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[[Senyawa]] '''karbondioksida''', atau CO<sub>2</sub>, adalah [[gas]] atmosfir yang terdiri dari satu atom [[karbon]] dan dua atom [[oksigen]]. Karbondioksida adalah hasil dari [[pembakaran]] [[senyawa organik]] jika cukup jumlah oksigen hadir. Juga dihasilkan oleh berbagai [[mikroorganisme]] dalam [[fermentasi]] dan dihembuskan oleh [[hewan]]. [[Tumbuhan]] menyerap karbondioksida selama [[fotosintesis]], memakai baik karbon maupun oksigen untuk membuat [[karbohidrat]]. Hadir di [[Atmosfer Bumi]] dengan konsentrasi rendah dan bertindak sebagai [[gas rumah kaca]]. Adalah bagian utama dari [[siklus karbon]].
{{dablink|This article is about the chemical element. For other meanings of "sulfur" or "sulphur", see [[sulphur (disambiguation)]]}}
{{Elementbox_header | number=16 | symbol=S | name=sulfur | left=[[phosphorus]] | right=[[chlorine]] | above=[[oxygen|O]] | below=[[selenium|Se]] | color1=#a0ffa0 | color2=black }}
{{Elementbox_series | [[nonmetal]]s }}
{{Elementbox_groupperiodblock | group=16 | period=3 | block=p }}
{{Elementbox_appearance | lemon yellow<br />[[Image:sulfur.jpg|125px| ]] }}
{{Elementbox_atomicmass_gpm | [[1 E-26 kg|32.065]][[List of elements by atomic mass|(5)]] }}
{{Elementbox_econfig | [[[neon|Ne]]] 3s<sup>2</sup> 3p<sup>4</sup> }}
{{Elementbox_epershell | 2, 8, 6 }}
{{Elementbox_section_physicalprop | color1=#a0ffa0 | color2=black }}
{{Elementbox_phase | [[solid]] }}
{{Elementbox_density_gpcm3nrt | (alpha) 2.07 }}
{{Elementbox_density_gpcm3nrt | (beta) 1.96 }}
{{Elementbox_density_gpcm3nrt | (gamma) 1.92 }}
{{Elementbox_densityliq_gpcm3mp | 1.819 }}
{{Elementbox_meltingpoint | k=388.36 | c=115.21 | f=239.38 }}
{{Elementbox_boilingpoint | k=717.8 | c=444.6 | f=832.3 }}
{{Elementbox_criticalpoint | k=1314 | mpa=20.7 }}
{{Elementbox_heatfusion_kjpmol | (mono) 1.727 }}
{{Elementbox_heatvaporiz_kjpmol | (mono) 45 }}
{{Elementbox_heatcapacity_jpmolkat25 | 22.75 }}
{{Elementbox_vaporpressure_katpa | 375 | 408 | 449 | 508 | 591 | 717 | comment= }}
{{Elementbox_section_atomicprop | color1=#a0ffa0 | color2=black }}
{{Elementbox_crystalstruct | orthorhombic }}
{{Elementbox_oxistates | −1, ±2, 4, '''6'''<br />(strongly [[acid]]ic oxide) }}
{{Elementbox_electroneg_pauling | 2.58 }}
{{Elementbox_ionizationenergies4 | 999.6 | 2252 | 3357 }}
{{Elementbox_atomicradius_pm | [[1 E-10 m|100]] }}
{{Elementbox_atomicradiuscalc_pm | [[1 E-11 m|88]] }}
{{Elementbox_covalentradius_pm | [[1 E-10 m|102]] }}
{{Elementbox_vanderwaalsrad_pm | [[1 E-10 m|180]] }}
{{Elementbox_section_miscellaneous | color1=#a0ffa0 | color2=black }}
{{Elementbox_magnetic | no data }}
{{Elementbox_eresist_ohmmat20 | (amorphous)<br />2×10<sup>15</sup> }}
{{Elementbox_thermalcond_wpmkat300k | (amorphous)<br />0.205 }}
{{Elementbox_bulkmodulus_gpa | 7.7 }}
{{Elementbox_mohshardness | 2.0 }}
{{Elementbox_cas_number | 7704-34-9 }}
{{Elementbox_isotopes_begin | isotopesof=sulfur | color1=#a0ffa0 | color2=black }}
{{Elementbox_isotopes_stable | mn=32 | sym=S | na=95.02% | n=16 }}
{{Elementbox_isotopes_stable | mn=33 | sym=S | na=0.75% | n=17 }}
