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<ul id="toc-Properties-sublist" class="vector-toc-list"> <li id="toc-Stability" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Stability"> <div class="vector-toc-text"> 5.1 Stability </div> </a> <ul id="toc-Stability-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Color" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Color"> <div class="vector-toc-text"> 5.2 Color </div> </a> <ul id="toc-Color-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chemical_properties" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chemical_properties"> <div class="vector-toc-text"> 5.3 Chemical properties </div> </a> <ul id="toc-Chemical_properties-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#See_also"> <div class="vector-toc-text"> 6 See 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role="note" class="hatnote navigation-not-searchable">Not to be confused with <a href="/wiki/Polyhalite" title="Polyhalite">Polyhalite</a>.</div> Polyhalogen ions are a group of polyatomic <a href="/wiki/Cation" class="mw-redirect" title="Cation">cations</a> and <a href="/wiki/Anion" class="mw-redirect" title="Anion">anions</a> containing <a href="/wiki/Halogen" title="Halogen">halogens</a> only. The ions can be classified into two classes, isopolyhalogen ions which contain one type of halogen only, and heteropolyhalogen ions with more than one type of halogen. <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Introduction">Introduction</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=1" title="Edit section: Introduction">edit</a>]</div> Numerous polyhalogen ions have been found, with their salts isolated in the solid state and structurally characterized. The following tables summarize the known species.<a href="#cite_note-Encyclo-1">[1]</a><a href="#cite_note-InorgChem-2">[2]</a><a href="#cite_note-Greenwood-3">[3]</a><a href="#cite_note-AdvInorgChem-4">[4]</a><a href="#cite_note-wiberg2001-5">[5]</a><a href="#cite_note-6">[6]</a> <div style="float:left; display:table; margin-left:1em; margin-right:1em"> <table class="wikitable left"> <caption>Isopolyhalogen cations </caption> <tbody><tr> <td>Diatomic species</td> <td><a href="#Symb1">*</a><style data-mw-deduplicate="TemplateStyles:r1123817410">.mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em}</style>[Cl2]+, [Br2]+, [I2]+ </td></tr> <tr> <td>Triatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]+, [Br3]+, [I3]+ </td></tr> <tr> <td>Tetraatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl4]+, [I4]2+ </td></tr> <tr> <td>Pentaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br5]+, [I5]+ </td></tr> <tr> <td>Heptaatomic species</td> <td><a href="#Symb2">†</a><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I7]+ </td></tr> <tr> <td>Higher species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I15]3+ </td></tr></tbody></table> <div style="display:table-caption; caption-side:bottom;"> <style data-mw-deduplicate="TemplateStyles:r1238216509">.mw-parser-output .vanchor>:target~.vanchor-text{background-color:#b1d2ff}@media screen{html.skin-theme-clientpref-night .mw-parser-output .vanchor>:target~.vanchor-text{background-color:#0f4dc9}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .vanchor>:target~.vanchor-text{background-color:#0f4dc9}}</style>* <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2]+ can only exist as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2O2]2+ at low temperatures, a <a href="/wiki/Charge-transfer_complex" title="Charge-transfer complex">charge-transfer complex</a> from <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">O2 to <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2]+.<a href="#cite_note-InorgChem-2">[2]</a> Free <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2]+ is only known from its electronic band spectrum obtained in a low-pressure discharge tube.<a href="#cite_note-Greenwood-3">[3]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238216509">† The existence of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I7]+ is possible but still uncertain.<a href="#cite_note-Encyclo-1">[1]</a> </div> </div> <table class="wikitable" style="float:left; margin-left:1em; margin-right:1em"> <caption>Heteropolyhalogen cations </caption> <tbody><tr> <td>Triatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF2]+, [Cl2F]+, [BrF2]+, [IF2]+, [ICl2]+, [IBrCl]+, [IBr2]+, [I2Cl]+, [I2Br]+ </td></tr> <tr> <td>Pentaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF4]+, [BrF4]+, [IF4]+, [I3Cl2]+ </td></tr> <tr> <td>Heptaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]+, [BrF6]+, [IF6]+ </td></tr></tbody></table> <table class="wikitable" style="float:left; margin-left:1em; margin-right:1em"> <caption>Isopolyhalogen anions </caption> <tbody><tr> <td>Triatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]−, [Br3]−, [I3]− </td></tr> <tr> <td>Tetraatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br4]2−, [I4]2− </td></tr> <tr> <td>Pentaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]− </td></tr> <tr> <td>Heptaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I7]− </td></tr> <tr> <td>Octaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br8]2−, [I8]2− </td></tr> <tr> <td>Higher species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I9]−, [I10]2−, [I10]4−, [I11]−, [I12]2−, [I13]3−, [I16]2−, [I22]4−, [I26]3−, [I26]4−, [I28]4−, [I29]3− </td></tr></tbody></table> <table class="wikitable" style="float:left; margin-left:1em; margin-right:1em"> <caption>Heteropolyhalogen anions </caption> <tbody><tr> <td>Triatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF2]−, [BrF2]−, [BrCl2]−, [IF2]−, [ICl2]−, [IBrF]−, [IBrCl]−, [IBr2]−, [I2Cl]−, [I2Br]−, [AtBrCl]−, [AtBr2]−, [AtICl]−, [AtIBr]−, [AtI2]− </td></tr> <tr> <td>Pentaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF4]−, [BrF4]−, [IF4]−, [ICl3F]−, [ICl4]−, [IBrCl3]−, [I2Cl3]−, [I2BrCl2]−, [I2Br2Cl]−, [I2Br3]−, [I4Cl]−, [I4Br]− </td></tr> <tr> <td>Hexaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF5]2− </td></tr> <tr> <td>Heptaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]−, [BrF6]−, [IF6]−, [I3Br4]− </td></tr> <tr> <td>Nonaatomic species</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF8]− </td></tr></tbody></table> <div style="clear:both;" class=""></div> <div class="mw-heading mw-heading2"><h2 id="Structure">Structure</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=2" title="Edit section: Structure">edit</a>]</div> <figure class="mw-halign-center" typeof="mw:File/Thumb"><a href="/wiki/File:Structures_of_some_isopolyhalogen_cations.