Iodine monochloride

Iodine monochloride
Names
Preferred IUPAC name
Iodine monochloride
Iodine(I) chloride
Systematic IUPAC name
Chloroiodane
Other names
Iodine chloride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.306
EC Number 232-236-7
MeSH Iodine-monochloride
UN number 1792
Properties
ICl
Molar mass 162.35 g/mol
Appearance reddish-brown
Density 3.10 g/cm3
Melting point 27.2 °C (81.0 °F; 300.3 K) (α-form)
13.9 °C (β-form)
Boiling point 97.4 °C (207.3 °F; 370.5 K)
Hydrolyzes
Solubility soluble in CS2
acetic acid
pyridine
alcohol, ether, HCl
−54.6·10−6 cm3/mol
Hazards
Main hazards corrosive
Safety data sheet External MSDS
Related compounds
Related interhalogen compounds
 Chlorine monofluoride
Bromine monochloride
Iodine monobromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

Iodine monochloride is an interhalogen compound with the formula ICl. It is a red-brown chemical compound that melts near room temperature. Because of the difference in the electronegativity of iodine and chlorine, ICl is highly polar and behaves as a source of I+.

Iodine monochloride is produced simply by combining the halogens in a 1:1 molar ratio, according to the equation

I2 + Cl2 → 2 ICl

When chlorine gas is passed through iodine crystals, one observes the brown vapor of iodine monochloride. Dark brown iodine monochloride liquid is collected. Excess chlorine converts iodine monochloride into iodine trichloride in a reversible reaction:

ICl + Cl2 ⇌ ICl3

Polymorphs

ICl has two polymorphs; α-ICl, which exists as black needles (red by transmitted light) with a melting point of 27.2 °C, and β-ICl, which exists as black platelets (red-brown by transmitted light) with a melting point 13.9 °C.[1]

In the crystal structures of both polymorphs the molecules are arranged in zig-zag chains. β-ICl is monoclinic with the space group P21/c.[2]

Reactions and uses

Iodine monochloride is soluble in acids such as HF and HCl but reacts with pure water to form HCl and HI:

ICl + H2O → HCl + HI + ½O2

ICl is a useful reagent in organic synthesis.[1] It is used as a source of electrophilic iodine in the synthesis of certain aromatic iodides.[3] It also cleaves C-Si bonds.

ICl will also add to the double bond in alkenes to give chloro-iodo alkanes.

When such reactions are conducted in the presence of sodium azide, the iodo-azide is obtained.[4]

The Wijs solution, iodine monochloride dissolved in acetic acid, is used to determine the iodine value of a substance.

It can also be used to make pure iodates, by reacting with a chlorate and releasing chlorine gas as byproduct.

References

  1. 1 2 Brisbois, R. G.; Wanke, R. A.; Stubbs, K. A.; Stick, R. V. "Iodine Monochloride" Encyclopedia of Reagents for Organic Synthesis, 2004 John Wiley & Sons. doi:10.1002/047084289X.ri014
  2. ↑ Carpenter, G. B.; Richards, S. M. (1 April 1962). "The crystal structure of β-iodine monochloride". Acta Crystallographica. 15 (4): 360–364. doi:10.1107/S0365110X62000882.
  3. ↑ Wallingford, V. H.; Krüger, P. A. (1943). "5-Iodo-anthranilic Acid". Organic Syntheses. ; Collective Volume, 2, p. 349
  4. ↑ Padwa, A.; Blacklock, T.; Tremper, A. "3-Phenyl-2H-Azirine-2-carboxaldehyde". Organic Syntheses. ; Collective Volume, 6, p. 893
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.