So3^2-

A handy guide a rough rationalization of the molecular geometry of SO3 2- (Sulfite ion) including an outline of the SO3 2- bond angles.Looking at the SO3 2- Lewis...SO3 does not have the extra 2 electrons (SO3) 2- has. Therefore, the lewis dot buildings will As proven under, The lewis structure of SO3 is being regarded as when no electrons will intervene with the...Sulfur trioxide (selection spelling sulphur trioxide) is the chemical compound with the formula SO3. It has been described as "unquestionably the most important economically" sulfur oxide.

What is the difference between the Lewis structure of SO3 vs... - Quora

SO42- + 4H+ + 2e =H2SO3 + H2O. (CH3)2SO2 + 2H+ + 2e = (CH3)2SO + H2O.Уравняйте S + SO3 = SO2 химическое уравнение или реакцию с помощью этого калькулятора! Трехокись серы Оксид серы Триоксид серы Серный газ Оксид серы VI SO3 Серы триоксид...

Sulfur trioxide - Wikipedia

Sulfur trioxide

Jump to navigation Jump to search For different makes use of, see SO3 (disambiguation). Sulfur trioxide Names Preferred IUPAC name Sulfur trioxide Systematic IUPAC title Sulfonylideneoxidane Other names Sulfuric anhydride, Sulfur(VI) oxide Identifiers CAS Number 7446-11-9  3D fashion (JSmol) monomer: Interactive imageγ-trimer: Interactive imageα/β polymer: Interactive symbol ChEBI CHEBI:29384  ChemSpider 23080  ECHA InfoCard 100.028.361 EC Number 231-197-3 Gmelin Reference 1448 PubChem CID 2468222235242 (hemihydrate)23035042 (monohydrate) RTECS quantity WT4830000 UNII HH2O7V4LYD  UN quantity UN 1829 CompTox Dashboard (EPA) DTXSID1029673 InChI InChI=1S/O3S/c1-4(2)3 Key: AKEJUJNQAAGONA-UHFFFAOYSA-N InChI=1S/O3S/c1-4(2)3Key: AKEJUJNQAAGONA-UHFFFAOYSA-NInChI=1/O3S/c1-4(2)3Key: AKEJUJNQAAGONA-UHFFFAOYAX SMILES monomer: O=S(=O)=Oγ-trimer: O=S0(=O)OS(=O)(=O)OS(=O)(=O)O0α/β polymer: OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)OS(=O)(=O)O Properties Chemical formula SO3 Molar mass 80.066 g/mol Appearance Colorless to white crystalline cast which is able to fume in air.[1] Colorless liquid and fuel.[2]Odor Varies. Vapor is stinky; like sulfur dioxide.[3] Mist is odorless.[2]Density 1.92 g/cm3, liquid Melting level 16.9 °C (62.4 °F; 290.0 Ok) Boiling point 45 °C (113 °F; 318 K) Solubility in water Reacts to give sulfuric acid Thermochemistry Std molarentropy (So298) 256.77 JK−1mol−1Std enthalpy offormation (ΔfH⦵298) −395.7 kJ/mol Hazards Main hazards Highly corrosive Safety data sheet ICSC 1202 GHS pictograms GHS Signal word Danger GHS danger statements H314, H335 GHS precautionary statements P261, P280, P305+351+338, P310[4]NFPA 704 (fireplace diamond) 3 0 3WOX Flash point Non-flammable Lethal dose or focus (LD, LC): LC50 (median concentration) rat, 4 hr 375 mg/m3Related compounds Other cations Selenium trioxideTellurium trioxide Related sulfur oxides Sulfur monoxideSulfur dioxide Related compounds Sulfuric acid Except the place in a different way famous, information are given for materials of their standard state (at 25 °C [77 °F], 100 kPa).  test (what is  ?) Infobox references

Sulfur trioxide (selection spelling sulphur trioxide) is the chemical compound with the formula SO3. It has been described as "unquestionably the most important economically" sulfur oxide.[5] It is ready on an industrial scale as a precursor to sulfuric acid.

