAW2021-2">[2]</a></li></ul></div></td></tr><tr style="display:none"><td colspan="2"> </td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Sulfur in the <a href="/wiki/Periodic_table" title="Periodic table">periodic table</a></th></tr><tr><td colspan="2" class="infobox-full-data"> <table class="wikitable" style="text-align:center; width:100%; margin:0; background:#f8f8f8; color:black;"> <tbody><tr> <td> <table class="periodictable" style="margin:0 auto"> <tbody><tr> <td style="border:none; width:5px"><div style="background-color:transparent; color:inherit; margin:0; padding:0; text-align:center; border:none;"> <table style="empty-cells:hidden; border:none; padding:0; border-spacing:1px; border-collapse:separate; margin:0;"> <tbody><tr> <td style="border:none;padding:0;"><a href="/wiki/Hydrogen" title="Hydrogen">Hydrogen</a> </td> <td colspan="30" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Helium" title="Helium">Helium</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Lithium" title="Lithium">Lithium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Beryllium" title="Beryllium">Beryllium</a> </td> <td colspan="24" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Boron" title="Boron">Boron</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Carbon" title="Carbon">Carbon</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nitrogen" title="Nitrogen">Nitrogen</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Oxygen" title="Oxygen">Oxygen</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Fluorine" title="Fluorine">Fluorine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neon" title="Neon">Neon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Sodium" title="Sodium">Sodium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Magnesium" title="Magnesium">Magnesium</a> </td> <td colspan="24" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Aluminium" title="Aluminium">Aluminium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Silicon" title="Silicon">Silicon</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Phosphorus" title="Phosphorus">Phosphorus</a> </td> <td style="border:none;padding:0;"><a class="mw-selflink selflink">Sulfur</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Chlorine" title="Chlorine">Chlorine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Argon" title="Argon">Argon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Potassium" title="Potassium">Potassium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Calcium" title="Calcium">Calcium</a> </td> <td colspan="14" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Scandium" title="Scandium">Scandium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Titanium" title="Titanium">Titanium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Vanadium" title="Vanadium">Vanadium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Chromium" title="Chromium">Chromium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Manganese" title="Manganese">Manganese</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iron" title="Iron">Iron</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cobalt" title="Cobalt">Cobalt</a> </td> <td style="border:none;padding:0;"><a 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href="/wiki/Actinium" title="Actinium">Actinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thorium" title="Thorium">Thorium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Protactinium" title="Protactinium">Protactinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Uranium" title="Uranium">Uranium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neptunium" title="Neptunium">Neptunium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Plutonium" title="Plutonium">Plutonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Americium" title="Americium">Americium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Curium" title="Curium">Curium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Berkelium" title="Berkelium">Berkelium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Californium" title="Californium">Californium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Einsteinium" title="Einsteinium">Einsteinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Fermium" title="Fermium">Fermium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Mendelevium" title="Mendelevium">Mendelevium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nobelium" title="Nobelium">Nobelium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lawrencium" title="Lawrencium">Lawrencium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rutherfordium" title="Rutherfordium">Rutherfordium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Dubnium" title="Dubnium">Dubnium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Seaborgium" title="Seaborgium">Seaborgium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bohrium" title="Bohrium">Bohrium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Hassium" title="Hassium">Hassium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Meitnerium" title="Meitnerium">Meitnerium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Darmstadtium" title="Darmstadtium">Darmstadtium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Roentgenium" title="Roentgenium">Roentgenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Copernicium" title="Copernicium">Copernicium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nihonium" title="Nihonium">Nihonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Flerovium" title="Flerovium">Flerovium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Moscovium" title="Moscovium">Moscovium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Livermorium" title="Livermorium">Livermorium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tennessine" title="Tennessine">Tennessine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Oganesson" title="Oganesson">Oganesson</a> </td></tr></tbody></table> </div> </td> <td style="vertical-align:middle; text-align:center; font-size:90%; line-height:100%; width:10px; border:none;"><a href="/wiki/Oxygen" title="Oxygen">O</a> ↑ S ↓ <a href="/wiki/Selenium" title="Selenium">Se</a> </td></tr> <tr> <td colspan="2" class="nowrap" style="text-align:center; font-size:90%; line-height:100%; padding-top:0; padding-bottom:1px; border:none;"><a href="/wiki/Phosphorus" title="Phosphorus">phosphorus</a> ← sulfur → <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> </td></tr></tbody></table> </td></tr></tbody></table></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Atomic_number" title="Atomic number">Atomic number</a> (Z)</th><td class="infobox-data">16</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Group_(periodic_table)" title="Group (periodic table)">Group</a></th><td class="infobox-data"><a href="/wiki/Chalcogen" title="Chalcogen">group 16 (chalcogens)</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Period_(periodic_table)" title="Period (periodic table)">Period</a></th><td class="infobox-data"><a href="/wiki/Period_3_element" title="Period 3 element">period 3</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Block_(periodic_table)" title="Block (periodic table)">Block</a></th><td class="infobox-data"> <a href="/wiki/Block_(periodic_table)#p-block" title="Block (periodic table)">p-block</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electron_configuration" title="Electron configuration">Electron configuration</a></th><td class="infobox-data">[<a href="/wiki/Neon" title="Neon">Ne</a>] 3s2 3p4</td></tr><tr><th scope="row" class="infobox-label">Electrons per shell</th><td class="infobox-data">2, 8, 6</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Physical properties</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Phase_(matter)" title="Phase (matter)">Phase</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r886047488">at <a href="/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure">STP</a></th><td class="infobox-data"><a href="/wiki/Solid" title="Solid">solid</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Melting_point" title="Melting point">Melting point</a></th><td class="infobox-data">alpha (α-S8): 388.36 <a href="/wiki/Kelvin" title="Kelvin">K</a> (115.21 °C, 239.38 °F) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Boiling_point" title="Boiling point">Boiling point</a></th><td class="infobox-data">717.8 K (444.6 °C, 832.3 °F) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Density" title="Density">Density</a> (near <a href="/wiki/Room_temperature" title="Room temperature">r.t.</a>)</th><td class="infobox-data">alpha (α-S8): 2.07 g/cm3 beta (β-S8): 1.96 g/cm3 gamma (γ-S8): 1.92 g/cm3 </td></tr><tr><th scope="row" class="infobox-label">when liquid (at <a href="/wiki/Melting_point" title="Melting point">m.p.</a>)</th><td class="infobox-data">1.819 g/cm3 </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Critical_point_(thermodynamics)" title="Critical point (thermodynamics)">Critical point</a></th><td class="infobox-data">1314 K, 20.7 MPa </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Enthalpy_of_fusion" title="Enthalpy of fusion">Heat of fusion</a></th><td class="infobox-data">beta (β-S8): 1.727 <a href="/wiki/Kilojoule_per_mole" class="mw-redirect" title="Kilojoule per mole">kJ/mol</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Enthalpy_of_vaporization" title="Enthalpy of vaporization">Heat of vaporization</a></th><td class="infobox-data">beta (β-S8): 45 kJ/mol </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Molar_heat_capacity" title="Molar heat capacity">Molar heat capacity</a></th><td class="infobox-data">22.75 J/(mol·K) </td></tr><tr><td colspan="2" class="infobox-full-data"><a href="/wiki/Vapor_pressure" title="Vapor pressure">Vapor pressure</a><div style="position:relative; margin:0 auto; padding:0; text-align:initial; width:-moz-fit-content;width:-webkit-fit-content;width:fit-content;"> <table class="wikitable" style="text-align:center; font-size:90%; border-collapse:collapse; margin:0"> <tbody><tr> <th><abbr title="Pressure">P</abbr> (Pa) </th> <th>1 </th> <th>10 </th> <th>100 </th> <th>1 k </th> <th>10 k </th> <th>100 k </th></tr> <tr> <th>at <abbr title="Temperature">T</abbr> (K) </th> <td>375 </td> <td>408 </td> <td>449 </td> <td>508 </td> <td>591 </td> <td>717 </td></tr></tbody></table> </div></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Atomic properties</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Oxidation_state" title="Oxidation state">Oxidation states</a></th><td class="infobox-data">common: −2, +2, +4, +6 −1,<a href="#cite_note-GE28-3">[3]</a> 0, +1,<a href="#cite_note-GE28-3">[3]</a> +3,<a href="#cite_note-GE28-3">[3]</a> +5<a href="#cite_note-GE28-3">[3]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electronegativity" title="Electronegativity">Electronegativity</a></th><td class="infobox-data">Pauling scale: 2.58 </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Ionization_energy" title="Ionization energy">Ionization energies</a></th><td class="infobox-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>1st: 999.6 kJ/mol </li><li>2nd: 2252 kJ/mol </li><li>3rd: 3357 kJ/mol </li><li>(<a href="/wiki/Molar_ionization_energies_of_the_elements#sulfur" title="Molar ionization energies of the elements">more</a>) </li></ul></div></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Covalent_radius" title="Covalent radius">Covalent radius</a></th><td class="infobox-data">105±3 <a href="/wiki/Picometre" title="Picometre">pm</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Van_der_Waals_radius" title="Van der Waals radius">Van der Waals radius</a></th><td class="infobox-data">180 pm </td></tr><tr><td colspan="2" class="infobox-full-data"><figure class="mw-default-size mw-halign-center" typeof="mw:File/Frameless"><a href="/wiki/File:Sulfur_spectrum_visible.png" class="mw-file-description"><img alt="Color lines in a spectral range" src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d4/Sulfur_spectrum_visible.png/240px-Sulfur_spectrum_visible.png" decoding="async" width="240" height="41" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d4/Sulfur_spectrum_visible.png/360px-Sulfur_spectrum_visible.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d4/Sulfur_spectrum_visible.png/480px-Sulfur_spectrum_visible.png 2x" data-file-width="7430" data-file-height="1280"></a><figcaption></figcaption></figure><a href="/wiki/Spectral_line" title="Spectral line">Spectral lines</a> of sulfur</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Other properties</th></tr><tr><th scope="row" class="infobox-label">Natural occurrence</th><td class="infobox-data"><a href="/wiki/Primordial_nuclide" title="Primordial nuclide">primordial</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Crystal_structure" title="Crystal structure">Crystal structure</a></th><td class="infobox-data">alpha (α-S8): <a href="/wiki/Orthorhombic_crystal_system" title="Orthorhombic crystal system">orthorhombic</a> (<a href="/wiki/Pearson_symbol" title="Pearson symbol">oF128</a>)</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Lattice_constant" title="Lattice constant">Lattice constants</a></th><td class="infobox-data"><div style="float:right;"><a href="/wiki/File:Orthorhombic.svg" class="mw-file-description"><img alt="Orthorhombic crystal structure for alpha (α-S8): sulfur" src="//upload.wikimedia.org/wikipedia/commons/thumb/d/dd/Orthorhombic.svg/50px-Orthorhombic.svg.png" decoding="async" width="50" height="66" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/dd/Orthorhombic.svg/75px-Orthorhombic.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/dd/Orthorhombic.svg/100px-Orthorhombic.svg.png 2x" data-file-width="108" data-file-height="142"></a></div>a = 1.0460 nm b = 1.2861 nm c = 2.4481 nm (at 20 °C)<a href="#cite_note-Arblaster_2018-4">[4]</a></td></tr><tr><th scope="row" class="infobox-label">Crystal structure</th><td class="infobox-data">beta (β-S8): <a href="/wiki/Monoclinic_crystal_system" title="Monoclinic crystal system">monoclinic</a> (<a href="/wiki/Pearson_symbol" title="Pearson symbol">mP48</a>)</td></tr><tr><th scope="row" class="infobox-label">Lattice constants</th><td class="infobox-data"><div style="float:right;"><a href="/wiki/File:Monoclinic.svg" class="mw-file-description"><img alt="Monoclinic crystal structure for beta (β-S8): sulfur" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f4/Monoclinic.svg/50px-Monoclinic.svg.png" decoding="async" width="50" height="63" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f4/Monoclinic.svg/75px-Monoclinic.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f4/Monoclinic.svg/100px-Monoclinic.svg.png 2x" data-file-width="114" data-file-height="143"></a></div>a = 1.0923 nm b = 1.0851 nm c = 1.0787 nm β = 95.905° (at 20 °C)<a href="#cite_note-Arblaster_2018-4">[4]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Thermal_conductivity" class="mw-redirect" title="Thermal conductivity">Thermal conductivity</a></th><td class="infobox-data">0.205 W/(m⋅K) (amorphous)</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electrical_resistivity_and_conductivity" title="Electrical resistivity and conductivity">Electrical resistivity</a></th><td class="infobox-data">2×1015 Ω⋅m (at 20 °C) (amorphous)</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Magnetism" title="Magnetism">Magnetic ordering</a></th><td class="infobox-data"><a href="/wiki/Diamagnetic" class="mw-redirect" title="Diamagnetic">diamagnetic</a><a href="#cite_note-magnet-5">[5]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Magnetic_susceptibility" title="Magnetic susceptibility">Molar magnetic susceptibility</a></th><td class="infobox-data">alpha (α-S8): −15.5×10−6 cm3/mol (298 K)<a href="#cite_note-6">[6]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Bulk_modulus" title="Bulk modulus">Bulk modulus</a></th><td class="infobox-data">7.7 GPa </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Mohs_scale_of_mineral_hardness" class="mw-redirect" title="Mohs scale of mineral hardness">Mohs hardness</a></th><td class="infobox-data">2.0 </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/CAS_Registry_Number" title="CAS Registry Number">CAS Number</a></th><td class="infobox-data">7704-34-9 </td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">History</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Timeline_of_chemical_element_discoveries" class="mw-redirect" title="Timeline of chemical element discoveries">Discovery</a></th><td class="infobox-data">before 2000 BCE<a href="#cite_note-7">[7]</a></td></tr><tr><th scope="row" class="infobox-label">Recognized as an <a href="/wiki/Chemical_element" title="Chemical element">element</a> by</th><td class="infobox-data"><a href="/wiki/Antoine_Lavoisier" title="Antoine Lavoisier">Antoine Lavoisier</a> (1777)</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c"><a href="/wiki/Isotopes_of_sulfur" title="Isotopes of sulfur">Isotopes of sulfur</a><style data-mw-deduplicate="TemplateStyles:r1129693374">.mw-parser-output .hlist dl,.mw-parser-output .hlist ol,.mw-parser-output .hlist ul{margin:0;padding:0}.mw-parser-output .hlist dd,.mw-parser-output .hlist dt,.mw-parser-output .hlist li{margin:0;display:inline}.mw-parser-output .hlist.inline,.mw-parser-output .hlist.inline dl,.mw-parser-output .hlist.inline ol,.mw-parser-output .hlist.inline ul,.mw-parser-output .hlist dl dl,.mw-parser-output .hlist dl ol,.mw-parser-output .hlist dl ul,.mw-parser-output .hlist ol dl,.mw-parser-output .hlist ol ol,.mw-parser-output .hlist ol ul,.mw-parser-output .hlist ul dl,.mw-parser-output .hlist ul ol,.mw-parser-output .hlist ul ul{display:inline}.mw-parser-output .hlist .mw-empty-li{display:none}.mw-parser-output .hlist dt::after{content:": "}.mw-parser-output .hlist dd::after,.mw-parser-output .hlist li::after{content:" · ";font-weight:bold}.mw-parser-output .hlist dd:last-child::after,.mw-parser-output .hlist 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.navbar a>span,.mw-parser-output .navbar a>abbr{text-decoration:inherit}.mw-parser-output .navbar-mini abbr{font-variant:small-caps;border-bottom:none;text-decoration:none;cursor:inherit}.mw-parser-output .navbar-ct-full{font-size:114%;margin:0 7em}.mw-parser-output .navbar-ct-mini{font-size:114%;margin:0 4em}html.skin-theme-clientpref-night .mw-parser-output .navbar li a abbr{color:var(--color-base)!important}@media(prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .navbar li a abbr{color:var(--color-base)!important}}@media print{.mw-parser-output .navbar{display:none!important}}</style><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Infobox_sulfur_isotopes" title="Template:Infobox sulfur isotopes"><abbr title="View this template">v</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_sulfur_isotopes" title="Special:EditPage/Template:Infobox sulfur isotopes"><abbr title="Edit this template">e</abbr></a></li></ul></div></th></tr><tr><td colspan="2" class="infobox-full-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1257001546"></td></tr><tr><td colspan="2" class="infobox-full-data"> <table class="wikitable" style="text-align: center; vertical-align: middle; width: 100%; border-collapse: collapse; margin: 0; padding: 0;"> <tbody><tr> <th colspan="3">Main isotopes </th> <th colspan="2"><a href="/wiki/Radioactive_decay" title="Radioactive decay">Decay</a> </th></tr> <tr> <th> </th> <th style="padding: 0.1em;"><a href="/wiki/Natural_abundance" title="Natural abundance">abundance</a> </th> <th style="padding: 0.1em;"><a href="/wiki/Half-life" title="Half-life">half-life</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r886047488">(t1/2) </th> <th style="padding: 0.1em;"><a href="/wiki/Radioactive_decay#Types_of_decay" title="Radioactive decay">mode</a> </th> <th style="padding: 0.1em;"><a href="/wiki/Decay_product" title="Decay product">product</a> </th></tr> <tr> <th rowspan="1" style="vertical-align: top;">32S </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">94.8% </td> <td rowspan="1" colspan="3" style="vertical-align: top; text-align: left;"><a href="/wiki/Stable_isotope" class="mw-redirect" title="Stable isotope">stable</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">33S </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">0.760% </td> <td rowspan="1" colspan="3" style="vertical-align: top; text-align: left;">stable </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">34S </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">4.37% </td> <td rowspan="1" colspan="3" style="vertical-align: top; text-align: left;">stable </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">35S </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;"><a href="/wiki/Trace_radioisotope" title="Trace radioisotope">trace</a> </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">87.37 d </td> <td style="text-align: left; vertical-align: top;"><a href="/wiki/Beta_minus_decay" class="mw-redirect" title="Beta minus decay">β−</a> </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Chlorine-35" class="mw-redirect" title="Chlorine-35">35Cl</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">36S </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">0.02% </td> <td rowspan="1" colspan="3" style="vertical-align: top; text-align: left;">stable </td></tr></tbody></table><div style="text-align:left; padding-left:0.5em; background: #F8F9FA;">34S abundances vary greatly (between 3.96 and 4.77 percent) in natural samples.</div></td></tr><tr style="display:none"><td colspan="2"> </td></tr><tr><td colspan="2" class="infobox-below noprint" style="color:inherit; background:#fdff8c"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/9/96/Symbol_category_class.svg/16px-Symbol_category_class.svg.png" decoding="async" width="16" height="16" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/96/Symbol_category_class.svg/23px-Symbol_category_class.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/96/Symbol_category_class.svg/31px-Symbol_category_class.svg.png 2x" data-file-width="180" data-file-height="185"> <a href="/wiki/Category:Sulfur" title="Category:Sulfur">Category: Sulfur</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist"><ul><li class="nv-view"><a href="/wiki/Template:Infobox_sulfur" title="Template:Infobox sulfur">view</a></li><li class="nv-talk"><a href="/wiki/Template_talk:Infobox_sulfur" title="Template talk:Infobox sulfur">talk</a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_sulfur" title="Special:EditPage/Template:Infobox sulfur">edit</a></li></ul></div> | <a href="/wiki/List_of_data_references_for_chemical_elements" title="List of data references for chemical elements">references</a></td></tr></tbody></table> Sulfur is the tenth most abundant element by mass in the universe and the fifth most common on Earth. Though sometimes found in pure, <a href="/wiki/Native_element_minerals" class="mw-redirect" title="Native element minerals">native</a> form, sulfur on Earth usually occurs as <a href="/wiki/Sulfide_minerals" class="mw-redirect" title="Sulfide minerals">sulfide</a> and <a href="/wiki/Sulfate_minerals" class="mw-redirect" title="Sulfate minerals">sulfate minerals</a>. Being abundant in native form, sulfur was known in ancient times, being mentioned for its uses in <a href="/wiki/Outline_of_ancient_India" title="Outline of ancient India">ancient India</a>, <a href="/wiki/Ancient_Greece" title="Ancient Greece">ancient Greece</a>, <a href="/wiki/History_of_China#Ancient_China" title="History of China">China</a>, and <a href="/wiki/Ancient_Egypt" title="Ancient Egypt">ancient Egypt</a>. Historically and in literature sulfur is also called brimstone,<a href="#cite_note-Greenwood-1997a-8">[8]</a> which means "burning stone".<a href="#cite_note-9">[9]</a> Almost all elemental sulfur is produced as a byproduct of removing sulfur-containing contaminants from <a href="/wiki/Natural_gas" title="Natural gas">natural gas</a> and <a href="/wiki/Petroleum" title="Petroleum">petroleum</a>.<a href="#cite_note-Knight-2014-10">[10]</a><a href="#cite_note-BBC_Elements-2014-11">[11]</a> The greatest commercial use of the element is the production of <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> for sulfate and phosphate <a href="/wiki/Fertilizer" title="Fertilizer">fertilizers</a>, and other chemical processes. Sulfur is used in <a href="/wiki/Match" title="Match">matches</a>, <a href="/wiki/Insecticide" title="Insecticide">insecticides</a>, and <a href="/wiki/Fungicide" title="Fungicide">fungicides</a>. Many sulfur compounds are odoriferous, and the smells of odorized natural gas, <a href="/wiki/Skunk" title="Skunk">skunk</a> scent, <a href="/wiki/Bad_breath" title="Bad breath">bad breath</a>, <a href="/wiki/Grapefruit" title="Grapefruit">grapefruit</a>, and <a href="/wiki/Garlic" title="Garlic">garlic</a> are due to <a href="/wiki/Organosulfur" class="mw-redirect" title="Organosulfur">organosulfur</a> compounds. <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">Hydrogen sulfide</a> gives the characteristic odor to rotting eggs and other biological processes. Sulfur is an <a href="/wiki/Mineral_(nutrient)" title="Mineral (nutrient)">essential element</a> for all life, almost always in the form of <a href="/wiki/Organosulfur_compounds" class="mw-redirect" title="Organosulfur compounds">organosulfur compounds</a> or metal sulfides. <a href="/wiki/Amino_acid" title="Amino acid">Amino acids</a> (two <a href="/wiki/Proteinogenic_amino_acid" title="Proteinogenic amino acid">proteinogenic</a>: <a href="/wiki/Cysteine" title="Cysteine">cysteine</a> and <a href="/wiki/Methionine" title="Methionine">methionine</a>, and many other <a href="/wiki/Non-proteinogenic_amino_acids" title="Non-proteinogenic amino acids">non-coded</a>: <a href="/wiki/Cystine" title="Cystine">cystine</a>, <a href="/wiki/Taurine" title="Taurine">taurine</a>, etc.) and two vitamins (<a href="/wiki/Biotin" title="Biotin">biotin</a> and <a href="/wiki/Thiamine" title="Thiamine">thiamine</a>) are organosulfur compounds crucial for life. Many <a href="/wiki/Cofactor_(biochemistry)" title="Cofactor (biochemistry)">cofactors</a> also contain sulfur, including <a href="/wiki/Glutathione" title="Glutathione">glutathione</a>, and <a href="/wiki/Iron%E2%80%93sulfur_protein" title="Iron–sulfur protein">iron–sulfur proteins</a>. <a href="/wiki/Disulfide" title="Disulfide">Disulfides</a>, S–S bonds, confer mechanical strength and insolubility of the (among others) protein <a href="/wiki/Keratin" title="Keratin">keratin</a>, found in outer skin, hair, and feathers. Sulfur is one of the core chemical elements needed for <a href="/wiki/Biochemical" class="mw-redirect" title="Biochemical">biochemical</a> functioning and is an elemental <a href="/wiki/Macronutrient" class="mw-redirect" title="Macronutrient">macronutrient</a> for all living organisms. <div id="toc" class="toc" role="navigation" aria-labelledby="mw-toc-heading"><input type="checkbox" role="button" id="toctogglecheckbox" class="toctogglecheckbox" style="display:none"><div class="toctitle" lang="en" dir="ltr"><h2 id="mw-toc-heading">Contents</h2><label class="toctogglelabel" for="toctogglecheckbox"></label></div> <ul> <li class="toclevel-1 tocsection-1"><a href="#Characteristics">1 Characteristics</a> <ul> <li class="toclevel-2 tocsection-2"><a href="#Physical_properties">1.1 Physical properties</a></li> <li class="toclevel-2 tocsection-3"><a href="#Chemical_properties">1.2 Chemical properties</a></li> <li class="toclevel-2 tocsection-4"><a href="#Allotropes">1.3 Allotropes</a></li> <li class="toclevel-2 tocsection-5"><a href="#Isotopes">1.4 Isotopes</a></li> <li class="toclevel-2 tocsection-6"><a href="#Natural_occurrence">1.5 Natural occurrence</a></li> </ul> </li> <li class="toclevel-1 tocsection-7"><a href="#Compounds">2 Compounds</a> <ul> <li class="toclevel-2 tocsection-8"><a href="#Electron_transfer_reactions">2.1 Electron transfer reactions</a></li> <li class="toclevel-2 tocsection-9"><a href="#Hydrogenation">2.2 Hydrogenation</a></li> <li class="toclevel-2 tocsection-10"><a href="#Combustion">2.3 Combustion</a></li> <li class="toclevel-2 tocsection-11"><a href="#Halogenation">2.4 Halogenation</a></li> <li class="toclevel-2 tocsection-12"><a href="#Pseudohalides">2.5 Pseudohalides</a></li> <li class="toclevel-2 tocsection-13"><a href="#Metal_sulfides">2.6 Metal sulfides</a></li> <li class="toclevel-2 tocsection-14"><a href="#Organic_compounds">2.7 Organic compounds</a></li> </ul> </li> <li class="toclevel-1 tocsection-15"><a href="#History">3 History</a> <ul> <li class="toclevel-2 tocsection-16"><a href="#Antiquity">3.1 Antiquity</a></li> <li class="toclevel-2 tocsection-17"><a href="#Modern_times">3.2 Modern times</a></li> <li class="toclevel-2 tocsection-18"><a href="#Spelling_and_etymology">3.3 Spelling and etymology</a></li> </ul> </li> <li class="toclevel-1 tocsection-19"><a href="#Production">4 Production</a></li> <li class="toclevel-1 tocsection-20"><a href="#Applications">5 Applications</a> <ul> <li class="toclevel-2 tocsection-21"><a href="#Sulfuric_acid">5.1 Sulfuric acid</a></li> <li class="toclevel-2 tocsection-22"><a href="#Other_important_sulfur_chemistry">5.2 Other important sulfur chemistry</a></li> <li class="toclevel-2 tocsection-23"><a href="#Fertilizer">5.3 Fertilizer</a></li> <li class="toclevel-2 tocsection-24"><a href="#Fungicide_and_pesticide">5.4 Fungicide and pesticide</a></li> <li class="toclevel-2 tocsection-25"><a href="#Pharmaceuticals">5.5 Pharmaceuticals</a></li> <li class="toclevel-2 tocsection-26"><a href="#Batteries">5.6 Batteries</a></li> </ul> </li> <li class="toclevel-1 tocsection-27"><a href="#Biological_role">6 Biological role</a> <ul> <li class="toclevel-2 tocsection-28"><a href="#Transferring_sulfur_between_inorganic_and_biomolecules">6.1 Transferring sulfur between inorganic and biomolecules</a></li> <li class="toclevel-2 tocsection-29"><a href="#Protein_and_organic_metabolites">6.2 Protein and organic metabolites</a></li> <li class="toclevel-2 tocsection-30"><a href="#Metalloproteins_and_inorganic_cofactors">6.3 Metalloproteins and inorganic cofactors</a></li> <li class="toclevel-2 tocsection-31"><a href="#Sulfate">6.4 Sulfate</a></li> <li class="toclevel-2 tocsection-32"><a href="#Deficiency">6.5 Deficiency</a></li> </ul> </li> <li class="toclevel-1 tocsection-33"><a href="#Precautions">7 Precautions</a> <ul> <li class="toclevel-2 tocsection-34"><a href="#Toxicity_of_sulfur_compounds">7.1 Toxicity of sulfur compounds</a></li> </ul> </li> <li class="toclevel-1 tocsection-35"><a href="#Notes">8 Notes</a></li> <li class="toclevel-1 tocsection-36"><a href="#See_also">9 See also</a></li> <li class="toclevel-1 tocsection-37"><a href="#References">10 References</a></li> <li class="toclevel-1 tocsection-38"><a href="#Further_reading">11 Further reading</a></li> <li class="toclevel-1 tocsection-39"><a href="#External_links">12 External links</a></li> </ul> </div> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(1)"><h2 id="Characteristics">Characteristics</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=1" title="Edit section: Characteristics" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-1 collapsible-block" id="mf-section-1"> <div class="mw-heading mw-heading3"><h3 id="Physical_properties">Physical properties</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=2" title="Edit section: Physical properties" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Burning-sulfur.png" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Burning-sulfur.png/170px-Burning-sulfur.png" decoding="async" width="170" height="204" class="mw-file-element" data-file-width="440" data-file-height="528"></noscript><span class="lazy-image-placeholder" style="width: 170px;height: 204px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Burning-sulfur.png/170px-Burning-sulfur.png" data-width="170" data-height="204" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Burning-sulfur.png/255px-Burning-sulfur.