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class="vector-toc-list"> </ul> </li> <li id="toc-Pnictogens" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Pnictogens"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.2</span> <span>Pnictogens</span> </div> </a> <ul id="toc-Pnictogens-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chalcogens" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chalcogens"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.3</span> <span>Chalcogens</span> </div> </a> <ul id="toc-Chalcogens-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Halogens" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Halogens"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.4</span> <span>Halogens</span> </div> </a> <ul id="toc-Halogens-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Noble_gases" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Noble_gases"> <div class="vector-toc-text"> <span class="vector-toc-numb">3.5</span> <span>Noble gases</span> </div> </a> <ul id="toc-Noble_gases-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Transition_metals_and_actinides" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Transition_metals_and_actinides"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Transition metals and actinides</span> </div> </a> <ul id="toc-Transition_metals_and_actinides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Minerals_and_ionic_compounds" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Minerals_and_ionic_compounds"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Minerals and ionic compounds</span> </div> </a> <ul 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class="vector-appearance vector-pinnable-element"> <div class="vector-pinnable-header vector-appearance-pinnable-header vector-pinnable-header-pinned" data-feature-name="appearance-pinned" data-pinnable-element-id="vector-appearance" data-pinned-container-id="vector-appearance-pinned-container" data-unpinned-container-id="vector-appearance-unpinned-container" > <div class="vector-pinnable-header-label">Appearance</div> <button class="vector-pinnable-header-toggle-button vector-pinnable-header-pin-button" data-event-name="pinnable-header.vector-appearance.pin">move to sidebar</button> <button class="vector-pinnable-header-toggle-button vector-pinnable-header-unpin-button" data-event-name="pinnable-header.vector-appearance.unpin">hide</button> </div> </div> </div> </nav> </div> </div> <div id="bodyContent" class="vector-body" aria-labelledby="firstHeading" data-mw-ve-target-container> <div class="vector-body-before-content"> <div class="mw-indicators"> </div> <div id="siteSub" class="noprint">From Wikipedia, the free encyclopedia</div> </div> <div id="contentSub"><div id="mw-content-subtitle"><span class="mw-redirectedfrom">(Redirected from <a href="/w/index.php?title=Oxyfluoride&redirect=no" class="mw-redirect" title="Oxyfluoride">Oxyfluoride</a>)</span></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compounds with oxygen and a halogen bonded to the same atom</div> <p>In <a href="/wiki/Chemistry" title="Chemistry">chemistry</a>, <b>molecular oxohalides</b> (<b>oxyhalides</b>) are a group of <a href="/wiki/Chemical_compound" title="Chemical compound">chemical compounds</a> in which both <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> and <a href="/wiki/Halogen" title="Halogen">halogen</a> atoms are attached to another <a href="/wiki/Chemical_element" title="Chemical element">chemical element</a> A in a single <a href="/wiki/Molecule" title="Molecule">molecule</a>. They have the general formula <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><span class="chemf nowrap">AO<sub class="template-chem2-sub"><i>m</i></sub>X<sub class="template-chem2-sub"><i>n</i></sub></span>, where X is a <a href="/wiki/Halogen" title="Halogen">halogen</a>. Known oxohalides have <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> (F), <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> (Cl), <a href="/wiki/Bromine" title="Bromine">bromine</a> (Br), and/or <a href="/wiki/Iodine" title="Iodine">iodine</a> (I) in their molecules. The element A may be a <a href="/wiki/Main_group" class="mw-redirect" title="Main group">main group</a> element, a <a href="/wiki/Transition_element" class="mw-redirect" title="Transition element">transition element</a>, a <a href="/wiki/Rare_earth_element" class="mw-redirect" title="Rare earth element">rare earth element</a> or an <a href="/wiki/Actinide" title="Actinide">actinide</a>. The term <i>oxohalide</i>, or <i>oxyhalide</i>, may also refer to <a href="/wiki/Mineral" title="Mineral">minerals</a> and other <a href="/wiki/Crystalline" class="mw-redirect" title="Crystalline">crystalline</a> substances with the same overall chemical formula, but having an <a href="/wiki/Ionic_crystal" title="Ionic crystal">ionic</a> structure. </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Synthesis">Synthesis</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=1" title="Edit section: Synthesis"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Chromyl_chloride.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/Chromyl_chloride.jpg/100px-Chromyl_chloride.jpg" decoding="async" width="100" height="133" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/Chromyl_chloride.jpg/150px-Chromyl_chloride.