{{Elementbox_isotopes_stable | mn=34 | sym=S | na=4.21% | n=18 }}
{{Elementbox_isotopes_decay | mn=35 | sym=S | na=[[synthetic radioisotope|syn]] | hl=[[1 E6 s|87.32 d]] | dm=[[beta emission|β<sup>-</sup>]] | de=0.167 | pn=35 | ps=[[chlorine|Cl]] }}
{{Elementbox_isotopes_stable | mn=36 | sym=S | na=0.02% | n=20 }}
{{Elementbox_isotopes_end}}
{{Elementbox_footer | color1=#a0ffa0 | color2=black }}
{{kimia-stub}}
'''Sulfur''' or '''sulphur''' ([[#Spelling|see spelling below]]) is the [[chemical element]] in the [[periodic table]] that has the symbol '''S''' and [[atomic number]] 16. It is an abundant, tasteless, odorless, [[Valency (chemistry)|multivalent]] [[non-metal]]. Sulfur, in its native form, is a yellow crystaline solid. In [[nature]], it can be found as the pure element or as [[sulfide]] and [[sulfate]] minerals. It is an essential element for life and is found in two [[amino acid]]s. Its commercial uses are primarily in [[fertilizer]]s but it is also widely used in [[gunpowder]], [[match]]es, [[insecticide]]s and [[fungicide]]s.
[[Kategori:Senyawa kimia]]
== Notable characteristics ==
[[ar:ثاني أكسيد الكربون]]
[[Image:Burning-sulfur.png|thumb|left|A piece of sulfur melts to a blood-red liquid. When burned, it emits a blue flame.]]
[[bg:Въглероден диоксид]]
At room temperature, sulfur is a soft bright yellow solid. Although sulfur is infamous for its smell - frequently compared to rotten eggs - the odor is actually characteristic of [[hydrogen sulfide]] (H<sub>2</sub>S); elemental sulfur is odorless. It burns with a blue flame that emits [[sulfur dioxide]], notable for its peculiar suffocating odor. Sulfur is insoluble in water but [[solubility|soluble]] in [[carbon disulfide]] and to a lesser extent in other organic solvents such as [[benzene]]. Common [[oxidation state]]s of sulfur include −2, +2, +4 and +6. Sulfur forms stable compounds with all elements except the noble gases.
[[bs:Ugljen dioksid]]
[[ca:Diòxid de carboni]]
Sulfur in the solid state ordinarily exists as cyclic crown-shaped S<sub>8</sub> molecules. Sulfur has many [[allotropy|allotrope]]s besides S<sub>8</sub>. Removing one atom from the crown gives S<sub>7</sub>, which is responsible for sulfur's distinctive yellow color. Many other rings have been prepared, including S<sub>12</sub> and S<sub>18</sub>. By contrast, its lighter neighbor [[oxygen]] only exists in two states of chemical significance: O<sub>2</sub> and O<sub>3</sub>. [[Selenium]], the heavier analogue of sulfur can form rings but is more often found as a polymer chain.
[[cs:Oxid uhličitý]]
[[da:Carbondioxid]]
The [[crystallography]] of sulfur is complex. Depending on the specific conditions, the sulfur [[allotrope]]s form several distinct [[crystal structure]]s, with '''[[rhombic]]''' and '''[[monoclinic]]''' S<sub>8</sub> best known.
[[de:Kohlenstoffdioxid]]
[[en:Carbon dioxide]]
A noteworthy property is that the [[viscosity]] of molten sulfur, unlike most other liquids, increases with temperature due to the formation of [[polymer]] chains. However, after a certain temperature is reached, the viscosity is reduced because there is enough energy to break the chains.
