Iridium(IV) oxide: Difference between revisions

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| OtherNames = Iridium dioxide

|Section1={{Chembox Identifiers

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

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

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

| UNII = CL6CQW9MWS

| PubChem = 82821

|Section2={{Chembox Properties

| Formula = IrO₂

| MolarMass = 224.22 g/mol

| Appearance = blue-black solid

| Density = 11.66 g/cm³

| MeltingPtC = 1100

| MeltingPt_notes = decomposes

| Solubility = insoluble

| MagSus = +224.0·10⁻⁶ cm³/mol

|Section3={{Chembox Structure

| Coordination = Octahedral (Ir); Trigonal (O)

| CrystalStruct = [[Rutile]] (tetragonal)

|Section7={{Chembox Hazards

| ExternalSDS =

| MainHazards =

| NFPA-H =

| NFPA-F =

| NFPA-R =

| NFPA-S =

| FlashPt = Non-flammable

|Section8={{Chembox Related

| OtherAnions = [[iridium(IV) fluoride]], [[iridium disulfide]]

| OtherCations = [[rhodium dioxide]], [[osmium dioxide]], [[platinum dioxide]]

| OtherCompounds =

'''Iridium(IV) oxide''', IrO₂, is the only well-characterised oxide of iridium. It is a blue-black solid. The compound adopts the TiO₂ [[rutile structure]], featuring six coordinate iridium and three coordinate oxygen.<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref>

It is used with other rare oxides in the coating of anode-electrodes for industrial electrolysis and in [[microelectrode]]s for [[electrophysiology]] research.<ref>{{cite journal

| last =Cogan |first=Stuart F.

| title =Neural Stimulation and Recording Electrodes|journal=Annual Review of Biomedical Engineering

| date =August 2008

| volume =10 |issue=1

| pages =275–309

| doi =10.1146/annurev.bioeng.10.061807.160518

| pmid=18429704

}}</ref>

As described by its discoverers, it can be formed by treating the green form of [[iridium trichloride]] with oxygen at high temperatures:

:2 IrCl₃ + 2 O₂ → 2 IrO₂ + 3 Cl₂

A hydrated form is also known.<ref>{{cite book|editor=G. Brauer|author=H. L. Grube|chapter=The Platinum Metals|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed.|publisher=Academic Press|year=1963|place=NY|page=1590}}</ref>

==Application==

Iridium dioxide can be used as an anode electrode for industrial electrolysis and as a microelectrode for electrophysiological studies.<ref>{{Cite journal|last=Cogan|first=Stuart F.|date=August 2008|title=Neural Stimulation and Recording Electrodes|url=http://www.annualreviews.org/doi/10.1146/annurev.bioeng.10.061807.160518|journal=Annual Review of Biomedical Engineering|language=en|volume=10|issue=1|pages=275–309|doi=10.1146/annurev.bioeng.10.061807.160518|pmid=18429704 |issn=1523-9829}}</ref>

Iridium dioxide can be used to make coated electrodes.<ref>{{Cite web|title=改性二氧化铱电极研制--《无机盐工业》1998年03期|url=https://www.cnki.com.cn/Article/CJFDTotal-WJYG803.005.htm|access-date=2021-05-21|website=www.cnki.com.cn}}</ref>

{{oxygen compounds}}

{{Authority control}}

[[Category:Transition metal oxides]]