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/18/Chromyl_chloride.jpg/200px-Chromyl_chloride.jpg 2x" data-file-width="500" data-file-height="667" /></a><figcaption>Chromyl chloride liquid and vapour</figcaption></figure> <p>Oxohalides can be seen as compounds intermediate between <a href="/wiki/Oxide" title="Oxide">oxides</a> and <a href="/wiki/Halide" title="Halide">halides</a>. There are three general methods of synthesis:<sup id="cite_ref-1" class="reference"><a href="#cite_note-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </p> <ul><li>Partial oxidation of a halide: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 PCl<sub class="template-chem2-sub">3</sub> + O<sub class="template-chem2-sub">2</sub> → 2 POCl<sub class="template-chem2-sub">3</sub></span></dd></dl> <ul><li>In this example, the <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation state</a> increases by two and the electrical charge is unchanged.</li></ul></li> <li>Partial halogenation of an oxide: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 V<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">5</sub> + 6 Cl<sub class="template-chem2-sub">2</sub> + 3 C → 4 VOCl<sub class="template-chem2-sub">3</sub> + 3 CO<sub class="template-chem2-sub">2</sub></span></dd></dl></li> <li>Oxide replacement: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">CrO<span class="template-chem2-su"><span>2−</span><span>4</span></span> + 2 Cl<sup class="template-chem2-sup">−</sup> + 4 H<sup class="template-chem2-sup">+</sup> → CrO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub> + 4 H<sub class="template-chem2-sub">2</sub>O</span></dd></dl></li></ul> <p>In addition, various oxohalides can be made by halogen exchange reactions and this reaction can also lead to the formation of mixed oxohalides such as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">POFCl<sub class="template-chem2-sub">2</sub></span> and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">CrO<sub class="template-chem2-sub">2</sub>FCl</span>. </p> <div class="mw-heading mw-heading2"><h2 id="Properties">Properties</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=2" title="Edit section: Properties"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>In relation to the oxide or halide, for a given oxidation state of an element A, if two halogen atoms replace one oxygen atom, or <i>vice versa</i>, the overall charge on the molecule is unchanged and the <a href="/wiki/Coordination_number" title="Coordination number">coordination number</a> of the central atom decreases by one. For example, both <a href="/wiki/Phosphorus_oxychloride" class="mw-redirect" title="Phosphorus oxychloride">phosphorus oxychloride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">POCl<sub class="template-chem2-sub">3</sub></span>) and <a href="/wiki/Phosphorus_pentachloride" title="Phosphorus pentachloride">phosphorus pentachloride</a>, (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">PCl<sub class="template-chem2-sub">5</sub></span>) are neutral <a href="/wiki/Covalent" class="mw-redirect" title="Covalent">covalent</a> compounds of <a href="/wiki/Phosphorus" title="Phosphorus">phosphorus</a> in the +5 <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation state</a>. If an oxygen atom is simply replaced by a halogen atom the charge increases by +1, but the coordination number is unchanged. This is illustrated by the reaction of a mixture of a <a href="/wiki/Chromate_and_dichromate" title="Chromate and dichromate">chromate or dichromate</a> salt and <a href="/wiki/Potassium_chloride" title="Potassium chloride">potassium chloride</a> with concentrated <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>. </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Cr<sub class="template-chem2-sub">2</sub>O<span class="template-chem2-su"><span>2−</span><span>7</span></span> + 4 Cl<sup class="template-chem2-sup">−</sup> + 6 H<sup class="template-chem2-sup">+</sup> → 2 CrO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub> + 3 H<sub class="template-chem2-sub">2</sub>O</span></dd></dl> <p>The <a href="/wiki/Chromyl_chloride" title="Chromyl chloride">chromyl chloride</a> produced has no electrical charge and is a volatile covalent molecule that can be distilled out of the reaction mixture.<sup id="cite_ref-2" class="reference"><a href="#cite_note-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> </p><p>Oxohalides of elements in high oxidation states are strong <a href="/wiki/Oxidizing_agent" title="Oxidizing agent">oxidizing agents</a>, with oxidizing power similar to the corresponding oxide or halide. Most oxohalides are easily <a href="/wiki/Hydrolysis" title="Hydrolysis">hydrolyzed</a>. For example, chromyl chloride is hydrolyzed to chromate in the reverse of the synthetic reaction, above. The driving force for this reaction is the formation of A-O bonds which are stronger than A-Cl bonds. This gives a favourable <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> contribution to the <a href="/wiki/Gibbs_free_energy" title="Gibbs free energy">Gibbs free energy</a> change for the reaction<sup id="cite_ref-3" class="reference"><a href="#cite_note-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </p><p>Many oxohalides can act as <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acids</a>. This