[[eo:Karbona dioksido]]
[[es:Dióxido de carbono]]
[[Amorphous]] or "plastic" sulfur can be produced through the rapid cooling of molten sulfur. [[X-ray crystallography]] studies show that the amorphous form may have a [[helix|helical]] structure with eight atoms per turn. This form is [[metastable]] at room temperature and gradually reverts back to crystalline form. This process happens within a matter of hours to days but can be rapidly catalyzed.
[[et:Süsihappegaas]]
[[fi:Hiilidioksidi]]
== Applications ==
[[fr:Dioxyde de carbone]]
[[gl:Dióxido de carbono]]
Sulfur has many industrial uses. Through its major derivative, [[sulfuric acid]] ([[hydrogen|H]]<sub>2</sub>S[[oxygen|O]]<sub>4</sub>), sulfur ranks as one of the more important elements used as an industrial raw material. It is of prime importance to every sector of the [[world economy|world's economies]].
[[he:פחמן דו חמצני]]
[[hr:Ugljični dioksid]]
Sulfuric acid production is the major end use for sulfur, and consumption of sulfuric acid has been regarded as one of the best indices of a nation's industrial development. More sulfuric acid is produced in the [[United States]] every year than any other industrial chemical.
[[hu:Szén-dioxid]]
[[io:Karbo dioxido]]
Sulfur is also used in [[battery (electricity)|batteries]], [[detergents]], the [[vulcanization]] of [[rubber]], [[fungicide]]s, and in the manufacture of [[phosphate]] fertilizers. [[Sulfite]]s are used to [[Bleach (chemical)|bleach]] [[paper]] and as a preservative in [[wine]] and dried [[fruit]]. Because of its flammable nature, sulfur also finds use in [[match]]es, [[gunpowder]], and [[firework]]s. Sodium or ammonium [[sodium thiosulfate|thiosulfate]] are used as photographic fixing agents. [[Magnesium sulfate]], better known as [[Epsom salts]], can be used as a [[laxative]], a bath additive, an [[exfoliant]], or a [[magnesium]] supplement for plants. Sulfur is used as the light-generating medium in the rare lighting fixtures known as [[sulfur lamp]]s.
[[is:Koldíoxíð]]
[[it:Anidride carbonica]]
In the late [[1700s]], [[furniture]] makers used molten sulfur to produce decorative [[inlay]]s in their craft. Because of the [[sulfur dioxide]] produced during the process of melting sulfur, the craft of sulfur inlays was soon abandoned.
[[ja:二酸化炭素]]
[[ko:이산화 탄소]]
== Biological role ==
[[la:Dioxidum carbonis]]
[[lt:Anglies dioksidas]]
The [[amino acid]]s [[cysteine]] and [[methionine]] contain sulfur, as do all [[polypeptide]]s, [[protein]]s, and [[enzyme]]s which contain these amino acids. This makes sulfur a necessary component of all living [[cell (biology)|cells]]. [[Disulfide bond]]s between polypeptides are very important in protein assembly and structure. [[Homocysteine]] and [[taurine]] are also sulfur containing amino acids but are not coded for by [[DNA]] nor are they part of the [[primary structure]] of proteins. Some forms of [[bacterium|bacteria]] use [[hydrogen sulfide]] (H<sub>2</sub>S) in the place of water as the [[electron]] donor in a primitive [[photosynthesis]]-like process. Sulfur is absorbed by [[plant]]s via the [[root]]s from soil as the [[sulfate]] [[ion]] and reduced to sulfide before it is incorporated into [[cysteine]] and other organic sulfur compounds ([[sulfur assimilation]]). Inorganic sulfur forms a part of [[iron-sulfur cluster]]s, and sulfur is the bridging ligand in the [[copper|Cu]]<sub>A</sub> site of [[cytochrome c oxidase]]. Sulfur is an important component of [[CoA|coenzyme A]].
