خامس أكسيد اليود
خامس أكسيد اليود هو مركب كيميائي بالصيغة I2O5. أكسيد اليود هذا هو 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]
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| الأسماء | ||
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| اسم أيوپاك
Iodine pentoxide
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| أسماء أخرى
Iodine(V) oxide
Iodic anhydride | ||
| Identifiers | ||
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3D model (JSmol)
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| ChEBI | ||
| ChemSpider | ||
| ECHA InfoCard | 100.031.569 
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PubChem CID
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| UNII | ||
CompTox Dashboard (EPA)
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| InChI | InChI={{{value}}} | |
| SMILES | ||
| الخصائص | ||
| الصيغة الجزيئية | I 2O 5 | |
| كتلة مولية | 333.81 g/mol | |
| المظهر | white crystalline solid[1] hygroscopic | |
| الكثافة | 4.980 g/cm3[1] | |
| نقطة الانصهار | ||
| قابلية الذوبان | soluble in water and nitric acid; insoluble in ethanol, ether and CS2 | |
| القابلية المغناطيسية | −79.4·10−6 cm3/mol | |
| Section4 = | المخاطر | |
| خطر رئيسي | oxidizer | |
| NFPA 704 (معيـَّن النار) | ||
| مركبات ذا علاقة | ||
أنيونات أخرى
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خامس فلوريد اليود | |
ما لم يُذكر غير ذلك، البيانات المعطاة للمواد في حالاتهم العيارية (عند 25 °س [77 °ف]، 100 kPa). | ||
 verify (what is  ?)
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| مراجع الجدول | ||
- 2HIO3 → I2O5 + H2O
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البنية
I2O5 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.[2]
التفاعلات
Iodine pentoxide easily oxidises carbon monoxide to carbon dioxide at room temperature:
- 5 CO + I2O5 → I2 + 5 CO2
This reaction can be used to analyze 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.[3]
المراجع
- ^ أ ب ت Greenwood, N. N. (1997). Chemistry of the Elements (2nd Edition ed.). Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
{{cite book}}:|edition=has extra text (help); Unknown parameter|coauthors=ignored (|author=suggested) (help) - ^ Selte, K.; Kjekshus, A. (1970). "Iodine Oxides: Part III. The Crystal Structure of I2O5" (PDF). Acta Chemica Scandinavica. 24 (6): 1912–1924. doi:10.3891/acta.chem.scand.24-1912.
- ^ 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. (Google Books)
| HI | He | ||||||||||||||||
| LiI | BeI2 | BI3 | CI4 | NI3 | I2O4, I2O5, I4O9 | IF, IF3, IF5, IF7 | Ne | ||||||||||
| NaI | MgI2 | AlI3 | SiI4 | PI3, P2I4 | S | ICl, ICl3 | Ar | ||||||||||
| KI | CaI2 | Sc | TiI4 | VI3 | Cr | MnI2 | Fe | CoI2 | NiI2 | CuI | ZnI2 | Ga2I6 | GeI2, GeI4 | AsI3 | Se | IBr | Kr |
| RbI | SrI2 | Y | ZrI4 | Nb | Mo | Tc | Ru | Rh | Pd | AgI | CdI2 | InI3 | SnI4, SnI2 | SbI3 | TeI4 | I | Xe |
| CsI | BaI2 | Hf | Ta | W | Re | Os | Ir | Pt | AuI | Hg2I2, HgI2 | TlI | PbI2 | Bi | Po | At | Rn | |
| Fr | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Uub | Uut | Uuq | Uup | Uuh | Uus | Uuo | |
| ↓ | |||||||||||||||||
| La | Ce | Pr | Nd | Pm | SmI2 | Eu | Gd | TbI3 | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | ThI4 | Pa | U | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||