is particularly so with oxohalides of <a href="/wiki/Coordination_number" title="Coordination number">coordination number</a> 3 or 4 which, in accepting one or more electron pairs from a <a href="/wiki/Lewis_base" class="mw-redirect" title="Lewis base">Lewis base</a>, become 5- or 6-coordinate. Oxohalide anions such as <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[VOCl<sub class="template-chem2-sub">4</sub>]<sup>2−</sup></span> can be seen as acid-base complexes of the oxohalide (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">VOCl<sub class="template-chem2-sub">2</sub></span>) with more halide ions acting as Lewis bases. Another example is <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">VOCl<sub class="template-chem2-sub">2</sub></span> which forms the <a href="/wiki/Trigonal_bipyramid" class="mw-redirect" title="Trigonal bipyramid">trigonal bipyramidal</a> complex <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">VOCl<sub class="template-chem2-sub">2</sub>(N(CH<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">2</sub></span> with the base <a href="/wiki/Trimethylamine" title="Trimethylamine">trimethylamine</a>.<sup id="cite_ref-4" class="reference"><a href="#cite_note-4"><span class="cite-bracket">[</span>4<span class="cite-bracket">]</span></a></sup> </p><p>The <a href="/wiki/Vibrational_spectroscopy" class="mw-redirect" title="Vibrational spectroscopy">vibrational spectra</a> of many oxohalides have been assigned in detail. They give useful information on relative bond strengths. For example, in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">CrO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></span>, the Cr–O stretching vibrations are at 1006 cm<sup>−1</sup> and 1016 cm<sup>−1</sup> and the Cr–F stretching vibrations are at 727 cm<sup>−1</sup> and 789 cm<sup>−1</sup>. The difference is much too large to be due to the different masses of O and F atoms. Rather, it shows that the Cr–O bond is much stronger than the Cr–F bond. M–O bonds are generally considered to be <a href="/wiki/Double_bond" title="Double bond">double bonds</a> and this is backed up by measurements of M–O bond lengths. It implies that the elements A and O are <a href="/wiki/Chemical_bond" title="Chemical bond">chemically bound</a> together by a σ bond and a π bond.<sup id="cite_ref-Nakamoto_5-0" class="reference"><a href="#cite_note-Nakamoto-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> </p><p>Oxohalides of elements in high oxidation states are intensely coloured owing to ligand to metal <a href="/wiki/Charge-transfer_complex" title="Charge-transfer complex">charge transfer</a> (LMCT) transitions.<sup id="cite_ref-6" class="reference"><a href="#cite_note-6"><span class="cite-bracket">[</span>6<span class="cite-bracket">]</span></a></sup> </p> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Boron-teflate-3D-balls.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/Boron-teflate-3D-balls.png/170px-Boron-teflate-3D-balls.png" decoding="async" width="170" height="160" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/Boron-teflate-3D-balls.png/255px-Boron-teflate-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/75/Boron-teflate-3D-balls.png/340px-Boron-teflate-3D-balls.png 2x" data-file-width="2000" data-file-height="1877" /></a><figcaption>Boron teflate. <style data-mw-deduplicate="TemplateStyles:r981673959">.mw-parser-output .legend{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .legend-color{display:inline-block;min-width:1.25em;height:1.25em;line-height:1.25;margin:1px 0;text-align:center;border:1px solid black;background-color:transparent;color:black}.mw-parser-output .legend-text{}</style><div class="legend"><span class="legend-color mw-no-invert" style="background-color:pink; color:black;"> </span> Boron</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:red; color:black;"> </span> Oxygen</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:#d2691e; color:black;"> </span> Tellurium</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:lime; color:black;"> </span> Fluorine</div></figcaption></figure> <div class="mw-heading mw-heading2"><h2 id="Main_group_elements">Main group elements</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=3" title="Edit section: Main group elements"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Sulfuryl-fluoride-2D-dimensions.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a9/Sulfuryl-fluoride-2D-dimensions.png/100px-Sulfuryl-fluoride-2D-dimensions.png" decoding="async" width="100" height="104" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a9/Sulfuryl-fluoride-2D-dimensions.png/150px-Sulfuryl-fluoride-2D-dimensions.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a9/Sulfuryl-fluoride-2D-dimensions.png/200px-Sulfuryl-fluoride-2D-dimensions.png 2x" data-file-width="1059" data-file-height="1100" /></a><figcaption>Sulfuryl fluoride</figcaption></figure> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Chalcooxyfluoride.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/Chalcooxyfluoride.png/170px-Chalcooxyfluoride.png" decoding="async" width="170" height="97" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/75/Chalcooxyfluoride.png/255px-Chalcooxyfluoride.