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Burning-sulfur.png/340px-Burning-sulfur.png 2x" data-class="mw-file-element"> </a><figcaption>As a solid, sulfur is a characteristic lemon yellow; when burned, sulfur melts into a blood-red liquid and emits a blue flame.</figcaption></figure> Sulfur forms several polyatomic molecules. The best-known allotrope is <a href="/wiki/Octasulfur" title="Octasulfur">octasulfur</a>, cyclo-S8. The <a href="/wiki/Point_group" title="Point group">point group</a> of cyclo-S8 is D4d and its dipole moment is 0 D.<a href="#cite_note-12">[12]</a> Octasulfur is a soft, bright-yellow solid that is odorless.<a href="#cite_note-13">[a]</a> It melts at 115.21 °C (239.38 °F),<a href="#cite_note-15">[b]</a> and boils at 444.6 °C (832.3 °F).<a href="#cite_note-Greenwood-1997a-8">[8]</a> At 95.2 °C (203.4 °F), below its melting temperature, cyclo-octasulfur begins slowly changing from α-octasulfur to the β-<a href="/wiki/Polymorphism_(materials_science)" class="mw-redirect" title="Polymorphism (materials science)">polymorph</a>.<a href="#cite_note-Greenwood-1997b-16">[14]</a> The structure of the S8 ring is virtually unchanged by this phase transition, which affects the intermolecular interactions. Cooling molten sulfur freezes at 119.6 °C (247.3 °F),<a href="#cite_note-17">[15]</a> as it predominantly consists of the β-S8 molecules.<a href="#cite_note-21">[c]</a> Between its melting and boiling temperatures, octasulfur changes its allotrope again, turning from β-octasulfur to γ-sulfur, again accompanied by a lower density but increased <a href="/wiki/Viscosity" title="Viscosity">viscosity</a> due to the formation of <a href="/wiki/Polymer" title="Polymer">polymers</a>.<a href="#cite_note-Greenwood-1997b-16">[14]</a> At higher temperatures, the viscosity decreases as depolymerization occurs. Molten sulfur assumes a dark red color above 200 °C (392 °F). The density of sulfur is about 2 g/cm3, depending on the allotrope; all of the stable allotropes are excellent electrical insulators. Sulfur <a href="/wiki/Sublimation_(phase_transition)" title="Sublimation (phase transition)">sublimes</a> more or less between 20 °C (68 °F) and 50 °C (122 °F).<a href="#cite_note-22">[19]</a> Sulfur is insoluble in water but soluble in <a href="/wiki/Carbon_disulfide" title="Carbon disulfide">carbon disulfide</a> and, to a lesser extent, in other <a href="/wiki/Chemical_polarity" title="Chemical polarity">nonpolar</a> organic solvents, such as <a href="/wiki/Benzene" title="Benzene">benzene</a> and <a href="/wiki/Toluene" title="Toluene">toluene</a>. <div class="mw-heading mw-heading3"><h3 id="Chemical_properties">Chemical properties</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=3" title="Edit section: Chemical properties" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Under normal conditions, sulfur <a href="/wiki/Hydrolysis" title="Hydrolysis">hydrolyzes</a> very slowly to mainly form <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a> and <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>: <style data-mw-deduplicate="TemplateStyles:r996643573">.mw-parser-output .block-indent{padding-left:3em;padding-right:0;overflow:hidden}</style><div class="block-indent"><style data-mw-deduplicate="TemplateStyles:r1154941027">.mw-parser-output .frac{white-space:nowrap}.mw-parser-output .frac .num,.mw-parser-output .frac .den{font-size:80%;line-height:0;vertical-align:super}.mw-parser-output .frac .den{vertical-align:sub}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}</style>1⁄2 S 8 + 4 H 2O → 3 H 2S + H 2SO 4</div> <style data-mw-deduplicate="TemplateStyles:r1237032888/mw-parser-output/.tmulti">.mw-parser-output .tmulti .multiimageinner{display:flex;flex-direction:column}.mw-parser-output .tmulti .trow{display:flex;flex-direction:row;clear:left;flex-wrap:wrap;width:100%;box-sizing:border-box}.mw-parser-output .tmulti .tsingle{margin:1px;float:left}.mw-parser-output .tmulti .theader{clear:both;font-weight:bold;text-align:center;align-self:center;background-color:transparent;width:100%}.mw-parser-output .tmulti .thumbcaption{background-color:transparent}.mw-parser-output .tmulti .text-align-left{text-align:left}.mw-parser-output .tmulti .text-align-right{text-align:right}.mw-parser-output .tmulti .text-align-center{text-align:center}@media all and (max-width:720px){.mw-parser-output .tmulti .thumbinner{width:100%!important;box-sizing:border-box;max-width:none!important;align-items:center}.mw-parser-output .tmulti .trow{justify-content:center}.mw-parser-output .tmulti .tsingle{float:none!important;max-width:100%!important;box-sizing:border-box;text-align:center}.mw-parser-output .tmulti .tsingle .thumbcaption{text-align:left}.mw-parser-output .tmulti .trow>.thumbcaption{text-align:center}}@media screen{html.skin-theme-clientpref-night .mw-parser-output .tmulti .multiimageinner img{background-color:white}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .tmulti .multiimageinner img{background-color:white}}</style><div class="thumb tmulti tleft"><div class="thumbinner multiimageinner" style="width:100px;max-width:100px"><div class="trow"><div class="tsingle" style="width:90px;max-width:90px"><div class="thumbimage" style="height:167px;overflow:hidden"><a href="/wiki/File:Liquid_hydrogen_sulfide.png" class="mw-file-description"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f8/Liquid_hydrogen_sulfide.png/88px-Liquid_hydrogen_sulfide.png" decoding="async" width="88" height="167" class="mw-file-element" data-file-width="426" data-file-height="810"></noscript><span class="lazy-image-placeholder" style="width: 88px;height: 167px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f8/Liquid_hydrogen_sulfide.png/88px-Liquid_hydrogen_sulfide.png" data-alt="" data-width="88" data-height="167" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f8/Liquid_hydrogen_sulfide.png/132px-Liquid_hydrogen_sulfide.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f8/Liquid_hydrogen_sulfide.png/176px-Liquid_hydrogen_sulfide.png 2x" data-class="mw-file-element"> </a></div></div></div><div class="trow"><div class="tsingle" style="width:90px;max-width:90px"><div class="thumbimage" style="height:124px;overflow:hidden"><a href="/wiki/File:Sulphuric_acid_96_percent_extra_pure.jpg" class="mw-file-description"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Sulphuric_acid_96_percent_extra_pure.jpg/88px-Sulphuric_acid_96_percent_extra_pure.jpg" decoding="async" width="88" height="124" class="mw-file-element" data-file-width="660" data-file-height="932"></noscript><span class="lazy-image-placeholder" style="width: 88px;height: 124px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Sulphuric_acid_96_percent_extra_pure.jpg/88px-Sulphuric_acid_96_percent_extra_pure.jpg" data-alt="" data-width="88" data-height="124" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Sulphuric_acid_96_percent_extra_pure.jpg/132px-Sulphuric_acid_96_percent_extra_pure.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Sulphuric_acid_96_percent_extra_pure.jpg/176px-Sulphuric_acid_96_percent_extra_pure.jpg 2x" data-class="mw-file-element"> </a></div></div></div><div class="trow" style="display:flex"><div class="thumbcaption">Left: Liquid hydrogen sulfide inside a test tube. Right: A bottle of sulfuric acid.</div></div></div></div> The reaction involves adsorption of protons onto S 8 clusters, followed by <a href="/wiki/Disproportionation" title="Disproportionation">disproportionation</a> into the reaction products.<a href="#cite_note-23">[20]</a> The second, fourth and sixth <a href="/wiki/Molar_ionization_energies_of_the_elements" title="Molar ionization energies of the elements">ionization energies</a> of sulfur are 2252 kJ/mol, 4556 kJ/mol and 8495.8 kJ/mol, respectively. The composition of reaction products of sulfur with oxidants (and its oxidation state) depends on whether releasing of reaction energy overcomes these thresholds. Applying <a href="/wiki/Catalysis" title="Catalysis">catalysts</a> and/or <a href="/wiki/Endothermic_process" title="Endothermic process">supply of external energy</a> may vary sulfur's oxidation state and the composition of reaction products. While reaction between sulfur and oxygen under normal conditions gives sulfur dioxide (oxidation state +4), formation of <a href="/wiki/Sulfur_trioxide" title="Sulfur trioxide">sulfur trioxide</a> (oxidation state +6) requires a temperature of 400–600 °C (750–1,100 °F) and presence of a catalyst. In reactions with elements of lesser <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a>, it reacts as an oxidant and forms sulfides, where it has oxidation state −2. Sulfur reacts with nearly all other elements except noble gases, even with the notoriously unreactive metal <a href="/wiki/Iridium" title="Iridium">iridium</a> (yielding <a href="/wiki/Iridium_disulfide" title="Iridium disulfide">iridium disulfide</a>).<a href="#cite_note-Munson-1968-24">[21]</a> Some of those reactions require elevated temperatures.<a href="#cite_note-Wiberg-2001-25">[22]</a> <div class="mw-heading mw-heading3"><h3 id="Allotropes">Allotropes</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=4" title="Edit section: Allotropes" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Allotropes_of_sulfur" title="Allotropes of sulfur">Allotropes of sulfur</a></div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Cyclooctasulfur-above-3D-balls.png" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7e/Cyclooctasulfur-above-3D-balls.png/220px-Cyclooctasulfur-above-3D-balls.png" decoding="async" width="220" height="161" class="mw-file-element" data-file-width="1100" data-file-height="804"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 161px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7e/Cyclooctasulfur-above-3D-balls.png/220px-Cyclooctasulfur-above-3D-balls.png" data-width="220" data-height="161" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/7e/Cyclooctasulfur-above-3D-balls.png/330px-Cyclooctasulfur-above-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/7e/Cyclooctasulfur-above-3D-balls.png/440px-Cyclooctasulfur-above-3D-balls.png 2x" data-class="mw-file-element"> </a><figcaption>The structure of the cyclooctasulfur molecule, S8</figcaption></figure> Sulfur forms over 30 solid <a href="/wiki/Allotropy" title="Allotropy">allotropes</a>, more than any other element.<a href="#cite_note-26">[23]</a> Besides S8, several other rings are known.<a href="#cite_note-27">[24]</a> Removing one atom from the crown gives S7, which is of a deeper yellow than S8. <a href="/wiki/High-performance_liquid_chromatography" title="High-performance liquid chromatography">HPLC</a> analysis of "elemental sulfur" reveals an equilibrium mixture of mainly S8, but with S7 and small amounts of S6.<a href="#cite_note-28">[25]</a> Larger rings have been prepared, including S12 and S18.<a href="#cite_note-29">[26]</a><a href="#cite_note-30">[27]</a> <a href="/wiki/Amorphous" class="mw-redirect" title="Amorphous">Amorphous</a> or "plastic" sulfur is produced by rapid cooling of molten sulfur—for example, by pouring it into cold water. <a href="/wiki/X-ray_crystallography" title="X-ray crystallography">X-ray crystallography</a> studies show that the amorphous form may have a <a href="/wiki/Helix" title="Helix">helical</a> structure with eight atoms per turn. The long coiled polymeric molecules make the brownish substance <a href="/wiki/Elasticity_(physics)" title="Elasticity (physics)">elastic</a>, and in bulk it has the feel of crude rubber. This form is <a href="/wiki/Metastability_in_molecules" class="mw-redirect" title="Metastability in molecules">metastable</a> at room temperature and gradually reverts to the crystalline molecular allotrope, which is no longer elastic. This process happens over a matter of hours to days, but can be rapidly catalyzed. <div style="clear:left;" class=""></div> <div class="mw-heading mw-heading3"><h3 id="Isotopes">Isotopes</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=5" title="Edit section: Isotopes" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Isotopes_of_sulfur" title="Isotopes of sulfur">Isotopes of sulfur</a></div> Sulfur has 23 known <a href="/wiki/Isotope" title="Isotope">isotopes</a>, four of which are stable: 32S (94.99%±0.26%), 33S (0.75%±0.02%), 34S (4.25%±0.24%), and 36S (0.01%±0.01%).<a href="#cite_note-31">[28]</a><a href="#cite_note-CRC-2011-32">[29]</a> Other than 35S, with a <a href="/wiki/Half-life" title="Half-life">half-life</a> of 87 days, the <a href="/wiki/Radioactivity" class="mw-redirect" title="Radioactivity">radioactive</a> isotopes of sulfur have half-lives less than 3 hours. The preponderance of 32S is explained by its production in the so-called alpha-process (one of the main classes of nuclear fusion reactions) in exploding stars. Other stable sulfur isotopes are produced in the bypass processes related with 34Ar, and their composition depends on a type of a stellar explosion. For example, proportionally more 33S comes from <a href="/wiki/Novae" class="mw-redirect" title="Novae">novae</a> than from <a href="/wiki/Supernovae" class="mw-redirect" title="Supernovae">supernovae</a>.<a href="#cite_note-33">[30]</a> On the planet Earth the sulfur isotopic composition was determined by the Sun. Though it was assumed that the distribution of different sulfur isotopes would be more or less equal, it has been found that proportions of the two most abundant sulfur isotopes 32S and 34S varies in different samples. Assaying of the isotope ratio (<a href="/wiki/%CE%9434S" title="Δ34S">δ34S</a>) in the samples suggests their chemical history, and with support of other methods, it allows to age-date the samples, estimate temperature of equilibrium between ore and water, determine pH and oxygen <a href="/wiki/Fugacity" title="Fugacity">fugacity</a>, identify the activity of sulfate-reducing bacteria in the time of formation of the sample, or suggest the main sources of sulfur in ecosystems.<a href="#cite_note-34">[31]</a> However, there are ongoing discussions over the real reason for the δ34S shifts, biological activity or postdeposit alteration.<a href="#cite_note-35">[32]</a> For example, when <a href="/wiki/Sulfide_mineral" title="Sulfide mineral">sulfide minerals</a> are precipitated, isotopic equilibration among solids and liquid may cause small differences in the δ34S values of co-genetic minerals. The differences between minerals can be used to estimate the temperature of equilibration. The <a href="/wiki/%CE%9413C" title="Δ13C">δ13C</a> and δ34S of coexisting <a href="/wiki/Carbonate_minerals" class="mw-redirect" title="Carbonate minerals">carbonate minerals</a> and sulfides can be used to determine the <a href="/wiki/PH" title="PH">pH</a> and oxygen fugacity of the ore-bearing fluid during ore formation. Scientists measure the <a href="/wiki/Sulfur_isotope_biogeochemistry" title="Sulfur isotope biogeochemistry">sulfur isotopes</a> of <a href="/wiki/Mineral" title="Mineral">minerals</a> in rocks and <a href="/wiki/Sediment" title="Sediment">sediments</a> to study the <a href="/wiki/Redox" title="Redox">redox</a> conditions in past oceans. <a href="/wiki/Sulfate-reducing_microorganism" title="Sulfate-reducing microorganism">Sulfate-reducing bacteria</a> in marine sediment fractionate <a href="/wiki/Sulfur_isotope_biogeochemistry" title="Sulfur isotope biogeochemistry">sulfur isotopes</a> as they take in <a href="/wiki/Sulfate" title="Sulfate">sulfate</a> and produce <a href="/wiki/Sulfide" title="Sulfide">sulfide</a>. Prior to the 2010s, it was thought that sulfate reduction could fractionate <a href="/wiki/Sulfur_isotope_biogeochemistry" title="Sulfur isotope biogeochemistry">sulfur isotopes</a> up to 46 <a href="/wiki/Permil" class="mw-redirect" title="Permil">permil</a><a href="#cite_note-36">[33]</a> and fractionation larger than 46 permil recorded in sediments must be due to <a href="/wiki/Disproportionation" title="Disproportionation">disproportionation</a> of sulfur compounds in the sediment. This view has changed since the 2010s as experiments showed that <a href="/wiki/Sulfate-reducing_microorganism" title="Sulfate-reducing microorganism">sulfate-reducing bacteria</a> can fractionate to 66 permil.<a href="#cite_note-37">[34]</a> As substrates for disproportionation are limited by the product of <a href="/wiki/Sulfate-reducing_microorganism" title="Sulfate-reducing microorganism">sulfate reduction</a>, the isotopic effect of disproportionation should be less than 16 permil in most sedimentary settings.<a href="#cite_note-38">[35]</a> In <a href="/wiki/Forest" title="Forest">forest</a> ecosystems, sulfate is derived mostly from the atmosphere; weathering of ore minerals and evaporites contribute some sulfur. Sulfur with a distinctive isotopic composition has been used to identify pollution sources, and enriched sulfur has been added as a tracer in <a href="/wiki/Hydrology" title="Hydrology">hydrologic</a> studies. Differences in the <a href="/wiki/Natural_abundance" title="Natural abundance">natural abundances</a> can be used in systems where there is sufficient variation in the 34S of ecosystem components. <a href="/wiki/Rocky_Mountain" class="mw-redirect" title="Rocky Mountain">Rocky Mountain</a> lakes thought to be dominated by atmospheric sources of sulfate have been found to have measurably different 34S values than lakes believed to be dominated by watershed sources of sulfate. The radioactive 35S is formed in <a href="/wiki/Cosmic_ray_spallation" title="Cosmic ray spallation">cosmic ray spallation</a> of the atmospheric <a href="/wiki/Argon-40" class="mw-redirect" title="Argon-40">40Ar</a>. This fact may be used to verify the presence of recent (up to 1 year) atmospheric sediments in various materials. This isotope may be obtained artificially by different ways. In practice, the reaction <a href="/wiki/Chlorine-35" class="mw-redirect" title="Chlorine-35">35Cl</a> + <a href="/wiki/Neutron" title="Neutron">n</a> → 35S + <a href="/wiki/Proton" title="Proton">p</a> is used by irradiating <a href="/wiki/Potassium_chloride" title="Potassium chloride">potassium chloride</a> with neutrons.<a href="#cite_note-39">[36]</a> The isotope 35S is used in various sulfur-containing compounds as a <a href="/wiki/Radioactive_tracer" title="Radioactive tracer">radioactive tracer</a> for many biological studies, for example, the <a href="/wiki/Hershey-Chase_experiment" class="mw-redirect" title="Hershey-Chase experiment">Hershey-Chase experiment</a>. Because of the weak <a href="/wiki/Beta_decay" title="Beta decay">beta activity</a> of 35S, its compounds are relatively safe as long as they are not ingested or absorbed by the body.<a href="#cite_note-40">[37]</a> <div class="mw-heading mw-heading3"><h3 id="Natural_occurrence">Natural occurrence</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=6" title="Edit section: Natural occurrence" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded,_Freeport_Sulphur_Co.,_Hoskins_Mound,_Texas,_1a35438v.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f3/Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg/220px-Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg" decoding="async" width="220" height="165" class="mw-file-element" data-file-width="6075" data-file-height="4550"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 165px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f3/Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg/220px-Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg" data-width="220" data-height="165" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f3/Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg/330px-Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f3/Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg/440px-Nearly_exhausted_sulphur_vat_from_which_railroad_cars_are_loaded%2C_Freeport_Sulphur_Co.%2C_Hoskins_Mound%2C_Texas%2C_1a35438v.jpg 2x" data-class="mw-file-element"> </a><figcaption>Sulfur vat from which railroad cars are loaded, Freeport Sulphur Co., Hoskins Mound, Texas (1943)</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Io_highest_resolution_true_color.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7b/Io_highest_resolution_true_color.jpg/220px-Io_highest_resolution_true_color.jpg" decoding="async" width="220" height="220" class="mw-file-element" data-file-width="3196" data-file-height="3196"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 220px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7b/Io_highest_resolution_true_color.jpg/220px-Io_highest_resolution_true_color.jpg" data-width="220" data-height="220" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/7b/Io_highest_resolution_true_color.jpg/330px-Io_highest_resolution_true_color.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/7b/Io_highest_resolution_true_color.jpg/440px-Io_highest_resolution_true_color.jpg 2x" data-class="mw-file-element"> </a><figcaption>Most of the yellow and orange hues of <a href="/wiki/Io_(moon)" title="Io (moon)">Io</a> are due to elemental sulfur and sulfur compounds deposited by active <a href="/wiki/Volcano" title="Volcano">volcanoes</a>.</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Menambang_Belerang.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/3/35/Menambang_Belerang.jpg/220px-Menambang_Belerang.jpg" decoding="async" width="220" height="146" class="mw-file-element" data-file-width="2500" data-file-height="1656"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 146px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/3/35/Menambang_Belerang.jpg/220px-Menambang_Belerang.jpg" data-width="220" data-height="146" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/35/Menambang_Belerang.jpg/330px-Menambang_Belerang.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/3/35/Menambang_Belerang.jpg/440px-Menambang_Belerang.jpg 2x" data-class="mw-file-element"> </a><figcaption>Sulfur extraction, East Java</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/ac/Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg/220px-Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg" decoding="async" width="220" height="147" class="mw-file-element" data-file-width="5616" data-file-height="3744"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 147px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/a/ac/Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg/220px-Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg" data-width="220" data-height="147" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/ac/Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg/330px-Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/ac/Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg/440px-Kawah_Ijen_-East_Java_-Indonesia_-sulphur-31July2009.jpg 2x" data-class="mw-file-element"> </a><figcaption>A man carrying sulfur blocks from <a href="/wiki/Kawah_Ijen" class="mw-redirect" title="Kawah Ijen">Kawah Ijen</a>, a volcano in East Java, Indonesia, 2009</figcaption></figure> 32S is created inside massive stars, at a depth where the temperature exceeds 2.5×109 K, by the <a href="/wiki/Silicon_burning" class="mw-redirect" title="Silicon burning">fusion</a> of one nucleus of silicon plus one nucleus of helium.<a href="#cite_note-41">[38]</a> As this nuclear reaction is part of the <a href="/wiki/Alpha_process" title="Alpha process">alpha process</a> that produces elements in abundance, sulfur is the 10th <a href="/wiki/Abundance_of_the_chemical_elements#Universe" title="Abundance of the chemical elements">most common element in the universe</a>. Sulfur, usually as sulfide, is present in many types of <a href="/wiki/Meteorite" title="Meteorite">meteorites</a>. <a href="/wiki/Ordinary_chondrite" title="Ordinary chondrite">Ordinary chondrites</a> contain on average 2.1% sulfur, and <a href="/wiki/Carbonaceous_chondrite" title="Carbonaceous chondrite">carbonaceous chondrites</a> may contain as much as 6.6%. It is normally present as <a href="/wiki/Troilite" title="Troilite">troilite</a> (FeS), but there are exceptions, with carbonaceous chondrites containing free sulfur, sulfates and other sulfur compounds.<a href="#cite_note-42">[39]</a> The distinctive colors of <a href="/wiki/Jupiter" title="Jupiter">Jupiter</a>'s <a href="/wiki/Volcano" title="Volcano">volcanic</a> moon <a href="/wiki/Io_(moon)" title="Io (moon)">Io</a> are attributed to various forms of molten, solid, and gaseous sulfur.<a href="#cite_note-43">[40]</a> In July 2024, elemental sulfur was accidentally discovered to exist on <a href="/wiki/Mars" title="Mars">Mars</a> after the <a href="/wiki/Curiosity_(rover)" title="Curiosity (rover)">Curiosity rover</a> drove over and crushed a rock, revealing sulfur crystals inside it.<a href="#cite_note-44">[41]</a> Sulfur is the fifth most common element by mass in the Earth. Elemental sulfur can be found near <a href="/wiki/Hot_spring" title="Hot spring">hot springs</a> and <a href="/wiki/Volcanic" class="mw-redirect" title="Volcanic">volcanic</a> regions in many parts of the world, especially along the <a href="/wiki/Pacific_Ring_of_Fire" class="mw-redirect" title="Pacific Ring of Fire">Pacific Ring of Fire</a>; such volcanic deposits are mined in Indonesia, Chile, and Japan. These deposits are polycrystalline, with the largest documented single crystal measuring 22 cm × 16 cm × 11 cm (8.7 in × 6.3 in × 4.3 in).<a href="#cite_note-45">[42]</a> Historically, <a href="/wiki/Sicily" title="Sicily">Sicily</a> was a major source of sulfur in the <a href="/wiki/Industrial_Revolution" title="Industrial Revolution">Industrial Revolution</a>.<a href="#cite_note-46">[43]</a> Lakes of molten sulfur up to about 200 m (660 ft) in diameter have been found on the sea floor, associated with <a href="/wiki/Submarine_volcano" title="Submarine volcano">submarine volcanoes</a>, at depths where the boiling point of water is higher than the melting point of sulfur.<a href="#cite_note-de_Ronde-2015-47">[44]</a> Native sulfur is synthesized by <a href="/wiki/Anaerobic_bacteria" class="mw-redirect" title="Anaerobic bacteria">anaerobic bacteria</a> acting on <a href="/wiki/Sulfate_minerals" class="mw-redirect" title="Sulfate minerals">sulfate minerals</a> such as <a href="/wiki/Gypsum" title="Gypsum">gypsum</a> in <a href="/wiki/Salt_dome" title="Salt dome">salt domes</a>.<a href="#cite_note-48">[45]</a><a href="#cite_note-49">[46]</a> Significant deposits in salt domes occur along the coast of the <a href="/wiki/Gulf_of_Mexico" title="Gulf of Mexico">Gulf of Mexico</a>, and in <a href="/wiki/Evaporite" title="Evaporite">evaporites</a> in eastern Europe and western Asia. Native sulfur may be produced by geological processes alone. Fossil-based sulfur deposits from salt domes were once the basis for commercial production in the United States, Russia, Turkmenistan, and Ukraine.<a href="#cite_note-Nehb-2006-50">[47]</a> Such sources have become of secondary commercial importance, and most are no longer worked but commercial production is still carried out in the <a href="/wiki/Osiek,_%C5%9Awi%C4%99tokrzyskie_Voivodeship" title="Osiek, Świętokrzyskie Voivodeship">Osiek</a> mine in Poland. Common naturally occurring sulfur compounds include the <a href="/wiki/Mineral#Sulfides" title="Mineral">sulfide minerals</a>, such as <a href="/wiki/Pyrite" title="Pyrite">pyrite</a> (iron sulfide), <a href="/wiki/Cinnabar" title="Cinnabar">cinnabar</a> (mercury sulfide), <a href="/wiki/Galena" title="Galena">galena</a> (lead sulfide), <a href="/wiki/Sphalerite" title="Sphalerite">sphalerite</a> (zinc sulfide), and <a href="/wiki/Stibnite" title="Stibnite">stibnite</a> (antimony sulfide); and the <a href="/wiki/Mineral#Sulfates" title="Mineral">sulfate minerals</a>, such as <a href="/wiki/Gypsum" title="Gypsum">gypsum</a> (calcium sulfate), <a href="/wiki/Alunite" title="Alunite">alunite</a> (potassium aluminium sulfate), and <a href="/wiki/Barite" class="mw-redirect" title="Barite">barite</a> (barium sulfate). On Earth, just as upon Jupiter's moon Io, elemental sulfur occurs naturally in volcanic emissions, including emissions from <a href="/wiki/Hydrothermal_vent" title="Hydrothermal vent">hydrothermal vents</a>. The main industrial source of sulfur has become <a href="/wiki/Petroleum" title="Petroleum">petroleum</a> and <a href="/wiki/Natural_gas" title="Natural gas">natural gas</a>.