Sulfur trioxide exists in several forms - gaseous monomer, crystalline trimer, and cast polymer. All are colorless bureaucracy. with a slightly slender liquid vary. Gaseous SO3 is the main precursor to acid rain.[6]

Molecular structure and bonding

The molecule SO3 is trigonal planar. As predicted by way of VSEPR idea, its construction belongs to the D3hpoint team. The sulfur atom has an oxidation state of +6 and a formal charge of 0. The S-O bonding is delocalized.[5] The electrical dipole second of gaseous sulfur trioxide is zero.

Chemical reactions

Sulfur trioxide undergoes many reactions.[5]

Hydration and hydrofluorination

SO3 is the anhydride of H2SO4. Thus, it is liable to hydration:

SO3 + H2O → H2SO4 (ΔHf = −Two hundred kJ mol−1)[7] Gaseous sulfur trioxide fumes profusely even in a rather dry setting owing to formation of a sulfuric acid mist.

Akin to the conduct of H2O, hydrogen fluoride provides to provide fluorosulfuric acid:

SO3 + HF → FSO3HDeoxyenation

SO3 reacts with dinitrogen pentoxide to present the nitronium salt of pyrosulfate:

2 SO3 + N2O5 → [NO2]2S2O7Oxidant

Sulfur trioxide is an oxidant. It oxidizes sulfur dichloride to thionyl chloride.

SO3 + SCl2 → SOCl2 + SO2Lewis acid

SO3 is a strong Lewis acid readily forming adducts with Lewis bases.[8] With pyridine, it give the sulfur trioxide pyridine advanced. Related adducts form from dioxane and trimethylamine.

Sulfonating agent

Sulfur trioxide is a potent sulfonating agent, i.e. it provides SO3 teams to substrates. Often the substrates are organic.[9] For activated substrates, Lewis base adducts of sulfur trioxide are efficient sulfonating agents.[10]

Preparation

The direct oxidation of sulfur dioxide to sulfur trioxide in air proceeds very slowly:

SO2 + ​1⁄2O2 = SO3  ΔH=-198.4Industrial

Industrially SO3 is made through the touch process. Sulfur dioxide, which in flip is produced by the burning of sulfur or iron pyrite (a sulfide ore of iron). After being purified by means of electrostatic precipitation, the SO2 is then oxidised through atmospheric oxygen at between 400 and 600 °C over a catalyst. A standard catalyst consists of vanadium pentoxide (V2O5) activated with potassium oxide K2O on kieselguhr or silica improve. Platinum additionally works rather well however is simply too expensive and is poisoned (rendered ineffective) much more simply by impurities.[11] The majority of sulfur trioxide made on this approach is transformed into sulfuric acid.

Laboratory

Sulfur trioxide can be prepared within the laboratory by the two-stage pyrolysis of sodium bisulfate. Sodium pyrosulfate is an intermediate product:[12]

Dehydration at 315 °C: 2 NaHSO4 → Na2S2O7 + H2O Cracking at 460 °C: Na2S2O7 → Na2SO4 + SO3

In contrast, KHSO4 does no longer undergo the same response.[12]

It will also be prepared via dehydrating sulfuric acid with phosphorus pentoxide.[13]

Applications

Sulfur trioxide is a reagent in sulfonation reactions. These processes have the funds for detergents, dyes, and prescribed drugs. Sulfur trioxide is generated in situ from sulfuric acid or is used as a solution within the acid.

Structure SO3

Ball-and-stick fashion of the cyclic trimer of SO3 An ampoule of sulfur trioxide

Both liquid and gaseous[14] SO3 exists in an equilibrium between the monomer and the cyclic trimer. The nature of forged SO3 is complicated and at least Three polymorphs are known, with conversion between them being depending on strains of water.[15]

Absolutely natural SO3 freezes at 16.8 °C to present the γ-SO3 form, which adopts the cyclic trimer configuration [S(=O)2(μ-O)]3.[16][17]