[[lv:Oglekļa dioksīds]]
[[mk:Јаглерод диоксид]]
== Environmental impact ==
[[ms:Karbon dioksida]]
[[nl:Kooldioxide]]
The burning of [[coal]] and [[petroleum]] by industry and power plants liberates huge amounts of [[sulfur dioxide]] (S[[oxygen|O]]<sub>2</sub>) which reacts with atmospheric water and oxygen to produce sulfuric acid. This sulfuric acid is a component of [[acid rain]], which lowers the [[pH]] of [[soil]] and freshwater bodies, resulting in substantial damage to the [[natural environment]] and [[chemical weathering]] of statues and architecture. Fuel standards increasingly require sulfur to be extracted from [[fossil fuel]]s to prevent the formation of acid rain. This extracted sulfur is then refined and represents a large portion of sulfur production.
[[nn:Karbondioksid]]
[[no:Karbondioksid]]
== History ==
[[oc:Dioxide de carbòni]]
[[pl:Dwutlenek węgla]]
[[Image:SulfurCrystal.jpg|thumb|left|Sulfur crystal]]
[[pt:Dióxido de carbono]]
Sulfur ([[Sanskrit]], ''sulvere''; [[Latin]] ''sulpur'') was known in ancient times, and is referred to in the [[Bible|Biblical]] [[Pentateuch]] ([[Genesis]]). The word itself is almost certainly from the [[Arabic language|Arabic]] ''sufra'' meaning yellow, from the bright color of the naturally-occurring form.
[[ru:Диоксид углерода]]
[[sc:Diòssidu de carboniu]]
English translations of the Bible commonly refer to sulfur as "brimstone", giving rise to the name of 'Fire and brimstone' [[sermon]]s, which sinners are reminded of their fate of eternal damnation. It is from this part of the Bible that [[Hell]] is implied to "smell of sulfur", although as mentioned above sulfur is in fact odorless. The "smell of sulfur" usually refers to the odor of [[hydrogen sulfide]], e.g. from rotten eggs. Burning sulfur produces [[sulfur dioxide]], the smell associated with burnt matches.
[[simple:Carbon dioxide]]
[[sk:Oxid uhličitý]]
[[Homer]] mentioned "pest-averting sulfur" in the [[8th century BC]] and in [[424 BC]], the tribe of [[Boeotia]] destroyed the walls of a city by burning a mixture of coal, sulfur, and tar under them. Sometime in the [[12th century]], the [[China|Chinese]] invented [[gun powder]] which is a mixture of [[potassium nitrate]] ([[potassium|K]][[nitrogen|N]][[oxygen|O]]<sub>3</sub>), [[carbon]], and sulfur. Early [[alchemy|alchemists]] gave sulfur its own alchemical symbol which was a triangle at the top of a cross. In the late [[1770s]], [[Antoine Lavoisier]] helped convince the scientific community that sulfur was an element and not a compound. In 1867, sulfur was discovered in underground deposits in [[Louisiana]] and [[Texas]]. The overlying layer of earth was [[quicksand]], prohibiting ordinary mining operations. Therefore the [[Frasch process]] was utilized.
[[sl:Ogljikov dioksid]]
[[sr:Угљен диоксид]]
== Occurrence ==
[[sv:Koldioxid]]
[[th:คาร์บอนไดออกไซด์]]
[[Image:SulfurUSGOV.jpg|thumb|left|Sulfur]]
[[tr:Karbondioksit]]
[[Image:NZ sulfur NI.jpg|thumb|right|Sulfur crystalites at [[Wai-o-tapu]] [[hot springs]], [[New Zealand]]]]
[[vi:Điôxít cacbon]]
[[wa:Diyocside di carbone]]
Elemental sulfur can be found near [[hot spring]]s and [[volcanic]] regions in many parts of the world, especially along the [[Pacific Ring of Fire]]. These occurrences are the basis for the traditional name brimstone, since sulfur could be found near the brims of volcanic craters. Such volcanic deposits are currently exploited in [[Indonesia]], [[Chile]], and [[Japan]].