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/96/Structures_of_some_isopolyhalogen_cations.png/650px-Structures_of_some_isopolyhalogen_cations.png" decoding="async" width="650" height="316" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/96/Structures_of_some_isopolyhalogen_cations.png/975px-Structures_of_some_isopolyhalogen_cations.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/96/Structures_of_some_isopolyhalogen_cations.png/1300px-Structures_of_some_isopolyhalogen_cations.png 2x" data-file-width="4380" data-file-height="2131" /></a><figcaption>Structures of some isopolyhalogen cations</figcaption></figure> <figure class="mw-halign-center" typeof="mw:File/Thumb"><a href="/wiki/File:Solid_state_structures_of_the_polyhalogen_ions_(BrF2)%2B._(ClF2)%2B,_(ICl2)%2B.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d7/Solid_state_structures_of_the_polyhalogen_ions_%28BrF2%29%2B._%28ClF2%29%2B%2C_%28ICl2%29%2B.png/950px-Solid_state_structures_of_the_polyhalogen_ions_%28BrF2%29%2B._%28ClF2%29%2B%2C_%28ICl2%29%2B.png" decoding="async" width="950" height="137" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d7/Solid_state_structures_of_the_polyhalogen_ions_%28BrF2%29%2B._%28ClF2%29%2B%2C_%28ICl2%29%2B.png/1425px-Solid_state_structures_of_the_polyhalogen_ions_%28BrF2%29%2B._%28ClF2%29%2B%2C_%28ICl2%29%2B.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d7/Solid_state_structures_of_the_polyhalogen_ions_%28BrF2%29%2B._%28ClF2%29%2B%2C_%28ICl2%29%2B.png/1900px-Solid_state_structures_of_the_polyhalogen_ions_%28BrF2%29%2B._%28ClF2%29%2B%2C_%28ICl2%29%2B.png 2x" data-file-width="6660" data-file-height="960" /></a><figcaption>Solid state structures of the polyhalogen ions <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF2]+, [ClF2]+, [ICl2]+ in their <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[SbF6]− salts.</figcaption></figure> <figure class="mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Solid_state_structure_of_the_(I3Cl2)%2B_ion.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/Solid_state_structure_of_the_%28I3Cl2%29%2B_ion.png/300px-Solid_state_structure_of_the_%28I3Cl2%29%2B_ion.png" decoding="async" width="300" height="167" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/Solid_state_structure_of_the_%28I3Cl2%29%2B_ion.png/450px-Solid_state_structure_of_the_%28I3Cl2%29%2B_ion.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/57/Solid_state_structure_of_the_%28I3Cl2%29%2B_ion.png/600px-Solid_state_structure_of_the_%28I3Cl2%29%2B_ion.png 2x" data-file-width="1970" data-file-height="1094" /></a><figcaption>Solid state structure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3Cl2]+ in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3Cl2]+[SbCl6]−.</figcaption></figure> <figure class="mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Structure_of_the_(I2F12)-_dimer.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/2b/Structure_of_the_%28I2F12%29-_dimer.png/200px-Structure_of_the_%28I2F12%29-_dimer.png" decoding="async" width="200" height="140" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/2b/Structure_of_the_%28I2F12%29-_dimer.png/300px-Structure_of_the_%28I2F12%29-_dimer.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/2b/Structure_of_the_%28I2F12%29-_dimer.png/400px-Structure_of_the_%28I2F12%29-_dimer.png 2x" data-file-width="1358" data-file-height="950" /></a><figcaption>Structure of the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2F12]2− dimer present in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Me4N]+[IF6]−.</figcaption></figure> Most of the structures of the ions have been determined by <a href="/wiki/IR_spectroscopy" class="mw-redirect" title="IR spectroscopy">IR spectroscopy</a>, <a href="/wiki/Raman_spectroscopy" title="Raman spectroscopy">Raman spectroscopy</a> and <a href="/wiki/X-ray_crystallography" title="X-ray crystallography">X-ray crystallography</a>. The polyhalogen ions always have the heaviest and least electronegative halogen present in the ion as the central atom, making the ion asymmetric in some cases. For example, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2F]+ has a structure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl−Cl−F]− but not <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl−F−Cl]−. In general, the structures of most heteropolyhalogen ions and lower isopolyhalogen ions were in agreement with the <a href="/wiki/VSEPR_model" class="mw-redirect" title="VSEPR model">VSEPR model</a>. However, there were exceptional cases. For example, when the central atom is heavy and has seven <a href="/wiki/Lone_pairs" class="mw-redirect" title="Lone pairs">lone pairs</a>, such as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF6]− and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF6]−, they have a regular octahedral arrangement of fluoride ligands instead of a distorted one due to the presence of a <a href="/wiki/Inert-pair_effect#Steric_activity_of_the_lone_pair" title="Inert-pair effect">stereochemically inert lone pair</a>. More deviations from the ideal VSEPR model were found in the solid state structures due to strong cation-anion interactions, which also complicates interpretation of <a href="/wiki/Vibrational_spectroscopy" class="mw-redirect" title="Vibrational spectroscopy">vibrational spectroscopic</a> data. In all known structures of the polyhalogen anion salts, the anions make very close contact, via halogen bridges, with the counter-cations.