Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Copper(I) iodide: Difference between pages

| Watchedfields = changed

| verifiedrevid = 477313922

| Name = Copper(I) iodide

| ImageFile = Copper(I) iodide sample.jpg

| ImageName = Copper(I) iodide

| IUPACName = Copper(I) iodide

| OtherNames = Cuprous iodide, [[marshite]]

|Section1={{Chembox Identifiers

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| CASNo_Ref = {{cascite|correct|CAS}}

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 7DE9CA6IL2

}}

|Section2={{Chembox Properties

| Formula = CuI

| Cu=1|I=1

| Appearance = White solid

| Odor = odorless

| Density = 5.67 g/cm³ <ref>{{RubberBible87th}}</ref>

| Solubility = 0.000042 g/100 mL

| SolubilityProduct = 1.27 x 10⁻¹² <ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=4–47|edition=99th |language=English}}</ref>

| SolubleOther = soluble in [[ammonia]] and [[iodide]] solutions <br> insoluble in dilute acids

| MeltingPtC = 606

| BoilingPtC = 1290

| BoilingPt_notes = (decomposes)

| RefractIndex = 2.346

| VaporPressure = 10 mm Hg (656 °C)

| MagSus = −63.0·10⁻⁶ cm³/mol

}}

|Section3={{Chembox Structure

| Coordination = Tetrahedral anions and cations

| CrystalStruct = [[Zincblende (crystal structure)|zincblende]]

}}

|Section7={{Chembox Hazards

| ExternalSDS = [https://www.sigmaaldrich.com/US/en/sds/aldrich/215554 Sigma Aldrich]

| GHSPictograms = {{GHS05}}{{GHS07}}{{GHS09}}

| GHSSignalWord = DANGER

| HPhrases = {{H-phrases|302|315|319|335|410}}

| PPhrases = {{P-phrases|261|273|305+351+338|501}}

| NFPA-H = 1

| NFPA-R = 0

| NFPA-F = 1

| NFPA-S =

| FlashPt = Non-flammable

| PEL = TWA 1 mg/m³ (as Cu)<ref name=PGCH>{{PGCH|0150}}</ref>

| REL = TWA 1 mg/m³ (as Cu)<ref name=PGCH/>

| IDLH = TWA 100 mg/m³ (as Cu)<ref name=PGCH/>

}}

|Section8={{Chembox Related

| OtherAnions = {{Ubl|[[Copper(I) fluoride]]|[[Copper(I) chloride]]|[[Copper(I) bromide]]}}

| OtherCations = {{ubl|[[Silver iodide]]|[[Gold monoiodide]]|[[Sodium iodide]]}}

}}

'''Copper(I) iodide''' is an [[inorganic compound]] with the [[chemical formula]] {{chem2|CuI|auto=1}}. 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.<ref name="Kauffman">{{cite book |doi=10.1002/9780470132531.ch20|year=1983|author=George B. Kauffman, Lawrence W. Fang|series=Inorganic Syntheses|volume=22|page=101|title=Copper(I) Iodide}}</ref><ref>{{Cite web|url=https://www.mindat.org/min-2580.html|title=Verification}}</ref><ref>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref>

== 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 [[zincblende (crystal structure)|zinc blende structure]] below 390&nbsp;°C (γ-CuI), a [[wurtzite]] structure between 390 and 440&nbsp;°C (β-CuI), and a [[Cubic (crystal system)|rock salt]] structure above 440&nbsp;°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&nbsp;°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.<ref>{{cite book | vauthors = Wells AF | title = Structural Inorganic Chemistry | publisher = Oxford University Press | location = Oxford | date = 1984 | edition = 5th | pages = 410 and 444}}</ref> Consistent with its covalency, CuI is a p-type semiconductor.<ref>{{cite journal |title=Novel approaches and scalability prospects of copper based hole transporting materials for planar perovskite solar cells |journal=Journal of Materials Chemistry C |year=2019 |doi=10.1039/c9tc04009a|doi-access=free |last1=Bidikoudi |first1=Maria |last2=Kymakis |first2=Emmanuel |volume=7 |issue=44 |pages=13680–13708}}</ref>

{| class="wikitable" style="margin:1em auto; text-align:center;"

|[[File:Copper(I)-iodide-unit-cell-3D-balls.png|150px]]||[[File:Copper(I)-iodide-(beta)-unit-cell-3D-balls.png|150px]]||[[File:Copper(I)-iodide-(alpha)-unit-cell-3D-balls.png|150px]]

|-

|γ-CuI||β-CuI||α-CuI

|}

==Preparation==

Copper(I) iodide can be prepared by heating iodine and copper in concentrated [[hydroiodic acid]].<ref>{{cite book | vauthors = Holleman AF, Wiberg E | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | date = 2001 | isbn = 0-12-352651-5}}</ref>

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]].<ref name="Kauffman"/>

:{{chem2|2 Cu(2+) + 4 I− → 2 CuI + I2}}

==Reactions==

Copper(I) iodide reacts with [[mercury (element)|mercury]] vapors to form brown copper(I) tetraiodomercurate(II):

:{{chem2|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 {{chem2|Cu2[HgI4]}} color change is dramatic.