[[zh:二氧化碳]]
Significant desposits of elemental sulfur also exist in [[salt domes]] along the coast of the [[Gulf of Mexico]], and in [[evaporite]]s in eastern Europe and western Asia. The sulfur in these deposits is believed to come from the action of [[anaerobic bacteria]] on [[sulfate]] minerals, especially [[gypsum]]. Such deposits are the basis for commercial production in the [[United States]], [[Poland]], [[Russia]], [[Turkmenistan]], and [[Ukraine]].
Sulfur extracted from oil, gas and the [[Athabasca Oil Sands]] has become a glut on the market, with huge stockpiles of sulfur in existence throughout Alberta.
[[Image:AlbertaSulfurAtVancouverBC.jpg|thumb|250px|right|Sulfur mined in [[Alberta]], prepared for shipment at [[Vancouver|Vancouver, B. C.]]]]
Common naturally-occurring sulfur compounds include the metal [[sulfide]]s, such as [[pyrite]] (iron sulfide), [[cinnabar]] (mercury sulfide), [[galena]] ([[lead sulfide]]), [[sphalerite]] (zinc sulfide) and [[stibnite]] (antimony sulfide); and the metal sulfates, such as gypsum (calcium sulfate), [[alunite]] (potassium aluminium sulfate), and [[barite]] (barium sulfate). [[Hydrogen sulfide]] is the gas responsible for the odor of rotten [[egg (biology)|eggs]]. It occurs naturally in volcanic emissions, such as from [[hydrothermal vent]]s, and from bacterial action on decaying sulfur-containing organic matter.
The distinctive colors of [[Jupiter (planet)|Jupiter]]'s [[volcano|volcanic]] moon, [[Io (moon)|Io]], are from various forms of molten, solid and gaseous sulfur. There is also a dark area near the [[Moon|Lunar]] [[Impact crater|crater]] [[Aristarchus (crater)|Aristarchus]] that may be a sulfur deposit. Sulfur is also present in many types of [[meteorite]]s.
''See also [[:Category:Sulfide minerals|Sulfide minerals]], [[:Category:Sulfate minerals|Sulfate minerals]].''
== Compounds ==
[[Hydrogen sulfide]] has the characteristic smell of rotten eggs. Dissolved in water, hydrogen sulfide is acidic and will react with metals to form a series of metal sulfides. Natural metal sulfides are common, especially those of iron. Iron sulfide is called [[pyrite]], the so called ''fool's gold''. Interestingly, pyrite can show semiconductor properties.[http://home.earthlink.net/~lenyr/iposc.htm] [[Galena]], a naturally occurring lead sulfide, was the first [[semiconductor]] discovered, and found a use as a signal [[rectifier]] in the "cat's whiskers" of early [[crystal radio]]s.
Many of the unpleasant odors of organic matter are based on sulfur-containing compounds such as [[Methanethiol|methyl]] and [[Ethanethiol|ethyl mercaptan]] used to scent natural gas so that leaks are easily detectable. The odor of [[garlic]] and "[[skunk]] stink" are also caused by sulfur-containing organic compounds. However, not all organic sulfur compounds smell unpleasant; for example, [[grapefruit mercaptan]], a sulfur-containing [[terpene|monoterpenoid]] is responsible for the characteristic scent of [[grapefruit]].
Polymeric sulfur nitride has metallic properties even though it does not contain any [[metal]] atoms. This compound also has unusual electrical and optical properties. This polymer can be made from [[tetrasulfur tetranitride]] S<sub>4</sub>N<sub>4</sub>.
Phosphorus sulfides are important in synthesis. For example, P<sub>4</sub>S<sub>10</sub> and its derivatives [[Lawesson's reagent]] and [[naphthalen-1,8-diyl 1,3,2,4-dithiadiphosphetane 2,4-disulfide]] are used to replace oxygen from some organic molecules with sulfur.
'''Inorganic sulfur compounds:'''
* [[Sulfide]]s (S<sup>2-</sup>), a complex family of compounds usually derived from S<sup>2-</sup>. [[Cadmium sulfide]] (CdS) is an example.