If SO3 is condensed above 27 °C, then α-SO3 paperwork, which has a melting level of 62.3 °C. α-SO3 is fibrous in appearance. Structurally, it's the polymer [S(=O)2(μ-O)]n. Each end of the polymer is terminated with OH teams. β-SO3, just like the alpha shape, is fibrous however of various molecular weight, consisting of an hydroxyl-capped polymer, but melts at 32.5 °C. Both the gamma and the beta bureaucracy are metastable, ultimately changing to the strong alpha form if left status for sufficient time. This conversion is brought about by means of traces of water.[18]

Relative vapor pressures of forged SO3 are alpha < beta < gamma at similar temperatures, indicative in their relative molecular weights. Liquid sulfur trioxide has a vapor power in line with the gamma form. Thus heating a crystal of α-SO3 to its melting level ends up in a sudden build up in vapor drive, which will also be forceful sufficient to shatter a tumbler vessel wherein it's heated. This impact is known as the "alpha explosion".[18]

SO3 is aggressively hygroscopic. The heat of hydration is enough that combos of SO3 and wooden or cotton can ignite. In such cases, SO3 dehydrates those carbohydrates.[18]

Safety

Along with being an oxidizing agent, sulfur trioxide is highly corrosive. It reacts violently with water to supply highly corrosive sulfuric acid.

