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Contents

   



(Top)
  


1 Structure  




2 Reactions  




3 References  













Iodine pentoxide






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From Wikipedia, the free encyclopedia
  

Iodine pentoxide
Names
IUPAC name

Iodine pentoxide

Other names

Iodine(V) oxide
Iodic anhydride

Identifiers

CAS Number

3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.031.569 Edit this at Wikidata

PubChem CID
UNII

CompTox Dashboard (EPA)

  • InChI=1S/I2O5/c3-1(4)7-2(5)6 checkY

    Key: BIZCJSDBWZTASZ-UHFFFAOYSA-N checkY

  • InChI=1/I2O5/c3-1(4)7-2(5)6

    Key: BIZCJSDBWZTASZ-UHFFFAOYAR

  • O=I(=O)OI(=O)=O

Properties

Chemical formula

 I
2O
5
Molar mass 333.81 g/mol
Appearance white crystalline solid[1]
hygroscopic
Density 4.980 g/cm3[1]
Melting point 300 °C (572 °F; 573 K)[2] (decomposes)
Solubility soluble in water and nitric acid;
insoluble in ethanol, ether and CS2

Magnetic susceptibility (χ)

 −79.4·10−6cm3/mol
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

 -173.0 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):

Main hazards

 oxidizer
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
3
0
0
OX
Related compounds

Other anions

 iodine pentafluoride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

☒N verify (what is checkY☒N ?)

Infobox references

Iodine pentoxide
Fresh iodine pentoxide

Iodine pentoxide is the chemical compound with the formulaI2O5. This iodine oxide is the anhydrideofiodic 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

Structure[edit]

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.[3]

Reactions[edit]

Iodine pentoxide easily oxidises carbon monoxidetocarbon 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.[4]

References[edit]

  1. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 851–852. ISBN 978-0-08-037941-8.
  • ^ Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. ISBN 0-07-049439-8.
  • ^ 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)

    • Retrieved from "https://en.wikipedia.org/w/index.php?title=Iodine_pentoxide&oldid=1145087138"
    Categories: 
    ●Iodine compounds
     ●Oxides
     ●Acidic oxides
     ●Oxidizing agents
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