* [[Sulfites]] (SO<sub>3</sub><sup>2-</sup>), the salts of [[sulfurous acid]] (H<sub>2</sub>SO<sub>3</sub>) which is generated by dissolving SO<sub>2</sub> in water. Sulfurous acid and the corresponding sulfites are fairly strong reducing agents. Other compounds derived from SO<sub>2</sub> include the pyrosulfite or metabisulfite ion (S<sub>2</sub>O<sub>5</sub><sup>2−</sup>).
* [[Sulfate]]s (SO<sub>4</sub><sup>2-</sup>), the salts of [[sulfuric acid]]. Sulfuric acid also reacts with SO<sub>3</sub> in equimolar ratios to form [[pyrosulfuric acid]] (H<sub>2</sub>S<sub>2</sub>O<sub>7</sub>).
* [[sodium thiosulfate|Thiosulfates]] (sometimes referred to as thiosulfites or "hyposulfites") (S<sub>2</sub>O<sub>3</sub><sup>2−</sup>). Thiosulfates are used in photographic fixing (HYPO) as reducing agents. Ammonium thiosulfate is being investigated as a [[cyanide]] replacement in leaching [[gold]].[http://doccopper.tripod.com/gold/AltLixiv.html]
* [[Sodium dithionite]], Na<sub>2</sub>S<sub>2</sub>O<sub>4</sub>, is the highly reducing dianion derived from hyposulfurous/dithionous acid.
* [[Sodium dithionate]] (Na<sub>2</sub>S<sub>2</sub>O<sub>6</sub>).
* [[Polythionic acid]]s (H<sub>2</sub>S<sub>''n''</sub>O<sub>6</sub>), where ''n'' can range from 3 to 80.
* [[Peroxymonosulfuric acid]] (H<sub>2</sub>SO<sub>5</sub>) and [[peroxydisulfuric acid]]s (H<sub>2</sub>S<sub>2</sub>O<sub>8</sub>), made from the action of SO<sub>3</sub> on concentrated [[hydrogen peroxide|H<sub>2</sub>O<sub>2</sub>]], and [[sulfuric acid|H<sub>2</sub>SO<sub>4</sub>]] on concentrated H<sub>2</sub>O<sub>2</sub> respectively.
* [[Sodium polysulfide]]s (Na<sub>2</sub>S<sub>x</sub>)
* [[Sulfur hexafluoride]], SF<sub>6</sub>, a dense gas at ambient conditions, is used as nonreactive and nontoxic propellant
* Sulfur nitrides are chain and cyclic compounds containing only S and N. [[Tetrasulfur tetranitride]] S<sub>4</sub>N<sub>4</sub> is an example.
* [[Thiocyanate]]s contain the SCN<sup>-</sup> group. Oxidation of thiocyanoate gives [[thiocyanogen]], (SCN)<sub>2</sub> with the connectivity NCS-SCN.
'''Organic sulfur compounds''' (where R, R', and R'' are organic groups such as CH<sub>3</sub>):
* [[Thioether]]s have the form ''R''-S-''R′''. These compounds are the sulfur equivalents of [[ether]]s.
* [[Sulfonium]] ions have the formula RR'S-'R'", i.e. where three groups are attached to the cationic sulfur center. [[Dimethylsulfoniopropionate]] ([[DMSP]]; (CH<sub>3</sub> )<sub>2</sub>S<sup>+</sup>CH<sub>2</sub>CH<sub>2</sub>COO<sup>-</sup>) is a sulfonium ion, which is important in the marine organic sulfur cycle.
* [[Thiol]]s (also known as mercaptans) have the form R-SH. These are the sulfur equivalents of [[alcohol]]s.
* [[Thiolate]]s ions s have the form R-S<sup>-</sup>. Such anions arise upon treatment of [[thiol]]s with base.
* [[Sulfoxide]]s have the form ''R''-S(=O)-''R''&prime. A common sulfoxide is [[dimethyl sulfoxide|DMSO]].
* [[Sulfone]]s have the form ''R''-S(=O)<sub>2</sub>-''R''&prime. A common sulfone is sulfolane C<sub>4</sub>H<sub>8</sub>SO<sub>2</sub>.