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/75/Chalcooxyfluoride.png/340px-Chalcooxyfluoride.png 2x" data-file-width="1178" data-file-height="670" /></a><figcaption><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">F<sub class="template-chem2-sub">5</sub>AOAF<sub class="template-chem2-sub">5</sub></span> (A = S, Se, Te)</figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Carbon_group">Carbon group</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=4" title="Edit section: Carbon group"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Carbon <a href="/wiki/Carbon_oxohalide" title="Carbon oxohalide">forms oxohalides</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">COX<sub class="template-chem2-sub">2</sub></span>, X = <a href="/wiki/Carbonyl_fluoride" title="Carbonyl fluoride">F</a>, <a href="/wiki/Carbonyl_bromide" title="Carbonyl bromide">Br</a>, and the very toxic <a href="/wiki/Phosgene" title="Phosgene">phosgene</a> (X = Cl), which is produced industrially by a carbon-catalyzed reaction of <a href="/wiki/Carbon_monoxide" title="Carbon monoxide">carbon monoxide</a> with <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>. It is a useful reagent in <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a> for the formation of <a href="/wiki/Carbonyl_compounds" class="mw-redirect" title="Carbonyl compounds">carbonyl compounds</a>.<sup id="cite_ref-7" class="reference"><a href="#cite_note-7"><span class="cite-bracket">[</span>7<span class="cite-bracket">]</span></a></sup> For example: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">COCl<sub class="template-chem2-sub">2</sub> + 2 ROH → CO(OR)<sub class="template-chem2-sub">2</sub> + 2 HCl</span></dd></dl> <p><a href="/wiki/Silicon_tetrafluoride" title="Silicon tetrafluoride">Silicon tetrafluoride</a> reacts with <a href="/wiki/Water" title="Water">water</a> to yield poorly-characterized oxyfluoride polymers, but slow and careful reaction at <a href="/wiki/Liquid_nitrogen" title="Liquid nitrogen">-196 °C</a> yields the oxyfluoride hexafluorodisiloxane as well.<sup id="cite_ref-8" class="reference"><a href="#cite_note-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Pnictogens">Pnictogens</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=5" title="Edit section: Pnictogens"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><a href="/wiki/Nitrogen" title="Nitrogen">Nitrogen</a> forms two series of oxohalides with nitrogen in oxidation states 3, NOX, X = <a href="/wiki/Nitrosyl_fluoride" title="Nitrosyl fluoride">F</a>, <a href="/wiki/Nitrosyl_chloride" title="Nitrosyl chloride">Cl</a>, <a href="/wiki/Nitrosyl_bromide" title="Nitrosyl bromide">Br</a> and 5, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">NO<sub class="template-chem2-sub">2</sub>X</span>, X = <a href="/wiki/Nitryl_fluoride" title="Nitryl fluoride">F</a>, Cl. They are made by halogenation of nitrogen oxides. Note that <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">NO<sub class="template-chem2-sub">2</sub>F</span> is <a href="/wiki/Isoelectronic" class="mw-redirect" title="Isoelectronic">isoelectronic</a> with the <a href="/wiki/Nitrate" title="Nitrate">nitrate</a> ion, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">NO<span class="template-chem2-su"><span>−</span><span>3</span></span></span>. Only oxohalides of <a href="/wiki/Phosphorus" title="Phosphorus">phosphorus</a>(V) are known.<sup id="cite_ref-9" class="reference"><a href="#cite_note-9"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Chalcogens">Chalcogens</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=6" title="Edit section: Chalcogens"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><a href="/wiki/Sulfur" title="Sulfur">Sulfur</a> forms oxohalides<sup id="cite_ref-10" class="reference"><a href="#cite_note-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> in oxidation state +4, such as <a href="/wiki/Thionyl_chloride" title="Thionyl chloride">thionyl chloride</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">SOCl<sub class="template-chem2-sub">2</sub></span> and oxidation state +6, such as <a href="/wiki/Sulfuryl_fluoride" title="Sulfuryl fluoride">sulfuryl fluoride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">SO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></span>), <a href="/wiki/Sulfuryl_chloride" title="Sulfuryl chloride">sulfuryl chloride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">SO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></span>), and <a href="/wiki/Thionyl_tetrafluoride" title="Thionyl tetrafluoride">thionyl tetrafluoride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">SOF<sub class="template-chem2-sub">4</sub></span>). All are easily hydrolyzed. Indeed, thionyl chloride can be used as a dehydration agent as the water molecules are converted into gaseous products, leaving behind the anhydrous solid chloride.<sup id="cite_ref-s397_11-0" class="reference"><a href="#cite_note-s397-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">MgCl<sub class="template-chem2-sub">2</sub>·6H<sub>2</sub>O + 6 SOCl<sub class="template-chem2-sub">2</sub> → MgCl<sub class="template-chem2-sub">2</sub> + 6 SO<sub class="template-chem2-sub">2</sub> + 12 HCl</span></dd></dl> <p><a href="/wiki/Selenium" title="Selenium">Selenium</a> and <a href="/wiki/Tellurium" title="Tellurium">tellurium</a> form similar compounds and also the oxo-bridged species <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">F<sub class="template-chem2-sub">5</sub>AOAF<sub class="template-chem2-sub">5</sub></span> (A = S, Se, Te). They are non-linear with the A-O-A angle of 142.5, 142.4 and 145.5° for S, Se and Te, respectively.