| 词条 | Iodine pentoxide |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 450595852 | ImageFile1 = Iodine-pentoxide-3D-balls.png | ImageSize1 = 120px | ImageFile2 = Iodine-pentoxide-3D-vdW.png | ImageSize2 = 120px | IUPACName = Diiodine pentoxide | OtherNames = Iodine(V) oxide Iodic anhydride |Section1={{Chembox Identifiers | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 140179 | InChI = 1/I2O5/c3-1(4)7-2(5)6 | InChIKey = BIZCJSDBWZTASZ-UHFFFAOYAR | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/I2O5/c3-1(4)7-2(5)6 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = BIZCJSDBWZTASZ-UHFFFAOYSA-N | CASNo_Ref = {{cascite|correct|??}} | CASNo = 12029-98-0 | PubChem = 159402 | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 29914 | SMILES = O=I(=O)OI(=O)=O |Section2={{Chembox Properties | Formula = {{Chem|I|2|O|5}} | MolarMass = 333.81 g/mol | Appearance = white crystalline solid[1] hygroscopic | Density = 4.980 g/cm3[1] | MeltingPtC = 300 | MeltingPt_notes = (decomposes) | MeltingPt_ref = [2] | Solubility = | SolubleOther = soluble in water and nitric acid; insoluble in ethanol, ether and CS2 | MagSus = −79.4·10−6 cm3/mol |Section3={{Chembox Hazards | MainHazards = oxidizer | FlashPt = | AutoignitionPt = | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 0 | NFPA-S = OX |Section8={{Chembox Related | OtherAnions = iodine pentafluoride }}Iodine pentoxide is the chemical compound with the formula I2O5. This iodine oxide is the anhydride of iodic acid, and the only stable oxide of iodine. It is produced by dehydrating iodic acid at 200 °C in a stream of dry air:[1] 2HIO3 → I2O5 + H2O StructureI2O5 is bent with an I-O-I angle of 139.2°, but the molecule has no mirror plane so its symmetry is C2 rather than C2v. The terminal I-O distances are around 1.80 Å and the bridging I-O distances are around 1.95 Å.[3] ReactionsIodine pentoxide easily oxidises carbon monoxide to carbon dioxide at room temperature: 5CO + I2O5 → I2 + 5CO2 This reaction can be used to analyse the concentration of CO in a gaseous sample. I2O5 forms iodyl salts, [IO2+], with SO3 and S2O6F2, but iodosyl salts, [IO+], with concentrated sulfuric acid. Iodine pentoxide decomposes to iodine (vapor) and oxygen when heated to about 350 °C.[4] Other compounds{{clear right}}
References1. ^1 2 {{Greenwood&Earnshaw | pages = 851–852 }} {{Iodine compounds}}{{oxygen compounds}}{{DEFAULTSORT:Iodine Pentoxide}}2. ^{{cite book | author = Patnaik, P. | title = Handbook of Inorganic Chemicals | publisher = McGraw-Hill | year = 2002 | isbn = 0-07-049439-8 }} 3. ^{{cite journal |author1=Selte, K. |author2=Kjekshus, A. | year = 1970 | title = Iodine Oxides: Part III. The Crystal Structure of I2O5 | journal = Acta Chemica Scandinavica | volume = 24 | issue = 6 | pages = 1912–1924 | doi = 10.3891/acta.chem.scand.24-1912 | url = http://actachemscand.org/pdf/acta_vol_24_p1912-1924.pdf | format = pdf }} 4. ^G. Baxter and G. Tilley, "A Revision of the Atomic Weights of Iodine and Silver," The Chemical News and Journal of Industrial Science; Volumes 99-100, Royal Society Anniversary Meeting, December 3, 1909, p. 276. ([https://books.google.com/books?id=Rco_AQAAIAAJ&pg=PA323-IA375&lpg=PA323-IA375&dq=decomposition+of+iodine+pentoxide&source=bl&ots=YQnICe63wz&sig=hkAwdjRbL5cCbq2MT-bZrK03XHc&hl=en&sa=X&ei=trWoUrDPIcv6qAG29oGoDQ&ved=0CEsQ6AEwBA#v=onepage&q=decomposition%20of%20iodine%20pentoxide Google Books]) 4 : Iodine compounds|Oxides|Acidic oxides|Oxidizing agents |
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