''See also [[:category:Sulfur compounds|Category: sulfur compounds]] and [[organosulfur chemistry]]''
== Isotopes ==
Sulfur has 18 [[isotope]]s, of which four are stable: <sup>32</sup>S (95.02%), <sup>33</sup>S (0.75%), <sup>34</sup>S (4.21%), and <sup>36</sup>S (0.02%). Other than <sup>35</sup>S, the [[radioactive isotopes]] of sulfur are all short lived. <sup>35</sup>S is formed from [[cosmic ray]] [[spallation]] of <sup>40</sup>[[argon|Ar]] in the [[Earth's atmosphere|atmosphere]]. It has a [[half-life]] of 87 days.
When sulfide [[mineral]]s are precipitated, isotopic equilibration among solids and liquid may cause small differences in the δS-34 values of co-genetic minerals. The differences between minerals can be used to estimate the temperature of equilibration. The δ[[carbon|C]]-13 and δS-34 of co-existing [[carbonate]]s and sulfides can be used to determine the [[pH]] and [[oxygen]] [[fugacity]] of the ore-bearing fluid during ore formation.
In most [[forest]] ecosystems, sulfate is derived mostly from the atmosphere; weathering of ore minerals and evaporites also 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 [[hydrology|hydrologic]] studies. Differences in the [[natural abundance]]s can also be used in systems where there is sufficient variation in the <sup>34</sup>S of ecosystem components. [[Rocky Mountain]] lakes thought to be dominated by atmospheric sources of sulfate have been found to have different δS-34 values from lakes believed to be dominated by watershed sources of sulfate.
== Precautions ==
Carbon disulfide, carbon oxysulfide, hydrogen sulfide, and sulfur dioxide should all be handled with care.
Although '''[[sulfur dioxide]]''' is sufficiently safe to be used as a [[food additive]] in small amounts, at high concentrations it reacts with moisture to form [[sulfurous acid]] which in sufficient quantities may harm the [[lungs]], [[eyes]] or other [[Biological tissue|tissues]]. In creatures without lungs such as insects or plants, it otherwise prevents [[Respiration (physiology)|respiration]].
'''[[Hydrogen sulfide]]''' is quite [[toxic]] (more toxic than [[cyanide]]). Although very pungent at first, it quickly deadens the sense of smell, so potential victims may be unaware of its presence until it is too late.
== Spelling ==
The element has traditionally been spelled ''sulphur'' in the [[United Kingdom]], [[Ireland]], and [[India]], but ''sulfur'' in the [[United States]], while both spellings are used in [[Australia]], [[Canada]] and [[New Zealand]]. The [[IUPAC]] adopted the spelling "sulfur" in 1990, as did the [[Royal Society of Chemistry]] Nomenclature Committee in 1992. This spelling has begun to replace its variant in official use, unlike ''aluminum'', a spelling which is not commonly used outside [[North America]].
== See also ==
* [[Sulfur cycle]]
* [[Disulfide bond]]
* [[Sulfonium]] S<sup>+</sup>, S<sup>+</sup>R<sub>3</sub>
== References ==
* [http://periodic.lanl.gov/elements/16.html Los Alamos National Laboratory – Sulfur]
* R. Steudel (ed.): Elemental Sulfur and Sulfur-Rich Compounds (part I & II), Topics in Current Chemistry Vol. 230 & 231, Springer, Berlin 2003.
== External links ==
{{Commons|Sulfur}}
{{wiktionary|sulfur}}
* [http://library.tedankara.k12.tr/chemistry/vol2/allotropy/z129.htm Sulfur phase diagram.]
* [http://www.webelements.com/webelements/elements/text/S/index.html WebElements.com – Sulfur]
*[http://www.chemicalelements.com/elements/s.html chemicalelements.com/sulfur]
[[Category:Chemical elements]]
[[Category:Nonmetals]]
[[Category:Chalcogens]]
[[Category:Pyrotechnic chemicals]]
[[Category:Sulfur compounds|*]]
{{Link FA|sr}}
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[[eo:Sulfuro]]
[[es:Azufre]]
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[[fr:Soufre]]
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[[id:Belerang]]
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