Iodine monochloride

Iodine monochloride  |

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Names
Preferred IUPAC name

Iodine monochloride
Iodine(I) chloride

Systematic IUPAC name

Chloroiodane

Other names

Iodine chloride

Identifiers

CAS Number

* 7790-99-0 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 23042 Y

EC Number |

* 232-236-7

MeSH | Iodine-monochloride

PubChem CID

* 24640

UNII |

* 0SMG5NLU45 Y

UN number | 1792

InChI

* InChI=1S/ClI/c1-2 Y

Key: QZRGKCOWNLSUDK-UHFFFAOYSA-N Y

* InChI=1S/ClI/c1-2

Key: QZRGKCOWNLSUDK-UHFFFAOYSA-N

* InChI=1/ClI/c1-2

Key: QZRGKCOWNLSUDK-UHFFFAOYAO

SMILES

* ClI

Properties

Chemical formula

| 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)

Solubility in water

| Hydrolyzes
Solubility | soluble in CS2
acetic acid
pyridine
alcohol, ether, HCl

Magnetic susceptibility (χ)

| −54.6×10−6 cm3/mol
Hazards
Main hazards | Corrosive, reacts with water to release HCl
Safety data sheet | https://chemicalsafety.com/sds1/sdsviewer.php?id=30683304
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 YN ?)
Infobox references

Tracking categories (test):

* SizeSet

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, this molecule is highly polar and behaves as a source of I+. Discovered in 1814 by Gay-Lussac, iodine monochloride is the first interhalogen compound discovered.[1]

## Contents

* 1 Preparation
* 2 Polymorphs
* 3 Reactions and uses
* 4 References

## Preparation

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

2 \+ Cl
2 → 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 + Cl
2 ⇌ ICl

## 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.[2]

In the crystal structures of both polymorphs the molecules are arranged in zigzag chains. β-ICl is monoclinic with the space group P21/c.[3]

## Reactions and uses

Iodine monochloride is soluble in acids such as HF and HCl but reacts with pure water to form HCl, iodine, and iodic acid:

ICl + H
2O → HCl + HI \+ ​1⁄2O2
2 ICl + H
2O → 2 HCl + I
2 \+ ​1⁄2O2
5 ICl + 3 H
2O → 5 HCl + HIO
3 \+ 2 I

ICl is a useful reagent in organic synthesis.[2] It is used as a source of electrophilic iodine in the synthesis of certain aromatic iodides.[4] It also cleaves C–Si bonds.

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

RCH=CHR′ + ICl → RCH(I)–CH(Cl)R′

When such reactions are conducted in the presence of sodium azide, the iodo-azide RCH(I)–CH(N3)R′ is obtained.[5]

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 prepare iodates, by reaction with a chlorate. Chlorine is released as a byproduct.

Iodine monochloride is a Lewis acid that forms 1:1 adducts with Lewis bases such as dimethylacetamide and benzene.

## References

1. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 790. ISBN 978-0-08-037941-8.
2. ↑ 2.0 2.1 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
3. ↑ 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.
4. ↑ Wallingford, V. H.; Krüger, P. A. (1943). "5-Iodo-anthranilic Acid". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=cv2p0349. ;  Collective Volume, 2, pp. 349
5. ↑ Padwa, A.; Blacklock, T.; Tremper, A.. "3-Phenyl-2H-Azirine-2-carboxaldehyde". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=cv6p0893. ;  Collective Volume, 6, pp. 893

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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

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Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

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