Copper(I) iodide
_iodide_sample.jpg)
| |
| Names | |
|---|---|
| IUPAC name
Copper(I) iodide
| |
| Other names
Cuprous iodide, marshite
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.028.795 |
PubChem CID
|
|
| UNII | |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| CuI | |
| Molar mass | 190.450 g·mol−1 |
| Appearance | White solid |
| Odor | odorless |
| Density | 5.67 g/cm3 [1] |
| Melting point | 606 °C (1,123 °F; 879 K) |
| Boiling point | 1,290 °C (2,350 °F; 1,560 K) (decomposes) |
| 0.000042 g/100 mL | |
Solubility product (Ksp)
|
1.27 x 10−12 [2] |
| Solubility | soluble in ammonia and iodide solutions insoluble in dilute acids |
| Vapor pressure | 10 mm Hg (656 °C) |
| −63.0·10−6 cm3/mol | |
Refractive index (nD)
|
2.346 |
| Structure | |
| zincblende | |
| Tetrahedral anions and cations | |
| Hazards | |
| GHS labelling: | |
  
| |
| Danger | |
| H302, H315, H319, H335, H410 | |
| P261, P273, P305+P351+P338, P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
|
TWA 1 mg/m3 (as Cu)[3] |
REL (Recommended)
|
TWA 1 mg/m3 (as Cu)[3] |
IDLH (Immediate danger)
|
TWA 100 mg/m3 (as Cu)[3] |
| Safety data sheet (SDS) | Sigma Aldrich |
| Related compounds | |
Other anions
|
|
Other cations
|
|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Copper(I) iodide is an inorganic compound with the chemical 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 often appear tan or even, when found in nature as rare mineral marshite, reddish brown, but such color is due to the presence of impurities. It is common for samples of iodide-containing compounds to become discolored due to the facile aerobic oxidation of the iodide anion to molecular iodine.[4][5][6]
Structure
[edit]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 (γ-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.[7] Consistent with its covalency, CuI is a p-type semiconductor.[8]
-iodide-unit-cell-3D-balls.png) |
-iodide-(beta)-unit-cell-3D-balls.png) |
-iodide-(alpha)-unit-cell-3D-balls.png)
|
| γ-CuI | β-CuI | α-CuI |
Preparation
[edit]Copper(I) iodide can be prepared by heating iodine and copper in concentrated hydroiodic acid.[9]
In the laboratory however, copper(I) iodide is prepared by simply mixing an aqueous solution of potassium iodide and a soluble copper(II) salt such as copper(II) sulfate.[4]
- 2 Cu2+ + 4 I− → 2 CuI + I2
Reactions
[edit]Copper(I) iodide reacts with mercury vapors to form brown copper(I) tetraiodomercurate(II):
- 4 CuI + Hg → (Cu+)2[HgI4]2− + 2 Cu
This reaction can be used for the detection of mercury since the white CuI to brown Cu2[HgI4] color change is dramatic.
Copper(I) iodide is used in the synthesis of Cu(I) clusters such as [Cu6I7]−.[10]
Copper(I) iodide dissolves in acetonitrile, yielding diverse complexes. Upon crystallization, molecular[11] or polymeric[12][13] compounds can be isolated. Dissolution is also observed when a solution of the appropriate complexing agent in acetone or chloroform is used. For example, thiourea and its derivatives can be used. Solids that crystallize out of those solutions are composed of hybrid inorganic chains.[14]
Uses
[edit]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 (see aromatic Finkelstein reaction).[15]
CuI is used as a co-catalyst with palladium catalyst in the Sonogashira coupling.[16]
CuI is used in cloud seeding,[17] 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.[citation needed]
CuI is used as a source of dietary iodine in table salt and animal feed.[17]
References
[edit]- ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, Florida: CRC Press. ISBN 0-8493-0487-3.
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99th ed.). CRC Press. pp. 4–47. ISBN 978-1138561632.
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH).