Copper(I) iodide is used in the synthesis of Cu(I) clusters such as {{chem2|[Cu6I7]-}}.<ref>{{Cite journal |doi = 10.1021/acs.chemmater.7b01790|title = Cation-Induced Strategy toward an Hourglass-Shaped Cu6I7– Cluster and its Color-Tunable Luminescence|journal = Chemistry of Materials|volume = 29|issue = 19|pages = 8093–8099|year = 2017|last1 = Yu|first1 = Muxin|last2 = Chen|first2 = Lian|last3 = Jiang|first3 = Feilong|last4 = Zhou|first4 = Kang|last5 = Liu|first5 = Caiping|last6 = Sun|first6 = Cai|last7 = Li|first7 = Xingjun|last8 = Yang|first8 = Yan|last9 = Hong|first9 = Maochun | name-list-style = vanc}}</ref>

Copper(I) iodide dissolves in [[acetonitrile]], yielding diverse complexes. Upon crystallization, molecular<ref>{{cite journal | vauthors = Barth ER, Golz C, Knorr M, Strohmann C | title = Crystal structure of di-μ-iodido-bis-[bis(aceto-nitrile-κN)copper(I)] | journal = Acta Crystallographica Section E | volume = 71 | issue = Pt 11 | pages = m189-90 | date = November 2015 | pmid = 26594527 | pmc = 4645014 | doi = 10.1107/S2056989015018149}}</ref> or polymeric<ref>{{Cite journal| vauthors = Healy PC, Kildea JD, Skelton BW, White AH |date=1989|title=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)|journal=Australian Journal of Chemistry|language=en|volume=42|issue=1|pages=79|doi=10.1071/CH9890079|issn=0004-9425}}</ref><ref>{{Cite journal| vauthors = Arkhireeva TM, Bulychev BM, Sizov AI, Sokolova TA, Belsky VK, Soloveichik GL |date=1990|title=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|journal=Inorganica Chimica Acta|language=en|volume=169|issue=1|pages=109–118|doi=10.1016/S0020-1693(00)82043-5}}</ref> 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 [[Metal–organic framework|hybrid inorganic chains]].<ref>{{cite journal | vauthors = Rosiak D, Okuniewski A, Chojnacki J | title = Copper(I) iodide ribbons coordinated with thiourea derivatives | journal = Acta Crystallographica Section C | volume = 74 | issue = Pt 12 | pages = 1650–1655 | date = December 2018 | pmid = 30516149 | doi = 10.1107/S2053229618015620 | s2cid = 54615309}}</ref>

==Uses==

In combination with 1,2- or 1,3-diamine ligands, CuI catalyzes the conversion of [[Aryl bromide|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]]).<ref>{{cite journal | vauthors = Klapars A, Buchwald SL | title = Copper-catalyzed halogen exchange in aryl halides: an aromatic Finkelstein reaction | journal = Journal of the American Chemical Society | volume = 124 | issue = 50 | pages = 14844–5 | date = December 2002 | pmid = 12475315 | doi = 10.1021/ja028865v | s2cid = 11338218}}</ref>

CuI is used as a co-catalyst with [[palladium]] catalyst in the [[Sonogashira coupling]].<ref name="Development">{{citation |author=Sonogashira, K. |journal=[[J. Organomet. Chem.]] |title= Development of Pd-Cu catalyzed cross-coupling of terminal acetylenes with sp²-carbon halides |year=2002 |volume=653 |issue=1–2 |pages=46–49 |doi= 10.1016/s0022-328x(02)01158-0}}</ref>

CuI is used in [[cloud seeding]],<ref name=Ullmann/> 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|date=January 2022}}

CuI is used as a source of dietary iodine in table salt and animal feed.<ref name=Ullmann>{{cite book | vauthors = Zhang J, Richardson HW | chapter = Copper compounds | title = Ullmann's Encyclopedia of Industrial Chemistry | date = June 2000 | pages = 1–31 | doi = 10.1002/14356007.a07_567

| publisher = Wiley-VCH | location = Weinheim | isbn = 3527306730}}</ref>

== References ==

{{reflist}}

== Further reading==

{{refbegin}}

*{{cite book | vauthors = Macintyre J | title = Dictionary of Inorganic Compounds | publisher = Chapman and Hall | location = London | date = 1992 | volume = 3 | pages = 3103}}

{{refend}}

== External links ==

{{commons category}}

*[https://archive.today/20130119043649/https://www.chemicalland21.com/arokorhi/industrialchem/inorganic/CUPROUS%20IODIDE.htm Chemicalland properties database]

*[https://web.archive.org/web/20080302034606/https://www.npi.gov.au/database/substance-info/profiles/27.html National Pollutant Inventory – Copper and compounds fact sheet]

{{Copper compounds}}

{{Iodides}}

[[Category:Copper(I) compounds]]

[[Category:Iodides]]

[[Category:Metal halides]]

[[Category:Zincblende crystal structure]]

[[Category:Wurtzite structure type]]

[[Category:Semiconductor materials]]