<a href="#cite_note-AdvInorgChem-4">[4]</a> For example, in the solid state, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF6]− is not regularly octahedral, as solid state structure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[(CH3)4N]+[IF6]− reveals loosely bound <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2F11]2− dimers. Significant cation-anion interactions were also found in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF2]+[SbF6]−, [ClF2]+[SbF6]−, [BrF4]+[Sb6F11]−.<a href="#cite_note-InorgChem-2">[2]</a> <div style="display:table; margin-left: auto; margin-right: auto; border: none;"> <table class="wikitable"> <caption>General structures of selected heteropolyhalogen ions </caption> <tbody><tr> <td>Linear (or almost linear)</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF2]−, [BrF2]−, [BrCl2]−, [IF2]−, [ICl2]−, [IBr2]−, [I2Cl]−, [I2Br]− </td></tr> <tr> <td>Bent</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF2]+, [Cl2F]+, [BrF2]+, [IF2]+, [ICl2]+, [I2Cl]+, [IBr2]+, [I2Br]+, [IBrCl]+ </td></tr> <tr> <td>Square planar</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF4]−, [BrF4]−, [IF4]−, [ICl4]− </td></tr> <tr> <td>Disphenoidal (or seesaw)</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF4]+, [BrF4]+, [IF4]+ </td></tr> <tr> <td>Pentagonal planar</td> <td><a href="#Symb3">‡</a><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF5]2− </td></tr> <tr> <td>Octahedral</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]+, [BrF6]+, [IF6]+, <a href="#Symb4">¶</a><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]−, [BrF6]−, [IF6]− </td></tr> <tr> <td>Square antiprismatic</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF8]− </td></tr></tbody></table> <div style="display:table-caption; caption-side:bottom;"> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238216509">‡ <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF5]2− is one of the two <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">XYn-type species known to have the rare pentagonal planar geometry, the other being <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[XeF5]−. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238216509">¶ <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]− is distorted octahedral as the stereochemical inert-pair effect is not significant in the chlorine atom. </div> </div> The <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3Cl2]+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3Br2]+ ions have a trans-Z-type structure, analogous to that of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]+. <figure class="mw-halign-center" typeof="mw:File/Thumb"><a href="/wiki/File:Solid_state_structure_of_the_(BrF4)%2B_ion.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f7/Solid_state_structure_of_the_%28BrF4%29%2B_ion.png/500px-Solid_state_structure_of_the_%28BrF4%29%2B_ion.png" decoding="async" width="500" height="173" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f7/Solid_state_structure_of_the_%28BrF4%29%2B_ion.png/750px-Solid_state_structure_of_the_%28BrF4%29%2B_ion.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f7/Solid_state_structure_of_the_%28BrF4%29%2B_ion.png/1000px-Solid_state_structure_of_the_%28BrF4%29%2B_ion.png 2x" data-file-width="3043" data-file-height="1051" /></a><figcaption>Solid state structure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF4]+ in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF4]+[Sb2F11]−.</figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Higher_polyiodides">Higher polyiodides</h3>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=3" title="Edit section: Higher polyiodides">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Polyiodide" title="Polyiodide">Polyiodide</a></div> The <a href="/wiki/Polyiodide" title="Polyiodide">polyiodide</a> ions have much more complicated structures. Discrete polyiodides usually have a linear sequence of iodine atoms and iodide ions, and are described in terms of association between <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">I2, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">I− and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3]− units, which reflects the origin of the polyiodide. In the solid states, the polyiodides can interact with each other to form chains, rings, or even complicated two-dimensional and three-dimensional networks. <div class="mw-heading mw-heading2"><h2 id="Bonding">Bonding</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=4" title="Edit section: Bonding">edit</a>]</div> The bonding in polyhalogen ions mostly invoke the predominant use of p-orbitals. Significant d-orbital participation in the bonding is improbable as much promotional energy will be required, while scant s-orbital participation is expected in iodine-containing species due to the <a href="/wiki/Inert-pair_effect" title="Inert-pair effect">inert-pair effect</a>, suggested by data from <a href="/wiki/M%C3%B6ssbauer_spectroscopy" title="Mössbauer spectroscopy">Mössbauer spectroscopy</a>. However, no bonding model has been capable of reproducing such wide range of bond lengths and angles observed so far.<a href="#cite_note-Greenwood-3">[3]</a> As expected from the fact that an electron is removed from the <a href="/wiki/Antibonding_orbital" class="mw-redirect" title="Antibonding orbital">antibonding orbital</a> when <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">X2 is ionized to <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[X2]+, the <a href="/wiki/Bond_order" title="Bond order">bond order</a> as well as the <a href="/wiki/Bond_strength" class="mw-redirect" title="Bond strength">bond strength</a> in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[X2]+ gets higher, consequently the interatomic distances in the molecular ion is less than those in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">X2. Linear or nearly-linear triatomic polyhalides have weaker and longer bonds compared with that in the corresponding diatomic interhalogen or halogen, consistent with the additional repulsion between atoms as the halide ion is added to the neutral molecule. Another model involving the use of <a href="/wiki/Resonance_(chemistry)" title="Resonance (chemistry)">resonance theory</a> exists, for example, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]− can be viewed as the <a href="/wiki/Resonance_hybrid" class="mw-redirect" title="Resonance hybrid">resonance hybrid</a> of the following <a href="/wiki/Resonance_(chemistry)#Use_of_contributing_structures" title="Resonance (chemistry)">canonical forms</a>: <figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Canonical_forms_of_(ICl2)-.