Iodine monochloride
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| Names | |||
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| Preferred IUPAC name
Iodine monochloride Iodine(I) chloride | |||
| Systematic IUPAC name
Chloroiodane | |||
| Other names
Iodine chloride
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| Identifiers | |||
3D model (JSmol)
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| ChemSpider | |||
| ECHA InfoCard | 100.029.306 | ||
| EC Number |
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| MeSH | Iodine-monochloride | ||
PubChem CID
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| UN number | 1792 | ||
CompTox Dashboard (EPA)
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| 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 | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
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corrosive | ||
| Safety data sheet (SDS) | External MSDS | ||
| Related compounds | |||
Related interhalogen compounds
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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).
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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
- ^ a b 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
- ^ 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.
- ^ Wallingford, V. H.; Krüger, P. A. (1943). "5-Iodo-anthranilic Acid". Organic Syntheses
{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 2, p. 349. - ^ Padwa, A.; Blacklock, T.; Tremper, A. "3-Phenyl-2H-Azirine-2-carboxaldehyde". Organic Syntheses
{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 6, p. 893.