<sup id="cite_ref-r3_12-0" class="reference"><a href="#cite_note-r3-12"><span class="cite-bracket">[</span>12<span class="cite-bracket">]</span></a></sup> The tellurium anion <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">F<sub class="template-chem2-sub">5</sub>TeO<sup class="template-chem2-sup">−</sup></span>, known as <a href="/wiki/Teflic_acid" title="Teflic acid">teflate</a>, is a large and rather stable anion, useful for forming stable salts with large cations.<sup id="cite_ref-s397_11-1" class="reference"><a href="#cite_note-s397-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Halogens">Halogens</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=7" title="Edit section: Halogens"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The halogens form various oxofluorides with formulae <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XO<sub class="template-chem2-sub">2</sub>F</span> (<a href="/wiki/Chloryl_fluoride" title="Chloryl fluoride">chloryl fluoride</a>), <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XO<sub class="template-chem2-sub">3</sub>F</span> (<a href="/wiki/Perchloryl_fluoride" title="Perchloryl fluoride">perchloryl fluoride</a>) and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XOF<sub class="template-chem2-sub">3</sub></span> with X = Cl, Br and I. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">IO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">3</sub></span> and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">IOF<sub class="template-chem2-sub">5</sub></span> are also known.<sup id="cite_ref-13" class="reference"><a href="#cite_note-13"><span class="cite-bracket">[</span>13<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Noble_gases">Noble gases</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=8" title="Edit section: Noble gases"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><a href="/wiki/Xenon" title="Xenon">Xenon</a> forms <a href="/wiki/Xenon_oxytetrafluoride" title="Xenon oxytetrafluoride">xenon oxytetrafluoride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XeOF<sub class="template-chem2-sub">4</sub></span>), <a href="/wiki/Xenon_dioxydifluoride" title="Xenon dioxydifluoride">xenon dioxydifluoride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XeO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></span>) and <a href="/wiki/Xenon_oxydifluoride" title="Xenon oxydifluoride">xenon oxydifluoride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XeOF<sub class="template-chem2-sub">2</sub></span>). </p> <div class="mw-heading mw-heading2"><h2 id="Transition_metals_and_actinides">Transition metals and actinides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=9" title="Edit section: Transition metals and actinides"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Ti(ClO4)4.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c1/Ti%28ClO4%294.png/220px-Ti%28ClO4%294.png" decoding="async" width="220" height="181" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c1/Ti%28ClO4%294.png/330px-Ti%28ClO4%294.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c1/Ti%28ClO4%294.png/440px-Ti%28ClO4%294.png 2x" data-file-width="1100" data-file-height="904" /></a><figcaption>Crystal structure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Ti(ClO<sub class="template-chem2-sub">4</sub>)<sub class="template-chem2-sub">4</sub></span>.<sup id="cite_ref-14" class="reference"><a href="#cite_note-14"><span class="cite-bracket">[</span>14<span class="cite-bracket">]</span></a></sup> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:silver; color:black;"> </span> Titanium</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:lime; color:black;"> </span> Chlorine</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:red; color:black;"> </span> Oxygen</div></figcaption></figure> <p>A selection of known oxohalides of <a href="/wiki/Transition_metal" title="Transition metal">transition metals</a> is shown below, and more detailed lists are available in the literature.<sup id="cite_ref-15" class="reference"><a href="#cite_note-15"><span class="cite-bracket">[</span>15<span class="cite-bracket">]</span></a></sup> X indicates various halides, most often F and Cl. </p> <table class="wikitable"> <tbody><tr> <th>Oxidation state</th> <th>oxohalides </th></tr> <tr> <td>3</td> <td>VOCl, VOBr,<sup id="cite_ref-16" class="reference"><a href="#cite_note-16"><span class="cite-bracket">[</span>16<span class="cite-bracket">]</span></a></sup> <a href="/wiki/FeOCl" class="mw-redirect" title="FeOCl">FeOCl</a> </td></tr> <tr> <td>4</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[TiOCl<sub class="template-chem2-sub">4</sub>]<sup>2−</sup></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Cl<sub class="template-chem2-sub">3</sub>TiOTiCl<sub class="template-chem2-sub">3</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Vanadium_oxydichloride" title="Vanadium oxydichloride">VOCl<sub class="template-chem2-sub">2</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[VOCl<sub class="template-chem2-sub">4</sub>]<sup>2−</sup></span> </td></tr> <tr> <td>5</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">VOX<sub