<a href="#cite_note-Knight-2014-10">[10]</a> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(2)"><h2 id="Compounds">Compounds</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=7" title="Edit section: Compounds" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-2 collapsible-block" id="mf-section-2"> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Sulfur_compounds" title="Sulfur compounds">Sulfur compounds</a></div> Common <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation states</a> of sulfur range from −2 to +6. Sulfur forms stable compounds with all elements except the <a href="/wiki/Noble_gas" title="Noble gas">noble gases</a>. <div class="mw-heading mw-heading3"><h3 id="Electron_transfer_reactions">Electron transfer reactions</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=8" title="Edit section: Electron transfer reactions" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Lapis_lazuli_block.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a6/Lapis_lazuli_block.jpg/170px-Lapis_lazuli_block.jpg" decoding="async" width="170" height="302" class="mw-file-element" data-file-width="673" data-file-height="1197"></noscript><span class="lazy-image-placeholder" style="width: 170px;height: 302px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a6/Lapis_lazuli_block.jpg/170px-Lapis_lazuli_block.jpg" data-width="170" data-height="302" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a6/Lapis_lazuli_block.jpg/255px-Lapis_lazuli_block.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a6/Lapis_lazuli_block.jpg/340px-Lapis_lazuli_block.jpg 2x" data-class="mw-file-element"> </a><figcaption><a href="/wiki/Lapis_lazuli" title="Lapis lazuli">Lapis lazuli</a> owes its blue color to a <a href="/wiki/Trisulfur" title="Trisulfur">trisulfur</a> radical anion (S− 3)</figcaption></figure> Sulfur polycations, <style data-mw-deduplicate="TemplateStyles:r1123817410">.mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em}</style>S2+8, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">S2+4 and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">S2+16 are produced when sulfur is reacted with oxidizing agents in a strongly acidic solution.<a href="#cite_note-51">[48]</a> The colored solutions produced by dissolving sulfur in <a href="/wiki/Oleum" title="Oleum">oleum</a> were first reported as early as 1804 by C. F. Bucholz, but the cause of the color and the structure of the polycations involved was only determined in the late 1960s. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">S2+8 is deep blue, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">S2+4 is yellow and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">S2+16 is red.<a href="#cite_note-Greenwood-1997b-16">[14]</a> Reduction of sulfur gives various <a href="/wiki/Polysulfide" title="Polysulfide">polysulfides</a> with the formula S2− x, many of which have been obtained in crystalline form. Illustrative is the production of <a href="/wiki/Sodium_tetrasulfide" title="Sodium tetrasulfide">sodium tetrasulfide</a>: <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">4 Na + S8 → 2 Na2S4</div> Some of these dianions dissociate to give <a href="/wiki/Radical_anion" title="Radical anion">radical anions</a>, such as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Trisulfur" title="Trisulfur">S−3</a> gives the blue color of the rock <a href="/wiki/Lapis_lazuli" title="Lapis lazuli">lapis lazuli</a>. <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:S@CNT.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/91/S%40CNT.jpg/220px-S%40CNT.jpg" decoding="async" width="220" height="260" class="mw-file-element" data-file-width="412" data-file-height="487"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 260px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/9/91/S%40CNT.jpg/220px-S%40CNT.jpg" data-width="220" data-height="260" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/91/S%40CNT.jpg/330px-S%40CNT.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/9/91/S%40CNT.jpg 2x" data-class="mw-file-element"> </a><figcaption>Two parallel sulfur chains grown inside a single-wall <a href="/wiki/Carbon_nanotube" title="Carbon nanotube">carbon nanotube</a> (CNT, a). Zig-zag (b) and straight (c) S chains inside double-wall CNTs<a href="#cite_note-52">[49]</a></figcaption></figure> This reaction highlights a distinctive property of sulfur: its ability to <a href="/wiki/Catenation" title="Catenation">catenate</a> (bind to itself by formation of chains). <a href="/wiki/Protonation" title="Protonation">Protonation</a> of these polysulfide anions produces the <a href="/wiki/Polysulfane" title="Polysulfane">polysulfanes</a>, H2Sx, where x = 2, 3, and 4.<a href="#cite_note-53">[50]</a> Ultimately, reduction of sulfur produces sulfide salts: <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">16 Na + S8 → 8 Na2S</div> The interconversion of these species is exploited in the <a href="/wiki/Sodium%E2%80%93sulfur_battery" title="Sodium–sulfur battery">sodium–sulfur battery</a>. <div class="mw-heading mw-heading3"><h3 id="Hydrogenation">Hydrogenation</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=9" title="Edit section: Hydrogenation" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Treatment of sulfur with hydrogen gives <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a>. When dissolved in water, hydrogen sulfide is mildly acidic:<a href="#cite_note-Greenwood-1997a-8">[8]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">H2S ⇌ HS− + H+</div> Hydrogen sulfide gas and the hydrosulfide anion are extremely toxic to mammals, due to their inhibition of the oxygen-carrying capacity of <a href="/wiki/Hemoglobin" title="Hemoglobin">hemoglobin</a> and certain <a href="/wiki/Cytochrome" title="Cytochrome">cytochromes</a> in a manner analogous to <a href="/wiki/Cyanide" title="Cyanide">cyanide</a> and <a href="/wiki/Azide" title="Azide">azide</a> (see below, under precautions). <div class="mw-heading mw-heading3"><h3 id="Combustion">Combustion</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=10" title="Edit section: Combustion" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> The two principal sulfur oxides are obtained by burning sulfur: <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">S + O2 → SO2 (<a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a>)</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">2 SO2 + O2 → 2 SO3 (<a href="/wiki/Sulfur_trioxide" title="Sulfur trioxide">sulfur trioxide</a>)</div> Many other sulfur oxides are observed including the <a href="/wiki/Lower_sulfur_oxides" title="Lower sulfur oxides">sulfur-rich oxides</a> include <a href="/wiki/Sulfur_monoxide" title="Sulfur monoxide">sulfur monoxide</a>, <a href="/wiki/Disulfur_monoxide" title="Disulfur monoxide">disulfur monoxide</a>, disulfur dioxides, and <a href="/wiki/Higher_sulfur_oxides" title="Higher sulfur oxides">higher oxides</a> containing peroxo groups. <div class="mw-heading mw-heading3"><h3 id="Halogenation">Halogenation</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=11" title="Edit section: Halogenation" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Sulfur reacts with <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> to give the highly reactive <a href="/wiki/Sulfur_tetrafluoride" title="Sulfur tetrafluoride">sulfur tetrafluoride</a> and the highly inert <a href="/wiki/Sulfur_hexafluoride" title="Sulfur hexafluoride">sulfur hexafluoride</a>.<a href="#cite_note-54">[51]</a> Whereas fluorine gives S(IV) and S(VI) compounds, chlorine gives S(II) and S(I) derivatives. Thus, <a href="/wiki/Sulfur_dichloride" title="Sulfur dichloride">sulfur dichloride</a>, <a href="/wiki/Disulfur_dichloride" title="Disulfur dichloride">disulfur dichloride</a>, and higher chlorosulfanes arise from the chlorination of sulfur. <a href="/wiki/Sulfuryl_chloride" title="Sulfuryl chloride">Sulfuryl chloride</a> and <a href="/wiki/Chlorosulfuric_acid" title="Chlorosulfuric acid">chlorosulfuric acid</a> are derivatives of sulfuric acid; <a href="/wiki/Thionyl_chloride" title="Thionyl chloride">thionyl chloride</a> (SOCl2) is a common reagent in <a href="/wiki/Organic_synthesis" title="Organic synthesis">organic synthesis</a>.<a href="#cite_note-Lauss-55">[52]</a> Bromine also oxidizes sulfur to form <a href="/wiki/Sulfur_dibromide" title="Sulfur dibromide">sulfur dibromide</a> and <a href="/wiki/Disulfur_dibromide" title="Disulfur dibromide">disulfur dibromide</a>.<a href="#cite_note-Lauss-55">[52]</a> <div class="mw-heading mw-heading3"><h3 id="Pseudohalides">Pseudohalides</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=12" title="Edit section: Pseudohalides" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Sulfur oxidizes <a href="/wiki/Cyanide" title="Cyanide">cyanide</a> and <a href="/wiki/Sulfite" title="Sulfite">sulfite</a> to give <a href="/wiki/Thiocyanate" title="Thiocyanate">thiocyanate</a> and <a href="/wiki/Thiosulfate" title="Thiosulfate">thiosulfate</a>, respectively. <div class="mw-heading mw-heading3"><h3 id="Metal_sulfides">Metal sulfides</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=13" title="Edit section: Metal sulfides" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Sulfur reacts with many metals. Electropositive metals give polysulfide salts. Copper, zinc, and silver are attacked by sulfur; see <a href="/wiki/Tarnishing" class="mw-redirect" title="Tarnishing">tarnishing</a>. Although many <a href="/wiki/Sulfide_mineral" title="Sulfide mineral">metal sulfides</a> are known, most are prepared by high temperature reactions of the elements.<a href="#cite_note-56">[53]</a> Geoscientists also study the isotopes of metal sulfides in rocks and sediment to study environmental conditions in the Earth's past.<a href="#cite_note-57">[54]</a> <div class="mw-heading mw-heading3"><h3 id="Organic_compounds">Organic compounds</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=14" title="Edit section: Organic compounds" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Organosulfur_compounds" class="mw-redirect" title="Organosulfur compounds">Organosulfur compounds</a></div> <ul class="gallery mw-gallery-traditional"> <li class="gallerycaption">Illustrative organosulfur compounds</li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:L-Cystein_-_L-Cysteine.svg" class="mw-file-description" title="(L)-cysteine, an amino acid containing a thiol group"><noscript><img alt="(L)-cysteine, an amino acid containing a thiol group" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1a/L-Cystein_-_L-Cysteine.svg/120px-L-Cystein_-_L-Cysteine.svg.png" decoding="async" width="120" height="78" class="mw-file-element" data-file-width="185" data-file-height="121"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 78px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1a/L-Cystein_-_L-Cysteine.svg/120px-L-Cystein_-_L-Cysteine.svg.png" data-alt="(L)-cysteine, an amino acid containing a thiol group" data-width="120" data-height="78" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1a/L-Cystein_-_L-Cysteine.svg/180px-L-Cystein_-_L-Cysteine.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1a/L-Cystein_-_L-Cysteine.svg/240px-L-Cystein_-_L-Cysteine.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext">(L)-<a href="/wiki/Cysteine" title="Cysteine">cysteine</a>, an <a href="/wiki/Amino_acid" title="Amino acid">amino acid</a> containing a thiol group</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Methionin_-_Methionine.svg" class="mw-file-description" title="Methionine, an amino acid containing a thioether"><noscript><img alt="Methionine, an amino acid containing a thioether" src="//upload.wikimedia.org/wikipedia/commons/thumb/2/23/Methionin_-_Methionine.svg/120px-Methionin_-_Methionine.svg.png" decoding="async" width="120" height="55" class="mw-file-element" data-file-width="265" data-file-height="121"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 55px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/2/23/Methionin_-_Methionine.svg/120px-Methionin_-_Methionine.svg.png" data-alt="Methionine, an amino acid containing a thioether" data-width="120" data-height="55" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/23/Methionin_-_Methionine.svg/180px-Methionin_-_Methionine.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/23/Methionin_-_Methionine.svg/240px-Methionin_-_Methionine.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Methionine" title="Methionine">Methionine</a>, an amino acid containing a thioether</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Thiamin.svg" class="mw-file-description" title="Thiamine or vitamin B1"><noscript><img alt="Thiamine or vitamin B1" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f0/Thiamin.svg/120px-Thiamin.svg.png" decoding="async" width="120" height="70" class="mw-file-element" data-file-width="346" data-file-height="201"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 70px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f0/Thiamin.svg/120px-Thiamin.svg.png" data-alt="Thiamine or vitamin B1" data-width="120" data-height="70" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f0/Thiamin.svg/180px-Thiamin.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f0/Thiamin.svg/240px-Thiamin.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Thiamine" title="Thiamine">Thiamine</a> or vitamin B1</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Biotin_structure.svg" class="mw-file-description" title="Biotin or vitamin B7"><noscript><img alt="Biotin or vitamin B7" src="//upload.wikimedia.org/wikipedia/commons/thumb/8/85/Biotin_structure.svg/120px-Biotin_structure.svg.png" decoding="async" width="120" height="67" class="mw-file-element" data-file-width="1200" data-file-height="670"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 67px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/8/85/Biotin_structure.svg/120px-Biotin_structure.svg.png" data-alt="Biotin or vitamin B7" data-width="120" data-height="67" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/85/Biotin_structure.svg/180px-Biotin_structure.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/85/Biotin_structure.svg/240px-Biotin_structure.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Biotin" title="Biotin">Biotin</a> or vitamin B7</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Penicillin_core.svg" class="mw-file-description" title='Penicillin, an antibiotic ("R" is the variable group)'><noscript><img alt='Penicillin, an antibiotic ("R" is the variable group)' src="//upload.wikimedia.org/wikipedia/commons/thumb/9/99/Penicillin_core.svg/120px-Penicillin_core.svg.png" decoding="async" width="120" height="80" class="mw-file-element" data-file-width="512" data-file-height="342"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 80px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/9/99/Penicillin_core.svg/120px-Penicillin_core.svg.png" data-alt='Penicillin, an antibiotic ("R" is the variable group)' data-width="120" data-height="80" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/99/Penicillin_core.svg/180px-Penicillin_core.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/99/Penicillin_core.svg/240px-Penicillin_core.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Penicillin" title="Penicillin">Penicillin</a>, an antibiotic ("R" is the variable group)</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Allicin_skeletal.svg" class="mw-file-description" title="Allicin, a chemical compound in garlic"><noscript><img alt="Allicin, a chemical compound in garlic" src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Allicin_skeletal.svg/120px-Allicin_skeletal.svg.png" decoding="async" width="120" height="43" class="mw-file-element" data-file-width="394" data-file-height="140"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 43px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Allicin_skeletal.svg/120px-Allicin_skeletal.svg.png" data-alt="Allicin, a chemical compound in garlic" data-width="120" data-height="43" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Allicin_skeletal.svg/180px-Allicin_skeletal.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Allicin_skeletal.svg/240px-Allicin_skeletal.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Allicin" title="Allicin">Allicin</a>, a chemical compound in garlic</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Diphenyl_disulfide.svg" class="mw-file-description" title="Diphenyl disulfide, a representative disulfide"><noscript><img alt="Diphenyl disulfide, a representative disulfide" src="//upload.wikimedia.org/wikipedia/commons/thumb/3/3c/Diphenyl_disulfide.svg/120px-Diphenyl_disulfide.svg.png" decoding="async" width="120" height="71" class="mw-file-element" data-file-width="453" data-file-height="269"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 71px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/3/3c/Diphenyl_disulfide.svg/120px-Diphenyl_disulfide.svg.png" data-alt="Diphenyl disulfide, a representative disulfide" data-width="120" data-height="71" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/3c/Diphenyl_disulfide.svg/180px-Diphenyl_disulfide.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/3/3c/Diphenyl_disulfide.svg/240px-Diphenyl_disulfide.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Diphenyl_disulfide" title="Diphenyl disulfide">Diphenyl disulfide</a>, a representative disulfide</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Dibenzothiophen_-_Dibenzothiophene.svg" class="mw-file-description" title="Dibenzothiophene, a component of crude oil"><noscript><img alt="Dibenzothiophene, a component of crude oil" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/19/Dibenzothiophen_-_Dibenzothiophene.svg/120px-Dibenzothiophen_-_Dibenzothiophene.svg.png" decoding="async" width="120" height="62" class="mw-file-element" data-file-width="197" data-file-height="101"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 62px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/1/19/Dibenzothiophen_-_Dibenzothiophene.svg/120px-Dibenzothiophen_-_Dibenzothiophene.svg.png" data-alt="Dibenzothiophene, a component of crude oil" data-width="120" data-height="62" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/19/Dibenzothiophen_-_Dibenzothiophene.svg/180px-Dibenzothiophen_-_Dibenzothiophene.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/19/Dibenzothiophen_-_Dibenzothiophene.svg/240px-Dibenzothiophen_-_Dibenzothiophene.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Dibenzothiophene" title="Dibenzothiophene">Dibenzothiophene</a>, a component of crude oil</div> </li> <li class="gallerybox" style="width: 155px"> <div class="thumb" style="width: 150px; height: 150px;"><a href="/wiki/File:Perfluorooctanesulfonic_acid_structure.svg" class="mw-file-description" title="Perfluorooctanesulfonic acid (PFOS), a surfactant"><noscript><img alt="Perfluorooctanesulfonic acid (PFOS), a surfactant" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Perfluorooctanesulfonic_acid_structure.svg/120px-Perfluorooctanesulfonic_acid_structure.svg.png" decoding="async" width="120" height="38" class="mw-file-element" data-file-width="570" data-file-height="180"></noscript><span class="lazy-image-placeholder" style="width: 120px;height: 38px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Perfluorooctanesulfonic_acid_structure.svg/120px-Perfluorooctanesulfonic_acid_structure.svg.png" data-alt="Perfluorooctanesulfonic acid (PFOS), a surfactant" data-width="120" data-height="38" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Perfluorooctanesulfonic_acid_structure.svg/180px-Perfluorooctanesulfonic_acid_structure.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/04/Perfluorooctanesulfonic_acid_structure.svg/240px-Perfluorooctanesulfonic_acid_structure.svg.png 2x" data-class="mw-file-element"> </a></div> <div class="gallerytext"><a href="/wiki/Perfluorooctanesulfonic_acid" title="Perfluorooctanesulfonic acid">Perfluorooctanesulfonic acid</a> (PFOS), a surfactant</div> </li> </ul> Some of the main classes of sulfur-containing organic compounds include the following:<a href="#cite_note-Cremlyn-1996-58">[55]</a> <ul><li><a href="/wiki/Thiol" title="Thiol">Thiols</a> or mercaptans (so called because they capture mercury as <a href="/wiki/Chelation" title="Chelation">chelators</a>) are the sulfur analogs of <a href="/wiki/Alcohol_(chemistry)" title="Alcohol (chemistry)">alcohols</a>; treatment of thiols with base gives <a href="/wiki/Thiolate" class="mw-redirect" title="Thiolate">thiolate</a> ions.</li> <li><a href="/wiki/Thioether" class="mw-redirect" title="Thioether">Thioethers</a> are the sulfur analogs of <a href="/wiki/Ether" title="Ether">ethers</a>.</li> <li><a href="/wiki/Sulfonium" title="Sulfonium">Sulfonium</a> ions have three groups attached to a cationic sulfur center. <a href="/wiki/Dimethylsulfoniopropionate" title="Dimethylsulfoniopropionate">Dimethylsulfoniopropionate</a> (DMSP) is one such compound, important in the marine organic <a href="/wiki/Sulfur_cycle" title="Sulfur cycle">sulfur cycle</a>.</li> <li><a href="/wiki/Sulfoxide" title="Sulfoxide">Sulfoxides</a> and <a href="/wiki/Sulfone" title="Sulfone">sulfones</a> are thioethers with one and two oxygen atoms attached to the sulfur atom, respectively. The simplest sulfoxide, <a href="/wiki/Dimethyl_sulfoxide" title="Dimethyl sulfoxide">dimethyl sulfoxide</a>, is a common solvent; a common sulfone is <a href="/wiki/Sulfolane" title="Sulfolane">sulfolane</a>.</li> <li><a href="/wiki/Sulfonic_acid" title="Sulfonic acid">Sulfonic acids</a> are used in many detergents.</li></ul> Compounds with carbon–sulfur multiple bonds are uncommon, an exception being <a href="/wiki/Carbon_disulfide" title="Carbon disulfide">carbon disulfide</a>, a volatile colorless liquid that is structurally similar to carbon dioxide. It is used as a reagent to make the polymer <a href="/wiki/Rayon" title="Rayon">rayon</a> and many organosulfur compounds. Unlike <a href="/wiki/Carbon_monoxide" title="Carbon monoxide">carbon monoxide</a>, <a href="/wiki/Carbon_monosulfide" title="Carbon monosulfide">carbon monosulfide</a> is stable only as an extremely dilute gas, found between solar systems.<a href="#cite_note-59">[56]</a> Organosulfur compounds are responsible for some of the unpleasant odors of decaying organic matter. They are widely known as the <a href="/wiki/Odorizer" title="Odorizer">odorant</a> in domestic natural gas, garlic odor, and skunk spray, as well as a component of <a href="/wiki/Bad_breath" title="Bad breath">bad breath</a> odor. Not all organic sulfur compounds smell unpleasant at all concentrations: the sulfur-containing <a href="/wiki/Terpene" title="Terpene">monoterpenoid</a> <a href="/wiki/Grapefruit_mercaptan" title="Grapefruit mercaptan">grapefruit mercaptan</a> in small concentrations is the characteristic scent of grapefruit, but has a generic thiol odor at larger concentrations. <a href="/wiki/Sulfur_mustard" class="mw-redirect" title="Sulfur mustard">Sulfur mustard</a>, a potent <a href="/wiki/Blister_agent" title="Blister agent">vesicant</a>, was <a href="/wiki/Chemical_weapons_in_World_War_I" title="Chemical weapons in World War I">used in World War I</a> as a disabling agent.<a href="#cite_note-60">[57]</a> Sulfur–sulfur bonds are a structural component used to stiffen rubber, similar to the disulfide bridges that rigidify proteins (see biological below). In the most common type of industrial "curing" or hardening and strengthening of natural <a href="/wiki/Rubber" class="mw-redirect" title="Rubber">rubber</a>, elemental sulfur is heated with the rubber to the point that chemical reactions form <a href="/wiki/Disulfide" title="Disulfide">disulfide</a> bridges between <a href="/wiki/Isoprene" title="Isoprene">isoprene</a> units of the polymer. This process, patented in 1843,[<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">citation needed</a>] made rubber a major industrial product, especially in automobile tires. Because of the heat and sulfur, the process was named <a href="/wiki/Vulcanization" title="Vulcanization">vulcanization</a>, after the Roman god of the forge and <a href="/wiki/Volcanism" title="Volcanism">volcanism</a>. </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(3)"><h2 id="History">History</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=15" title="Edit section: History" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-3 collapsible-block" id="mf-section-3"> <div class="mw-heading mw-heading3"><h3 id="Antiquity">Antiquity</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=16" title="Edit section: Antiquity" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:MODOAzufre.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/MODOAzufre.jpg/220px-MODOAzufre.jpg" decoding="async" width="220" height="164" class="mw-file-element" data-file-width="1853" data-file-height="1384"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 164px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/MODOAzufre.jpg/220px-MODOAzufre.jpg" data-width="220" data-height="164" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/MODOAzufre.jpg/330px-MODOAzufre.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/75/MODOAzufre.jpg/440px-MODOAzufre.jpg 2x" data-class="mw-file-element"> </a><figcaption>Pharmaceutical container for sulfur from the first half of the 20th century. From the <a href="/wiki/Museo_del_Objeto_del_Objeto" title="Museo del Objeto del Objeto">Museo del Objeto del Objeto</a> collection</figcaption></figure> Being abundantly available in native form, sulfur was known in ancient times and is referred to in the <a href="/wiki/Torah" title="Torah">Torah</a> (<a href="/wiki/Book_of_Genesis" title="Book of Genesis">Genesis</a>). <a href="/wiki/English_translations_of_the_Bible" class="mw-redirect" title="English translations of the Bible">English translations of the Christian Bible</a> commonly referred to burning sulfur as "brimstone", giving rise to the term "<a href="/wiki/Fire_and_brimstone" title="Fire and brimstone">fire-and-brimstone</a>" <a href="/wiki/Sermon" title="Sermon">sermons</a>, in which listeners are reminded of the fate of <a href="/wiki/Damnation" title="Damnation">eternal damnation</a> that await the unbelieving and unrepentant. It is from this part of the Bible<a href="#cite_note-61">[58]</a> that <a href="/wiki/Hell" title="Hell">Hell</a> is implied to "smell of sulfur" (likely due to its association with volcanic activity). According to the <a href="/wiki/Ebers_Papyrus" title="Ebers Papyrus">Ebers Papyrus</a>, a sulfur ointment was used in ancient <a href="/wiki/Egypt" title="Egypt">Egypt</a> to treat granular eyelids. Sulfur was used for <a href="/wiki/Fumigation" title="Fumigation">fumigation</a> in preclassical <a href="/wiki/Greece" title="Greece">Greece</a>;<a href="#cite_note-62">[59]</a> this is mentioned in the <a href="/wiki/Odyssey" title="Odyssey">Odyssey</a>.<a href="#cite_note-63">[60]</a> <a href="/wiki/Pliny_the_Elder" title="Pliny the Elder">Pliny the Elder</a> discusses sulfur in book 35 of his <a href="/wiki/Natural_History_(Pliny)" title="Natural History (Pliny)">Natural History</a>, saying that its best-known source is the island of <a href="/wiki/Melos" class="mw-redirect" title="Melos">Melos</a>. He mentions its use for fumigation, medicine, and bleaching cloth.<a href="#cite_note-64">[61]</a> A natural form of sulfur known as shiliuhuang (石硫黄) was known in China since the 6th century BC and found in <a href="/wiki/Hanzhong" title="Hanzhong">Hanzhong</a>.<a href="#cite_note-Zhang-1986-65">[62]</a> By the 3rd century, the Chinese had discovered that sulfur could be extracted from <a href="/wiki/Pyrite" title="Pyrite">pyrite</a>.<a href="#cite_note-Zhang-1986-65">[62]</a> Chinese <a href="/wiki/Daoists" class="mw-redirect" title="Daoists">Daoists</a> were interested in sulfur's flammability and its reactivity with certain metals, yet its earliest practical uses were found in <a href="/wiki/Traditional_Chinese_medicine" title="Traditional Chinese medicine">traditional Chinese medicine</a>.<a href="#cite_note-Zhang-1986-65">[62]</a> The <a href="/wiki/Wujing_Zongyao" title="Wujing Zongyao">Wujing Zongyao</a> of 1044 AD described various formulas for Chinese <a href="/wiki/Black_powder" class="mw-redirect" title="Black powder">black powder</a>, which is a mixture of <a href="/wiki/Potassium_nitrate" title="Potassium nitrate">potassium nitrate</a> (KNO 3), <a href="/wiki/Charcoal" title="Charcoal">charcoal</a>, and sulfur.<a href="#cite_note-66">[63]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1237032888/mw-parser-output/.tmulti"><div class="thumb tmulti tright"><div class="thumbinner multiimageinner" style="width:272px;max-width:272px"><div class="trow"><div class="tsingle" style="width:134px;max-width:134px"><div class="thumbimage" style="height:132px;overflow:hidden"><a href="/wiki/File:Sulphur_symbol_(fixed_width).svg" class="mw-file-description"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Sulphur_symbol_%28fixed_width%29.svg/132px-Sulphur_symbol_%28fixed_width%29.svg.png" decoding="async" width="132" height="132" class="mw-file-element" data-file-width="16" data-file-height="16"></noscript><span class="lazy-image-placeholder" style="width: 132px;height: 132px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Sulphur_symbol_%28fixed_width%29.svg/132px-Sulphur_symbol_%28fixed_width%29.svg.png" data-alt="" data-width="132" data-height="132" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Sulphur_symbol_%28fixed_width%29.svg/198px-Sulphur_symbol_%28fixed_width%29.