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/26/Canonical_forms_of_%28ICl2%29-.png/400px-Canonical_forms_of_%28ICl2%29-.png" decoding="async" width="400" height="79" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/26/Canonical_forms_of_%28ICl2%29-.png/600px-Canonical_forms_of_%28ICl2%29-.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/26/Canonical_forms_of_%28ICl2%29-.png/800px-Canonical_forms_of_%28ICl2%29-.png 2x" data-file-width="2467" data-file-height="485" /></a><figcaption></figcaption></figure> Evidence supporting this theory comes from the bond lengths (255 pm in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]− and 232 pm in <a href="/wiki/Iodine_monochloride" title="Iodine monochloride">ICl</a>(g)) and bond stretching <a href="/wiki/Wavenumbers" class="mw-redirect" title="Wavenumbers">wavenumbers</a> (267 and 222 cm−1 for symmetric and asymmetric stretching in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]− compared with 384 cm−1 in ICl), which suggests a bond order of about 0.5 for each I–Cl bonds in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]−, consistent with the interpretation using the resonance theory. Other triatomic species <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[XY2]− can be similarly interpreted.<a href="#cite_note-InorgChem-2">[2]</a> Even though they have a reduced bond order, all three halogen atoms are tightly bound. The fluorine–fluorine bond of trifluoride, with bond order 0.5, has a bond-strength is 30 kcal/mol, only 8 kcal/mol less than the fluorine–fluorine bond in <a href="/wiki/Difluorine" class="mw-redirect" title="Difluorine">difluorine</a> whose bond order is 1.<a href="#cite_note-7">[7]</a> <div class="mw-heading mw-heading2"><h2 id="Synthesis">Synthesis</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=5" title="Edit section: Synthesis">edit</a>]</div> The formation of polyhalogen ions can be viewed as the <a href="/wiki/Molecular_autoionization" title="Molecular autoionization">self-dissociation</a> of their parent <a href="/wiki/Interhalogen" title="Interhalogen">interhalogens</a> or <a href="/wiki/Halogen" title="Halogen">halogens</a>: <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 XYn ⇌ [XYn−1]+ + [XYn+1]−</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">3 X2 ⇌ [X3]+ + [X3]−</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">4 X2 ⇌ [X5]+ + [X3]−</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">5 X2 ⇌ 2 [X2]+ + 2 [X3]−</li></ul> <div class="mw-heading mw-heading3"><h3 id="Polyhalogen_cations">Polyhalogen cations</h3>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=6" title="Edit section: Polyhalogen cations">edit</a>]</div> There are two general strategies for preparing polyhalogen cations: <ul><li>By reacting the appropriate <a href="/wiki/Interhalogen" title="Interhalogen">interhalogen</a> with a <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acid</a> (such as the halides of <a href="/wiki/Boron" title="Boron">B</a>, <a href="/wiki/Aluminum" class="mw-redirect" title="Aluminum">Al</a>, <a href="/wiki/Phosphorus" title="Phosphorus">P</a>, <a href="/wiki/Arsenic" title="Arsenic">As</a>, <a href="/wiki/Antimony" title="Antimony">Sb</a>) either in an inert or oxidizing solvent (such as anhydrous <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">HF</a>) or without one, to give a heteropolyhalogen cation.</li></ul> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">XYn + MYm → [XYn−1]+ + [MYm+1]−</dd></dl> <ul><li>By an oxidative process, in which the halogen or interhalogen is reacted with an oxidizer and a Lewis acid to give the cation:</li></ul> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cl2 + ClF + AsF5 → [Cl3]+[AsF6]−</dd></dl> In some cases the Lewis acid (the <a href="/wiki/Fluoride" title="Fluoride">fluoride</a> acceptor) itself acts as an oxidant: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">3 I2 + 3 <a href="/wiki/Antimony_pentafluoride" title="Antimony pentafluoride">SbF5</a> → 2 [I3]+[SbF6]− + SbF3</dd></dl> Usually the first method is employed for preparing heteropolyhalogen cations, and the second one is applicable to both. The oxidative process is useful in the preparation of the cations <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IBr2]+, [ClF6]+, [BrF6]+, as their parent interhalogens, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IBr3, ClF7, BrF7 respectively, has never been isolated: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Br2 + IOSO2F → [IBr2]+[SO3F]−</dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 ClF5 + 2 PtF6 → [ClF6]+[PtF6]− + [ClF4]+[PtF6]−</dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">BrF5 + [KrF]+[AsF6]− → [BrF6]+[AsF6]− + Kr</dd></dl> The preparation of some individual species are briefly summarized in the table below with equations:<a href="#cite_note-Encyclo-1">[1]</a><a href="#cite_note-InorgChem-2">[2]</a><a href="#cite_note-Greenwood-3">[3]</a><a href="#cite_note-AdvInorgChem-4">[4]</a> <div style="display:table; margin-left: auto; margin-right: auto; border: none;"> <table class="wikitable"> <caption>Synthesis of some polyhalogen cations </caption> <tbody><tr> <th>Species</th> <th>Relevant chemical equation</th> <th>Additional conditions required </th></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2]+ (as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2O2]+)</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cl2 + [O2]+[SbF6]− → [Cl2O2]+[SbF6]−</td> <td>in anhydrous HF at low temperatures </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Br2 (in BrSO3F) + 3 SbF5 → [Br2]+[Sb3F16]− (not balanced)</td> <td>at room temperature </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 I2 + S2O6F2 → 2 [I2]+[SO3F]−</td> <td>in <a href="/wiki/Fluorosulfuric_acid" title="Fluorosulfuric acid"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">HSO3F</a> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cl2 + ClF + AsF5 → [Cl3]+[AsF6]−</td> <td>at a temperature of 195 K (-78 °C) </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br3]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">3 Br2 + 2 [O2]+[AsF6]− → 2 [Br3]+[AsF6]− + 2 O2</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">3 I2 + S2O6F2 → 2 [I3]+[SO3F]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl4]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 Cl2 + IrF6 → [Cl4]+[IrF6]−</td> <td>in anhydrous HF, at a temperature below 193 K (-80 °C) </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I4]2+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 I2 + 3 AsF5 → [I4]2+[AsF6]−2 + AsF3</td> <td>in liquid <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SO2 </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br5]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">8 Br2 + 3 [XeF]+[AsF6]− → 3 [Br5]+[AsF6]− + 3 Xe + BrF3</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 I2 + ICl + AlCl3 → [I5]+[AlCl4]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I7]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">7 I2 + S2O6F2 → 2 I7SO3F</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">ClF3 + AsF5 → [ClF2]+[AsF6]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2F]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 ClF + AsF5 → [Cl2F]+[AsF6]−</td> <td>at a temperature below 197 K </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">5 BrF3 + 2 Au → 3 BrF + 2 [BrF2]+[AuF4]−</td> <td>with excess <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">BrF3 required </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IF3 + AsF5 → [IF2]+[AsF6]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">ICl3 + SbCl5 → [ICl2]+[SbCl6]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IBr2]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Br2 + IOSO2F → [IBr2]+[SO3F]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF4]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">ClF5 + SbF5 → [ClF4]+[SbF6]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF4]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">BrF5 + AsF5 → [BrF4]+[AsF6]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF4]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IF5 + 2 SbF5 → [IF4]+[Sb2F11]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]+</td> <td><a href="#Symb5">‡</a><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cs2[NiF6] + 5 AsF5 + ClF5 → [ClF6]+[AsF6]− + Ni[AsF6]2 + 2 Cs[AsF6]</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF6]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[KrF]+[AsF6]− + BrF5 → [BrF6]+[AsF6]− + Kr</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF6]+</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IF7 + BrF3 → [IF6]+[BrF4]−[<a href="/wiki/Wikipedia:Accuracy_dispute#Disputed_statement" title="Wikipedia:Accuracy dispute"><span title="The article interhalogen states that “No interhalogen compounds containing three or more different halogens are definitely known”, but the product here is a interhalogen compound containing three diffetent halogens. (November 2023)">dubious</a> – <a href="/wiki/Talk:Polyhalogen_ions#Dubious" title="Talk:Polyhalogen ions">discuss</a>]</td> <td> </td></tr></tbody></table> <div style="display:table-caption;caption-side:bottom;"> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238216509">‡ In this reaction, the active oxidizing species is <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[NiF3]+, which is formed in situ in the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cs2[NiF6]/<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">AsF5/HF system. It is an even more powerful oxidizing and fluorinating agent than <a href="/wiki/Platinum_hexafluoride" title="Platinum hexafluoride"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">PtF6</a>. </div> </div> <div class="mw-heading mw-heading3"><h3 id="Polyhalogen_anions">Polyhalogen anions</h3>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=7" title="Edit section: Polyhalogen anions">edit</a>]</div> For polyhalogen anions, there are two general preparation strategies as well: <ul><li>By reacting an interhalogen or halogen with a <a href="/wiki/Lewis_base" class="mw-redirect" title="Lewis base">Lewis base</a>, most likely a fluoride: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[(CH3CH2)4N]+Y− + XYn → [(CH3CH2)4N]+[XYn+1]−</dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">X2 + X− → [X3]−</dd></dl></li> <li>By oxidation of simple <a href="/wiki/Halide" title="Halide">halides</a>: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">KI + Cl2 → K+[ICl2]−</dd></dl></li></ul> The preparation of some individual species are briefly summarized in the table below with equations:<a href="#cite_note-Encyclo-1">[1]</a><a href="#cite_note-InorgChem-2">[2]</a><a href="#cite_note-Greenwood-3">[3]</a><a href="#cite_note-AdvInorgChem-4">[4]</a> <table class="wikitable" style="margin-left: auto; margin-right: auto; border: none;"> <caption>Synthesis of some polyhalogen anions </caption> <tbody><tr> <th>Species</th> <th>Relevant chemical equation</th> <th>Additional conditions required </th></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]−, [Br3]−, [I3]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">X2 + X− → [X3]− (X = Cl, Br, I)</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br3]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Br2 + [(CH3CH2CH2CH2)4N]+Br− → [(CH3CH2CH2CH2)4N]+[Br3]−</td> <td>in <a href="/wiki/1,2-dichloroethane" class="mw-redirect" title="1,2-dichloroethane">1,2-dichloroethane</a> or liquid <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a>. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br3]− does not exist in solution and is only formed when the salt crystallizes out. </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br5]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 Br2 + [(CH3CH2CH2CH2)4N]+Br− → [(CH3CH2CH2CH2)4N]+[Br5]−</td> <td>in 1,2-dichloroethane or liquid sulfur dioxide, with excess <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Br2 </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF2]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">ClF + CsF → Cs+[ClF2]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrCl2]−<a href="#cite_note-Brauer-8">[8]</a>: v1p294 </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Br2 + Cl2 + 2 CsCl → 2 Cs+[BrCl2]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]−<a href="#cite_note-Brauer-8">[8]</a>: v1p295 </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">KI + Cl2 → K+[ICl2]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IBr2]−<a href="#cite_note-Brauer-8">[8]</a>: v1p297 </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">CsI + Br2 → Cs+[IBr2]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[AtBr2]−, [AtICl]−, [AtIBr]−, [AtI2]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Astatine" title="Astatine">At</a>Y + X− → [AtXY]− (X = I, Br, Cl; Y = I, Br)</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF4]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">NOF + ClF3 → [NO]+[ClF4]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF4]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">6 KCl + 8 BrF3 → 6 K+[BrF4]− + 3 Cl2 + Br2</td> <td>excess <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">BrF3 needed </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF4]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 XeF2 + [(CH3)4N]+I− → [(CH3)4N]+[IF4]− + 2 Xe</td> <td>the reactants were mixed at 242 K, then warmed to 298 K for the reaction to proceed </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl4]−<a href="#cite_note-Brauer-8">[8]</a>: v1p298 </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">KI + ICl3 → K+[ICl4]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF5]2−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IF3 + 2 [(CH3)4N]+F− → [(CH3)4N+]2[IF5]2−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF6]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IF5 + CsF → Cs+[IF6]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3Br4]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Phenyl_group" title="Phenyl group">Ph</a>4P]+Br− + 3 IBr → [Ph4P]+[I3Br4]−</td> <td> </td></tr> <tr> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF8]−</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">IF7 + [(CH3)4N]+F− → [(CH3)4N]+[IF8]−</td> <td>in <a href="/wiki/Acetonitrile" title="Acetonitrile">acetonitrile</a> </td></tr></tbody></table> The higher polyiodides were formed upon crystallization of solutions containing various concentrations of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">I− and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">I2. For instance, the monohydrate of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">K+[I3]− crystallizes when a saturated solution containing appropriate amounts of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">I2 and <a href="/wiki/Potassium_iodide" title="Potassium iodide">KI</a> is cooled.<a href="#cite_note-Brauer-8">[8]</a>: v1p294  <div class="mw-heading mw-heading2"><h2 id="Properties">Properties</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=8" title="Edit section: Properties">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Stability">Stability</h3>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=9" title="Edit section: Stability">edit</a>]</div> In general, a large counter cation or anion (such as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Caesium" title="Caesium">Cs</a>+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[SbF6]−) can help stabilize the polyhalogen ions formed in the solid state from <a href="/wiki/Lattice_energy" title="Lattice energy">lattice energy</a> considerations, as the packing efficiency increases. The polyhalogen cations are strong oxidizing agents, as indicated by the fact that they can only be prepared in oxidative liquids as a solvent, such as <a href="/wiki/Oleum" title="Oleum">oleum</a>. The most oxidizing and therefore most unstable ones are the species <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[X2]+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[XF6]+ (X = Cl, Br), followed by <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[X3]+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF6]+. The stability of the <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[X2]+ salts (X = Br, I) are thermodynamically quite stable. However, their stability in solution depends on the <a href="/wiki/Superacid" title="Superacid">superacid</a> solvent. For example, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+ is stable in <a href="/wiki/Fluoroantimonic_acid" title="Fluoroantimonic acid">fluoroantimonic acid</a> (HF with 0.2 N <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SbF5, <a href="/wiki/Hammett_acidity_function" title="Hammett acidity function">H0</a> = −20.65), but disproportionates to <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3]+, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">I2 when weaker fluoride acceptors, like <a href="/wiki/Niobium_pentafluoride" class="mw-redirect" title="Niobium pentafluoride"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">NbF5</a>, <a href="/wiki/Tantalum_pentafluoride" class="mw-redirect" title="Tantalum pentafluoride"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">TaF5</a> or <a href="/wiki/Sodium_fluoride" title="Sodium fluoride">NaF</a>, are added instead of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SbF5.