- ^ a b George B. Kauffman, Lawrence W. Fang (1983). Copper(I) Iodide. Inorganic Syntheses. Vol. 22. p. 101. doi:10.1002/9780470132531.ch20.
- ^ "Verification".
- ^ "List of Minerals". 21 March 2011.
- ^ Wells AF (1984). Structural Inorganic Chemistry (5th ed.). Oxford: Oxford University Press. pp. 410 and 444.
- ^ Bidikoudi, Maria; Kymakis, Emmanuel (2019). "Novel approaches and scalability prospects of copper based hole transporting materials for planar perovskite solar cells". Journal of Materials Chemistry C. 7 (44): 13680–13708. doi:10.1039/c9tc04009a.
- ^ Holleman AF, Wiberg E (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
- ^ Yu M, Chen L, Jiang F, Zhou K, Liu C, Sun C, Li X, Yang Y, Hong M (2017). "Cation-Induced Strategy toward an Hourglass-Shaped Cu6I7– Cluster and its Color-Tunable Luminescence". Chemistry of Materials. 29 (19): 8093–8099. doi:10.1021/acs.chemmater.7b01790.
- ^ Barth ER, Golz C, Knorr M, Strohmann C (November 2015). "Crystal structure of di-μ-iodido-bis-[bis(aceto-nitrile-κN)copper(I)]". Acta Crystallographica Section E. 71 (Pt 11): m189-90. doi:10.1107/S2056989015018149. PMC 4645014. PMID 26594527.
- ^ Healy PC, Kildea JD, Skelton BW, White AH (1989). "Lewis-Base Adducts of Group 11 Metal(I) Compounds. XL. Conformational Systematics of [(N-base)1(CuX)1]∞ Orthogonal' Stair' Polymers (N-base = 'One-Dimensional Aceto-nitrile, Benzo-nitrile Ligand)". Australian Journal of Chemistry. 42 (1): 79. doi:10.1071/CH9890079. ISSN 0004-9425.
- ^ Arkhireeva TM, Bulychev BM, Sizov AI, Sokolova TA, Belsky VK, Soloveichik GL (1990). "Copper(I) complexes with metal-metal (d10–d10) bond. Crystal and molecular structures of adducts of tantalocene trihydride with copper(I) iodide of composition: (η5-C5H5)2TaH[(μ2-H)Cu(μ2-I)2Cu(μ2-H)]2HTa(η5-C5H5)2, (η5-C5H4But)2TaH(μ2-H)2Cu(μ2-I)2Cu(μ2-H)2HTa(η5-C5H4But)2·CH3CN and {Cu(μ3-I)·P[N(CH3)2]3}4". Inorganica Chimica Acta. 169 (1): 109–118. doi:10.1016/S0020-1693(00)82043-5.
- ^ Rosiak D, Okuniewski A, Chojnacki J (December 2018). "Copper(I) iodide ribbons coordinated with thiourea derivatives". Acta Crystallographica Section C. 74 (Pt 12): 1650–1655. doi:10.1107/S2053229618015620. PMID 30516149. S2CID 54615309.
- ^ Klapars A, Buchwald SL (December 2002). "Copper-catalyzed halogen exchange in aryl halides: an aromatic Finkelstein reaction". Journal of the American Chemical Society. 124 (50): 14844–5. doi:10.1021/ja028865v. PMID 12475315. S2CID 11338218.
- ^ Sonogashira, K. (2002), "Development of Pd-Cu catalyzed cross-coupling of terminal acetylenes with sp2-carbon halides", J. Organomet. Chem., 653 (1–2): 46–49, doi:10.1016/s0022-328x(02)01158-0
- ^ a b Zhang J, Richardson HW (June 2000). "Copper compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 1–31. doi:10.1002/14356007.a07_567. ISBN 3527306730.
Further reading
[edit]- Macintyre J (1992). Dictionary of Inorganic Compounds. Vol. 3. London: Chapman and Hall. p. 3103.
External links
[edit]