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Sulphur_symbol_%28fixed_width%29.svg/264px-Sulphur_symbol_%28fixed_width%29.svg.png 2x" data-class="mw-file-element"> </a></div><div class="thumbcaption">Sulfur</div></div><div class="tsingle" style="width:134px;max-width:134px"><div class="thumbimage" style="height:132px;overflow:hidden"><a href="/wiki/File:Black_sulfur_symbol_(fixed_width).svg" class="mw-file-description"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5d/Black_sulfur_symbol_%28fixed_width%29.svg/132px-Black_sulfur_symbol_%28fixed_width%29.svg.png" decoding="async" width="132" height="132" class="mw-file-element" data-file-width="16" data-file-height="16"></noscript><span class="lazy-image-placeholder" style="width: 132px;height: 132px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5d/Black_sulfur_symbol_%28fixed_width%29.svg/132px-Black_sulfur_symbol_%28fixed_width%29.svg.png" data-alt="" data-width="132" data-height="132" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/5d/Black_sulfur_symbol_%28fixed_width%29.svg/198px-Black_sulfur_symbol_%28fixed_width%29.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/5d/Black_sulfur_symbol_%28fixed_width%29.svg/264px-Black_sulfur_symbol_%28fixed_width%29.svg.png 2x" data-class="mw-file-element"> </a></div><div class="thumbcaption">Brimstone</div></div></div><div class="trow" style="display:flex"><div class="thumbcaption">Alchemical signs for sulfur, or the <a href="/wiki/Combustibility_and_flammability" title="Combustibility and flammability">combustible</a> elements, and brimstone, an older/archaic name for sulfur<a href="#cite_note-67">[64]</a></div></div></div></div> Indian alchemists, practitioners of the "science of chemicals" (<a href="/wiki/Sanskrit_language" class="mw-redirect" title="Sanskrit language">Sanskrit</a>: रसशास्त्र, <a href="/wiki/Romanization_of_Sanskrit" class="mw-redirect" title="Romanization of Sanskrit">romanized</a>: rasaśāstra), wrote extensively about the use of sulfur in alchemical operations with mercury, from the eighth century AD onwards.<a href="#cite_note-White-1996-68">[65]</a> In the <a href="/wiki/Rasa_shastra" class="mw-redirect" title="Rasa shastra">rasaśāstra</a> tradition, sulfur is called "the smelly" (गन्धक, gandhaka). Early <a href="/wiki/Europe" title="Europe">European</a> <a href="/wiki/Alchemy" title="Alchemy">alchemists</a> gave sulfur a unique <a href="/wiki/Alchemical_symbol" title="Alchemical symbol">alchemical symbol</a>, a triangle atop a cross (🜍). (This is sometimes confused with the astronomical crossed-spear symbol ⚴ for <a href="/wiki/2_Pallas" title="2 Pallas">2 Pallas</a>.) The variation known as brimstone has a symbol combining a <a href="/wiki/Two-barred_cross" title="Two-barred cross">two-barred cross</a> atop a <a href="/wiki/Infinity_symbol" title="Infinity symbol">lemniscate</a> (🜏). In traditional skin treatment, elemental sulfur was used (mainly in creams) to alleviate such conditions as <a href="/wiki/Scabies" title="Scabies">scabies</a>, <a href="/wiki/Ringworm" class="mw-redirect" title="Ringworm">ringworm</a>, <a href="/wiki/Psoriasis" title="Psoriasis">psoriasis</a>, <a href="/wiki/Eczema" class="mw-redirect" title="Eczema">eczema</a>, and <a href="/wiki/Acne" title="Acne">acne</a>. The mechanism of action is unknown—though elemental sulfur does oxidize slowly to sulfurous acid, which is (through the action of <a href="/wiki/Sulfite" title="Sulfite">sulfite</a>) a mild reducing and antibacterial agent.<a href="#cite_note-69">[66]</a><a href="#cite_note-70">[67]</a><a href="#cite_note-71">[68]</a> <div class="mw-heading mw-heading3"><h3 id="Modern_times">Modern times</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=17" title="Edit section: Modern times" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e9/18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png/280px-18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png" decoding="async" width="280" height="205" class="mw-file-element" data-file-width="1117" data-file-height="819"></noscript><span class="lazy-image-placeholder" style="width: 280px;height: 205px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e9/18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png/280px-18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png" data-width="280" data-height="205" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e9/18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png/420px-18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/e9/18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png/560px-18810703_Sulphur_Soap_-_advertisement_in_The_Helena_Independent.png 2x" data-class="mw-file-element"> </a><figcaption>Sulfur has antifungal, antibacterial, and <a href="/wiki/Keratolytic" title="Keratolytic">keratolytic</a> activity; in the past it was used against acne vulgaris, rosacea, seborrheic dermatitis, dandruff, pityriasis versicolor, scabies, and warts.<a href="#cite_note-Gupta-2004-72">[69]</a> This 1881 advertisement baselessly claims efficacy against rheumatism, gout, baldness, and graying of hair.</figcaption></figure> Sulfur appears in a column of fixed (non-acidic) <a href="/wiki/Alkali" title="Alkali">alkali</a> in a chemical table of 1718.<a href="#cite_note-73">[70]</a> <a href="/wiki/Antoine_Lavoisier" title="Antoine Lavoisier">Antoine Lavoisier</a> used sulfur in combustion experiments, writing of some of these in 1777.<a href="#cite_note-74">[71]</a> Sulfur deposits in <a href="/wiki/Sicily" title="Sicily">Sicily</a> were the dominant source for more than a century. By the late 18th century, about 2,000 tonnes per year of sulfur were imported into <a href="/wiki/Marseille" title="Marseille">Marseille</a>, France, for the production of <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> for use in the <a href="/wiki/Leblanc_process" title="Leblanc process">Leblanc process</a>. In <a href="/wiki/Industrial_Revolution" title="Industrial Revolution">industrializing</a> Britain, with the repeal of <a href="/wiki/Tariff" title="Tariff">tariffs</a> on salt in 1824, demand for sulfur from Sicily surged. The increasing British control and exploitation of the mining, refining, and transportation of sulfur, coupled with the failure of this lucrative export to transform Sicily's backward and impoverished economy, led to the <a href="/wiki/Sulfur_Crisis_of_1840" class="mw-redirect" title="Sulfur Crisis of 1840">Sulfur Crisis of 1840</a>, when <a href="/wiki/Ferdinand_II_of_the_Two_Sicilies" title="Ferdinand II of the Two Sicilies">King Ferdinand II</a> gave a monopoly of the sulfur industry to a French firm, violating an earlier 1816 trade agreement with Britain. A peaceful solution was eventually negotiated by France.<a href="#cite_note-75">[72]</a><a href="#cite_note-76">[73]</a> In 1867, elemental sulfur was discovered in underground deposits in <a href="/wiki/Louisiana" title="Louisiana">Louisiana</a> and <a href="/wiki/Texas" title="Texas">Texas</a>. The highly successful <a href="/wiki/Frasch_process" title="Frasch process">Frasch process</a> was developed to extract this resource.<a href="#cite_note-Botsch-2001-77">[74]</a> In the late 18th century, <a href="/wiki/Furniture" title="Furniture">furniture</a> makers used molten sulfur to produce <a href="/wiki/Sulfur_inlay" title="Sulfur inlay">decorative inlays</a>.<a href="#cite_note-Mass-2003-78">[75]</a> Molten sulfur is sometimes still used for setting steel bolts into drilled concrete holes where high shock resistance is desired for floor-mounted equipment attachment points. Pure powdered sulfur was used as a medicinal tonic and laxative.<a href="#cite_note-Nehb-2006-50">[47]</a> Since the advent of the <a href="/wiki/Contact_process" title="Contact process">contact process</a>, the majority of sulfur is used to make sulfuric acid for a wide range of uses, particularly fertilizer.<a href="#cite_note-79">[76]</a> In recent times, the main source of sulfur has become <a href="/wiki/Petroleum" title="Petroleum">petroleum</a> and <a href="/wiki/Natural_gas" title="Natural gas">natural gas</a>. This is due to the requirement to remove sulfur from fuels in order to prevent <a href="/wiki/Acid_rain" title="Acid rain">acid rain</a>, and has resulted in a surplus of sulfur.<a href="#cite_note-Knight-2014-10">[10]</a> <div class="mw-heading mw-heading3"><h3 id="Spelling_and_etymology">Spelling and etymology</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=18" title="Edit section: Spelling and etymology" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Sulfur is derived from the Latin word sulpur, which was <a href="/wiki/Hellenized" class="mw-redirect" title="Hellenized">Hellenized</a> to sulphur in the erroneous belief that the Latin word came from Greek. This spelling was later reinterpreted as representing an /f/ sound and resulted in the spelling sulfur, which appears in Latin toward the end of the <a href="/wiki/Classical_antiquity" title="Classical antiquity">Classical period</a>. The true Ancient Greek word for sulfur, θεῖον, theîon (from earlier θέειον, théeion), is the source of the international chemical prefix <a href="/wiki/Thio-" title="Thio-">thio-</a>. The Modern Standard Greek word for sulfur is θείο, theío. In 12th-century <a href="/wiki/Anglo-Norman_language" title="Anglo-Norman language">Anglo-French</a>, it was sulfre. In the 14th century, the erroneously Hellenized Latin -ph- was restored in Middle English sulphre. By the 15th century, both full Latin spelling variants sulfur and sulphur became common in English. The parallel f~ph spellings continued in Britain until the 19th century, when the word was standardized as sulphur.<a href="#cite_note-OED-80">[77]</a> On the other hand, sulfur was the form chosen in the United States, whereas Canada uses both. The <a href="/wiki/International_Union_of_Pure_and_Applied_Chemistry" title="International Union of Pure and Applied Chemistry">IUPAC</a> adopted the spelling sulfur in 1990<a href="#cite_note-81">[78]</a><a href="#cite_note-82">[79]</a> as did the Nomenclature Committee of the <a href="/wiki/Royal_Society_of_Chemistry" title="Royal Society of Chemistry">Royal Society of Chemistry</a> in 1992, restoring the spelling sulfur to Britain.<a href="#cite_note-83">[80]</a> <a href="/wiki/Oxford_English_Dictionary" title="Oxford English Dictionary">Oxford Dictionaries</a> note that "in chemistry and other technical uses ... the -f- spelling is now the standard form for this and related words in British as well as US contexts, and is increasingly used in general contexts as well."<a href="#cite_note-84">[81]</a> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(4)"><h2 id="Production">Production</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=19" title="Edit section: Production" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-4 collapsible-block" id="mf-section-4"> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Soufre_extraction_1.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c8/Soufre_extraction_1.jpg/220px-Soufre_extraction_1.jpg" decoding="async" width="220" height="196" class="mw-file-element" data-file-width="1643" data-file-height="1464"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 196px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c8/Soufre_extraction_1.jpg/220px-Soufre_extraction_1.jpg" data-width="220" data-height="196" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c8/Soufre_extraction_1.jpg/330px-Soufre_extraction_1.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c8/Soufre_extraction_1.jpg/440px-Soufre_extraction_1.jpg 2x" data-class="mw-file-element"> </a><figcaption>Sicilian kiln used to obtain sulfur from volcanic rock (diagram from a 1906 chemistry book)</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Bergelut_dengan_asap_nan_beracun.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4a/Bergelut_dengan_asap_nan_beracun.jpg/170px-Bergelut_dengan_asap_nan_beracun.jpg" decoding="async" width="170" height="257" class="mw-file-element" data-file-width="1656" data-file-height="2500"></noscript><span class="lazy-image-placeholder" style="width: 170px;height: 257px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4a/Bergelut_dengan_asap_nan_beracun.jpg/170px-Bergelut_dengan_asap_nan_beracun.jpg" data-width="170" data-height="257" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4a/Bergelut_dengan_asap_nan_beracun.jpg/255px-Bergelut_dengan_asap_nan_beracun.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4a/Bergelut_dengan_asap_nan_beracun.jpg/340px-Bergelut_dengan_asap_nan_beracun.jpg 2x" data-class="mw-file-element"> </a><figcaption>Traditional sulfur mining at <a href="/wiki/Ijen" title="Ijen">Ijen Volcano</a>, East Java, Indonesia. This image shows the dangerous and rugged conditions the miners face, including toxic smoke and high drops, as well as their lack of protective equipment. The pipes over which they are standing are for condensing sulfur vapors.</figcaption></figure> Sulfur may be found by itself and historically was usually obtained in this form; <a href="/wiki/Pyrite" title="Pyrite">pyrite</a> has also been a source of sulfur.<a href="#cite_note-85">[82]</a> In volcanic regions in <a href="/wiki/Sicily" title="Sicily">Sicily</a>, in ancient times, it was found on the surface of the Earth, and the "<a href="/wiki/Sicilian_method" title="Sicilian method">Sicilian process</a>" was used: sulfur deposits were piled and stacked in brick kilns built on sloping hillsides, with airspaces between them. Then, some sulfur was pulverized, spread over the stacked ore and ignited, causing the free sulfur to melt down the hills. Eventually the surface-borne deposits played out, and miners excavated veins that ultimately dotted the Sicilian landscape with labyrinthine mines. Mining was unmechanized and labor-intensive, with pickmen freeing the ore from the rock, and mine-boys or <a href="/wiki/Carusu" title="Carusu">carusi</a> carrying baskets of ore to the surface, often through a mile or more of tunnels. Once the ore was at the surface, it was reduced and extracted in smelting ovens. The conditions in <a href="/wiki/Sulfur_mining_in_Sicily" title="Sulfur mining in Sicily">Sicilian sulfur mines</a> were horrific, prompting <a href="/wiki/Booker_T._Washington" title="Booker T. Washington">Booker T. Washington</a> to write "I am not prepared just now to say to what extent I believe in a physical hell in the next world, but a sulfur mine in Sicily is about the nearest thing to hell that I expect to see in this life."<a href="#cite_note-86">[83]</a> Sulfur is still mined from surface deposits in poorer nations with volcanoes, such as <a href="/wiki/Indonesia" title="Indonesia">Indonesia</a>, and worker conditions have not improved much since Booker T. Washington's days.<a href="#cite_note-87">[84]</a> Elemental sulfur was extracted from <a href="/wiki/Salt_dome" title="Salt dome">salt domes</a> (where it sometimes occurs in nearly pure form) until the late 20th century, when it became a side product of other industrial processes such as in oil refining, in which sulfur is undesired. As a mineral, native sulfur under salt domes is thought to be a fossil mineral resource, produced by the action of anaerobic bacteria on sulfate deposits. It was removed from such salt-dome mines mainly by the <a href="/wiki/Frasch_process" title="Frasch process">Frasch process</a>.<a href="#cite_note-Nehb-2006-50">[47]</a> In this method, superheated water was pumped into a native sulfur deposit to melt the sulfur, and then compressed air returned the 99.5% pure melted product to the surface. Throughout the 20th century this procedure produced elemental sulfur that required no further purification. Due to a limited number of such sulfur deposits and the high cost of working them, this process for mining sulfur has not had significant use anywhere in the world since 2002.<a href="#cite_note-Eow-2002-88">[85]</a><a href="#cite_note-Schreiner-2008-89">[86]</a> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:AlbertaSulfurAtVancouverBC.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/AlbertaSulfurAtVancouverBC.jpg/220px-AlbertaSulfurAtVancouverBC.jpg" decoding="async" width="220" height="122" class="mw-file-element" data-file-width="1350" data-file-height="750"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 122px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/AlbertaSulfurAtVancouverBC.jpg/220px-AlbertaSulfurAtVancouverBC.jpg" data-width="220" data-height="122" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/AlbertaSulfurAtVancouverBC.jpg/330px-AlbertaSulfurAtVancouverBC.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/AlbertaSulfurAtVancouverBC.jpg/440px-AlbertaSulfurAtVancouverBC.jpg 2x" data-class="mw-file-element"> </a><figcaption>Sulfur recovered from hydrocarbons in <a href="/wiki/Alberta" title="Alberta">Alberta</a>, stockpiled for shipment in <a href="/wiki/North_Vancouver_(city)" title="North Vancouver (city)">North Vancouver</a>, British Columbia</figcaption></figure> Since then, sulfur has typically been produced from petroleum, <a href="/wiki/Natural_gas" title="Natural gas">natural gas</a>, and related fossil resources, from which it is obtained mainly as <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a>.<a href="#cite_note-Knight-2014-10">[10]</a> <a href="/wiki/Organosulfur_compound" class="mw-redirect" title="Organosulfur compound">Organosulfur compounds</a>, undesirable impurities in petroleum, may be upgraded by subjecting them to <a href="/wiki/Hydrodesulfurization" title="Hydrodesulfurization">hydrodesulfurization</a>, which cleaves the C–S bonds:<a href="#cite_note-Eow-2002-88">[85]</a><a href="#cite_note-Schreiner-2008-89">[86]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">R-S-R + 2 H2 → 2 RH + H2S</div> The resulting hydrogen sulfide from this process, and also as it occurs in natural gas, is converted into elemental sulfur by the <a href="/wiki/Claus_process" title="Claus process">Claus process</a>, which entails oxidation of some hydrogen sulfide to sulfur dioxide and then the <a href="/wiki/Comproportionation" title="Comproportionation">comproportionation</a> of the two:<a href="#cite_note-Eow-2002-88">[85]</a><a href="#cite_note-Schreiner-2008-89">[86]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">3 O2 + 2 H2S → 2 SO2 + 2 H2O</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">SO2 + 2 H2S → 3 S + 2 H2O</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Sulfur_price_world_production.svg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6e/Sulfur_price_world_production.svg/300px-Sulfur_price_world_production.svg.png" decoding="async" width="300" height="159" class="mw-file-element" data-file-width="1251" data-file-height="663"></noscript><span class="lazy-image-placeholder" style="width: 300px;height: 159px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6e/Sulfur_price_world_production.svg/300px-Sulfur_price_world_production.svg.png" data-width="300" data-height="159" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6e/Sulfur_price_world_production.svg/450px-Sulfur_price_world_production.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6e/Sulfur_price_world_production.svg/600px-Sulfur_price_world_production.svg.png 2x" data-class="mw-file-element"> </a><figcaption>Production and price (US market) of elemental sulfur</figcaption></figure> Due to the high sulfur content of the <a href="/wiki/Athabasca_Oil_Sands" class="mw-redirect" title="Athabasca Oil Sands">Athabasca Oil Sands</a>, stockpiles of elemental sulfur from this process exist throughout <a href="/wiki/Alberta" title="Alberta">Alberta</a>, Canada.<a href="#cite_note-Hyndman-1982-90">[87]</a> Another way of storing sulfur is as a <a href="/wiki/Binder_(material)" title="Binder (material)">binder</a> for concrete, the resulting product having some desirable properties (see <a href="/wiki/Sulfur_concrete" title="Sulfur concrete">sulfur concrete</a>).<a href="#cite_note-Mohamed-2010-91">[88]</a> The world production of sulfur in 2011 amounted to 69 million tonnes (Mt), with more than 15 countries contributing more than 1 Mt each. Countries producing more than 5 Mt are <a href="/wiki/China" title="China">China</a> (9.6), the <a href="/wiki/United_States" title="United States">United States</a> (8.8), <a href="/wiki/Canada" title="Canada">Canada</a> (7.1) and <a href="/wiki/Russia" title="Russia">Russia</a> (7.1).<a href="#cite_note-92">[89]</a> Production has been slowly increasing from 1900 to 2010; the price was unstable in the 1980s and around 2010.<a href="#cite_note-Apodaca-2010-93">[90]</a> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(5)"><h2 id="Applications">Applications</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=20" title="Edit section: Applications" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-5 collapsible-block" id="mf-section-5"> <div class="mw-heading mw-heading3"><h3 id="Sulfuric_acid">Sulfuric acid</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=21" title="Edit section: Sulfuric acid" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Elemental sulfur is used mainly as a precursor to other chemicals. Approximately 85% (1989) is converted to <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> (H2SO4): <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1154941027">1⁄8 <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">S8 + <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1154941027">3⁄2 <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">O2 + <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2O → <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2SO4</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Sulfuric_acid_2000.png" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Sulfuric_acid_2000.png/300px-Sulfuric_acid_2000.png" decoding="async" width="300" height="132" class="mw-file-element" data-file-width="1425" data-file-height="625"></noscript><span class="lazy-image-placeholder" style="width: 300px;height: 132px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Sulfuric_acid_2000.png/300px-Sulfuric_acid_2000.png" data-width="300" data-height="132" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Sulfuric_acid_2000.png/450px-Sulfuric_acid_2000.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c5/Sulfuric_acid_2000.png/600px-Sulfuric_acid_2000.png 2x" data-class="mw-file-element"> </a><figcaption>Sulfuric acid production in 2000</figcaption></figure> In 2010, the United States produced more sulfuric acid than any other inorganic industrial chemical.<a href="#cite_note-Apodaca-2010-93">[90]</a> The principal use for the acid is the extraction of phosphate ores for the production of fertilizer manufacturing. Other applications of sulfuric acid include oil refining, wastewater processing, and mineral extraction.<a href="#cite_note-Nehb-2006-50">[47]</a> <div class="mw-heading mw-heading3"><h3 id="Other_important_sulfur_chemistry">Other important sulfur chemistry</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=22" title="Edit section: Other important sulfur chemistry" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Sulfur reacts directly with methane to give <a href="/wiki/Carbon_disulfide" title="Carbon disulfide">carbon disulfide</a>, which is used to manufacture <a href="/wiki/Cellophane" title="Cellophane">cellophane</a> and <a href="/wiki/Rayon" title="Rayon">rayon</a>.<a href="#cite_note-Nehb-2006-50">[47]</a> One of the uses of elemental sulfur is in <a href="/wiki/Vulcanization" title="Vulcanization">vulcanization</a> of rubber, where <a href="/wiki/Polysulfide" title="Polysulfide">polysulfide</a> chains crosslink organic polymers. Large quantities of <a href="/wiki/Sulfite" title="Sulfite">sulfites</a> are used to <a href="/wiki/Bleach_(chemical)" class="mw-redirect" title="Bleach (chemical)">bleach</a> <a href="/wiki/Paper" title="Paper">paper</a> and to preserve <a href="/wiki/Dried_fruit" title="Dried fruit">dried fruit</a>. Many <a href="/wiki/Surfactant" title="Surfactant">surfactants</a> and <a href="/wiki/Detergent" title="Detergent">detergents</a> (e.g. <a href="/wiki/Sodium_lauryl_sulfate" class="mw-redirect" title="Sodium lauryl sulfate">sodium lauryl sulfate</a>) are sulfate derivatives. <a href="/wiki/Calcium_sulfate" title="Calcium sulfate">Calcium sulfate</a>, gypsum (CaSO4·2H2O) is mined on the scale of 100 million <a href="/wiki/Tonne" title="Tonne">tonnes</a> each year for use in <a href="/wiki/Portland_cement" title="Portland cement">Portland cement</a> and fertilizers. When silver-based <a href="/wiki/Photography" title="Photography">photography</a> was widespread, sodium and ammonium <a href="/wiki/Sodium_thiosulfate" title="Sodium thiosulfate">thiosulfate</a> were widely used as "fixing agents". Sulfur is a component of <a href="/wiki/Gunpowder" title="Gunpowder">gunpowder</a> ("black powder"). <div class="mw-heading mw-heading3"><h3 id="Fertilizer">Fertilizer</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=23" title="Edit section: Fertilizer" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <a href="/wiki/Amino_acid" title="Amino acid">Amino acids</a> synthesized by <a href="/wiki/Organism" title="Organism">living organisms</a> such as <a href="/wiki/Methionine" title="Methionine">methionine</a> and <a href="/wiki/Cysteine" title="Cysteine">cysteine</a> contain <a href="/wiki/Organosulfur_compounds" class="mw-redirect" title="Organosulfur compounds">organosulfur</a> groups (<a href="/wiki/Thioester" title="Thioester">thioester</a> and <a href="/wiki/Thiol" title="Thiol">thiol</a> respectively). The <a href="/wiki/Antioxidant" title="Antioxidant">antioxidant</a> <a href="/wiki/Glutathione" title="Glutathione">glutathione</a> protecting many living organisms against <a href="/wiki/Free_radical" class="mw-redirect" title="Free radical">free radicals</a> and <a href="/wiki/Oxidative_stress" title="Oxidative stress">oxidative stress</a> also contains organic sulfur. Some <a href="/wiki/Crop" title="Crop">crops</a> such as <a href="/wiki/Onion" title="Onion">onion</a> and <a href="/wiki/Garlic" title="Garlic">garlic</a> also produce different <a href="/wiki/Organosulfur_compounds" class="mw-redirect" title="Organosulfur compounds">organosulfur compounds</a> such as <a href="/wiki/Syn-Propanethial-S-oxide" title="Syn-Propanethial-S-oxide">syn-propanethial-S-oxide</a> responsible of lacrymal irritation (onions), or <a href="/wiki/Diallyl_disulfide" title="Diallyl disulfide">diallyl disulfide</a> and <a href="/wiki/Allicin" title="Allicin">allicin</a> (garlic). <a href="/wiki/Sulfate" title="Sulfate">Sulfates</a>, commonly found in <a href="/wiki/Soil" title="Soil">soils</a> and <a href="/wiki/Groundwater" title="Groundwater">groundwaters</a> are often a sufficient natural source of sulfur for plants and bacteria. <a href="/wiki/Deposition_(aerosol_physics)" title="Deposition (aerosol physics)">Atmospheric deposition</a> of <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a> (SO2) is also a common artificial source (<a href="/wiki/Coal_combustion_products" title="Coal combustion products">coal combustion</a>) of sulfur for the soils. Under normal circumstances, in most agricultural soils, sulfur is not a <a href="/wiki/Limiting_factor" title="Limiting factor">limiting nutrient</a> for plants and <a href="/wiki/Microorganism" title="Microorganism">microorganisms</a> (see <a href="/wiki/Liebig%27s_law_of_the_minimum#Liebig's_barrel" title="Liebig's law of the minimum">Liebig's barrel</a>). However, in some circumstances, soils can be depleted in <a href="/wiki/Sulfate" title="Sulfate">sulfate</a>, e.g. if this later is leached by <a href="/wiki/Meteoric_water" title="Meteoric water">meteoric water</a> (<a href="/wiki/Rain" title="Rain">rain</a>) or if the requirements in sulfur for some types of crops are high. This explains that sulfur is increasingly recognized and used as a component of <a href="/wiki/Fertilizer" title="Fertilizer">fertilizers</a>. The most important form of sulfur for fertilizer is <a href="/wiki/Calcium_sulfate" title="Calcium sulfate">calcium sulfate</a>, commonly found in nature as the mineral <a href="/wiki/Gypsum" title="Gypsum">gypsum</a> (CaSO4·2H2O). Elemental sulfur is <a href="/wiki/Hydrophobic" class="mw-redirect" title="Hydrophobic">hydrophobic</a> (not soluble in water) and cannot be used directly by plants. Elemental sulfur (ES) is sometimes mixed with <a href="/wiki/Bentonite" title="Bentonite">bentonite</a> to amend depleted soils for crops with high requirement in organo-sulfur. Over time, <a href="/wiki/Redox" title="Redox">oxidation</a> <a href="/wiki/Abiotic_component" title="Abiotic component">abiotic</a> processes with <a href="/wiki/Earth_atmosphere" class="mw-redirect" title="Earth atmosphere">atmospheric</a> <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> and <a href="/wiki/Soil_microbiology" title="Soil microbiology">soil bacteria</a> can <a href="/wiki/Redox" title="Redox">oxidize</a> and convert elemental sulfur to soluble derivatives, which can then be used by microorganisms and plants. Sulfur improves the efficiency of other essential plant nutrients, particularly <a href="/wiki/Nitrate" title="Nitrate">nitrogen</a> and phosphorus.<a href="#cite_note-sulphurinstitute-2020-94">[91]</a> Biologically produced sulfur particles are naturally <a href="/wiki/Hydrophile" title="Hydrophile">hydrophilic</a> due to a <a href="/wiki/Biopolymer" title="Biopolymer">biopolymer</a> coating and are easier to disperse over the land in a spray of diluted slurry, resulting in a faster uptake by plants. The plants requirement for sulfur equals or exceeds the requirement for <a href="/wiki/Phosphorus" title="Phosphorus">phosphorus</a>. It is an <a href="/wiki/Plant_nutrition" title="Plant nutrition">essential nutrient for plant</a> growth, <a href="/wiki/Root_nodule" title="Root nodule">root nodule</a> formation of legumes, and immunity and defense systems. Sulfur deficiency has become widespread in many countries in Europe.<a href="#cite_note-95">[92]</a><a href="#cite_note-96">[93]</a><a href="#cite_note-97">[94]</a> Because atmospheric inputs of sulfur continue to decrease, the deficit in the sulfur input/output is likely to increase unless sulfur fertilizers are used. Atmospheric inputs of sulfur decrease because of actions taken to limit <a href="/wiki/Acid_rain" title="Acid rain">acid rains</a>.