<a href="#cite_note-AdvInorgChem-4">[4]</a> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">14 [I2]+ + 5 F− → 9 [I3]+ + IF5</dd></dl> For polyhalogen anions with the same number of atoms, the more stable ones are those with a heavier halogen at the center, <a href="/wiki/Molecular_symmetry" title="Molecular symmetry">symmetric</a> ions are also more stable than asymmetric ones. therefore the stability of the anions decrease in the order: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3]− > [IBr2]− > [ICl2]− > [I2Br]− > [Br3]− > [BrCl2]− > [Br2Cl]−</dd></dl> Heteropolyhalogen ions with a coordination number larger than or equal to four can only exist with fluoride ligands. <div class="mw-heading mw-heading3"><h3 id="Color">Color</h3>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=10" title="Edit section: Color">edit</a>]</div> Most polyhalogen ions are intensely colored, with deepened color as the atomic weight of the constituent element increases. The well-known <a href="/wiki/Starch" title="Starch">starch</a>-iodine complex has a deep blue color due to the linear <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]− ions present in the <a href="/wiki/Amylose" title="Amylose">amylose</a> helix.<a href="#cite_note-AdvInorgChem-4">[4]</a> Some colors of the common species were listed below:<a href="#cite_note-Greenwood-3">[3]</a> <ul><li><a href="/w/index.php?title=Fluorocations&action=edit&redlink=1" class="new" title="Fluorocations (page does not exist)">fluorocations</a> tend to be colorless or pale yellow, other heteropolyhalogen ions are orange, red or deep purple<a href="#cite_note-AdvInorgChem-4">[4]</a></li> <li>compounds of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]+ are wine red to bright orange; while that of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2Cl]+ are dark brown to purplish black</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]+ is yellow</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl4]+ is blue<a href="#cite_note-InorgChem-2">[2]</a></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br2]+ is cherry red</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br3]+ is brown</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Br5]+ is dark brown</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+ is bright blue</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I3]+ is dark brown to black</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I4]2+ is red to brown</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]+ is green or black, the salt <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I5]+[AlCl4]− exists as greenish-black needles, but appears brown-red in thin sections</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I7]+ is black, if its existence in the compound <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I7]+[SO3F]− has been firmly established</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I15]3+ is black<a href="#cite_note-wiberg2001-5">[5]</a></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl2]− is scarlet red</li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ICl4]− is golden-yellow</li> <li><a href="/wiki/Polyiodides" class="mw-redirect" title="Polyiodides">polyiodides</a> have very dark colors, either dark brown or dark blue</li></ul> <div class="mw-heading mw-heading3"><h3 id="Chemical_properties">Chemical properties</h3>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=11" title="Edit section: Chemical properties">edit</a>]</div> The heteropolyhalogen cations are explosively reactive oxidants, and the cations often have higher reactivity than their parent interhalogens and decompose by reductive pathways. As expected from the highest oxidation state of +7 in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]+, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF6]+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[IF6]+, these species are extremely strong oxidizing agents, demonstrated by the reactions shown below: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 O2 + 2 [BrF6]+[AsF6]− → 2 <a href="/wiki/Dioxygenyl" title="Dioxygenyl">[O2]+</a>[AsF6]− + 2 BrF5 + F2</dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><a href="/wiki/Radon" title="Radon">Rn</a> + [IF6]+[SbF6]− → [RnF]+[SbF6]− + IF5</dd></dl> Polyhalogen cations with lower oxidation states tend to <a href="/wiki/Disproportionation" title="Disproportionation">disproportionate</a>. For example, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2F]+ is unstable in solution and disproportionate completely in <a href="/wiki/Fluoroantimonic_acid" title="Fluoroantimonic acid">HF/<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">SbF5</a> mixture even at 197 K: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 [Cl2F]+ → [ClF2]+ + [Cl3]+</dd></dl> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+ reversibly dimerizes at 193 K, and is observed as the blue color of <a href="/wiki/Paramagnetic" class="mw-redirect" title="Paramagnetic">paramagnetic</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+ dramatically shifts to the red-brown color of <a href="/wiki/Diamagnetic" class="mw-redirect" title="Diamagnetic">diamagnetic</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+, together with a drop in <a href="/wiki/Magnetochemistry#Magnetic_susceptibility" title="Magnetochemistry">paramagnetic susceptibility</a> and <a href="/wiki/Electrical_conductivity" class="mw-redirect" title="Electrical conductivity">electrical conductivity</a> when the solution is cooled to below 193 K:<a href="#cite_note-InorgChem-2">[2]</a> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">2 [I2]+ ⇌ [I4]2+</dd></dl> The dimerization can be attributed to the overlapping of the half-filled π* orbitals in two <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I2]+. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl4]+ in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl4]+[IrF6]− is structurally analogous to <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[I4]2+, but decomposes at 195 K to give <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cl2, and salts of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]+ instead of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl2]+.