Copper(I) iodide

Copper(I) iodide
IUPAC name	Copper(I) iodide
Other names	Cuprous iodide
Identifiers
CAS number	7681-65-4 Y
PubChem	6432705
Properties
Molecular formula	CuI
Molar mass	190.45 g/mol
Appearance	White powder when impure: tan or brownish
Density	5.67 g/cm3 [2]
Melting point	606 °C
Boiling point	1290 °C (decomposes)
Solubility in water	insoluble
Solubility product, Ksp	1 x 10-12 [1]
Solubility	soluble in 3.5 M KI soln.
Refractive index (nD)	2.346
Structure
Crystal structure	zincblende
Coordination geometry	Tetrahedral anions and cations
Hazards
EU Index	Not listed
NFPA 704	1 1 0
Flash point	Non-flammable
Related compounds
Other anions	Copper(I) fluoride Copper(I) chloride Copper(I) bromide
Other cations	silver(I) iodide
Y (what is this?)  (verify) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Copper(I) iodide is the chemical compound with the formula CuI; it is also known as cuprous iodide. It is useful in a variety of applications ranging from organic synthesis to cloud seeding.

Copper(I) iodide is white, but samples are often tan or even, when found in nature as rare mineral marshite, reddish brown, but such color is due to impurities.^[3] It is common for iodides to become discolored because of the easy oxidation of the iodide anion to iodine.

Structure

Copper(I) iodide, like most "binary" (containing only two elements) metal halides, is an inorganic polymer. It has a rich phase diagram, meaning that it exists in several crystalline forms. It adopts a zinc blende structure below 390 °C (ɣ-CuI), a wurtzite structure between 390 and 440 °C (β-CuI), and a rock salt structure above 440 °C (α-CuI). The ions are tetrahedrally coordinated when in the zinc blende or the wurtzite structure, with a Cu-I distance of 2.338 Å. Copper(I) bromide and copper(I) chloride also transform from the zinc blende structure to the wurtzite structure at 405 and 435 °C, respectively. Therefore, the longer the copper - halide bond length, the lower the temperature needs to be to change the structure from the zinc blende structure to the wurtzite structure. The interatomic distances in copper(I) bromide and copper(I) chloride are 2.173 and 2.051 Å, respectively.^[4]

ɣ-CuI	β-CuI	α-CuI

Preparation

In the laboratory, copper(I) iodide is prepared by simply mixing an aqueous solutions of sodium or potassium iodide and a soluble copper(II) salt such copper sulfate.

2Cu²⁺ + 4I⁻ → 2CuI₂

The CuI₂ immediately decomposes to iodine and insoluble copper(I) iodide, releasing I₂.^[5]

2 CuI₂ → 2 CuI + I₂

This reaction has been employed as a means of assaying copper(II) samples, since the evolved I₂ can be analyzed by redox titration. Copper(I) iodide can also be prepared by heating iodine and copper in concentrated hydriodic acid, HI.

CuI is poorly soluble in water (0.00042 g/L at 25 °C), but it dissolves in the presence of NaI or KI to give the linear anion [CuI₂]⁻. Dilution of such solutions with water reprecipitates CuI. This dissolution-precipitation process is employed to purify CuI, affording colorless samples.^[6]

Uses

CuI has several uses:

• CuI is used as a reagent in organic synthesis. In combination with 1,2- or 1,3 diamine ligands, CuI catalyzes the conversion of aryl, heteroaryl, and vinyl bromides into the corresponding iodides. NaI is the typical iodide source and dioxane is a typical solvent. Aryl halides are used to form carbon-carbon and carbon-heteroatom bonds in process such as the Heck, Stille, Suzuki, and Ullman type coupling reactions. Aryl iodides, however, are more reactive than the corresponding aryl bromides or aryl chlorides.^[7] 2-Bromo-1-octen-3-ol and 1-nonyne are coupled when combined with dichlorobis(triphenylphosphine)palladium(II), CuI, and diethylamine to form 7-methylene-8-hexadecyn-6-ol.^[8]
• CuI is used in cloud seeding,^[3] altering the amount or type of precipitation of a cloud, or their structure by dispersing substances into the atmosphere which increase water's ability to form droplets or crystals. CuI provides a sphere for moisture in the cloud to condense around, causing precipitation to increase and cloud density to decrease.
• The structural properties of CuI allow CuI to stabilize heat in nylon in commercial and residential carpet industries, automotive engine accessories, and other markets where durability and weight are a factor.
• CuI is used as a source of dietary iodine in table salt and animal feed.^[3]

References

1. ^ Skoog West Holler Crouch. Fundamentals of Inorganic Chemistry. Brooks/Cole, 2004, pp. A-6 ISBN 978-0-03-035523-3
2. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
3. ^ ^{a b c} Patnaik, Pradyot (2003) (Google Books excerpt). Handbook of inorganic chemicals. New York: McGraw-Hill. pp. 268-269. ISBN 0-07-049439-8. http://books.google.com.sg/books?id=Xqj-TTzkvTEC&pg=PA268. 
4. ^ Wells, A. F. Structural Inorganic Chemistry Oxford University Press, Oxford, (1984). 5th ed., p. 410 and 444.
5. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
6. ^ Kauffman, G. B.; Fang, L. Y. (1983). "Purification of Copper(I) Iodide". Inorg. Synth. 22: 101–103. doi:10.1002/9780470132531.ch20. 
7. ^ Klapars, A.; Buchwald, S. L. (2002). "Copper-Cataylzed Halogen Exchange in Aryl Halides: an Aromatic Finkelstein Reaction". J. Am. Chem. Soc. 124: 14845. doi:10.1021/ja028865v. 
8. ^ Marshall, J. A.; Sehon, C. A., "Isomerization of Β-Alkynyl Allylic Alcohols to Furans Catalyzed by Silver Nitrate on Silica Gel: 2-Pentyl-3-methyl-5-heptylfuran", Org. Synth. 76: 263, http://www.orgsyn.org/orgsyn/orgsyn/prepContent.asp?prep=v76p0263 

Sources

• Macintyre, J. Dictionary of Inorganic Compounds. Chapman and Hall, London, (1992). Vol. 3, p.3103.

External links

Wikimedia Commons has media related to: Copper(I) iodide

• Chemicalland properties database
• National Pollutant Inventory - Copper and compounds fact sheet