<a href="#cite_note-NASA-2011-98">[95]</a><a href="#cite_note-sulphurinstitute-2020-94">[91]</a> <div class="mw-heading mw-heading3"><h3 id="Fungicide_and_pesticide">Fungicide and pesticide</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=24" title="Edit section: Fungicide and pesticide" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Sulphur_Candle.jpg" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4f/Sulphur_Candle.jpg/180px-Sulphur_Candle.jpg" decoding="async" width="180" height="221" class="mw-file-element" data-file-width="343" data-file-height="422"></noscript><span class="lazy-image-placeholder" style="width: 180px;height: 221px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4f/Sulphur_Candle.jpg/180px-Sulphur_Candle.jpg" data-width="180" data-height="221" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4f/Sulphur_Candle.jpg/270px-Sulphur_Candle.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/4/4f/Sulphur_Candle.jpg 2x" data-class="mw-file-element"> </a><figcaption>Sulfur candle originally sold for home fumigation</figcaption></figure> Elemental sulfur is one of the oldest fungicides and <a href="/wiki/Pesticide" title="Pesticide">pesticides</a>. "Dusting sulfur", elemental sulfur in powdered form, is a common fungicide for grapes, strawberry, many vegetables and several other crops. It has a good efficacy against a wide range of <a href="/wiki/Powdery_mildew" title="Powdery mildew">powdery mildew</a> diseases as well as black spot. In organic production, sulfur is the most important fungicide. It is the only fungicide used in <a href="/wiki/Organic_agriculture" class="mw-redirect" title="Organic agriculture">organically</a> farmed apple production against the main disease <a href="/wiki/Apple_scab" title="Apple scab">apple scab</a> under colder conditions. Biosulfur (biologically produced elemental sulfur with hydrophilic characteristics) can also be used for these applications. Standard-formulation dusting sulfur is applied to crops with a sulfur duster or <a href="/wiki/Aerial_application" title="Aerial application">from a dusting plane</a>. Wettable sulfur is the commercial name for dusting sulfur formulated with additional ingredients to make it water <a href="/wiki/Miscibility" title="Miscibility">miscible</a>.<a href="#cite_note-Mohamed-2010-91">[88]</a><a href="#cite_note-99">[96]</a> It has similar applications and is used as a <a href="/wiki/Fungicide" title="Fungicide">fungicide</a> against <a href="/wiki/Mildew" title="Mildew">mildew</a> and other mold-related problems with plants and soil. Elemental sulfur powder is used as an "<a href="/wiki/Organic_farming" title="Organic farming">organic</a>" (i.e., "green") <a href="/wiki/Insecticide" title="Insecticide">insecticide</a> (actually an <a href="/wiki/Acaricide" title="Acaricide">acaricide</a>) against <a href="/wiki/Tick" title="Tick">ticks</a> and <a href="/wiki/Mite" title="Mite">mites</a>. A common method of application is dusting the clothing or limbs with sulfur powder. A diluted solution of <a href="/wiki/Lime_sulfur" title="Lime sulfur">lime sulfur</a> (made by combining <a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide">calcium hydroxide</a> with elemental sulfur in water) is used as a dip for pets to destroy <a href="/wiki/Ringworm" class="mw-redirect" title="Ringworm">ringworm (fungus)</a>, <a href="/wiki/Mange" title="Mange">mange</a>, and other <a href="/wiki/Cutaneous_conditions" class="mw-redirect" title="Cutaneous conditions">dermatoses</a> and <a href="/wiki/Parasitism" title="Parasitism">parasites</a>. Sulfur candles of almost pure sulfur were burned to <a href="/wiki/Fumigant" class="mw-redirect" title="Fumigant">fumigate</a> structures and wine barrels, but are now considered too toxic for residences. <div class="mw-heading mw-heading3"><h3 id="Pharmaceuticals">Pharmaceuticals</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=25" title="Edit section: Pharmaceuticals" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Sulfur_(pharmacy)" class="mw-redirect" title="Sulfur (pharmacy)">Sulfur (pharmacy)</a></div> Sulfur (specifically <a href="/wiki/Octasulfur" title="Octasulfur">octasulfur</a>, S8) is used in pharmaceutical skin preparations for the treatment of <a href="/wiki/Acne" title="Acne">acne</a> and other conditions. It acts as a <a href="/wiki/Keratolytic" title="Keratolytic">keratolytic</a> agent and also kills bacteria, fungi, <a href="/wiki/Scabies" title="Scabies">scabies</a> mites, and other parasites.<a href="#cite_note-Springer-1978-100">[97]</a> Precipitated sulfur and colloidal sulfur are used, in form of <a href="/wiki/Lotion" title="Lotion">lotions</a>, creams, powders, soaps, and bath additives, for the treatment of <a href="/wiki/Acne_vulgaris" class="mw-redirect" title="Acne vulgaris">acne vulgaris</a>, <a href="/wiki/Acne_rosacea" class="mw-redirect" title="Acne rosacea">acne rosacea</a>, and <a href="/wiki/Seborrhoeic_dermatitis" title="Seborrhoeic dermatitis">seborrhoeic dermatitis</a>.<a href="#cite_note-Arzneibuch-Kommentar-101">[98]</a> Many drugs contain sulfur.<a href="#cite_note-102">[99]</a> Early examples include antibacterial <a href="/wiki/Sulfonamide_(medicine)" title="Sulfonamide (medicine)">sulfonamides</a>, known as sulfa drugs. A more recent example is mucolytic <a href="/wiki/Acetylcysteine" title="Acetylcysteine">acetylcysteine</a>. Sulfur is a part of many bacterial defense molecules. Most <a href="/wiki/%CE%92-lactam" class="mw-redirect" title="Β-lactam">β-lactam</a> antibiotics, including the <a href="/wiki/Penicillin" title="Penicillin">penicillins</a>, <a href="/wiki/Cephalosporins" class="mw-redirect" title="Cephalosporins">cephalosporins</a> and <a href="/wiki/Monobactam" title="Monobactam">monobactams</a> contain sulfur.<a href="#cite_note-Cremlyn-1996-58">[55]</a> <div class="mw-heading mw-heading3"><h3 id="Batteries">Batteries</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=26" title="Edit section: Batteries" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Due to their high energy density and the availability of sulfur, there is ongoing research in creating rechargeable <a href="/wiki/Lithium%E2%80%93sulfur_battery" title="Lithium–sulfur battery">lithium–sulfur batteries</a>. Until now, carbonate electrolytes have caused failures in such batteries after a single cycle. In February 2022, researchers at <a href="/wiki/Drexel_University" title="Drexel University">Drexel University</a> have not only created a prototypical battery that lasted 4000 recharge cycles, but also found the first monoclinic gamma sulfur that remained stable below 95 degrees Celsius.<a href="#cite_note-103">[100]</a> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(6)"><h2 id="Biological_role">Biological role</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=27" title="Edit section: Biological role" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-6 collapsible-block" id="mf-section-6"> Sulfur is an essential component of all living <a href="/wiki/Cell_(biology)" title="Cell (biology)">cells</a>. It is the eighth most abundant element in the human body by weight,<a href="#cite_note-sulphurinstitute-2021-104">[101]</a> about equal in abundance to <a href="/wiki/Potassium" title="Potassium">potassium</a>, and slightly greater than <a href="/wiki/Sodium" title="Sodium">sodium</a> and <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>.<a href="#cite_note-105">[102]</a> A 70 kg (150 lb) human body contains about 140 grams (4.9 oz) of sulfur.<a href="#cite_note-106">[103]</a> The main dietary source of sulfur for humans is sulfur-containing amino-acids,<a href="#cite_note-Parcell-2002-107">[104]</a> which can be found in plant and animal proteins.<a href="#cite_note-Ingenbleek-2013-108">[105]</a> <div class="mw-heading mw-heading3"><h3 id="Transferring_sulfur_between_inorganic_and_biomolecules">Transferring sulfur between inorganic and biomolecules</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=28" title="Edit section: Transferring sulfur between inorganic and biomolecules" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Sulfur_cycle" title="Sulfur cycle">Sulfur cycle</a> and <a href="/wiki/Sulfur_metabolism" title="Sulfur metabolism">Sulfur metabolism</a></div> In the 1880s, while studying <a href="/wiki/Beggiatoa" title="Beggiatoa">Beggiatoa</a> (a bacterium living in a sulfur rich environment), <a href="/wiki/Sergei_Winogradsky" title="Sergei Winogradsky">Sergei Winogradsky</a> found that it oxidized <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a> (H2S) as an energy source, forming intracellular sulfur droplets. Winogradsky referred to this form of metabolism as inorgoxidation (oxidation of inorganic compounds).<a href="#cite_note-109">[106]</a> Another contributor, who continued to study it was <a href="/wiki/Selman_Waksman" title="Selman Waksman">Selman Waksman</a>.<a href="#cite_note-110">[107]</a> Primitive bacteria that live around deep ocean <a href="/wiki/Hydrothermal_vent" title="Hydrothermal vent">volcanic vents</a> oxidize hydrogen sulfide for their nutrition, as discovered by <a href="/wiki/Robert_Ballard" title="Robert Ballard">Robert Ballard</a>.<a href="#cite_note-BBC_Elements-2014-11">[11]</a> Sulfur oxidizers can use as energy sources reduced sulfur compounds, including hydrogen sulfide, elemental sulfur, <a href="/wiki/Sulfite" title="Sulfite">sulfite</a>, <a href="/wiki/Thiosulfate" title="Thiosulfate">thiosulfate</a>, and various <a href="/wiki/Polythionates" title="Polythionates">polythionates</a> (e.g., <a href="/wiki/Tetrathionate" title="Tetrathionate">tetrathionate</a>).<a href="#cite_note-111">[108]</a> They depend on enzymes such as <a href="/wiki/Sulfur_dioxygenase" title="Sulfur dioxygenase">sulfur oxygenase</a> and <a href="/wiki/Sulfite_oxidase" title="Sulfite oxidase">sulfite oxidase</a> to oxidize sulfur to sulfate. Some <a href="/wiki/Lithotroph" title="Lithotroph">lithotrophs</a> can even use the energy contained in sulfur compounds to produce sugars, a process known as <a href="/wiki/Chemosynthesis" title="Chemosynthesis">chemosynthesis</a>. Some <a href="/wiki/Bacteria" title="Bacteria">bacteria</a> and <a href="/wiki/Archaea" title="Archaea">archaea</a> use hydrogen sulfide in place of water as the <a href="/wiki/Electron_donor" title="Electron donor">electron donor</a> in chemosynthesis, a process similar to <a href="/wiki/Photosynthesis" title="Photosynthesis">photosynthesis</a> that produces sugars and uses oxygen as the <a href="/wiki/Electron_acceptor" title="Electron acceptor">electron acceptor</a>. Sulfur-based chemosynthesis may be simplifiedly compared with photosynthesis: <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">H2S + CO2 → sugars + S</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">H2O + CO2 → sugars + O2</div> There are bacteria combining these two ways of nutrition: <a href="/wiki/Green_sulfur_bacteria" title="Green sulfur bacteria">green sulfur bacteria</a> and <a href="/wiki/Purple_sulfur_bacteria" title="Purple sulfur bacteria">purple sulfur bacteria</a>.<a href="#cite_note-112">[109]</a> Also sulfur-oxidizing bacteria can go into symbiosis with larger organisms, enabling the later to use hydrogen sulfide as food to be oxidized. Example: the <a href="/wiki/Giant_tube_worm" class="mw-redirect" title="Giant tube worm">giant tube worm</a>.<a href="#cite_note-113">[110]</a> There are <a href="/wiki/Sulfate-reducing_bacteria" class="mw-redirect" title="Sulfate-reducing bacteria">sulfate-reducing bacteria</a>, that, by contrast, "breathe sulfate" instead of oxygen. They use organic compounds or molecular hydrogen as the energy source. They use sulfur as the electron acceptor, and reduce various oxidized sulfur compounds back into sulfide, often into hydrogen sulfide. They can grow on other partially oxidized sulfur compounds (e.g. thiosulfates, thionates, polysulfides, sulfites). There are studies pointing that many deposits of native sulfur in places that were the bottom of <a href="/wiki/Tethys_Ocean" title="Tethys Ocean">the ancient oceans</a> have biological origin.<a href="#cite_note-114">[111]</a><a href="#cite_note-115">[112]</a><a href="#cite_note-116">[113]</a> These studies indicate that this native sulfur have been obtained through biological activity, but what is responsible for that (sulfur-oxidizing bacteria or sulfate-reducing bacteria) is still unknown for sure. Sulfur is absorbed by <a href="/wiki/Plant" title="Plant">plants</a> <a href="/wiki/Root" title="Root">roots</a> from soil as <a href="/wiki/Sulfate" title="Sulfate">sulfate</a> and transported as a phosphate ester. Sulfate is reduced to sulfide via sulfite before it is incorporated into <a href="/wiki/Cysteine" title="Cysteine">cysteine</a> and other organosulfur compounds.<a href="#cite_note-Heldt-1996-117">[114]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SO2−4 → <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SO2−3 → <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">H2S → cysteine (thiol) → methionine (thioether)</div> While the plants' role in transferring sulfur to animals by <a href="/wiki/Food_chain" title="Food chain">food chains</a> is more or less understood, the role of sulfur bacteria is just getting investigated.<a href="#cite_note-118">[115]</a><a href="#cite_note-119">[116]</a> <div class="mw-heading mw-heading3"><h3 id="Protein_and_organic_metabolites">Protein and organic metabolites</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=29" title="Edit section: Protein and organic metabolites" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> In all forms of life, most of the sulfur is contained in two <a href="/wiki/Proteinogenic_amino_acid" title="Proteinogenic amino acid">proteinogenic amino acids</a> (<a href="/wiki/Cysteine" title="Cysteine">cysteine</a> and <a href="/wiki/Methionine" title="Methionine">methionine</a>), thus the element is present in all <a href="/wiki/Protein" title="Protein">proteins</a> that contain these amino acids, as well as in respective <a href="/wiki/Peptide" title="Peptide">peptides</a>.<a href="#cite_note-120">[117]</a> Some of the sulfur is comprised in certain metabolites—many of which are <a href="/wiki/Cofactor_(biochemistry)" title="Cofactor (biochemistry)">cofactors</a>—and sulfated polysaccharides of <a href="/wiki/Connective_tissue" title="Connective tissue">connective tissue</a> (<a href="/wiki/Chondroitin_sulfate" title="Chondroitin sulfate">chondroitin sulfates</a>, <a href="/wiki/Heparin" title="Heparin">heparin</a>). <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Disulfide-bridges-made-in-Avogadro.png" class="mw-file-description"><noscript><img alt="Disulfide bonds between two alpha-helix" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5e/Disulfide-bridges-made-in-Avogadro.png/220px-Disulfide-bridges-made-in-Avogadro.png" decoding="async" width="220" height="334" class="mw-file-element" data-file-width="792" data-file-height="1201"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 334px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5e/Disulfide-bridges-made-in-Avogadro.png/220px-Disulfide-bridges-made-in-Avogadro.png" data-alt="Disulfide bonds between two alpha-helix" data-width="220" data-height="334" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/5e/Disulfide-bridges-made-in-Avogadro.png/330px-Disulfide-bridges-made-in-Avogadro.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/5e/Disulfide-bridges-made-in-Avogadro.png/440px-Disulfide-bridges-made-in-Avogadro.png 2x" data-class="mw-file-element"> </a><figcaption>Schematic representation of disulfide bridges (in yellow) between two protein helices</figcaption></figure> Proteins, to execute their <a href="/wiki/Protein#Cellular_functions" title="Protein">biological function</a>, need to have specific space geometry. Formation of this geometry is performed in a process called <a href="/wiki/Protein_folding" title="Protein folding">protein folding</a>, and is provided by intra- and inter-molecular bonds. The process has several stages. While at premier stages a polypeptide chain folds due to <a href="/wiki/Hydrogen_bond" title="Hydrogen bond">hydrogen bonds</a>, at later stages folding is provided (apart from hydrogen bonds) by <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bonds</a> between two sulfur atoms of two cysteine residues (so called disulfide bridges) at different places of a chain (tertiary protein structure) as well as between two cysteine residues in two separated protein subunits (quaternary protein structure). Both structures easily may be seen in <a href="/wiki/Insulin" title="Insulin">insulin</a>. As the <a href="/wiki/Bond_energy" title="Bond energy">bond energy</a> of a covalent disulfide bridge is higher than the energy of a <a href="/wiki/Coordinate_covalent_bond" title="Coordinate covalent bond">coordinate bond</a> or hydrophobic interaction, higher disulfide bridges content leads to higher energy needed for protein <a href="/wiki/Denaturation_(biochemistry)" title="Denaturation (biochemistry)">denaturation</a>. In general disulfide bonds are necessary in proteins functioning outside cellular space, and they do not change proteins' conformation (geometry), but serve as its stabilizers.<a href="#cite_note-121">[118]</a> Within <a href="/wiki/Cytoplasm" title="Cytoplasm">cytoplasm</a> cysteine residues of proteins are saved in reduced state (i.e. in -SH form) by <a href="/wiki/Thioredoxin" title="Thioredoxin">thioredoxins</a>.<a href="#cite_note-122">[119]</a> This property manifests in following examples. <a href="/wiki/Lysozyme" title="Lysozyme">Lysozyme</a> is stable enough to be applied as a drug.<a href="#cite_note-123">[120]</a> Feathers and hair have relative strength, and consisting in them <a href="/wiki/Keratin" title="Keratin">keratin</a> is considered indigestible by most organisms. However, there are fungi and bacteria containing <a href="/wiki/Keratinase" title="Keratinase">keratinase</a>, and are able to destruct keratin. Many important cellular enzymes use prosthetic groups ending with -SH moieties to handle reactions involving acyl-containing biochemicals: two common examples from basic metabolism are <a href="/wiki/Coenzyme_A" title="Coenzyme A">coenzyme A</a> and <a href="/wiki/Alpha-lipoic_acid" class="mw-redirect" title="Alpha-lipoic acid">alpha-lipoic acid</a>.<a href="#cite_note-Nelson-2000-124">[121]</a> Cysteine-related metabolites <a href="/wiki/Homocysteine" title="Homocysteine">homocysteine</a> and <a href="/wiki/Taurine" title="Taurine">taurine</a> are other sulfur-containing amino acids that are similar in structure, but not coded by <a href="/wiki/DNA" title="DNA">DNA</a>, and are not part of the <a href="/wiki/Primary_structure" class="mw-redirect" title="Primary structure">primary structure</a> of proteins, take part in various locations of mammalian physiology.<a href="#cite_note-125">[122]</a><a href="#cite_note-126">[123]</a> Two of the 13 classical vitamins, <a href="/wiki/Biotin" title="Biotin">biotin</a> and <a href="/wiki/Thiamine" title="Thiamine">thiamine</a>, contain sulfur, and serve as cofactors to several enzymes.<a href="#cite_note-127">[124]</a><a href="#cite_note-128">[125]</a> In intracellular chemistry, sulfur operates as a carrier of reducing hydrogen and its electrons for cellular repair of oxidation. Reduced <a href="/wiki/Glutathione" title="Glutathione">glutathione</a>, a sulfur-containing tripeptide, is a reducing agent through its sulfhydryl (–SH) moiety derived from <a href="/wiki/Cysteine" title="Cysteine">cysteine</a>. <a href="/wiki/Methanogenesis" title="Methanogenesis">Methanogenesis</a>, the route to most of the world's methane, is a multistep biochemical transformation of <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a>. This conversion requires several organosulfur cofactors. These include <a href="/wiki/Coenzyme_M" title="Coenzyme M">coenzyme M</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CH3SCH2CH2SO−3, the immediate precursor to <a href="/wiki/Methane" title="Methane">methane</a>.<a href="#cite_note-129">[126]</a> <div class="mw-heading mw-heading3"><h3 id="Metalloproteins_and_inorganic_cofactors">Metalloproteins and inorganic cofactors</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=30" title="Edit section: Metalloproteins and inorganic cofactors" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> Metalloproteins—in which the active site is a transition metal ion (or metal-sulfide cluster) often coordinated by sulfur atoms of cysteine residues<a href="#cite_note-130">[127]</a>—are essential components of enzymes involved in electron transfer processes. Examples include <a href="/wiki/Plastocyanin" title="Plastocyanin">plastocyanin</a> (Cu2+) and <a href="/wiki/Nitrous-oxide_reductase" title="Nitrous-oxide reductase">nitrous oxide reductase</a> (Cu–S). The function of these enzymes is dependent on the fact that the transition metal ion can undergo <a href="/wiki/Redox_reaction" class="mw-redirect" title="Redox reaction">redox reactions</a>. Other examples include many zinc proteins,<a href="#cite_note-131">[128]</a> as well as <a href="/wiki/Iron%E2%80%93sulfur_cluster" title="Iron–sulfur cluster">iron–sulfur clusters</a>. Most pervasive are the <a href="/wiki/Ferrodoxin" class="mw-redirect" title="Ferrodoxin">ferrodoxins</a>, which serve as electron shuttles in cells. In bacteria, the important <a href="/wiki/Nitrogenase" title="Nitrogenase">nitrogenase</a> enzymes contain an Fe–Mo–S cluster and is a <a href="/wiki/Catalyst" class="mw-redirect" title="Catalyst">catalyst</a> that performs the important function of <a href="/wiki/Nitrogen_fixation" title="Nitrogen fixation">nitrogen fixation</a>, converting atmospheric nitrogen to ammonia that can be used by microorganisms and plants to make proteins, DNA, RNA, alkaloids, and the other organic nitrogen compounds necessary for life.<a href="#cite_note-132">[129]</a> Sulfur is also present in <a href="/wiki/Molybdenum_cofactor" title="Molybdenum cofactor">molybdenum cofactor</a>.<a href="#cite_note-133">[130]</a> <dl><dd><figure class="mw-default-size mw-halign-center" typeof="mw:File/Thumb"><a href="/wiki/File:FdRedox.png" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6b/FdRedox.png/660px-FdRedox.png" decoding="async" width="660" height="150" class="mw-file-element" data-file-width="1904" data-file-height="434"></noscript><span class="lazy-image-placeholder" style="width: 660px;height: 150px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6b/FdRedox.png/660px-FdRedox.png" data-width="660" data-height="150" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6b/FdRedox.png/990px-FdRedox.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6b/FdRedox.png/1320px-FdRedox.png 2x" data-class="mw-file-element"> </a><figcaption>Easiness of electron flow in a cluster provides catalytic effect of a respective enzyme.</figcaption></figure></dd></dl> <div class="mw-heading mw-heading3"><h3 id="Sulfate">Sulfate</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=31" title="Edit section: Sulfate" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Sulfation#Sulfation_in_biology" title="Sulfation">Sulfation § Sulfation in biology</a></div> <div class="mw-heading mw-heading3"><h3 id="Deficiency">Deficiency</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=32" title="Edit section: Deficiency" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> In humans <a href="/wiki/Methionine" title="Methionine">methionine</a> is an <a href="/wiki/Essential_amino_acid" title="Essential amino acid">essential amino acid</a>; <a href="/wiki/Cysteine" title="Cysteine">cysteine</a> is conditionally essential and may be synthesized from non-essential <a href="/wiki/Serine" title="Serine">serine</a> (sulfur donor would be methionine in this case). Dietary deficiency rarely happens in common conditions. Artificial methionine deficiency is attempted to apply in cancer treatment,<a href="#cite_note-134">[131]</a> but the method is still potentially dangerous.<a href="#cite_note-135">[132]</a> <a href="/w/index.php?title=Isolated_sulfite_oxidase_deficiency&action=edit&redlink=1" class="new" title="Isolated sulfite oxidase deficiency (page does not exist)">Isolated sulfite oxidase deficiency</a> is a rare, fatal genetic disease preventing production of <a href="/wiki/Sulfite_oxidase" title="Sulfite oxidase">sulfite oxidase</a>, needed to metabolize sulfites to sulfates.<a href="#cite_note-136">[133]</a> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(7)"><h2 id="Precautions">Precautions</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=33" title="Edit section: Precautions" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-7 collapsible-block" id="mf-section-7"> <style data-mw-deduplicate="TemplateStyles:r1084375498">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}</style> <table class="infobox ib-chembox"> <caption>Sulfur </caption> <tbody><tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Hazards </th></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals" title="Globally Harmonized System of Classification and Labelling of Chemicals">GHS labelling</a>: </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_hazard_pictograms" title="GHS hazard pictograms">Pictograms</a></div> </td> <td><a href="/wiki/File:GHS-pictogram-exclam.svg" class="mw-file-description" title="GHS07: Exclamation mark"><noscript><img alt="GHS07: Exclamation mark" src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/50px-GHS-pictogram-exclam.svg.png" decoding="async" width="50" height="50" class="mw-file-element" data-file-width="512" data-file-height="512"></noscript><span class="lazy-image-placeholder" style="width: 50px;height: 50px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/50px-GHS-pictogram-exclam.svg.png" data-alt="GHS07: Exclamation mark" data-width="50" data-height="50" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/75px-GHS-pictogram-exclam.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/100px-GHS-pictogram-exclam.svg.png 2x" data-class="mw-file-element"> </a> <a href="/wiki/File:GHS-pictogram-flamme.svg" class="mw-file-description" title="GHS02: Flammable"><noscript><img alt="GHS02: Flammable" src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/GHS-pictogram-flamme.svg/50px-GHS-pictogram-flamme.svg.png" decoding="async" width="50" height="50" class="mw-file-element" data-file-width="512" data-file-height="512"></noscript><span class="lazy-image-placeholder" style="width: 50px;height: 50px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/GHS-pictogram-flamme.svg/50px-GHS-pictogram-flamme.svg.png" data-alt="GHS02: Flammable" data-width="50" data-height="50" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/GHS-pictogram-flamme.svg/75px-GHS-pictogram-flamme.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6d/GHS-pictogram-flamme.svg/100px-GHS-pictogram-flamme.svg.png 2x" data-class="mw-file-element"> </a> </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals#Signal_word" title="Globally Harmonized System of Classification and Labelling of Chemicals">Signal word</a></div> </td> <td>Warning </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_hazard_statements" title="GHS hazard statements">Hazard statements</a></div> </td> <td><abbr class="abbr" title="H315: Causes skin irritation">H315</abbr><a href="#cite_note-137">[134]</a> </td></tr> <tr> <td><a href="/wiki/NFPA_704" title="NFPA 704">NFPA 704</a> (fire diamond) </td> <td><style data-mw-deduplicate="TemplateStyles:r1170367383">.mw-parser-output .nfpa-704-diamond-ref{float:right;padding:1px;text-align:right}.mw-parser-output .nfpa-704-diamond-container{width:82px;font-family:sans-serif;margin:0 auto}.mw-parser-output .nfpa-704-diamond-container-ref{float:left;margin-left:1em}.mw-parser-output .nfpa-704-diamond-images{float:left;font-size:20px;text-align:center;position:relative;height:80px;width:80px;padding:1px}.mw-parser-output .nfpa-704-diamond-map{position:absolute;height:80px;width:80px}.mw-parser-output .nfpa-704-diamond .noresize{margin:0 auto}.mw-parser-output .nfpa-704-diamond-code{line-height:1em;text-align:center;position:absolute}.mw-parser-output .nfpa-704-diamond-code>a{color:black}.mw-parser-output .nfpa-704-diamond-blue{width:13px;top:31px;left:15px}.mw-parser-output .nfpa-704-diamond-red{width:12px;top:12px;left:35px}.mw-parser-output .nfpa-704-diamond-yellow{width:13px;top:31px;left:54px}.mw-parser-output .nfpa-704-diamond-white-image{position:relative;top:51px;left:0}.mw-parser-output .nfpa-704-diamond-white-text{vertical-align:middle;text-align:center;line-height:80%;position:absolute;top:52px}.mw-parser-output .nfpa-704-diamond-white-text a>span{position:absolute;color:black}.mw-parser-output .nfpa-704-diamond-white-wors{font-size:15px;width:23px;left:29px}.mw-parser-output .nfpa-704-diamond-white-wox{font-size:15px;font-stretch:condensed;width:21px;line-height:80%;top:-4px;left:29px}.mw-parser-output .nfpa-704-diamond-white-abcp{font-size:13.5px;font-stretch:condensed;width:28px;left:26px}.mw-parser-output .nfpa-704-diamond-white-ac{font-size:10px;width:30px;left:25px}.mw-parser-output .nfpa-704-diamond-white-strike{text-decoration:line-through}</style><div class="nfpa-704-diamond notheme"><div class="nfpa-74-diamond-refs"><a href="#cite_note-138">[135]</a></div><div class="nfpa-704-diamond-container nfpa-704-diamond-container-ref"><div class="nfpa-704-diamond-images nounderlines"> <div class="nfpa-704-diamond-map"><figure class="noresize" typeof="mw:File"><noscript><img alt="NFPA 704 four-colored diamond" src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/80px-NFPA_704.svg.png" decoding="async" width="80" height="80" class="mw-file-element" data-file-width="512" data-file-height="512" usemap="#ImageMap_482e25fdfe95519d"></noscript><span class="lazy-image-placeholder" style="width: 80px;height: 80px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/80px-NFPA_704.svg.png" data-alt="NFPA 704 four-colored diamond" data-width="80" data-height="80" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/120px-NFPA_704.