class="template-chem2-sub">3</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Vanadium_dioxide_fluoride" title="Vanadium dioxide fluoride">VO<sub class="template-chem2-sub">2</sub>F</a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[CrOF<sub class="template-chem2-sub">4</sub>]<sup class="template-chem2-sup">−</sup></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[CrOF<sub class="template-chem2-sub">5</sub>]<sup>2−</sup></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">MnOCl<sub class="template-chem2-sub">3</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">TcOCl<sub class="template-chem2-sub">3</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Vanadium(V)_oxytrifluoride" title="Vanadium(V) oxytrifluoride">VOF<sub class="template-chem2-sub">3</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Vanadium_oxytrichloride" title="Vanadium oxytrichloride">VOCl<sub class="template-chem2-sub">3</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Niobium_oxychloride" title="Niobium oxychloride">NbOCl<sub class="template-chem2-sub">3</sub></a></span> </td></tr> <tr> <td>6</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Chromyl_chloride" title="Chromyl chloride">CrO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[CrO<sub class="template-chem2-sub">3</sub>Cl]<sup class="template-chem2-sup">−</sup></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Chromium_oxytetrafluoride" title="Chromium oxytetrafluoride">CrOF<sub class="template-chem2-sub">4</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">ReOX<sub class="template-chem2-sub">4</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">ReO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">OsOF<sub class="template-chem2-sub">4</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Chromyl_fluoride" title="Chromyl fluoride">CrO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Molybdenum_oxytetrafluoride" title="Molybdenum oxytetrafluoride">MoOF<sub class="template-chem2-sub">4</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Molybdenum_oxytetrachloride" title="Molybdenum oxytetrachloride">MoOCl<sub class="template-chem2-sub">4</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Molybdenum_dichloride_dioxide" title="Molybdenum dichloride dioxide">MoO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Molybdenum_difluoride_dioxide" title="Molybdenum difluoride dioxide">MoO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Tungsten_dichloride_dioxide" title="Tungsten dichloride dioxide">WO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">WO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">2</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Tungsten(VI)_oxytetrafluoride" class="mw-redirect" title="Tungsten(VI) oxytetrafluoride">WOF<sub class="template-chem2-sub">4</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Tungsten(VI)_oxytetrachloride" title="Tungsten(VI) oxytetrachloride">WOCl<sub class="template-chem2-sub">4</sub></a></span> </td></tr> <tr> <td>7</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Manganese_trioxide_fluoride" title="Manganese trioxide fluoride">MnO<sub class="template-chem2-sub">3</sub>F</a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">ReOF<sub class="template-chem2-sub">5</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Rhenium_dioxide_trifluoride" title="Rhenium dioxide trifluoride">ReO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">3</sub></a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Rhenium_trioxide_fluoride" title="Rhenium trioxide fluoride">ReO<sub class="template-chem2-sub">3</sub>F</a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Rhenium_trioxide_chloride" title="Rhenium trioxide chloride">ReO<sub class="template-chem2-sub">3</sub>Cl</a></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">OsOF<sub class="template-chem2-sub">5</sub></span> </td></tr> <tr> <td>8</td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">OsO<sub class="template-chem2-sub">2</sub>F<sub class="template-chem2-sub">4</sub></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">OsO<sub class="template-chem2-sub">3</sub>F<sub class="template-chem2-sub">2</sub></span> </td></tr></tbody></table> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Ta2OCl10_2-.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5a/Ta2OCl10_2-.svg/220px-Ta2OCl10_2-.svg.png" decoding="async" width="220" height="122" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/5a/Ta2OCl10_2-.svg/330px-Ta2OCl10_2-.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/5a/Ta2OCl10_2-.svg/440px-Ta2OCl10_2-.svg.png 2x" data-file-width="164" data-file-height="91" /></a><figcaption>Structure of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[Ta<sub class="template-chem2-sub">2</sub>OCl<sub class="template-chem2-sub">10</sub>]<sup>2−</sup></span>. Ru, Os form similar complexes.</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Agteflate.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/67/Agteflate.png/220px-Agteflate.png" decoding="async" width="220" height="207" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/67/Agteflate.png/330px-Agteflate.