Sources

NIST Standard Reference Database ChemSub Online

See additionally

Hypervalent molecule Sulfur trioxide pyridine advanced

References

^ .mw-parser-output cite.citationfont-style:inherit.mw-parser-output .citation qquotes:"\"""\"""'""'".mw-parser-output .id-lock-free a,.mw-parser-output .quotation .cs1-lock-free abackground:linear-gradient(clear,transparent),url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat.mw-parser-output .id-lock-limited a,.mw-parser-output .id-lock-registration a,.mw-parser-output .quotation .cs1-lock-limited a,.mw-parser-output .quotation .cs1-lock-registration abackground:linear-gradient(transparent,transparent),url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")correct 0.1em center/9px no-repeat.mw-parser-output .id-lock-subscription a,.mw-parser-output .citation .cs1-lock-subscription abackground:linear-gradient(clear,clear),url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")appropriate 0.1em center/9px no-repeat.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolour:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:lend a hand.mw-parser-output .cs1-ws-icon abackground:linear-gradient(clear,clear),url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat.mw-parser-output code.cs1-codecolour:inherit;background:inherit;border:none;padding:inherit.mw-parser-output .cs1-hidden-errorshow:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-maintshow:none;color:#33aa33;margin-left:0.3em.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em.mw-parser-output .quotation .mw-selflinkfont-weight:inherit"SULFUR TRIOXIDE CAMEO Chemicals NOAA". Cameochemicals.noaa.gov. ^ a b Lerner, L. (2011). Small-Scale Synthesis of Laboratory Reagents with Reaction Modeling. CRC Press. p. 10. ISBN 9781439813133. LCCN 2010038460. ^ "Substance:Sulfur trioxide - Learn Chemistry Wiki". Rsc.org. ^ "Sulfur trioxide 227692" (PDF). SO3. Archived from the original on 2020-09-01. Retrieved 1 September 2020. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2d ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. ^ Thomas Loerting; Klaus R. Liedl (2000). "Toward elimination of descrepancies between theory and experiment: The rate constant of the atmospheric conversion of SO3 to H2SO4". Proceedings of the National Academy of Sciences of the United States of America. 97 (16): 8874–8878. Bibcode:2000PNAS...97.8874L. doi:10.1073/pnas.97.16.8874. PMC 16788. PMID 10922048. ^ "The Manufacture of Sulfuric Acid and Superphosphate" (PDF). Chemical Processes in New Zealand. ^ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5 ^ Weil, J. Ok.; Bistline, Jr., R. G.; Stirton, A. J. (1956). "α-Sulfopalmitic Acid". Organic Syntheses. 36: 83. doi:10.15227/orgsyn.036.0083. ^ Rondestvedt, Jr., Christian S.; Bordwell, F. G. (1954). "Sodium β-Styrenesulfonate and β-Styrenesulfonyl Chloride". Organic Syntheses. 34: 85. doi:10.15227/orgsyn.034.0085. ^ Hermann Müller "Sulfuric Acid and Sulfur Trioxide" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. 2000 doi:10.1002/14356007.a25_635 ^ a b Okay.J. de Vries; P.J. Gellings (May 1969). "The thermal decomposition of potassium and sodium-pyrosulfate". Journal of Inorganic and Nuclear Chemistry. 31 (5): 1307–1313. doi:10.1016/0022-1902(69)80241-1. ^ "How to make sulfur trioxide - YouTube". www.youtube.com. Retrieved 1 September 2020. ^ Lovejoy, R. W.; Colwell, J. H.; Eggers, D. F.; Halsey, G. D. (February 1962). "Infrared Spectrum and Thermodynamic Properties of Gaseous Sulfur Trioxide". The Journal of Chemical Physics. 36 (3): 612–617. doi:10.1063/1.1732581. ^ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated through Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5 ^ Westrik, R.; Mac Gillavry, C. H. (1941). "The crystal structure of the ice-like form of sulphur trioxide (γ-modification)". Recueil des Travaux Chimiques des Pays-Bas. 60 (11): 794–810. doi:10.1002/recl.19410601102. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (second ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. ^ a b c Merck Index of Chemicals and Drugs, 9th ed. monograph 8775 vteOxidesBlended oxidation states Antimony tetroxide (Sb2O4) Cobalt(II,III) oxide (Co3O4) Lead(II,IV) oxide (Pb3O4) Manganese(II,III) oxide Iron(II,III) oxide (Fe3O4)se+1 oxidation state Copper(I) oxide (Cu2O) Caesium oxide (Cs2O) Dicarbon monoxide (C2O) Dichlorine monoxide (Cl2O) Gallium(I) oxide (Ga2O) Lithium oxide (Li2O) Potassium oxide (K2O) Rubidium oxide (Rb2O) Silver oxide (Ag2O) Thallium(I) oxide (Tl2O) Sodium oxide (Na2O) Water (hydrogen oxide) (H2O)+2 oxidation state Aluminium(II) oxide (AlO) Barium oxide (BaO) Beryllium oxide (BeO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N2O2) Germanium monoxide (GeO)) Iron(II) oxide (FeO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S2O2) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Zinc oxide (ZnO)+Three oxidation state Actinium(III) oxide (Ac2O3) Aluminium oxide (Al2O3) Antimony trioxide (Sb2O3) Arsenic trioxide (As2O3) Bismuth(III) oxide (Bi2O3) Boron trioxide (B2O3) Cerium(III) oxide (Ce2O3) Chromium(III) oxide (Cr2O3) Cobalt(III) oxide (Co2O3) Dinitrogen trioxide (N2O3) Dysprosium(III) oxide (Dy2O3) Erbium(III) oxide (Er2O3) Europium(III) oxide (Eu2O3) Gadolinium(III) oxide (Gd2O3) Gallium(III) oxide (Ga2O3) Holmium(III) oxide (Ho2O3) Indium(III) oxide (In2O3) Iron(III) oxide (Fe2O3) Lanthanum oxide (La2O3) Lutetium(III) oxide (Lu2O3) Manganese(III) oxide (Mn2O3) Neodymium(III) oxide (Nd2O3) Nickel(III) oxide (Ni2O3) Phosphorus monoxide (PO) Phosphorus trioxide (P4O6) Praseodymium(III) oxide (Pr2O3) Promethium(III) oxide (Pm2O3) Rhodium(III) oxide (Rh2O3) Samarium(III) oxide (Sm2O3) Scandium oxide (Sc2O3) Terbium(III) oxide (Tb2O3) Thallium(III) oxide (Tl2O3) Thulium(III) oxide (Tm2O3) Titanium(III) oxide (Ti2O3) Tungsten(III) oxide (W2O3) Vanadium(III) oxide (V2O3) Ytterbium(III) oxide (Yb2O3) Yttrium(III) oxide (Y2O3)+Four oxidation state Americium dioxide (AmO2) Carbon dioxide (CO2) Carbon trioxide (CO3) Cerium(IV) oxide (CeO2) Chlorine dioxide (ClO2) Chromium(IV) oxide (CrO2) Dinitrogen tetroxide (N2O4) Germanium dioxide (GeO2) Hafnium(IV) oxide (HfO2) Lead dioxide (PbO2) Manganese dioxide (MnO2) Neptunium(IV) oxide (NpO2) Nitrogen dioxide (NO2) Osmium dioxide (OsO2) Plutonium(IV) oxide (PuO2) Praseodymium(IV) oxide (PrO2) Protactinium(IV) oxide (PaO2) Rhodium(IV) oxide (RhO2) Ruthenium(IV) oxide (RuO2) Selenium dioxide (SeO2) Silicon dioxide (SiO2) Sulfur dioxide (SO2) Tellurium dioxide (TeO2) Terbium(IV) oxide (TbO2) Thorium dioxide (ThO2) Tin dioxide (SnO2) Titanium dioxide (TiO2) Tungsten(IV) oxide (WO2) Uranium dioxide (UO2) Vanadium(IV) oxide (VO2) Zirconium dioxide (ZrO2)+Five oxidation state Antimony pentoxide (Sb2O5) Arsenic pentoxide (As2O5) Dinitrogen pentoxide (N2O5) Niobium pentoxide (Nb2O5) Phosphorus pentoxide (P2O5) Protactinium(V) oxide (Pa2O5) Tantalum pentoxide (Ta2O5) Vanadium(V) oxide (V2O5)+6 oxidation state Chromium trioxide (CrO3) Molybdenum trioxide (MoO3) Rhenium trioxide (ReO3) Selenium trioxide (SeO3) Sulfur trioxide (SO3) Tellurium trioxide (TeO3) Tungsten trioxide (WO3) Uranium trioxide (UO3) Xenon trioxide (XeO3)+7 oxidation state Dichlorine heptoxide (Cl2O7) Manganese heptoxide (Mn2O7) Rhenium(VII) oxide (Re2O7) Technetium(VII) oxide (Tc2O7)+Eight oxidation state Osmium tetroxide (OsO4) Ruthenium tetroxide (RuO4) Xenon tetroxide (XeO4) Iridium tetroxide (IrO4)Related Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide OxypnictideOxides are taken care of via oxidation state. Category:Oxides vteSulfur compoundsSulfides and disulfides Al2S3 As2S2 As2S3 As2S5 As4S4 Au2S Au2S3 B2S3 BaS BeS Bi2S3 CS2 C3S2 C6S6 CaS CdS CeS CoS Cr2S3 CSSe CSTe CuFeS2 CuS D2S Dy2S3 Er2S3 EuS FeS2 GaS H2S HfS2 HgS In2S3 K2S LaS LiS MgS MoS3 NaHS Na2S NH4HS NiS P4Sx PbS PbS2 PSCl3 PSI3 PtS ReS2 Re2S7 SiS SrS TlS VS SeS2 S2U WS2 Sb2S3 Sb2S5 Sb4S3O3 Sm2S3 Y2S3 ZrS2Sulfur halides S2Br2 SBr2 S2Cl2 SCl2 SCl4 SF4 S2F10 SF6 SI2Sulfur oxides and oxyhalides SO2 SO3 SOBr2 SOCl2 SOF2 H2SO3 H2SO4 H2S2O7 H2SO5Sulfites CdSO3 K2SO3Sulfates Ag2SO4 CaSO4 Cs2O4S Er2(SO4)3 Eu2(SO4)3 HgSO4 K2SO4 KAl(SO4)2 NaAl(SO4)2 RaSO4 SnSO4 SrSO4 Ti(SO4)2 Tm2(SO4)3 Yb2(SO4)3 Zr(SO4)2 Thiocyanates HSCN KSCN Co(SCN)2Organosulfur compounds C2H4S C2H6S3 C4H4S C32H66S2 CHCl3S C2H3SNChemical formulation Retrieved from "https://en.wikipedia.org/w/index.php?title=Sulfur_trioxide&oldid=1013477526"

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