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/160px-NFPA_704.svg.png 2x" data-class="mw-file-element" data-usemap="#ImageMap_482e25fdfe95519d"> <map name="ImageMap_482e25fdfe95519d"><area href="/wiki/NFPA_704#Blue" shape="poly" coords="23,23,47,47,23,70,0,47" alt="Health 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroform" title="Health 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroform"><area href="/wiki/NFPA_704#Red" shape="poly" coords="47,0,70,23,47,47,23,23" alt="Flammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oil" title="Flammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oil"><area href="/wiki/NFPA_704#Yellow" shape="poly" coords="70,23,94,47,70,70,47,47" alt="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen"><area href="/wiki/NFPA_704#White" shape="poly" coords="47,47,70,70,47,94,23,70" alt="Special hazards (white): no code" title="Special hazards (white): no code"></map><figcaption></figcaption></figure></div><div class="nfpa-704-diamond-code nfpa-704-diamond-blue"> <a href="/wiki/NFPA_704#Blue" title="NFPA 704">2</a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-red"> <a href="/wiki/NFPA_704#Red" title="NFPA 704">1</a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-yellow"> <a href="/wiki/NFPA_704#Yellow" title="NFPA 704">0</a></div></div></div></div> </td></tr> </tbody></table> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Acid_rain_woods1.JPG" class="mw-file-description"><noscript><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Acid_rain_woods1.JPG/220px-Acid_rain_woods1.JPG" decoding="async" width="220" height="165" class="mw-file-element" data-file-width="960" data-file-height="720"></noscript><span class="lazy-image-placeholder" style="width: 220px;height: 165px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Acid_rain_woods1.JPG/220px-Acid_rain_woods1.JPG" data-width="220" data-height="165" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Acid_rain_woods1.JPG/330px-Acid_rain_woods1.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Acid_rain_woods1.JPG/440px-Acid_rain_woods1.JPG 2x" data-class="mw-file-element"> </a><figcaption>Effect of acid rain on a forest, Jizera Mountains, Czech Republic</figcaption></figure> Though elemental sulfur is only minimally absorbed through the skin and is of low toxicity to humans, inhalation of sulfur dust or contact with eyes or skin may cause irritation. Excessive ingestion of sulfur can cause a burning sensation or diarrhea,<a href="#cite_note-139">[136]</a> and cases of life-threatening metabolic acidosis have been reported after patients deliberately consumed sulfur as a folk remedy.<a href="#cite_note-140">[137]</a><a href="#cite_note-141">[138]</a> <div class="mw-heading mw-heading3"><h3 id="Toxicity_of_sulfur_compounds">Toxicity of sulfur compounds</h3> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=34" title="Edit section: Toxicity of sulfur compounds" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div> When sulfur burns in air, it produces <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a>. In water, this gas produces sulfurous acid and sulfites; sulfites are antioxidants that inhibit growth of aerobic bacteria and a useful <a href="/wiki/Food_additive" title="Food additive">food additive</a> in small amounts. At high concentrations these acids harm the <a href="/wiki/Human_lungs" class="mw-redirect" title="Human lungs">lungs</a>, <a href="/wiki/Human_eyes" class="mw-redirect" title="Human eyes">eyes</a>, or other <a href="/wiki/Biological_tissue" class="mw-redirect" title="Biological tissue">tissues</a>.<a href="#cite_note-142">[139]</a> In organisms without lungs such as insects, sulfite in high concentration prevents <a href="/wiki/Respiration_(physiology)" title="Respiration (physiology)">respiration</a>.<a href="#cite_note-143">[140]</a> <a href="/wiki/Sulfur_trioxide" title="Sulfur trioxide">Sulfur trioxide</a> (made by catalysis from sulfur dioxide) and <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> are similarly highly acidic and corrosive in the presence of water. Concentrated sulfuric acid is a strong dehydrating agent that can strip available water molecules and water components from sugar and organic tissue.<a href="#cite_note-144">[141]</a> The burning of <a href="/wiki/Coal" title="Coal">coal</a> and/or <a href="/wiki/Petroleum" title="Petroleum">petroleum</a> by industry and <a href="/wiki/Power_plants" class="mw-redirect" title="Power plants">power plants</a> generates sulfur dioxide (SO2) that reacts with atmospheric water and oxygen to produce <a href="/wiki/Sulfurous_acid" title="Sulfurous acid">sulfurous acid</a> (H2SO3).<a href="#cite_note-145">[142]</a> These acids are components of <a href="/wiki/Acid_rain" title="Acid rain">acid rain</a>, lowering the <a href="/wiki/PH" title="PH">pH</a> of <a href="/wiki/Soil" title="Soil">soil</a> and freshwater bodies, sometimes resulting in substantial damage to the <a href="/wiki/Environment_(biophysical)" class="mw-redirect" title="Environment (biophysical)">environment</a> and <a href="/wiki/Chemical_weathering" class="mw-redirect" title="Chemical weathering">chemical weathering</a> of statues and structures. Fuel standards increasingly require that fuel producers extract sulfur from <a href="/wiki/Fossil_fuel" title="Fossil fuel">fossil fuels</a> to prevent acid rain formation. This extracted and refined sulfur represents a large portion of sulfur production. In coal-fired power plants, <a href="/wiki/Flue_gas" title="Flue gas">flue gases</a> are sometimes purified. More modern power plants that use <a href="/wiki/Synthesis_gas" class="mw-redirect" title="Synthesis gas">synthesis gas</a> extract the sulfur before they burn the gas. <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">Hydrogen sulfide</a> is about one-half as <a href="/wiki/Toxic" class="mw-redirect" title="Toxic">toxic</a> as <a href="/wiki/Hydrogen_cyanide" title="Hydrogen cyanide">hydrogen cyanide</a>, and intoxicates by the same mechanism (inhibition of the respiratory enzyme <a href="/wiki/Cytochrome_oxidase" class="mw-redirect" title="Cytochrome oxidase">cytochrome oxidase</a>),<a href="#cite_note-146">[143]</a> though hydrogen sulfide is less likely to cause sudden poisonings from small inhaled amounts (near its <a href="/wiki/Permissible_exposure_limit" title="Permissible exposure limit">permissible exposure limit</a> (PEL) of 20 ppm) because of its disagreeable odor.<a href="#cite_note-147">[144]</a> However, its presence in ambient air at concentration over 100–150 ppm quickly deadens the sense of smell,<a href="#cite_note-148">[145]</a> and a victim may breathe increasing quantities without noticing until severe symptoms cause death. Dissolved <a href="/wiki/Sulfide" title="Sulfide">sulfide</a> and <a href="/wiki/Hydrosulfide" class="mw-redirect" title="Hydrosulfide">hydrosulfide</a> salts are toxic by the same mechanism. </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(8)"><h2 id="Notes">Notes</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=35" title="Edit section: Notes" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-8 collapsible-block" id="mf-section-8"> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist reflist-lower-alpha"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-13"><a href="#cite_ref-13">^</a> But impure samples have an odor similar to that of <a href="/wiki/Match" title="Match">matches</a>. A strong odor called "smell of sulfur" actually is given off by several sulfur compounds, such as <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a> and <a href="/wiki/Organosulfur" class="mw-redirect" title="Organosulfur">organosulfur</a> compounds. </li> <li id="cite_note-15"><a href="#cite_ref-15">^</a> Sulfur's melting point at 115.21°C was determined by two laboratories of the US Department of Energy (Jefferson Lab and Los Alamos National Lab).<a href="#cite_note-14">[13]</a> Greenwood and Earnshaw say that at fast heating for microcrystalline α-S8 the melting point is 115.1 °C (239.2 °F).<a href="#cite_note-Greenwood-1997a-8">[8]</a> </li> <li id="cite_note-21"><a href="#cite_ref-21">^</a> Historically, it was rather difficult to find the exact melting point of sulfur.<a href="#cite_note-18">[16]</a> When heated slowly, the melting point may range from 114.6 °C (238.3 °F) to 120.4 °C (248.7 °F)<a href="#cite_note-Greenwood-1997a-8">[8]</a> (factors that interfere with a definite melting point, are the <a href="/wiki/Crystallization_of_polymers" title="Crystallization of polymers">polymerlike nature</a> of sulfur<a href="#cite_note-19">[17]</a> and a large number of allotropes.<a href="#cite_note-20">[18]</a>) Melting point may be presented as a temperature range, depending on the allotropic composition of a sample at the time of melting. </li> </ol></div></div> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(9)"><h2 id="See_also">See also</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=36" title="Edit section: See also" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-9 collapsible-block" id="mf-section-9"> <style data-mw-deduplicate="TemplateStyles:r1239009302">.mw-parser-output .portalbox{padding:0;margin:0.5em 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sulfur aerosols">Stratospheric sulfur aerosols</a></li> <li><a href="/wiki/Sulfur_assimilation" title="Sulfur assimilation">Sulfur assimilation</a></li> <li><a href="/wiki/Sulfur_isotope_biogeochemistry" title="Sulfur isotope biogeochemistry">Sulfur isotope biogeochemistry</a></li> <li><a href="/wiki/Ultra-low_sulfur_diesel" class="mw-redirect" title="Ultra-low sulfur diesel">Ultra-low sulfur diesel</a></li></ul> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(10)"><h2 id="References">References</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=37" title="Edit section: References" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-10 collapsible-block" id="mf-section-10"> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239543626"><div class="reflist"> <div class="mw-references-wrap mw-references-columns"><ol class="references"> <li id="cite_note-1"><a href="#cite_ref-1">^</a> <style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.ciaaw.org/sulfur.htm">"Standard Atomic Weights: Sulfur"</a>. <a href="/wiki/Commission_on_Isotopic_Abundances_and_Atomic_Weights" title="Commission on Isotopic Abundances and Atomic Weights">CIAAW</a>. 2009.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Standard+Atomic+Weights%3A+Sulfur&rft.pub=CIAAW&rft.date=2009&rft_id=https%3A%2F%2Fwww.ciaaw.org%2Fsulfur.htm&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-CIAAW2021-2"><a href="#cite_ref-CIAAW2021_2-0">^</a> <link 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H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (4 May 2022). <a rel="nofollow" class="external text" href="https://www.degruyter.com/document/doi/10.1515/pac-2019-0603/html">"Standard atomic weights of the elements 2021 (IUPAC Technical Report)"</a>. Pure and Applied Chemistry. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1515%2Fpac-2019-0603">10.1515/pac-2019-0603</a>. <a href="/wiki/ISSN_(identifier)" class="mw-redirect" title="ISSN (identifier)">ISSN</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/issn/1365-3075">1365-3075</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Pure+and+Applied+Chemistry&rft.atitle=Standard+atomic+weights+of+the+elements+2021+%28IUPAC+Technical+Report%29&rft.date=2022-05-04&rft_id=info%3Adoi%2F10.1515%2Fpac-2019-0603&rft.issn=1365-3075&rft.aulast=Prohaska&rft.aufirst=Thomas&rft.au=Irrgeher%2C+Johanna&rft.au=Benefield%2C+Jacqueline&rft.au=B%C3%B6hlke%2C+John+K.&rft.au=Chesson%2C+Lesley+A.&rft.au=Coplen%2C+Tyler+B.&rft.au=Ding%2C+Tiping&rft.au=Dunn%2C+Philip+J.+H.&rft.au=Gr%C3%B6ning%2C+Manfred&rft.au=Holden%2C+Norman+E.&rft.au=Meijer%2C+Harro+A.+J.&rft_id=https%3A%2F%2Fwww.degruyter.com%2Fdocument%2Fdoi%2F10.1515%2Fpac-2019-0603%2Fhtml&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-GE28-3">^ <a href="#cite_ref-GE28_3-0">a</a> <a href="#cite_ref-GE28_3-1">b</a> <a href="#cite_ref-GE28_3-2">c</a> <a href="#cite_ref-GE28_3-3">d</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1"><a href="/wiki/Norman_Greenwood" title="Norman Greenwood">Greenwood, Norman N.</a>; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). <a href="/wiki/Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. p. 28. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-08-037941-8" title="Special:BookSources/978-0-08-037941-8"><bdi>978-0-08-037941-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry+of+the+Elements&rft.pages=28&rft.edition=2nd&rft.pub=Butterworth-Heinemann&rft.date=1997&rft.isbn=978-0-08-037941-8&rft.aulast=Greenwood&rft.aufirst=Norman+N.&rft.au=Earnshaw%2C+Alan&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-Arblaster_2018-4">^ <a href="#cite_ref-Arblaster_2018_4-0">a</a> <a href="#cite_ref-Arblaster_2018_4-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFArblaster2018" class="citation book cs1">Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-1-62708-155-9" title="Special:BookSources/978-1-62708-155-9"><bdi>978-1-62708-155-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Selected+Values+of+the+Crystallographic+Properties+of+Elements&rft.place=Materials+Park%2C+Ohio&rft.pub=ASM+International&rft.date=2018&rft.isbn=978-1-62708-155-9&rft.aulast=Arblaster&rft.aufirst=John+W.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-magnet-5"><a href="#cite_ref-magnet_5-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFLide,_D._R.2005" class="citation book cs1">Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". <a rel="nofollow" class="external text" href="https://web.archive.org/web/20110303222309/http://www-d0.fnal.gov/hardware/cal/lvps_info/engineering/elementmagn.pdf">CRC Handbook of Chemistry and Physics</a> (PDF) (86th ed.). Boca Raton (FL): CRC Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-8493-0486-5" title="Special:BookSources/0-8493-0486-5"><bdi>0-8493-0486-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Magnetic+susceptibility+of+the+elements+and+inorganic+compounds&rft.btitle=CRC+Handbook+of+Chemistry+and+Physics&rft.place=Boca+Raton+%28FL%29&rft.edition=86th&rft.pub=CRC+Press&rft.date=2005&rft.isbn=0-8493-0486-5&rft_id=https%3A%2F%2Fweb.archive.org%2Fweb%2F20110303222309%2Fhttp%3A%2F%2Fwww-d0.fnal.gov%2Fhardware%2Fcal%2Flvps_info%2Fengineering%2Felementmagn.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-6"><a href="#cite_ref-6">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWeast1984" class="citation book cs1">Weast, Robert (1984). 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Georgiagulfsulfur.com. Retrieved 12 February 2022.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Sulfur+History&rft.pub=Georgiagulfsulfur.com&rft_id=http%3A%2F%2Fwww.georgiagulfsulfur.com%2Fsulfur%2Fhistory&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-Greenwood-1997a-8">^ <a href="#cite_ref-Greenwood-1997a_8-0">a</a> <a href="#cite_ref-Greenwood-1997a_8-1">b</a> <a href="#cite_ref-Greenwood-1997a_8-2">c</a> <a href="#cite_ref-Greenwood-1997a_8-3">d</a> <a href="#cite_ref-Greenwood-1997a_8-4">e</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1">Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). 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Cambridge University Press. p. 571.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Brimstone&rft.btitle=Encyclop%C3%A6dia+Britannica&rft.pages=571&rft.edition=11th&rft.pub=Cambridge+University+Press&rft.date=1911&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-Knight-2014-10">^ <a href="#cite_ref-Knight-2014_10-0">a</a> <a href="#cite_ref-Knight-2014_10-1">b</a> <a href="#cite_ref-Knight-2014_10-2">c</a> <a href="#cite_ref-Knight-2014_10-3">d</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFLaurence_Knight2014" class="citation web cs1">Laurence Knight (19 July 2014). <a rel="nofollow" class="external text" href="https://www.bbc.com/news/magazine-28369829">"Sulphur surplus: Up to our necks in a diabolical element"</a>. BBC.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Sulphur+surplus%3A+Up+to+our+necks+in+a+diabolical+element&rft.pub=BBC&rft.date=2014-07-19&rft.au=Laurence+Knight&rft_id=https%3A%2F%2Fwww.bbc.com%2Fnews%2Fmagazine-28369829&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-BBC_Elements-2014-11">^ <a href="#cite_ref-BBC_Elements-2014_11-0">a</a> <a href="#cite_ref-BBC_Elements-2014_11-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.bbc.co.uk/programmes/p027xnp2">"Sulfur"</a>. Elements. BBC. 11 October 2014.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=Elements&rft.atitle=Sulfur&rft.date=2014-10-11&rft_id=https%3A%2F%2Fwww.bbc.co.uk%2Fprogrammes%2Fp027xnp2&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988">. Download <a rel="nofollow" class="external text" href="https://open.live.bbc.co.uk/mediaselector/6/redir/version/2.0/mediaset/audio-nondrm-download/proto/https/vpid/p02rc2q5.mp3">here</a>. </li> <li id="cite_note-12"><a href="#cite_ref-12">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFRettigTrotter1987" class="citation journal cs1">Rettig, S. J.; Trotter, J. (15 December 1987). <a rel="nofollow" class="external text" href="http://journals.iucr.org/c/issues/1987/12/00/a27614/a27614.pdf">"Refinement of the structure of orthorhombic sulfur, α-S8"</a> (PDF). 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Chemie in unserer Zeit (in German). 35 (5): 324–331. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F1521-3781%28200110%2935%3A5%3C324%3A%3AAID-CIUZ324%3E3.0.CO%3B2-9">10.1002/1521-3781(200110)35:5<324::AID-CIUZ324>3.0.CO;2-9</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chemie+in+unserer+Zeit&rft.atitle=Chemiker%2C+Techniker%2C+Unternehmer%3A+Zum+150.+Geburtstag+von+Hermann+Frasch&rft.volume=35&rft.issue=5&rft.pages=324-331&rft.date=2001&rft_id=info%3Adoi%2F10.1002%2F1521-3781%28200110%2935%3A5%3C324%3A%3AAID-CIUZ324%3E3.0.CO%3B2-9&rft.aulast=Botsch&rft.aufirst=Walter&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-Mass-2003-78"><a href="#cite_ref-Mass-2003_78-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMassAnderson2003" class="citation journal cs1">Mass, Jennifer L; Anderson, Mark J (2003). 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Eric; Coe, Fredric L. (13 January 2010). <a rel="nofollow" class="external text" href="https://www.nejm.org/doi/10.1056/NEJM197710202971606">"Metabolic Acidosis after Sulfur Ingestion"</a>. New England Journal of Medicine. 297 (16): 869–870. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1056%2Fnejm197710202971606">10.1056/nejm197710202971606</a>. <a href="/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/904661">904661</a>. 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Retrieved 24 October 2023.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=Centers+for+Disease+Control+and+Prevention&rft.atitle=Sulfur+Dioxide+%7C+Toxicological+Profile+%7C+ATSDR&rft.date=2014-03-26&rft_id=https%3A%2F%2Fwwwn.cdc.gov%2FTSP%2FToxProfiles%2FToxProfiles.aspx%3Fid%3D253%26tid%3D46&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-143"><a href="#cite_ref-143">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="http://npic.orst.edu/factsheets/sulfurgen.html#:~:text=However,%20the%20main%20theory%20is,cells%20and%20affects%20cell%20respiration.&text=Sulfur%20can%20kill%20insects%20if%20they%20touch%20it%20or%20eat%20it.&text=It%20disrupts%20their%20normal%20body,their%20ability%20to%20produce%20energy.">"Sulfur General Fact Sheet"</a>. npic.orst.edu. 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Medscape. 30 March 2017 – via eMedicine.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Medscape&rft.atitle=Hydrogen+Sulfide+Toxicity%3A+Practice+Essentials%2C+Pathophysiology%2C+Etiology&rft.date=2017-03-30&rft_id=https%3A%2F%2Femedicine.medscape.com%2Farticle%2F815139-overview%23a4&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> <li id="cite_note-147"><a href="#cite_ref-147">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSummers2017" class="citation web cs1">Summers, Vincent (8 April 2017). <a rel="nofollow" class="external text" href="https://www.quirkyscience.com/hydrogen-sulfide-or-hydrogen-cyanide/">"Hydrogen Sulfide or Hydrogen Cyanide: Which is More Dangerous?"</a>. Quirky Science. 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Retrieved 23 August 2022.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=www.osha.gov&rft.atitle=Hydrogen+Sulfide+%E2%80%93+Hazards+%7C+Occupational+Safety+and+Health+Administration&rft_id=https%3A%2F%2Fwww.osha.gov%2Fhydrogen-sulfide%2Fhazards&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </li> </ol></div></div> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(11)"><h2 id="Further_reading">Further reading</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=38" title="Edit section: Further reading" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-11 collapsible-block" id="mf-section-11"> <style data-mw-deduplicate="TemplateStyles:r1235681985">.mw-parser-output .side-box{margin:4px 0;box-sizing:border-box;border:1px solid #aaa;font-size:88%;line-height:1.25em;background-color:var(--background-color-interactive-subtle,#f8f9fa);display:flow-root}.mw-parser-output .side-box-abovebelow,.mw-parser-output .side-box-text{padding:0.25em 0.9em}.mw-parser-output .side-box-image{padding:2px 0 2px 0.9em;text-align:center}.mw-parser-output .side-box-imageright{padding:2px 0.9em 2px 0;text-align:center}@media(min-width:500px){.mw-parser-output .side-box-flex{display:flex;align-items:center}.mw-parser-output .side-box-text{flex:1;min-width:0}}@media(min-width:720px){.mw-parser-output .side-box{width:238px}.mw-parser-output .side-box-right{clear:right;float:right;margin-left:1em}.mw-parser-output .side-box-left{margin-right:1em}}</style><style data-mw-deduplicate="TemplateStyles:r1237033735">@media print{body.ns-0 .mw-parser-output .sistersitebox{display:none!important}}@media screen{html.skin-theme-clientpref-night .mw-parser-output .sistersitebox img[src*="Wiktionary-logo-en-v2.svg"]{background-color:white}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .sistersitebox img[src*="Wiktionary-logo-en-v2.svg"]{background-color:white}}</style><div class="side-box side-box-right plainlinks sistersitebox"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"> <div class="side-box-flex"> <div class="side-box-image"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/34px-Wikiquote-logo.svg.png" decoding="async" width="34" height="40" class="mw-file-element" data-file-width="300" data-file-height="355"></noscript><span class="lazy-image-placeholder" style="width: 34px;height: 40px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/34px-Wikiquote-logo.svg.png" data-alt="" data-width="34" data-height="40" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/51px-Wikiquote-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/68px-Wikiquote-logo.svg.png 2x" data-class="mw-file-element"> </div> <div class="side-box-text plainlist">Wikiquote has quotations related to <a href="https://en.wikiquote.org/wiki/Special:Search/Sulfur" class="extiw" title="q:Special:Search/Sulfur">Sulfur</a>.</div></div> </div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSigelFreisingerSigel2020" class="citation book cs1">Sigel, Astrid; Freisinger, Eva; Sigel, Roland K.O., eds. (2020). Transition Metals and Sulfur: A Strong Relationship for Life. Guest Editors Martha E Sosa Torres and Peter M.H.Kroneck. Berlin/Boston: de Gruyter. pp. xlv+455. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3-11-058889-7" title="Special:BookSources/978-3-11-058889-7"><bdi>978-3-11-058889-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Transition+Metals+and+Sulfur%3A+A+Strong+Relationship+for+Life&rft.place=Berlin%2FBoston&rft.pages=xlv%2B455&rft.pub=de+Gruyter&rft.date=2020&rft.isbn=978-3-11-058889-7&rfr_id=info%3Asid%2Fen.wikipedia.org%3ASulfur" class="Z3988"> </section><div class="mw-heading mw-heading2 section-heading" onclick="mfTempOpenSection(12)"><h2 id="External_links">External links</h2> <a role="button" href="/w/index.php?title=Sulfur&action=edit&section=39" title="Edit section: External links" class="cdx-button cdx-button--size-large cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--icon-only cdx-button--weight-quiet "> edit </a> </div><section class="mf-section-12 collapsible-block" id="mf-section-12"> <ul><li><a rel="nofollow" class="external text" href="http://www.periodicvideos.com/videos/016.htm">Sulfur</a> at <a href="/wiki/The_Periodic_Table_of_Videos" class="mw-redirect" title="The Periodic Table of Videos">The Periodic Table of Videos</a> (University of Nottingham)</li> <li><a rel="nofollow" class="external text" href="https://physics.nist.gov/PhysRefData/Handbook/Tables/sulfurtable1.htm">Atomic Data for Sulfur</a>, <a href="/wiki/NIST" class="mw-redirect" title="NIST">NIST</a> Physical Measurement Laboratory</li> <li><a rel="nofollow" class="external text" href="https://library.tedankara.k12.tr/chemistry/vol2/allotropy/z129.htm">Sulfur phase diagram</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100223201329/http://library.tedankara.k12.tr/chemistry/vol2/allotropy/z129.htm">Archived</a> 23 February 2010 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a>, Introduction to Chemistry for Ages 13–17</li> <li><a rel="nofollow" class="external text" href="https://www.swisseduc.ch/stromboli/perm/vulcano/sulphur-vulcano-en.html">Crystalline, liquid and polymerization of sulfur on Vulcano Island, Italy</a></li> <li><a rel="nofollow" class="external text" href="http://extoxnet.orst.edu/pips/sulfur.htm">Sulfur and its use as a pesticide</a></li> <li><a rel="nofollow" class="external text" href="https://www.sulphurinstitute.org/">The Sulphur Institute</a></li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20140714221502/http://www.nutrientstewardship.com/partners/products-and-services/sulfur-institute">Nutrient Stewardship and The Sulphur Institute</a></li></ul> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><style data-mw-deduplicate="TemplateStyles:r1236075235">.mw-parser-output .navbox{box-sizing:border-box;border:1px solid #a2a9b1;width:100%;clear:both;font-size:88%;text-align:center;padding:1px;margin:1em auto 0}.mw-parser-output .navbox .navbox{margin-top:0}.mw-parser-output .navbox+.navbox,.mw-parser-output .navbox+.navbox-styles+.navbox{margin-top:-1px}.mw-parser-output .navbox-inner,.mw-parser-output .navbox-subgroup{width:100%}.mw-parser-output .navbox-group,.mw-parser-output .navbox-title,.mw-parser-output .navbox-abovebelow{padding:0.25em 1em;line-height:1.5em;text-align:center}.mw-parser-output .navbox-group{white-space:nowrap;text-align:right}.mw-parser-output .navbox,.mw-parser-output .navbox-subgroup{background-color:#fdfdfd}.mw-parser-output .navbox-list{line-height:1.5em;border-color:#fdfdfd}.mw-parser-output .navbox-list-with-group{text-align:left;border-left-width:2px;border-left-style:solid}.mw-parser-output tr+tr>.navbox-abovebelow,.mw-parser-output tr+tr>.navbox-group,.mw-parser-output tr+tr>.navbox-image,.mw-parser-output tr+tr>.navbox-list{border-top:2px solid #fdfdfd}.mw-parser-output .navbox-title{background-color:#ccf}.mw-parser-output .navbox-abovebelow,.mw-parser-output .navbox-group,.mw-parser-output .navbox-subgroup .navbox-title{background-color:#ddf}.mw-parser-output .navbox-subgroup .navbox-group,.mw-parser-output .navbox-subgroup .navbox-abovebelow{background-color:#e6e6ff}.mw-parser-output .navbox-even{background-color:#f7f7f7}.mw-parser-output .navbox-odd{background-color:transparent}.mw-parser-output .navbox .hlist td dl,.mw-parser-output .navbox .hlist td ol,.mw-parser-output .navbox .hlist td ul,.mw-parser-output .navbox td.hlist dl,.mw-parser-output .navbox td.hlist ol,.mw-parser-output .navbox td.hlist ul{padding:0.125em 0}.mw-parser-output .navbox .navbar{display:block;font-size:100%}.mw-parser-output .navbox-title .navbar{float:left;text-align:left;margin-right:0.5em}body.skin--responsive .mw-parser-output .navbox-image img{max-width:none!important}@media print{body.ns-0 .mw-parser-output .navbox{display:none!important}}</style></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"></div> <style data-mw-deduplicate="TemplateStyles:r1130092004">.mw-parser-output .portal-bar{font-size:88%;font-weight:bold;display:flex;justify-content:center;align-items:baseline}.mw-parser-output .portal-bar-bordered{padding:0 2em;background-color:#fdfdfd;border:1px solid #a2a9b1;clear:both;margin:1em auto 0}.mw-parser-output .portal-bar-related{font-size:100%;justify-content:flex-start}.mw-parser-output .portal-bar-unbordered{padding:0 1.7em;margin-left:0}.mw-parser-output .portal-bar-header{margin:0 1em 0 0.5em;flex:0 0 auto;min-height:24px}.mw-parser-output .portal-bar-content{display:flex;flex-flow:row wrap;flex:0 1 auto;padding:0.15em 0;column-gap:1em;align-items:baseline;margin:0;list-style:none}.mw-parser-output .portal-bar-content-related{margin:0;list-style:none}.mw-parser-output .portal-bar-item{display:inline-block;margin:0.15em 0.2em;min-height:24px;line-height:24px}@media screen and (max-width:768px){.mw-parser-output .portal-bar{font-size:88%;font-weight:bold;display:flex;flex-flow:column wrap;align-items:baseline}.mw-parser-output .portal-bar-header{text-align:center;flex:0;padding-left:0.5em;margin:0 auto}.mw-parser-output .portal-bar-related{font-size:100%;align-items:flex-start}.mw-parser-output .portal-bar-content{display:flex;flex-flow:row wrap;align-items:center;flex:0;column-gap:1em;border-top:1px solid #a2a9b1;margin:0 auto;list-style:none}.mw-parser-output .portal-bar-content-related{border-top:none;margin:0;list-style:none}}.mw-parser-output .navbox+link+.portal-bar,.mw-parser-output .navbox+style+.portal-bar,.mw-parser-output .navbox+link+.portal-bar-bordered,.mw-parser-output .navbox+style+.portal-bar-bordered,.mw-parser-output .sister-bar+link+.portal-bar,.mw-parser-output .sister-bar+style+.portal-bar,.mw-parser-output .portal-bar+.navbox-styles+.navbox,.mw-parser-output .portal-bar+.navbox-styles+.sister-bar{margin-top:-1px}</style><div class="portal-bar noprint metadata noviewer portal-bar-bordered" role="navigation" aria-label="Portals"><a href="/wiki/Wikipedia:Contents/Portals" title="Wikipedia:Contents/Portals">Portal</a>:<ul class="portal-bar-content"><li class="portal-bar-item"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/19px-Papapishu-Lab-icon-6.svg.png" decoding="async" width="19" height="19" class="mw-file-element" data-file-width="512" data-file-height="512"></noscript><span class="lazy-image-placeholder" style="width: 19px;height: 19px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/19px-Papapishu-Lab-icon-6.svg.png" data-alt="" data-width="19" data-height="19" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/29px-Papapishu-Lab-icon-6.