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/67/Agteflate.png/440px-Agteflate.png 2x" data-file-width="772" data-file-height="725" /></a><figcaption><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[AgOTeF<sub class="template-chem2-sub">5</sub>-(C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">5</sub>CH<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">2</sub>]<sub class="template-chem2-sub">2</sub></span> molecule.<sup id="cite_ref-r2_17-0" class="reference"><a href="#cite_note-r2-17"><span class="cite-bracket">[</span>17<span class="cite-bracket">]</span></a></sup> (Hydrogen atoms not shown.) <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:black; color:white;"> </span> Carbon (C)</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:lime; color:black;"> </span> Fluorine (F)</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:red; color:black;"> </span> Oxygen (O)</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:#b8860b; color:black;"> </span> Tellurium (Te)</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r981673959"><div class="legend"><span class="legend-color mw-no-invert" style="background-color:gray; color:black;"> </span> Silver (Ag)</div></figcaption></figure> <p>High oxidation states of the metal are dictated by the fact that <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> is a strong <a href="/wiki/Oxidizing_agent" title="Oxidizing agent">oxidizing agent</a>, as is <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>. <a href="/wiki/Bromine" title="Bromine">Bromine</a> and <a href="/wiki/Iodine" title="Iodine">iodine</a> are relatively weak oxidizing agents, so fewer oxobromides and oxoiodides are known. Structures for compounds with d<sup>0</sup> configuration are predicted by <a href="/wiki/VSEPR_theory" title="VSEPR theory">VSEPR theory</a>. Thus, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">CrO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></span> is <a href="/wiki/Tetrahedral" class="mw-redirect" title="Tetrahedral">tetrahedral</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">OsO<sub class="template-chem2-sub">3</sub>F<sub class="template-chem2-sub">2</sub></span> is <a href="/wiki/Trigonal_bipyramid" class="mw-redirect" title="Trigonal bipyramid">trigonal bipyramidal</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">XeOF<sub class="template-chem2-sub">4</sub></span> is <a href="/wiki/Square_pyramid" title="Square pyramid">square pyramidal</a> and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">OsOF<sub class="template-chem2-sub">5</sub></span> is <a href="/wiki/Octahedral" class="mw-redirect" title="Octahedral">octahedral</a>.<sup id="cite_ref-18" class="reference"><a href="#cite_note-18"><span class="cite-bracket">[</span>18<span class="cite-bracket">]</span></a></sup> The d<sup>1</sup> complex <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">ReOCl<sub class="template-chem2-sub">4</sub></span> is square pyramidal. </p><p>The compounds <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[Ta<sub class="template-chem2-sub">2</sub>OX<sub class="template-chem2-sub">10</sub>]<sup>2−</sup></span> and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[M<sub class="template-chem2-sub">2</sub>OCl<sub class="template-chem2-sub">10</sub>]<sup>4−</sup></span> (M = W, Ru, Os) have two <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">MX<sub class="template-chem2-sub">5</sub></span> groups joined by a bridging oxygen atom.<sup id="cite_ref-19" class="reference"><a href="#cite_note-19"><span class="cite-bracket">[</span>19<span class="cite-bracket">]</span></a></sup> Each metal has an octahedral environment. The unusual linear <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">M−O−M</span> structure can be rationalized in terms of <a href="/wiki/Molecular_orbital" title="Molecular orbital">molecular orbital</a> theory, indicating the presence of d<sub>π</sub> — p<sub>π</sub> bonding between the metal and oxygen atoms.<sup id="cite_ref-20" class="reference"><a href="#cite_note-20"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup> Oxygen bridges are present in more complex configurations like <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">M(cp)<sub class="template-chem2-sub">2</sub>(OTeF<sub class="template-chem2-sub">5</sub>)<sub class="template-chem2-sub">2</sub></span> (M = Ti, Zr, Hf, Mo or W; cp = <a href="/wiki/Cyclopentadienyl_complex" title="Cyclopentadienyl complex">cyclopentadienyl</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">η<sup>5</sup>-C<sub class="template-chem2-sub">5</sub>H<sub class="template-chem2-sub">5</sub></span>)<sup id="cite_ref-r1_21-0" class="reference"><a href="#cite_note-r1-21"><span class="cite-bracket">[</span>21<span class="cite-bracket">]</span></a></sup> or <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[AgOTeF<sub class="template-chem2-sub">5</sub>-(C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">5</sub>CH<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">2</sub>]<sub class="template-chem2-sub">2</sub></span>.