Iodine pentoxide

Iodine pentoxide
Names


IUPAC name Diiodine pentoxide
Other names Iodine(V) oxide Iodic anhydride
Identifiers
CAS Number	12029-98-0^Y
3D model (Jmol)	Interactive image
ChEBI	CHEBI:29914^Y
ChemSpider	140179^Y
ECHA InfoCard	100.031.569
PubChem	159402
InChI InChI=1S/I2O5/c3-1(4)7-2(5)6^Y Key: BIZCJSDBWZTASZ-UHFFFAOYSA-N^Y InChI=1/I2O5/c3-1(4)7-2(5)6 Key: BIZCJSDBWZTASZ-UHFFFAOYAR
SMILES 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 nitric acid; insoluble in ethanol, ether and CS₂
Hazards
Main hazards	oxidizer
NFPA 704	0 3 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 ^YN ?)
Infobox references

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

Structure

I₂O₅ is bent with an I-O-I angle of 139.2°, but the molecule has no mirror plane so its symmetry is not C_2v. The terminal I-O distances are around 1.80 Å and the bridging I-O distances are around 1.95 Å.^[3]

Reactions

Iodine 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

Other compounds of iodine with elements in the periodic table:

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	CrI₃	MnI₂	FeI₂	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	BiI₃	Po	AtI	Rn
Fr	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts	Og
		↓
		La	Ce	Pr	Nd	Pm	SmI₂	Eu	Gd	TbI₃	Dy	Ho	Er	Tm	Yb	Lu
		Ac	ThI₄	Pa	UI₃, UI₄	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr

References

1 2 3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 851–852. ISBN 0-08-037941-9.
↑ 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)

Iodine compounds

Iodine(-I)	HI AtI ICN I⁻

Iodine(I)	HIO ICl IF IBr

Iodine(III)	HIO₂ ICl₃ IF₃

Iodine(V)	HIO₃ IF₅ I₂O₅

Iodine(VII)	HIO₄ H₅IO₆ IF₇

Oxygen compounds

AgO Al₂O₃ AmO₂ Am₂O₃ As₂O₃ As₂O₅ Au₂O₃ B₂O₃ BaO BeO Bi₂O₃ BiO₂ Bi₂O₅ BrO₂ Br₂O₃ Br₂O₅ CO CO₂ C₂O₃ CaO CaO₂ CdO CeO₂ Ce₂O₃ ClO₂ Cl₂O Cl₂O₃ Cl₂O₄ Cl₂O₆ Cl₂O₇ CoO Co₂O₃ Co₃O₄ CrO₃ Cr₂O₃ Cr₂O₅ Cr₅O₁₂ CsO₂ Cs₂O₃ CuO D₂O Dy₂O₃ Er₂O₃ Eu₂O₃ F₂O F₂O₂ F₂O₄ FeO Fe₂O₃ Fe₃O₄ Ga₂O Ga₂O₃ GeO GeO₂ H₂O H₂¹⁸O H₂O₂ HfO₂ HgO Hg₂O Ho₂O₃ I₂O₄ I₂O₅ I₂O₆ I₄O₉ In₂O₃ InO₂ KO₂ K₂O₂ La₂O₃ Li₂O Li₂O₂ Lu₂O₃ MgO Mg₂O₃ MnO MnO₂ Mn₂O₃ Mn₂O₇ MoO₂ MoO₃ Mo₂O₃ NO NO₂ N₂O N₂O₃ N₂O₄ N₂O₅ NaO₂ Na₂O Na₂O₂ NbO NbO₂ Nd₂O₃

Chemical formulas

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