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/38px-Papapishu-Lab-icon-6.svg.png 2x" data-class="mw-file-element">  <a href="/wiki/Portal:Chemistry" title="Portal:Chemistry">Chemistry</a></li></ul></div><style data-mw-deduplicate="TemplateStyles:r1236088147">.mw-parser-output .sister-bar{display:flex;justify-content:center;align-items:baseline;font-size:88%;background-color:#fdfdfd;border:1px solid #a2a9b1;clear:both;margin:1em 0 0;padding:0 2em}.mw-parser-output .sister-bar-header{margin:0 1em 0 0.5em;padding:0.2em 0;flex:0 0 auto;min-height:24px;line-height:22px}.mw-parser-output .sister-bar-content{display:flex;flex-flow:row wrap;flex:0 1 auto;align-items:baseline;padding:0.2em 0;column-gap:1em;margin:0;list-style:none}.mw-parser-output .sister-bar-item{display:flex;align-items:baseline;margin:0.15em 0;min-height:24px;text-align:left}.mw-parser-output .sister-bar-logo{width:22px;line-height:22px;margin:0 0.2em;text-align:right}.mw-parser-output .sister-bar-link{margin:0 0.2em;text-align:left}@media screen and (max-width:960px){.mw-parser-output .sister-bar{flex-flow:column wrap;margin:1em auto 0}.mw-parser-output .sister-bar-header{flex:0 1}.mw-parser-output .sister-bar-content{flex:1;border-top:1px solid #a2a9b1;margin:0;list-style:none}.mw-parser-output .sister-bar-item{flex:0 0 20em;min-width:20em}}.mw-parser-output .navbox+link+.sister-bar,.mw-parser-output .navbox+style+.sister-bar,.mw-parser-output .portal-bar+link+.sister-bar,.mw-parser-output .portal-bar+style+.sister-bar,.mw-parser-output .sister-bar+.navbox-styles+.navbox,.mw-parser-output .sister-bar+.navbox-styles+.portal-bar{margin-top:-1px}@media print{body.ns-0 .mw-parser-output .sister-bar{display:none!important}}</style><div class="noprint metadata sister-bar" role="navigation" aria-label="sister-projects"><div class="sister-bar-header">Sulfur at Wikipedia's <a href="/wiki/Wikipedia:Wikimedia_sister_projects" title="Wikipedia:Wikimedia sister projects">sister projects</a>:</div><ul class="sister-bar-content"><li class="sister-bar-item"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/19px-Wiktionary-logo-v2.svg.png" decoding="async" width="19" height="19" class="mw-file-element" data-file-width="391" data-file-height="391"></noscript><span class="lazy-image-placeholder" style="width: 19px;height: 19px;" data-src="//upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/19px-Wiktionary-logo-v2.svg.png" data-alt="" data-width="19" data-height="19" data-srcset="//upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/29px-Wiktionary-logo-v2.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/38px-Wiktionary-logo-v2.svg.png 2x" data-class="mw-file-element"> <a href="https://en.wiktionary.org/wiki/sulfur" class="extiw" title="wikt:sulfur">Definitions</a> from Wiktionary</li><li class="sister-bar-item"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/14px-Commons-logo.svg.png" decoding="async" width="14" height="19" class="mw-file-element" data-file-width="1024" data-file-height="1376"></noscript><span class="lazy-image-placeholder" style="width: 14px;height: 19px;" data-src="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/14px-Commons-logo.svg.png" data-alt="" data-width="14" data-height="19" data-srcset="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/21px-Commons-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/28px-Commons-logo.svg.png 2x" data-class="mw-file-element"> <a href="https://commons.wikimedia.org/wiki/Sulfur" class="extiw" title="c:Sulfur">Media</a> from Commons</li><li class="sister-bar-item"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/19px-Wikibooks-logo.svg.png" decoding="async" width="19" height="19" class="mw-file-element" data-file-width="300" data-file-height="300"></noscript><span class="lazy-image-placeholder" style="width: 19px;height: 19px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/19px-Wikibooks-logo.svg.png" data-alt="" data-width="19" data-height="19" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/29px-Wikibooks-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/38px-Wikibooks-logo.svg.png 2x" data-class="mw-file-element"> <a href="https://en.wikibooks.org/wiki/Wikijunior:The_Elements/Sulfur" class="extiw" title="b:Wikijunior:The Elements/Sulfur">Textbooks</a> from Wikibooks</li><li class="sister-bar-item"><noscript><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/21px-Wikiversity_logo_2017.svg.png" decoding="async" width="21" height="17" class="mw-file-element" data-file-width="626" data-file-height="512"></noscript><span class="lazy-image-placeholder" style="width: 21px;height: 17px;" data-src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/21px-Wikiversity_logo_2017.svg.png" data-alt="" data-width="21" data-height="17" data-srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/32px-Wikiversity_logo_2017.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/42px-Wikiversity_logo_2017.svg.png 2x" data-class="mw-file-element"> <a href="https://en.wikiversity.org/wiki/Sulfur_atom" class="extiw" title="v:Sulfur atom">Resources</a> from Wikiversity</li></ul></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"><style data-mw-deduplicate="TemplateStyles:r1038841319">.mw-parser-output .tooltip-dotted{border-bottom:1px dotted;cursor:help}</style></div></section></div> <noscript><img src="https://login.m.wikimedia.org/wiki/Special:CentralAutoLogin/start?type=1x1&mobile=1" alt="" width="1" height="1" style="border: none; position: absolute;"></noscript> <div class="printfooter" data-nosnippet="">Retrieved from "<a dir="ltr" href="https://en.wikipedia.org/w/index.php?title=Sulfur&oldid=1258684905">https://en.wikipedia.org/w/index.php?title=Sulfur&oldid=1258684905</a>"</div></div> </div> <div class="post-content" id="page-secondary-actions"> </div> </main> <footer class="mw-footer minerva-footer" role="contentinfo"> <a class="last-modified-bar" href="/w/index.php?title=Sulfur&action=history"> <div class="post-content last-modified-bar__content"> Last edited on 21 November 2024, at 01:07 </div> </a> <div class="post-content footer-content"> <div id='mw-data-after-content'> <div class="read-more-container"></div> </div> <div id="p-lang"> <h4>Languages</h4> <section> <ul id="p-variants" class="minerva-languages"></ul> <ul class="minerva-languages"><li class="interlanguage-link interwiki-af mw-list-item"><a href="https://af.wikipedia.org/wiki/Swawel" title="Swawel – Afrikaans" lang="af" hreflang="af" data-title="Swawel" data-language-autonym="Afrikaans" data-language-local-name="Afrikaans" class="interlanguage-link-target">Afrikaans</a></li><li class="interlanguage-link interwiki-am mw-list-item"><a href="https://am.wikipedia.org/wiki/%E1%8B%B5%E1%8A%9D" title="ድኝ – Amharic" lang="am" hreflang="am" data-title="ድኝ" data-language-autonym="አማርኛ" data-language-local-name="Amharic" class="interlanguage-link-target">አማርኛ</a></li><li class="interlanguage-link interwiki-anp mw-list-item"><a href="https://anp.wikipedia.org/wiki/%E0%A4%97%E0%A4%A8%E0%A5%8D%E0%A4%A7%E0%A4%95" title="गन्धक – Angika" lang="anp" hreflang="anp" data-title="गन्धक" data-language-autonym="अंगिका" data-language-local-name="Angika" class="interlanguage-link-target">अंगिका</a></li><li class="interlanguage-link interwiki-ar badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://ar.wikipedia.org/wiki/%D9%83%D8%A8%D8%B1%D9%8A%D8%AA" title="كبريت – Arabic" lang="ar" hreflang="ar" data-title="كبريت" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target">العربية</a></li><li class="interlanguage-link interwiki-an mw-list-item"><a href="https://an.wikipedia.org/wiki/Ixufre" title="Ixufre – Aragonese" lang="an" hreflang="an" data-title="Ixufre" data-language-autonym="Aragonés" data-language-local-name="Aragonese" class="interlanguage-link-target">Aragonés</a></li><li class="interlanguage-link interwiki-hyw mw-list-item"><a href="https://hyw.wikipedia.org/wiki/%D4%BE%D5%AE%D5%B8%D6%82%D5%B4%D5%A2" title="Ծծումբ – Western Armenian" lang="hyw" hreflang="hyw" data-title="Ծծումբ" data-language-autonym="Արեւմտահայերէն" data-language-local-name="Western Armenian" class="interlanguage-link-target">Արեւմտահայերէն</a></li><li class="interlanguage-link interwiki-roa-rup mw-list-item"><a href="https://roa-rup.wikipedia.org/wiki/Sulfu" title="Sulfu – Aromanian" lang="rup" hreflang="rup" data-title="Sulfu" data-language-autonym="Armãneashti" data-language-local-name="Aromanian" class="interlanguage-link-target">Armãneashti</a></li><li class="interlanguage-link interwiki-ast mw-list-item"><a href="https://ast.wikipedia.org/wiki/Azufre" title="Azufre – Asturian" lang="ast" hreflang="ast" data-title="Azufre" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target">Asturianu</a></li><li class="interlanguage-link interwiki-awa mw-list-item"><a href="https://awa.wikipedia.org/wiki/%E0%A4%B8%E0%A4%B2%E0%A5%8D%E0%A4%AB%E0%A4%B0" title="सल्फर – Awadhi" lang="awa" hreflang="awa" data-title="सल्फर" data-language-autonym="अवधी" data-language-local-name="Awadhi" class="interlanguage-link-target">अवधी</a></li><li class="interlanguage-link interwiki-gn mw-list-item"><a href="https://gn.wikipedia.org/wiki/Itaysy" title="Itaysy – Guarani" lang="gn" hreflang="gn" data-title="Itaysy" data-language-autonym="Avañe'ẽ" data-language-local-name="Guarani" class="interlanguage-link-target">Avañe'ẽ</a></li><li class="interlanguage-link interwiki-av mw-list-item"><a href="https://av.wikipedia.org/wiki/%D0%A7%D3%80%D0%B0%D0%B1%D0%B0%D1%82%D3%80" title="ЧӀабатӀ – Avaric" lang="av" hreflang="av" data-title="ЧӀабатӀ" data-language-autonym="Авар" data-language-local-name="Avaric" class="interlanguage-link-target">Авар</a></li><li class="interlanguage-link interwiki-ay mw-list-item"><a href="https://ay.wikipedia.org/wiki/Asuphri" title="Asuphri – Aymara" lang="ay" hreflang="ay" data-title="Asuphri" data-language-autonym="Aymar aru" data-language-local-name="Aymara" class="interlanguage-link-target">Aymar aru</a></li><li class="interlanguage-link interwiki-az mw-list-item"><a href="https://az.wikipedia.org/wiki/K%C3%BCk%C3%BCrd" title="Kükürd – Azerbaijani" lang="az" hreflang="az" data-title="Kükürd" data-language-autonym="Azərbaycanca" data-language-local-name="Azerbaijani" class="interlanguage-link-target">Azərbaycanca</a></li><li class="interlanguage-link interwiki-ban mw-list-item"><a href="https://ban.wikipedia.org/wiki/Urirang" title="Urirang – Balinese" lang="ban" hreflang="ban" data-title="Urirang" data-language-autonym="Basa Bali" data-language-local-name="Balinese" class="interlanguage-link-target">Basa Bali</a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%97%E0%A6%A8%E0%A7%8D%E0%A6%A7%E0%A6%95" title="গন্ধক – Bangla" lang="bn" hreflang="bn" data-title="গন্ধক" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target">বাংলা</a></li><li class="interlanguage-link interwiki-zh-min-nan mw-list-item"><a href="https://zh-min-nan.wikipedia.org/wiki/Li%C3%BB-h%C3%B4ng" title="Liû-hông – Minnan" lang="nan" hreflang="nan" data-title="Liû-hông" data-language-autonym="閩南語 / Bân-lâm-gú" data-language-local-name="Minnan" class="interlanguage-link-target">閩南語 / Bân-lâm-gú</a></li><li class="interlanguage-link interwiki-ba mw-list-item"><a href="https://ba.wikipedia.org/wiki/%D0%9A%D3%A9%D0%BA%D3%A9%D1%80%D1%82" title="Көкөрт – Bashkir" lang="ba" hreflang="ba" data-title="Көкөрт" data-language-autonym="Башҡортса" data-language-local-name="Bashkir" class="interlanguage-link-target">Башҡортса</a></li><li class="interlanguage-link interwiki-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%A1%D0%B5%D1%80%D0%B0" title="Сера – Belarusian" lang="be" hreflang="be" data-title="Сера" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target">Беларуская</a></li><li class="interlanguage-link interwiki-be-x-old mw-list-item"><a href="https://be-tarask.wikipedia.org/wiki/%D0%A1%D0%B5%D1%80%D0%BA%D0%B0" title="Серка – Belarusian (Taraškievica orthography)" lang="be-tarask" hreflang="be-tarask" data-title="Серка" data-language-autonym="Беларуская (тарашкевіца)" data-language-local-name="Belarusian (Taraškievica orthography)" class="interlanguage-link-target">Беларуская (тарашкевіца)</a></li><li class="interlanguage-link interwiki-bh mw-list-item"><a href="https://bh.wikipedia.org/wiki/%E0%A4%97%E0%A4%82%E0%A4%A7%E0%A4%95" title="गंधक – Bhojpuri" lang="bh" hreflang="bh" data-title="गंधक" data-language-autonym="भोजपुरी" data-language-local-name="Bhojpuri" class="interlanguage-link-target">भोजपुरी</a></li><li class="interlanguage-link interwiki-bcl mw-list-item"><a href="https://bcl.wikipedia.org/wiki/Asupre" title="Asupre – Central Bikol" lang="bcl" hreflang="bcl" data-title="Asupre" data-language-autonym="Bikol Central" data-language-local-name="Central Bikol" class="interlanguage-link-target">Bikol Central</a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%A1%D1%8F%D1%80%D0%B0" title="Сяра – Bulgarian" lang="bg" hreflang="bg" data-title="Сяра" data-language-autonym="Български" data-language-local-name="Bulgarian" class="interlanguage-link-target">Български</a></li><li class="interlanguage-link interwiki-bo mw-list-item"><a href="https://bo.wikipedia.org/wiki/%E0%BD%98%E0%BD%B4%E0%BC%8B%E0%BD%9F%E0%BD%B2%E0%BC%8D" title="མུ་ཟི། – Tibetan" lang="bo" hreflang="bo" data-title="མུ་ཟི།" data-language-autonym="བོད་ཡིག" data-language-local-name="Tibetan" class="interlanguage-link-target">བོད་ཡིག</a></li><li class="interlanguage-link interwiki-bs badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://bs.wikipedia.org/wiki/Sumpor" title="Sumpor – Bosnian" lang="bs" hreflang="bs" data-title="Sumpor" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target">Bosanski</a></li><li class="interlanguage-link interwiki-br mw-list-item"><a href="https://br.wikipedia.org/wiki/Sulfur" title="Sulfur – Breton" lang="br" hreflang="br" data-title="Sulfur" data-language-autonym="Brezhoneg" data-language-local-name="Breton" class="interlanguage-link-target">Brezhoneg</a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Sofre" title="Sofre – Catalan" lang="ca" hreflang="ca" data-title="Sofre" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target">Català</a></li><li class="interlanguage-link interwiki-cv mw-list-item"><a href="https://cv.wikipedia.org/wiki/%D0%9A%D3%B3%D0%BA%C4%95%D1%80%D1%82" title="Кӳкĕрт – Chuvash" lang="cv" hreflang="cv" data-title="Кӳкĕрт" data-language-autonym="Чӑвашла" data-language-local-name="Chuvash" class="interlanguage-link-target">Чӑвашла</a></li><li class="interlanguage-link interwiki-ceb mw-list-item"><a href="https://ceb.wikipedia.org/wiki/Asupri" title="Asupri – Cebuano" lang="ceb" hreflang="ceb" data-title="Asupri" data-language-autonym="Cebuano" data-language-local-name="Cebuano" class="interlanguage-link-target">Cebuano</a></li><li class="interlanguage-link interwiki-cs mw-list-item"><a href="https://cs.wikipedia.org/wiki/S%C3%ADra" title="Síra – Czech" lang="cs" hreflang="cs" data-title="Síra" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target">Čeština</a></li><li class="interlanguage-link interwiki-co mw-list-item"><a href="https://co.wikipedia.org/wiki/Zolfu" title="Zolfu – Corsican" lang="co" hreflang="co" data-title="Zolfu" data-language-autonym="Corsu" data-language-local-name="Corsican" class="interlanguage-link-target">Corsu</a></li><li class="interlanguage-link interwiki-cy mw-list-item"><a href="https://cy.wikipedia.org/wiki/Sylffwr" title="Sylffwr – Welsh" lang="cy" hreflang="cy" data-title="Sylffwr" data-language-autonym="Cymraeg" data-language-local-name="Welsh" class="interlanguage-link-target">Cymraeg</a></li><li class="interlanguage-link interwiki-dag mw-list-item"><a href="https://dag.wikipedia.org/wiki/Chilibi" title="Chilibi – Dagbani" lang="dag" hreflang="dag" data-title="Chilibi" data-language-autonym="Dagbanli" data-language-local-name="Dagbani" class="interlanguage-link-target">Dagbanli</a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Svovl" title="Svovl – Danish" lang="da" hreflang="da" data-title="Svovl" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target">Dansk</a></li><li class="interlanguage-link interwiki-ary mw-list-item"><a href="https://ary.wikipedia.org/wiki/%D9%83%D8%A8%D8%B1%D9%8A%D8%AA" title="كبريت – Moroccan Arabic" lang="ary" hreflang="ary" data-title="كبريت" data-language-autonym="الدارجة" data-language-local-name="Moroccan Arabic" class="interlanguage-link-target">الدارجة</a></li><li class="interlanguage-link interwiki-de badge-Q17437798 badge-goodarticle mw-list-item" title="good article badge"><a href="https://de.wikipedia.org/wiki/Schwefel" title="Schwefel – German" lang="de" hreflang="de" data-title="Schwefel" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target">Deutsch</a></li><li class="interlanguage-link interwiki-dv mw-list-item"><a href="https://dv.wikipedia.org/wiki/%DE%90%DE%A6%DE%8D%DE%B0%DE%8A%DE%A6%DE%83%DE%AA" title="ސަލްފަރު – Divehi" lang="dv" hreflang="dv" data-title="ސަލްފަރު" data-language-autonym="ދިވެހިބަސް" data-language-local-name="Divehi" class="interlanguage-link-target">ދިވެހިބަސް</a></li><li class="interlanguage-link interwiki-nv mw-list-item"><a href="https://nv.wikipedia.org/wiki/%C5%81eetsoii" title="Łeetsoii – Navajo" lang="nv" hreflang="nv" data-title="Łeetsoii" data-language-autonym="Diné bizaad" data-language-local-name="Navajo" class="interlanguage-link-target">Diné bizaad</a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/V%C3%A4%C3%A4vel" title="Väävel – Estonian" lang="et" hreflang="et" data-title="Väävel" data-language-autonym="Eesti" data-language-local-name="Estonian" class="interlanguage-link-target">Eesti</a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%98%CE%B5%CE%AF%CE%BF" title="Θείο – Greek" lang="el" hreflang="el" data-title="Θείο" data-language-autonym="Ελληνικά" data-language-local-name="Greek" class="interlanguage-link-target">Ελληνικά</a></li><li class="interlanguage-link interwiki-myv mw-list-item"><a href="https://myv.wikipedia.org/wiki/%D0%9F%D0%B0%D0%BB%D1%8B%D0%BA%D0%B0%D0%BD%D0%B4%D0%B0%D0%BB" title="Палыкандал – Erzya" lang="myv" hreflang="myv" data-title="Палыкандал" data-language-autonym="Эрзянь" data-language-local-name="Erzya" class="interlanguage-link-target">Эрзянь</a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Azufre" title="Azufre – Spanish" lang="es" hreflang="es" data-title="Azufre" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target">Español</a></li><li class="interlanguage-link interwiki-eo mw-list-item"><a href="https://eo.wikipedia.org/wiki/Sulfuro" title="Sulfuro – Esperanto" lang="eo" hreflang="eo" data-title="Sulfuro" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target">Esperanto</a></li><li class="interlanguage-link interwiki-ext mw-list-item"><a href="https://ext.wikipedia.org/wiki/Azufri" title="Azufri – Extremaduran" lang="ext" hreflang="ext" data-title="Azufri" data-language-autonym="Estremeñu" data-language-local-name="Extremaduran" class="interlanguage-link-target">Estremeñu</a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Sufre" title="Sufre – Basque" lang="eu" hreflang="eu" data-title="Sufre" data-language-autonym="Euskara" data-language-local-name="Basque" class="interlanguage-link-target">Euskara</a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%DA%AF%D9%88%DA%AF%D8%B1%D8%AF" title="گوگرد – Persian" lang="fa" hreflang="fa" data-title="گوگرد" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target">فارسی</a></li><li class="interlanguage-link interwiki-hif mw-list-item"><a href="https://hif.wikipedia.org/wiki/Sulfur" title="Sulfur – Fiji Hindi" lang="hif" hreflang="hif" data-title="Sulfur" data-language-autonym="Fiji Hindi" data-language-local-name="Fiji Hindi" class="interlanguage-link-target">Fiji Hindi</a></li><li class="interlanguage-link interwiki-fo mw-list-item"><a href="https://fo.wikipedia.org/wiki/Sv%C3%A1vul" title="Svávul – Faroese" lang="fo" hreflang="fo" data-title="Svávul" data-language-autonym="Føroyskt" data-language-local-name="Faroese" class="interlanguage-link-target">Føroyskt</a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Soufre" title="Soufre – French" lang="fr" hreflang="fr" data-title="Soufre" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target">Français</a></li><li class="interlanguage-link interwiki-fur mw-list-item"><a href="https://fur.wikipedia.org/wiki/Solfar" title="Solfar – Friulian" lang="fur" hreflang="fur" data-title="Solfar" data-language-autonym="Furlan" data-language-local-name="Friulian" class="interlanguage-link-target">Furlan</a></li><li class="interlanguage-link interwiki-ga mw-list-item"><a href="https://ga.wikipedia.org/wiki/Sulfar" title="Sulfar – Irish" lang="ga" hreflang="ga" data-title="Sulfar" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target">Gaeilge</a></li><li class="interlanguage-link interwiki-gv mw-list-item"><a href="https://gv.wikipedia.org/wiki/Sulfur" title="Sulfur – Manx" lang="gv" hreflang="gv" data-title="Sulfur" data-language-autonym="Gaelg" data-language-local-name="Manx" class="interlanguage-link-target">Gaelg</a></li><li class="interlanguage-link interwiki-gd mw-list-item"><a href="https://gd.wikipedia.org/wiki/Sulfar" title="Sulfar – Scottish Gaelic" lang="gd" hreflang="gd" data-title="Sulfar" data-language-autonym="Gàidhlig" data-language-local-name="Scottish Gaelic" class="interlanguage-link-target">Gàidhlig</a></li><li class="interlanguage-link interwiki-gl mw-list-item"><a href="https://gl.wikipedia.org/wiki/Xofre" title="Xofre – Galician" lang="gl" hreflang="gl" data-title="Xofre" data-language-autonym="Galego" data-language-local-name="Galician" class="interlanguage-link-target">Galego</a></li><li class="interlanguage-link interwiki-gan mw-list-item"><a href="https://gan.wikipedia.org/wiki/%E7%A1%AB" title="硫 – Gan" lang="gan" hreflang="gan" data-title="硫" data-language-autonym="贛語" data-language-local-name="Gan" class="interlanguage-link-target">贛語</a></li><li class="interlanguage-link interwiki-gu mw-list-item"><a href="https://gu.wikipedia.org/wiki/%E0%AA%97%E0%AA%82%E0%AA%A7%E0%AA%95" title="ગંધક – Gujarati" lang="gu" hreflang="gu" data-title="ગંધક" data-language-autonym="ગુજરાતી" data-language-local-name="Gujarati" class="interlanguage-link-target">ગુજરાતી</a></li><li class="interlanguage-link interwiki-hak mw-list-item"><a href="https://hak.wikipedia.org/wiki/Li%C3%B9-v%C3%B2ng" title="Liù-vòng – Hakka Chinese" lang="hak" hreflang="hak" data-title="Liù-vòng" data-language-autonym="客家語 / Hak-kâ-ngî" data-language-local-name="Hakka Chinese" class="interlanguage-link-target">客家語 / Hak-kâ-ngî</a></li><li class="interlanguage-link interwiki-xal mw-list-item"><a href="https://xal.wikipedia.org/wiki/%D0%9A%D2%AF%D0%BA%D1%80" title="Күкр – Kalmyk" lang="xal" hreflang="xal" data-title="Күкр" data-language-autonym="Хальмг" data-language-local-name="Kalmyk" class="interlanguage-link-target">Хальмг</a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%ED%99%A9" title="황 – Korean" lang="ko" hreflang="ko" data-title="황" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target">한국어</a></li><li class="interlanguage-link interwiki-haw mw-list-item"><a href="https://haw.wikipedia.org/wiki/Sulufura" title="Sulufura – Hawaiian" lang="haw" hreflang="haw" data-title="Sulufura" data-language-autonym="Hawaiʻi" data-language-local-name="Hawaiian" class="interlanguage-link-target">Hawaiʻi</a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D4%BE%D5%AE%D5%B8%D6%82%D5%B4%D5%A2" title="Ծծումբ – Armenian" lang="hy" hreflang="hy" data-title="Ծծումբ" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target">Հայերեն</a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%97%E0%A4%82%E0%A4%A7%E0%A4%95" title="गंधक – Hindi" lang="hi" hreflang="hi" data-title="गंधक" data-language-autonym="हिन्दी" data-language-local-name="Hindi" class="interlanguage-link-target">हिन्दी</a></li><li class="interlanguage-link interwiki-hsb mw-list-item"><a href="https://hsb.wikipedia.org/wiki/Syrik" title="Syrik – Upper Sorbian" lang="hsb" hreflang="hsb" data-title="Syrik" data-language-autonym="Hornjoserbsce" data-language-local-name="Upper Sorbian" class="interlanguage-link-target">Hornjoserbsce</a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Sumpor" title="Sumpor – Croatian" lang="hr" hreflang="hr" data-title="Sumpor" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target">Hrvatski</a></li><li class="interlanguage-link interwiki-io mw-list-item"><a href="https://io.wikipedia.org/wiki/Sulfo" title="Sulfo – Ido" lang="io" hreflang="io" data-title="Sulfo" data-language-autonym="Ido" data-language-local-name="Ido" class="interlanguage-link-target">Ido</a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Belerang" title="Belerang – Indonesian" lang="id" hreflang="id" data-title="Belerang" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target">Bahasa Indonesia</a></li><li class="interlanguage-link interwiki-ia mw-list-item"><a href="https://ia.wikipedia.org/wiki/Sulfure" title="Sulfure – Interlingua" lang="ia" hreflang="ia" data-title="Sulfure" data-language-autonym="Interlingua" data-language-local-name="Interlingua" class="interlanguage-link-target">Interlingua</a></li><li class="interlanguage-link interwiki-os mw-list-item"><a href="https://os.wikipedia.org/wiki/%D0%A1%D0%BE%D0%BD%D0%B4%D0%BE%D0%BD" title="Сондон – Ossetic" lang="os" hreflang="os" data-title="Сондон" data-language-autonym="Ирон" data-language-local-name="Ossetic" class="interlanguage-link-target">Ирон</a></li><li class="interlanguage-link interwiki-xh mw-list-item"><a href="https://xh.wikipedia.org/wiki/I-sulphur" title="I-sulphur – Xhosa" lang="xh" hreflang="xh" data-title="I-sulphur" data-language-autonym="IsiXhosa" data-language-local-name="Xhosa" class="interlanguage-link-target">IsiXhosa</a></li><li class="interlanguage-link interwiki-zu mw-list-item"><a href="https://zu.wikipedia.org/wiki/Isibabuli" title="Isibabuli – Zulu" lang="zu" hreflang="zu" data-title="Isibabuli" data-language-autonym="IsiZulu" data-language-local-name="Zulu" class="interlanguage-link-target">IsiZulu</a></li><li class="interlanguage-link interwiki-is mw-list-item"><a href="https://is.wikipedia.org/wiki/Brennisteinn" title="Brennisteinn – Icelandic" lang="is" hreflang="is" data-title="Brennisteinn" data-language-autonym="Íslenska" data-language-local-name="Icelandic" class="interlanguage-link-target">Íslenska</a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Zolfo" title="Zolfo – Italian" lang="it" hreflang="it" data-title="Zolfo" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target">Italiano</a></li><li class="interlanguage-link interwiki-he mw-list-item"><a href="https://he.wikipedia.org/wiki/%D7%92%D7%95%D7%A4%D7%A8%D7%99%D7%AA" title="גופרית – Hebrew" lang="he" hreflang="he" data-title="גופרית" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target">עברית</a></li><li class="interlanguage-link interwiki-jv mw-list-item"><a href="https://jv.wikipedia.org/wiki/Wlirang" title="Wlirang – Javanese" lang="jv" hreflang="jv" data-title="Wlirang" data-language-autonym="Jawa" data-language-local-name="Javanese" class="interlanguage-link-target">Jawa</a></li><li class="interlanguage-link interwiki-kbp mw-list-item"><a href="https://kbp.wikipedia.org/wiki/S%CA%8Af%C9%A9r%C9%A9" title="Sʊfɩrɩ – Kabiye" lang="kbp" hreflang="kbp" data-title="Sʊfɩrɩ" data-language-autonym="Kabɩyɛ" data-language-local-name="Kabiye" class="interlanguage-link-target">Kabɩyɛ</a></li><li class="interlanguage-link interwiki-kn mw-list-item"><a href="https://kn.wikipedia.org/wiki/%E0%B2%97%E0%B2%82%E0%B2%A7%E0%B2%95" title="ಗಂಧಕ – Kannada" lang="kn" hreflang="kn" data-title="ಗಂಧಕ" data-language-autonym="ಕನ್ನಡ" data-language-local-name="Kannada" class="interlanguage-link-target">ಕನ್ನಡ</a></li><li class="interlanguage-link interwiki-ka mw-list-item"><a href="https://ka.wikipedia.org/wiki/%E1%83%92%E1%83%9D%E1%83%92%E1%83%98%E1%83%A0%E1%83%93%E1%83%98" title="გოგირდი – Georgian" lang="ka" hreflang="ka" data-title="გოგირდი" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target">ქართული</a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%9A%D2%AF%D0%BA%D1%96%D1%80%D1%82" title="Күкірт – Kazakh" lang="kk" hreflang="kk" data-title="Күкірт" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target">Қазақша</a></li><li class="interlanguage-link interwiki-kw mw-list-item"><a href="https://kw.wikipedia.org/wiki/Sulfur" title="Sulfur – Cornish" lang="kw" hreflang="kw" data-title="Sulfur" data-language-autonym="Kernowek" data-language-local-name="Cornish" class="interlanguage-link-target">Kernowek</a></li><li class="interlanguage-link interwiki-sw mw-list-item"><a href="https://sw.wikipedia.org/wiki/Sulfuri" title="Sulfuri – Swahili" lang="sw" hreflang="sw" data-title="Sulfuri" data-language-autonym="Kiswahili" data-language-local-name="Swahili" class="interlanguage-link-target">Kiswahili</a></li><li class="interlanguage-link interwiki-kv mw-list-item"><a href="https://kv.wikipedia.org/wiki/%D0%A2%D1%8D%D0%B3" title="Тэг – Komi" lang="kv" hreflang="kv" data-title="Тэг" data-language-autonym="Коми" data-language-local-name="Komi" class="interlanguage-link-target">Коми</a></li><li class="interlanguage-link interwiki-ht mw-list-item"><a href="https://ht.wikipedia.org/wiki/Souf_(eleman)" title="Souf (eleman) – Haitian Creole" lang="ht" hreflang="ht" data-title="Souf (eleman)" data-language-autonym="Kreyòl ayisyen" data-language-local-name="Haitian Creole" class="interlanguage-link-target">Kreyòl ayisyen</a></li><li class="interlanguage-link interwiki-ku mw-list-item"><a href="https://ku.wikipedia.org/wiki/Kewkurd" title="Kewkurd – Kurdish" lang="ku" hreflang="ku" data-title="Kewkurd" data-language-autonym="Kurdî" data-language-local-name="Kurdish" class="interlanguage-link-target">Kurdî</a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%9A%D2%AF%D0%BA%D2%AF%D1%80%D1%82" title="Күкүрт – Kyrgyz" lang="ky" hreflang="ky" data-title="Күкүрт" data-language-autonym="Кыргызча" data-language-local-name="Kyrgyz" class="interlanguage-link-target">Кыргызча</a></li><li class="interlanguage-link interwiki-mrj mw-list-item"><a href="https://mrj.wikipedia.org/wiki/%D0%A1%D0%B5%D1%80%D0%B0" title="Сера – Western Mari" lang="mrj" hreflang="mrj" data-title="Сера" data-language-autonym="Кырык мары" data-language-local-name="Western Mari" class="interlanguage-link-target">Кырык мары</a></li><li class="interlanguage-link interwiki-lld mw-list-item"><a href="https://lld.wikipedia.org/wiki/Solper" title="Solper – Ladin" lang="lld" hreflang="lld" data-title="Solper" data-language-autonym="Ladin" data-language-local-name="Ladin" class="interlanguage-link-target">Ladin</a></li><li class="interlanguage-link interwiki-lo mw-list-item"><a href="https://lo.wikipedia.org/wiki/%E0%BA%8A%E0%BA%B9%E0%BA%99%E0%BA%9F%E0%BA%B9%E0%BA%A3%E0%BA%B4%E0%BA%81" title="ຊູນຟູຣິກ – Lao" lang="lo" hreflang="lo" data-title="ຊູນຟູຣິກ" data-language-autonym="ລາວ" data-language-local-name="Lao" class="interlanguage-link-target">ລາວ</a></li><li class="interlanguage-link interwiki-la mw-list-item"><a href="https://la.wikipedia.org/wiki/Sulphur" title="Sulphur – Latin" lang="la" hreflang="la" data-title="Sulphur" data-language-autonym="Latina" data-language-local-name="Latin" class="interlanguage-link-target">Latina</a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/S%C4%93rs" title="Sērs – Latvian" lang="lv" hreflang="lv" data-title="Sērs" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target">Latviešu</a></li><li class="interlanguage-link interwiki-lb mw-list-item"><a href="https://lb.wikipedia.org/wiki/Schwiefel" title="Schwiefel – Luxembourgish" lang="lb" hreflang="lb" data-title="Schwiefel" data-language-autonym="Lëtzebuergesch" data-language-local-name="Luxembourgish" class="interlanguage-link-target">Lëtzebuergesch</a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Siera" title="Siera – Lithuanian" lang="lt" hreflang="lt" data-title="Siera" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target">Lietuvių</a></li><li class="interlanguage-link interwiki-lij mw-list-item"><a href="https://lij.wikipedia.org/wiki/Sorfano" title="Sorfano – Ligurian" lang="lij" hreflang="lij" data-title="Sorfano" data-language-autonym="Ligure" data-language-local-name="Ligurian" class="interlanguage-link-target">Ligure</a></li><li class="interlanguage-link interwiki-li mw-list-item"><a href="https://li.wikipedia.org/wiki/Solfer" title="Solfer – Limburgish" lang="li" hreflang="li" data-title="Solfer" data-language-autonym="Limburgs" data-language-local-name="Limburgish" class="interlanguage-link-target">Limburgs</a></li><li class="interlanguage-link interwiki-olo mw-list-item"><a href="https://olo.wikipedia.org/wiki/Rikki" title="Rikki – Livvi-Karelian" lang="olo" hreflang="olo" data-title="Rikki" data-language-autonym="Livvinkarjala" data-language-local-name="Livvi-Karelian" class="interlanguage-link-target">Livvinkarjala</a></li><li class="interlanguage-link interwiki-jbo mw-list-item"><a href="https://jbo.wikipedia.org/wiki/sliri" title="sliri – Lojban" lang="jbo" hreflang="jbo" data-title="sliri" data-language-autonym="La .lojban." data-language-local-name="Lojban" class="interlanguage-link-target">La .lojban.