<a href="#cite_note-InorgChem-2">[2]</a> Attempts to prepare <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">ClF7 and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">BrF7 by fluorinating <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]+ and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF6]+ using <a href="/wiki/Nitrosyl_fluoride" title="Nitrosyl fluoride">NOF</a> have met with failure, because the following reactions occurred:<a href="#cite_note-Greenwood-3">[3]</a> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]+[PtF6]− + NOF → [NO]+[PtF6]− + ClF5 + F2</dd></dl> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[BrF6]+[AsF6]− + 2 NOF → [NO]+[AsF6]− + [NO]+[BrF6]− + F2</dd></dl> The anions are less reactive compared to the cations, and are generally weaker oxidants than their parent interhalogens. They are less reactive towards organic compounds, and some salts are of quite high thermal stability. Salts containing polyhalogen anions of the type <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">M+[XmYnZp]−, where m + n + p = {3, 5, 7, 9...}, tend to dissociate into simple monohalide salts between <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">M+ and the most <a href="/wiki/Electronegative" class="mw-redirect" title="Electronegative">electronegative</a> halogen, so that the monohalide has the highest lattice energy. An interhalogen is usually formed as the other product. The salt <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[(CH3)4N]+[ClF4]− decomposes at about 100 °C, and salts of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[ClF6]− are thermally unstable and can explode even at −31 °C.<a href="#cite_note-AdvInorgChem-4">[4]</a> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=12" title="Edit section: See also">edit</a>]</div> <ul><li><a href="/wiki/Polyiodide" title="Polyiodide">Polyiodide</a></li> <li><a href="/wiki/Halogen_bond" title="Halogen bond">Halogen bond</a></li> <li><a href="/wiki/Inorganic_polymer" title="Inorganic polymer">Inorganic polymer</a></li> <li><a href="/wiki/Catenation" title="Catenation">Catenation</a></li> <li><a href="/wiki/Allotropy" title="Allotropy">Allotropy</a></li></ul> <div class="mw-heading mw-heading2"><h2 id="References">References</h2>[<a href="/w/index.php?title=Polyhalogen_ions&action=edit&section=13" title="Edit section: References">edit</a>]</div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-Encyclo-1">^ <a href="#cite_ref-Encyclo_1-0">a</a> <a href="#cite_ref-Encyclo_1-1">b</a> <a href="#cite_ref-Encyclo_1-2">c</a> <a href="#cite_ref-Encyclo_1-3">d</a> <style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite id="CITEREFKing2005" class="citation book cs1">King, R. Bruce (2005). "Chlorine, Bromine, Iodine, & Astatine: Inorganic Chemistry". Encyclopedia of Inorganic Chemistry (2nd ed.). Wiley. p. 747. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9780470862100" title="Special:BookSources/9780470862100"><bdi>9780470862100</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Chlorine%2C+Bromine%2C+Iodine%2C+%26+Astatine%3A+Inorganic+Chemistry&rft.btitle=Encyclopedia+of+Inorganic+Chemistry&rft.pages=747&rft.edition=2nd&rft.pub=Wiley&rft.date=2005&rft.isbn=9780470862100&rft.aulast=King&rft.aufirst=R.+Bruce&rfr_id=info%3Asid%2Fen.wikipedia.org%3APolyhalogen+ions" class="Z3988"> </li> <li id="cite_note-InorgChem-2">^ <a href="#cite_ref-InorgChem_2-0">a</a> <a href="#cite_ref-InorgChem_2-1">b</a> <a href="#cite_ref-InorgChem_2-2">c</a> <a href="#cite_ref-InorgChem_2-3">d</a> <a href="#cite_ref-InorgChem_2-4">e</a> <a href="#cite_ref-InorgChem_2-5">f</a> <a href="#cite_ref-InorgChem_2-6">g</a> <a href="#cite_ref-InorgChem_2-7">h</a> <a href="#cite_ref-InorgChem_2-8">i</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFHousecroftSharpe2008" class="citation book cs1">Housecroft, Catherine E.; Sharpe, Alan G. (2008). "Chapter 17: The group 17 elements". Inorganic Chemistry (3rd ed.). Pearson. p. 547. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-13-175553-6" title="Special:BookSources/978-0-13-175553-6"><bdi>978-0-13-175553-6</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Chapter+17%3A+The+group+17+elements&rft.btitle=Inorganic+Chemistry&rft.pages=547&rft.edition=3rd&rft.pub=Pearson&rft.date=2008&rft.isbn=978-0-13-175553-6&rft.aulast=Housecroft&rft.aufirst=Catherine+E.&rft.au=Sharpe%2C+Alan+G.&rfr_id=info%3Asid%2Fen.wikipedia.org%3APolyhalogen+ions" class="Z3988"> </li> <li id="cite_note-Greenwood-3">^ <a href="#cite_ref-Greenwood_3-0">a</a> <a href="#cite_ref-Greenwood_3-1">b</a> <a href="#cite_ref-Greenwood_3-2">c</a> <a href="#cite_ref-Greenwood_3-3">d</a> <a href="#cite_ref-Greenwood_3-4">e</a> <a href="#cite_ref-Greenwood_3-5">f</a> <a href="#cite_ref-Greenwood_3-6">g</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1"><a href="/wiki/Norman_Greenwood" title="Norman Greenwood">Greenwood, Norman N.</a>; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). <a href="/wiki/Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. p. 835. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-08-037941-8" title="Special:BookSources/978-0-08-037941-8"><bdi>978-0-08-037941-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry+of+the+Elements&rft.pages=835&rft.edition=2nd&rft.pub=Butterworth-Heinemann&rft.date=1997&rft.isbn=978-0-08-037941-8&rft.aulast=Greenwood&rft.aufirst=Norman+N.&rft.au=Earnshaw%2C+Alan&rfr_id=info%3Asid%2Fen.wikipedia.org%3APolyhalogen+ions" class="Z3988"> </li> <li id="cite_note-AdvInorgChem-4">^ <a href="#cite_ref-AdvInorgChem_4-0">a</a> <a href="#cite_ref-AdvInorgChem_4-1">b</a> <a href="#cite_ref-AdvInorgChem_4-2">c</a> <a href="#cite_ref-AdvInorgChem_4-3">d</a> <a href="#cite_ref-AdvInorgChem_4-4">e</a> <a href="#cite_ref-AdvInorgChem_4-5">f</a> <a href="#cite_ref-AdvInorgChem_4-6">g</a> <a href="#cite_ref-AdvInorgChem_4-7">h</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFCottonWilkinsonMurilloBochmann1999" class="citation book cs1">Cotton, F. 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