</a></li><li class="interlanguage-link interwiki-lmo mw-list-item"><a href="https://lmo.wikipedia.org/wiki/Solfer" title="Solfer – Lombard" lang="lmo" hreflang="lmo" data-title="Solfer" data-language-autonym="Lombard" data-language-local-name="Lombard" class="interlanguage-link-target">Lombard</a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/K%C3%A9n" title="Kén – Hungarian" lang="hu" hreflang="hu" data-title="Kén" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target">Magyar</a></li><li class="interlanguage-link interwiki-mk mw-list-item"><a href="https://mk.wikipedia.org/wiki/%D0%A1%D1%83%D0%BB%D1%84%D1%83%D1%80" title="Сулфур – Macedonian" lang="mk" hreflang="mk" data-title="Сулфур" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target">Македонски</a></li><li class="interlanguage-link interwiki-mg mw-list-item"><a href="https://mg.wikipedia.org/wiki/Solifara" title="Solifara – Malagasy" lang="mg" hreflang="mg" data-title="Solifara" data-language-autonym="Malagasy" data-language-local-name="Malagasy" class="interlanguage-link-target">Malagasy</a></li><li class="interlanguage-link interwiki-ml mw-list-item"><a href="https://ml.wikipedia.org/wiki/%E0%B4%97%E0%B4%A8%E0%B5%8D%E0%B4%A7%E0%B4%95%E0%B4%82" title="ഗന്ധകം – Malayalam" lang="ml" hreflang="ml" data-title="ഗന്ധകം" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target">മലയാളം</a></li><li class="interlanguage-link interwiki-mi mw-list-item"><a href="https://mi.wikipedia.org/wiki/Pungatara" title="Pungatara – Māori" lang="mi" hreflang="mi" data-title="Pungatara" data-language-autonym="Māori" data-language-local-name="Māori" class="interlanguage-link-target">Māori</a></li><li class="interlanguage-link interwiki-mr mw-list-item"><a href="https://mr.wikipedia.org/wiki/%E0%A4%97%E0%A4%82%E0%A4%A7%E0%A4%95" title="गंधक – Marathi" lang="mr" hreflang="mr" data-title="गंधक" data-language-autonym="मराठी" data-language-local-name="Marathi" class="interlanguage-link-target">मराठी</a></li><li class="interlanguage-link interwiki-arz mw-list-item"><a href="https://arz.wikipedia.org/wiki/%D9%83%D8%A8%D8%B1%D9%8A%D8%AA" title="كبريت – Egyptian Arabic" lang="arz" hreflang="arz" data-title="كبريت" data-language-autonym="مصرى" data-language-local-name="Egyptian Arabic" class="interlanguage-link-target">مصرى</a></li><li class="interlanguage-link interwiki-ms mw-list-item"><a href="https://ms.wikipedia.org/wiki/Belerang" title="Belerang – Malay" lang="ms" hreflang="ms" data-title="Belerang" data-language-autonym="Bahasa Melayu" data-language-local-name="Malay" class="interlanguage-link-target">Bahasa Melayu</a></li><li class="interlanguage-link interwiki-mni mw-list-item"><a href="https://mni.wikipedia.org/wiki/%EA%AF%81%EA%AF%9C%EA%AF%90%EA%AF%94" title="ꯁꯜꯐꯔ – Manipuri" lang="mni" hreflang="mni" data-title="ꯁꯜꯐꯔ" data-language-autonym="ꯃꯤꯇꯩ ꯂꯣꯟ" data-language-local-name="Manipuri" class="interlanguage-link-target">ꯃꯤꯇꯩ ꯂꯣꯟ</a></li><li class="interlanguage-link interwiki-min mw-list-item"><a href="https://min.wikipedia.org/wiki/Balerang" title="Balerang – Minangkabau" lang="min" hreflang="min" data-title="Balerang" data-language-autonym="Minangkabau" data-language-local-name="Minangkabau" class="interlanguage-link-target">Minangkabau</a></li><li class="interlanguage-link interwiki-cdo mw-list-item"><a href="https://cdo.wikipedia.org/wiki/Li%C3%B9-u%C3%B2ng" title="Liù-uòng – Mindong" lang="cdo" hreflang="cdo" data-title="Liù-uòng" data-language-autonym="閩東語 / Mìng-dĕ̤ng-ngṳ̄" data-language-local-name="Mindong" class="interlanguage-link-target">閩東語 / Mìng-dĕ̤ng-ngṳ̄</a></li><li class="interlanguage-link interwiki-mwl mw-list-item"><a href="https://mwl.wikipedia.org/wiki/Alxofre" title="Alxofre – Mirandese" lang="mwl" hreflang="mwl" data-title="Alxofre" data-language-autonym="Mirandés" data-language-local-name="Mirandese" class="interlanguage-link-target">Mirandés</a></li><li class="interlanguage-link interwiki-mn mw-list-item"><a href="https://mn.wikipedia.org/wiki/%D0%A5%D2%AF%D1%85%D1%8D%D1%80" title="Хүхэр – Mongolian" lang="mn" hreflang="mn" data-title="Хүхэр" data-language-autonym="Монгол" data-language-local-name="Mongolian" class="interlanguage-link-target">Монгол</a></li><li class="interlanguage-link interwiki-my mw-list-item"><a href="https://my.wikipedia.org/wiki/%E1%80%80%E1%80%94%E1%80%B7%E1%80%BA" title="ကန့် – Burmese" lang="my" hreflang="my" data-title="ကန့်" data-language-autonym="မြန်မာဘာသာ" data-language-local-name="Burmese" class="interlanguage-link-target">မြန်မာဘာသာ</a></li><li class="interlanguage-link interwiki-nah mw-list-item"><a href="https://nah.wikipedia.org/wiki/Tlequiquiztl%C4%81lli" title="Tlequiquiztlālli – Nahuatl" lang="nah" hreflang="nah" data-title="Tlequiquiztlālli" data-language-autonym="Nāhuatl" data-language-local-name="Nahuatl" class="interlanguage-link-target">Nāhuatl</a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Zwavel" title="Zwavel – Dutch" lang="nl" hreflang="nl" data-title="Zwavel" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target">Nederlands</a></li><li class="interlanguage-link interwiki-ne mw-list-item"><a href="https://ne.wikipedia.org/wiki/%E0%A4%97%E0%A4%A8%E0%A5%8D%E0%A4%A7%E0%A4%95" title="गन्धक – Nepali" lang="ne" hreflang="ne" data-title="गन्धक" data-language-autonym="नेपाली" data-language-local-name="Nepali" class="interlanguage-link-target">नेपाली</a></li><li class="interlanguage-link interwiki-new mw-list-item"><a href="https://new.wikipedia.org/wiki/%E0%A4%97%E0%A4%A8%E0%A5%8D%E0%A4%A7%E0%A4%95" title="गन्धक – Newari" lang="new" hreflang="new" data-title="गन्धक" data-language-autonym="नेपाल भाषा" data-language-local-name="Newari" class="interlanguage-link-target">नेपाल भाषा</a></li><li class="interlanguage-link interwiki-ja mw-list-item"><a href="https://ja.wikipedia.org/wiki/%E7%A1%AB%E9%BB%84" title="硫黄 – Japanese" lang="ja" hreflang="ja" data-title="硫黄" data-language-autonym="日本語" data-language-local-name="Japanese" class="interlanguage-link-target">日本語</a></li><li class="interlanguage-link interwiki-frr mw-list-item"><a href="https://frr.wikipedia.org/wiki/Swaawel" title="Swaawel – Northern Frisian" lang="frr" hreflang="frr" data-title="Swaawel" data-language-autonym="Nordfriisk" data-language-local-name="Northern Frisian" class="interlanguage-link-target">Nordfriisk</a></li><li class="interlanguage-link interwiki-no mw-list-item"><a href="https://no.wikipedia.org/wiki/Svovel" title="Svovel – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Svovel" data-language-autonym="Norsk bokmål" data-language-local-name="Norwegian Bokmål" class="interlanguage-link-target">Norsk bokmål</a></li><li class="interlanguage-link interwiki-nn mw-list-item"><a href="https://nn.wikipedia.org/wiki/Svovel" title="Svovel – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Svovel" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target">Norsk nynorsk</a></li><li class="interlanguage-link interwiki-nov mw-list-item"><a href="https://nov.wikipedia.org/wiki/Sulfre" title="Sulfre – Novial" lang="nov" hreflang="nov" data-title="Sulfre" data-language-autonym="Novial" data-language-local-name="Novial" class="interlanguage-link-target">Novial</a></li><li class="interlanguage-link interwiki-oc mw-list-item"><a href="https://oc.wikipedia.org/wiki/Sofre" title="Sofre – Occitan" lang="oc" hreflang="oc" data-title="Sofre" data-language-autonym="Occitan" data-language-local-name="Occitan" class="interlanguage-link-target">Occitan</a></li><li class="interlanguage-link interwiki-or mw-list-item"><a href="https://or.wikipedia.org/wiki/%E0%AC%97%E0%AC%A8%E0%AD%8D%E0%AC%A7%E0%AC%95" title="ଗନ୍ଧକ – Odia" lang="or" hreflang="or" data-title="ଗନ୍ଧକ" data-language-autonym="ଓଡ଼ିଆ" data-language-local-name="Odia" class="interlanguage-link-target">ଓଡ଼ିଆ</a></li><li class="interlanguage-link interwiki-om mw-list-item"><a href="https://om.wikipedia.org/wiki/Waalgaa" title="Waalgaa – Oromo" lang="om" hreflang="om" data-title="Waalgaa" data-language-autonym="Oromoo" data-language-local-name="Oromo" class="interlanguage-link-target">Oromoo</a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Oltingugurt" title="Oltingugurt – Uzbek" lang="uz" hreflang="uz" data-title="Oltingugurt" data-language-autonym="Oʻzbekcha / ўзбекча" data-language-local-name="Uzbek" class="interlanguage-link-target">Oʻzbekcha / ўзбекча</a></li><li class="interlanguage-link interwiki-pa mw-list-item"><a href="https://pa.wikipedia.org/wiki/%E0%A8%97%E0%A9%B0%E0%A8%A7%E0%A8%95" title="ਗੰਧਕ – Punjabi" lang="pa" hreflang="pa" data-title="ਗੰਧਕ" data-language-autonym="ਪੰਜਾਬੀ" data-language-local-name="Punjabi" class="interlanguage-link-target">ਪੰਜਾਬੀ</a></li><li class="interlanguage-link interwiki-pi mw-list-item"><a href="https://pi.wikipedia.org/wiki/%E0%A4%B8%E0%A4%B2%E0%A5%8D%E0%A4%AB%E0%A4%B0" title="सल्फर – Pali" lang="pi" hreflang="pi" data-title="सल्फर" data-language-autonym="पालि" data-language-local-name="Pali" class="interlanguage-link-target">पालि</a></li><li class="interlanguage-link interwiki-pnb mw-list-item"><a href="https://pnb.wikipedia.org/wiki/%DA%AF%D9%86%D8%AF%DA%BE%DA%A9" title="گندھک – Western Punjabi" lang="pnb" hreflang="pnb" data-title="گندھک" data-language-autonym="پنجابی" data-language-local-name="Western Punjabi" class="interlanguage-link-target">پنجابی</a></li><li class="interlanguage-link interwiki-blk mw-list-item"><a href="https://blk.wikipedia.org/wiki/%E1%80%80%E1%80%94%E1%80%BA%EA%A9%BB" title="ကန်ꩻ – Pa'O" lang="blk" hreflang="blk" data-title="ကန်ꩻ" data-language-autonym="ပအိုဝ်ႏဘာႏသာႏ" data-language-local-name="Pa'O" class="interlanguage-link-target">ပအိုဝ်ႏဘာႏသာႏ</a></li><li class="interlanguage-link interwiki-ps mw-list-item"><a href="https://ps.wikipedia.org/wiki/%DA%AF%D9%88%DA%AF%DA%93" title="گوگړ – Pashto" lang="ps" hreflang="ps" data-title="گوگړ" data-language-autonym="پښتو" data-language-local-name="Pashto" class="interlanguage-link-target">پښتو</a></li><li class="interlanguage-link interwiki-jam mw-list-item"><a href="https://jam.wikipedia.org/wiki/Solfa" title="Solfa – Jamaican Creole English" lang="jam" hreflang="jam" data-title="Solfa" data-language-autonym="Patois" data-language-local-name="Jamaican Creole English" class="interlanguage-link-target">Patois</a></li><li class="interlanguage-link interwiki-pms mw-list-item"><a href="https://pms.wikipedia.org/wiki/Sorfo" title="Sorfo – Piedmontese" lang="pms" hreflang="pms" data-title="Sorfo" data-language-autonym="Piemontèis" data-language-local-name="Piedmontese" class="interlanguage-link-target">Piemontèis</a></li><li class="interlanguage-link interwiki-nds mw-list-item"><a href="https://nds.wikipedia.org/wiki/Swevel" title="Swevel – Low German" lang="nds" hreflang="nds" data-title="Swevel" data-language-autonym="Plattdüütsch" data-language-local-name="Low German" class="interlanguage-link-target">Plattdüütsch</a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/Siarka" title="Siarka – Polish" lang="pl" hreflang="pl" data-title="Siarka" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target">Polski</a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Enxofre" title="Enxofre – Portuguese" lang="pt" hreflang="pt" data-title="Enxofre" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target">Português</a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Sulf" title="Sulf – Romanian" lang="ro" hreflang="ro" data-title="Sulf" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target">Română</a></li><li class="interlanguage-link interwiki-qu mw-list-item"><a href="https://qu.wikipedia.org/wiki/Sallina" title="Sallina – Quechua" lang="qu" hreflang="qu" data-title="Sallina" data-language-autonym="Runa Simi" data-language-local-name="Quechua" class="interlanguage-link-target">Runa Simi</a></li><li class="interlanguage-link interwiki-rue mw-list-item"><a href="https://rue.wikipedia.org/wiki/%D0%A1%D1%83%D0%BB%D1%84%D1%83%D1%80" title="Сулфур – Rusyn" lang="rue" hreflang="rue" data-title="Сулфур" data-language-autonym="Русиньскый" data-language-local-name="Rusyn" class="interlanguage-link-target">Русиньскый</a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%A1%D0%B5%D1%80%D0%B0" title="Сера – Russian" lang="ru" hreflang="ru" data-title="Сера" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target">Русский</a></li><li class="interlanguage-link interwiki-sah mw-list-item"><a href="https://sah.wikipedia.org/wiki/%D0%9A%D2%AF%D0%BA%D1%8D%D1%80" title="Күкэр – Yakut" lang="sah" hreflang="sah" data-title="Күкэр" data-language-autonym="Саха тыла" data-language-local-name="Yakut" class="interlanguage-link-target">Саха тыла</a></li><li class="interlanguage-link interwiki-sa mw-list-item"><a href="https://sa.wikipedia.org/wiki/%E0%A4%97%E0%A4%A8%E0%A5%8D%E0%A4%A7%E0%A4%95%E0%A4%83" title="गन्धकः – Sanskrit" lang="sa" hreflang="sa" data-title="गन्धकः" data-language-autonym="संस्कृतम्" data-language-local-name="Sanskrit" class="interlanguage-link-target">संस्कृतम्</a></li><li class="interlanguage-link interwiki-sc mw-list-item"><a href="https://sc.wikipedia.org/wiki/S%C3%B9rfuru" title="Sùrfuru – Sardinian" lang="sc" hreflang="sc" data-title="Sùrfuru" data-language-autonym="Sardu" data-language-local-name="Sardinian" class="interlanguage-link-target">Sardu</a></li><li class="interlanguage-link interwiki-stq mw-list-item"><a href="https://stq.wikipedia.org/wiki/Swieuwel" title="Swieuwel – Saterland Frisian" lang="stq" hreflang="stq" data-title="Swieuwel" data-language-autonym="Seeltersk" data-language-local-name="Saterland Frisian" class="interlanguage-link-target">Seeltersk</a></li><li class="interlanguage-link interwiki-sq mw-list-item"><a href="https://sq.wikipedia.org/wiki/Sulfuri" title="Sulfuri – Albanian" lang="sq" hreflang="sq" data-title="Sulfuri" data-language-autonym="Shqip" data-language-local-name="Albanian" class="interlanguage-link-target">Shqip</a></li><li class="interlanguage-link interwiki-scn mw-list-item"><a href="https://scn.wikipedia.org/wiki/S%C3%B9rfuru" title="Sùrfuru – Sicilian" lang="scn" hreflang="scn" data-title="Sùrfuru" data-language-autonym="Sicilianu" data-language-local-name="Sicilian" class="interlanguage-link-target">Sicilianu</a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B6%9C%E0%B7%99%E0%B6%B1%E0%B7%8A%E0%B6%AF%E0%B6%9C%E0%B6%B8%E0%B7%8A" title="ගෙන්දගම් – Sinhala" lang="si" hreflang="si" data-title="ගෙන්දගම්" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target">සිංහල</a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Sulfur" title="Sulfur – Simple English" lang="en-simple" hreflang="en-simple" data-title="Sulfur" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target">Simple English</a></li><li class="interlanguage-link interwiki-sd mw-list-item"><a href="https://sd.wikipedia.org/wiki/%DA%AF%D9%86%D8%AF%D8%B1%D9%81" title="گندرف – Sindhi" lang="sd" hreflang="sd" data-title="گندرف" data-language-autonym="سنڌي" data-language-local-name="Sindhi" class="interlanguage-link-target">سنڌي</a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/S%C3%ADra" title="Síra – Slovak" lang="sk" hreflang="sk" data-title="Síra" data-language-autonym="Slovenčina" data-language-local-name="Slovak" class="interlanguage-link-target">Slovenčina</a></li><li class="interlanguage-link interwiki-sl mw-list-item"><a href="https://sl.wikipedia.org/wiki/%C5%BDveplo" title="Žveplo – Slovenian" lang="sl" hreflang="sl" data-title="Žveplo" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target">Slovenščina</a></li><li class="interlanguage-link interwiki-so mw-list-item"><a href="https://so.wikipedia.org/wiki/Salfar" title="Salfar – Somali" lang="so" hreflang="so" data-title="Salfar" data-language-autonym="Soomaaliga" data-language-local-name="Somali" class="interlanguage-link-target">Soomaaliga</a></li><li class="interlanguage-link interwiki-ckb mw-list-item"><a href="https://ckb.wikipedia.org/wiki/%DA%AF%DB%86%DA%AF%D8%B1%D8%AF" title="گۆگرد – Central Kurdish" lang="ckb" hreflang="ckb" data-title="گۆگرد" data-language-autonym="کوردی" data-language-local-name="Central Kurdish" class="interlanguage-link-target">کوردی</a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/%D0%A1%D1%83%D0%BC%D0%BF%D0%BE%D1%80" title="Сумпор – Serbian" lang="sr" hreflang="sr" data-title="Сумпор" data-language-autonym="Српски / srpski" data-language-local-name="Serbian" class="interlanguage-link-target">Српски / srpski</a></li><li class="interlanguage-link interwiki-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Sumpor" title="Sumpor – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Sumpor" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target">Srpskohrvatski / српскохрватски</a></li><li class="interlanguage-link interwiki-su mw-list-item"><a href="https://su.wikipedia.org/wiki/Walirang" title="Walirang – Sundanese" lang="su" hreflang="su" data-title="Walirang" data-language-autonym="Sunda" data-language-local-name="Sundanese" class="interlanguage-link-target">Sunda</a></li><li class="interlanguage-link interwiki-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Rikki" title="Rikki – Finnish" lang="fi" hreflang="fi" data-title="Rikki" data-language-autonym="Suomi" data-language-local-name="Finnish" class="interlanguage-link-target">Suomi</a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/Svavel" title="Svavel – Swedish" lang="sv" hreflang="sv" data-title="Svavel" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target">Svenska</a></li><li class="interlanguage-link interwiki-tl mw-list-item"><a href="https://tl.wikipedia.org/wiki/Asupre" title="Asupre – Tagalog" lang="tl" hreflang="tl" data-title="Asupre" data-language-autonym="Tagalog" data-language-local-name="Tagalog" class="interlanguage-link-target">Tagalog</a></li><li class="interlanguage-link interwiki-ta mw-list-item"><a href="https://ta.wikipedia.org/wiki/%E0%AE%95%E0%AE%A8%E0%AF%8D%E0%AE%A4%E0%AE%95%E0%AE%AE%E0%AF%8D" title="கந்தகம் – Tamil" lang="ta" hreflang="ta" data-title="கந்தகம்" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target">தமிழ்</a></li><li class="interlanguage-link interwiki-kab mw-list-item"><a href="https://kab.wikipedia.org/wiki/Akebri" title="Akebri – Kabyle" lang="kab" hreflang="kab" data-title="Akebri" data-language-autonym="Taqbaylit" data-language-local-name="Kabyle" class="interlanguage-link-target">Taqbaylit</a></li><li class="interlanguage-link interwiki-tt mw-list-item"><a href="https://tt.wikipedia.org/wiki/%D0%9A%D2%AF%D0%BA%D0%B5%D1%80%D1%82" title="Күкерт – Tatar" lang="tt" hreflang="tt" data-title="Күкерт" data-language-autonym="Татарча / tatarça" data-language-local-name="Tatar" class="interlanguage-link-target">Татарча / tatarça</a></li><li class="interlanguage-link interwiki-te mw-list-item"><a href="https://te.wikipedia.org/wiki/%E0%B0%97%E0%B0%82%E0%B0%A7%E0%B0%95%E0%B0%AE%E0%B1%81" title="గంధకము – Telugu" lang="te" hreflang="te" data-title="గంధకము" data-language-autonym="తెలుగు" data-language-local-name="Telugu" class="interlanguage-link-target">తెలుగు</a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%81%E0%B8%B3%E0%B8%A1%E0%B8%B0%E0%B8%96%E0%B8%B1%E0%B8%99" title="กำมะถัน – Thai" lang="th" hreflang="th" data-title="กำมะถัน" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target">ไทย</a></li><li class="interlanguage-link interwiki-tg mw-list-item"><a href="https://tg.wikipedia.org/wiki/%D0%A1%D1%83%D0%BB%D1%84%D1%83%D1%80" title="Сулфур – Tajik" lang="tg" hreflang="tg" data-title="Сулфур" data-language-autonym="Тоҷикӣ" data-language-local-name="Tajik" class="interlanguage-link-target">Тоҷикӣ</a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/K%C3%BCk%C3%BCrt" title="Kükürt – Turkish" lang="tr" hreflang="tr" data-title="Kükürt" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target">Türkçe</a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%A1%D1%96%D1%80%D0%BA%D0%B0" title="Сірка – Ukrainian" lang="uk" hreflang="uk" data-title="Сірка" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target">Українська</a></li><li class="interlanguage-link interwiki-ur mw-list-item"><a href="https://ur.wikipedia.org/wiki/%DA%AF%D9%86%D8%AF%DA%BE%DA%A9" title="گندھک – Urdu" lang="ur" hreflang="ur" data-title="گندھک" data-language-autonym="اردو" data-language-local-name="Urdu" class="interlanguage-link-target">اردو</a></li><li class="interlanguage-link interwiki-ug mw-list-item"><a href="https://ug.wikipedia.org/wiki/%DA%AF%DB%88%DA%AD%DA%AF%DB%88%D8%B1%D8%AA" title="گۈڭگۈرت – Uyghur" lang="ug" hreflang="ug" data-title="گۈڭگۈرت" data-language-autonym="ئۇيغۇرچە / Uyghurche" data-language-local-name="Uyghur" class="interlanguage-link-target">ئۇيغۇرچە / Uyghurche</a></li><li class="interlanguage-link interwiki-za mw-list-item"><a href="https://za.wikipedia.org/wiki/Vuengzcungq" title="Vuengzcungq – Zhuang" lang="za" hreflang="za" data-title="Vuengzcungq" data-language-autonym="Vahcuengh" data-language-local-name="Zhuang" class="interlanguage-link-target">Vahcuengh</a></li><li class="interlanguage-link interwiki-vep mw-list-item"><a href="https://vep.wikipedia.org/wiki/Rik" title="Rik – Veps" lang="vep" hreflang="vep" data-title="Rik" data-language-autonym="Vepsän kel’" data-language-local-name="Veps" class="interlanguage-link-target">Vepsän kel’</a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/L%C6%B0u_hu%E1%BB%B3nh" title="Lưu huỳnh – Vietnamese" lang="vi" hreflang="vi" data-title="Lưu huỳnh" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target">Tiếng Việt</a></li><li class="interlanguage-link interwiki-vo mw-list-item"><a href="https://vo.wikipedia.org/wiki/Sulfin" title="Sulfin – Volapük" lang="vo" hreflang="vo" data-title="Sulfin" data-language-autonym="Volapük" data-language-local-name="Volapük" class="interlanguage-link-target">Volapük</a></li><li class="interlanguage-link interwiki-wa mw-list-item"><a href="https://wa.wikipedia.org/wiki/Shoufe" title="Shoufe – Walloon" lang="wa" hreflang="wa" data-title="Shoufe" data-language-autonym="Walon" data-language-local-name="Walloon" class="interlanguage-link-target">Walon</a></li><li class="interlanguage-link interwiki-zh-classical mw-list-item"><a href="https://zh-classical.wikipedia.org/wiki/%E7%A1%AB" title="硫 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="硫" data-language-autonym="文言" data-language-local-name="Literary Chinese" class="interlanguage-link-target">文言</a></li><li class="interlanguage-link interwiki-vls mw-list-item"><a href="https://vls.wikipedia.org/wiki/Sulfer_(element)" title="Sulfer (element) – West Flemish" lang="vls" hreflang="vls" data-title="Sulfer (element)" data-language-autonym="West-Vlams" data-language-local-name="West Flemish" class="interlanguage-link-target">West-Vlams</a></li><li class="interlanguage-link interwiki-war mw-list-item"><a href="https://war.wikipedia.org/wiki/Asupre" title="Asupre – Waray" lang="war" hreflang="war" data-title="Asupre" data-language-autonym="Winaray" data-language-local-name="Waray" class="interlanguage-link-target">Winaray</a></li><li class="interlanguage-link interwiki-wuu mw-list-item"><a href="https://wuu.wikipedia.org/wiki/%E7%A1%AB" title="硫 – Wu" lang="wuu" hreflang="wuu" data-title="硫" data-language-autonym="吴语" data-language-local-name="Wu" class="interlanguage-link-target">吴语</a></li><li class="interlanguage-link interwiki-yi mw-list-item"><a href="https://yi.wikipedia.org/wiki/%D7%A9%D7%95%D7%95%D7%A2%D7%91%D7%9C" title="שוועבל – Yiddish" lang="yi" hreflang="yi" data-title="שוועבל" data-language-autonym="ייִדיש" data-language-local-name="Yiddish" class="interlanguage-link-target">ייִדיש</a></li><li class="interlanguage-link interwiki-yo mw-list-item"><a href="https://yo.wikipedia.org/wiki/S%C3%BAlf%C3%BAr%C3%B9" title="Súlfúrù – Yoruba" lang="yo" hreflang="yo" data-title="Súlfúrù" data-language-autonym="Yorùbá" data-language-local-name="Yoruba" class="interlanguage-link-target">Yorùbá</a></li><li class="interlanguage-link interwiki-zh-yue mw-list-item"><a href="https://zh-yue.wikipedia.org/wiki/%E7%A1%AB" title="硫 – Cantonese" lang="yue" hreflang="yue" data-title="硫" data-language-autonym="粵語" data-language-local-name="Cantonese" class="interlanguage-link-target">粵語</a></li><li class="interlanguage-link interwiki-zh mw-list-item"><a href="https://zh.wikipedia.org/wiki/%E7%A1%AB" title="硫 – Chinese" lang="zh" hreflang="zh" data-title="硫" data-language-autonym="中文" data-language-local-name="Chinese" class="interlanguage-link-target">中文</a></li><li class="interlanguage-link interwiki-zgh mw-list-item"><a href="https://zgh.wikipedia.org/wiki/%E2%B4%B0%E2%B5%A1%E2%B4%B9%E2%B5%89%E2%B5%99" title="ⴰⵡⴹⵉⵙ – Standard Moroccan Tamazight" lang="zgh" hreflang="zgh" data-title="ⴰⵡⴹⵉⵙ" data-language-autonym="ⵜⴰⵎⴰⵣⵉⵖⵜ ⵜⴰⵏⴰⵡⴰⵢⵜ" data-language-local-name="Standard Moroccan Tamazight" class="interlanguage-link-target">ⵜⴰⵎⴰⵣⵉⵖⵜ ⵜⴰⵏⴰⵡⴰⵢⵜ</a></li></ul> </section> </div> <div class="minerva-footer-logo"><img src="/static/images/mobile/copyright/wikipedia-wordmark-en.svg" alt="Wikipedia" width="120" height="18" style="width: 7.5em; height: 1.125em;"/> 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<script>(RLQ=window.RLQ||[]).push(function(){mw.config.set({"wgHostname":"mw-web.codfw.main-f69cdc8f6-6xdtf","wgBackendResponseTime":309,"wgPageParseReport":{"limitreport":{"cputime":"2.836","walltime":"3.386","ppvisitednodes":{"value":36418,"limit":1000000},"postexpandincludesize":{"value":814262,"limit":2097152},"templateargumentsize":{"value":45764,"limit":2097152},"expansiondepth":{"value":56,"limit":100},"expensivefunctioncount":{"value":23,"limit":500},"unstrip-depth":{"value":1,"limit":20},"unstrip-size":{"value":594556,"limit":5000000},"entityaccesscount":{"value":1,"limit":400},"timingprofile":["100.00% 2953.402 1 -total"," 48.88% 1443.587 3 Template:Infobox"," 34.05% 1005.714 1 Template:Infobox_sulfur"," 33.98% 1003.479 1 Template:Infobox_element"," 28.82% 851.026 2 Template:Reflist"," 10.28% 303.746 61 Template:Cite_journal"," 10.18% 300.769 135 Template:Trim"," 9.48% 279.989 1 Template:Infobox_sulfur_isotopes"," 9.42% 278.308 1 Template:Infobox_isotopes_(meta)"," 9.09% 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