<sup id="cite_ref-r2_17-1" class="reference"><a href="#cite_note-r2-17"><span class="cite-bracket">[</span>17<span class="cite-bracket">]</span></a></sup> </p><p>In the <a href="/wiki/Actinide" title="Actinide">actinide</a> series, <a href="/wiki/Uranyl" title="Uranyl">uranyl</a> compounds such as <a href="/wiki/Uranyl_chloride" title="Uranyl chloride">uranyl chloride</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">UO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></span>) and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[UO<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">4</sub>]<sup>2−</sup></span> are well known and contain the linear <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">UO<sub class="template-chem2-sub">2</sub></span> moiety. Similar species exist for <a href="/wiki/Neptunium" title="Neptunium">neptunium</a> and <a href="/wiki/Plutonium" title="Plutonium">plutonium</a>. The species <a href="/wiki/Uranyl_fluoride" title="Uranyl fluoride">uranyl fluoride</a> is a complicating contaminant in samples <a href="/wiki/Uranium_hexafluoride" title="Uranium hexafluoride">uranium hexafluoride</a>. </p> <div class="mw-heading mw-heading2"><h2 id="Minerals_and_ionic_compounds">Minerals and ionic compounds</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=10" title="Edit section: Minerals and ionic compounds"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:MatlockiteStructure.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d8/MatlockiteStructure.png/220px-MatlockiteStructure.png" decoding="async" width="220" height="190" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d8/MatlockiteStructure.png/330px-MatlockiteStructure.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d8/MatlockiteStructure.png/440px-MatlockiteStructure.png 2x" data-file-width="1047" data-file-height="904" /></a><figcaption>Crystal structure of bismoclite. Colours: red – O, green – Cl, grey – Bi.</figcaption></figure> <p><a href="/wiki/Bismuth_oxychloride" title="Bismuth oxychloride">Bismuth oxochloride</a> (BiOCl, <a href="/wiki/Bismoclite" title="Bismoclite">bismoclite</a>) is a rare example of a mineral oxohalide. The <a href="/wiki/Crystal_structure" title="Crystal structure">crystal structure</a> has a <a href="/wiki/Tetragonal" class="mw-redirect" title="Tetragonal">tetragonal</a> symmetry and can be thought of as consisting of layers of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Cl<sup class="template-chem2-sup">−</sup></span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Bi<sup>3+</sup></span> and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">O<sup>2−</sup></span> ions, in the order Cl-Bi-O-Bi-Cl-Cl-Bi-O-Bi-Cl. This layered, graphite-like structure results in a relatively low hardness of bismoclite (<a href="/wiki/Mohs_scale_of_mineral_hardness" class="mw-redirect" title="Mohs scale of mineral hardness">Mohs</a> 2–2.5) and most other oxohalide minerals.<sup id="cite_ref-handbook_22-0" class="reference"><a href="#cite_note-handbook-22"><span class="cite-bracket">[</span>22<span class="cite-bracket">]</span></a></sup> Those other minerals include <a href="/wiki/Terlinguaite" title="Terlinguaite">terlinguaite</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Hg<sub class="template-chem2-sub">2</sub>OCl</span>, formed by the weathering of mercury-containing minerals.<sup id="cite_ref-23" class="reference"><a href="#cite_note-23"><span class="cite-bracket">[</span>23<span class="cite-bracket">]</span></a></sup> <a href="/wiki/Mendipite" title="Mendipite">Mendipite</a>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Pb<sub class="template-chem2-sub">3</sub>O<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">2</sub></span>, formed from an original deposit of <a href="/wiki/Lead(II)_sulfide" title="Lead(II) sulfide">lead sulfide</a> in a number of stages is another example of a secondary oxohalide mineral. </p><p>The elements <a href="/wiki/Iron" title="Iron">iron</a>, <a href="/wiki/Antimony" title="Antimony">antimony</a>, <a href="/wiki/Bismuth" title="Bismuth">bismuth</a> and <a href="/wiki/Lanthanum" title="Lanthanum">lanthanum</a> form oxochlorides of general formula MOCl. MOBr and MOI are also known for Sb and Bi. Many of their crystal structures have been determined.<sup id="cite_ref-24" class="reference"><a href="#cite_note-24"><span class="cite-bracket">[</span>24<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=11" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><a href="/wiki/Transition_metal_oxo_complex" title="Transition metal oxo complex">Transition metal oxo complex</a></li></ul> <div class="mw-heading mw-heading2"><h2 id="References">References</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=12" title="Edit section: References"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></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 reflist-columns references-column-width" style="column-width: 30em;"> <ol class="references"> <li id="cite_note-1"><span class="mw-cite-backlink"><b><a href="#cite_ref-1">^</a></b></span> <span class="reference-text">Synthesis of individual compounds can be found in Housecroft & Sharpe and Greenwood & Earnshaw in sections relating to the specific element, A</span> </li> <li id="cite_note-2"><span class="mw-cite-backlink"><b><a href="#cite_ref-2">^</a></b></span> <span class="reference-text">Sisler, H. H. "Chromyl Chloride" <i>Inorganic Synthesis</i> McGraw-Hill: New York, 1946; Vol. 2, pp. 205–207.</span> </li> <li id="cite_note-3"><span class="mw-cite-backlink"><b><a href="#cite_ref-3">^</a></b></span> <span class="reference-text">Greenwood & Earnshaw, p. 1023</span> </li> <li id="cite_note-4"><span class="mw-cite-backlink"><b><a href="#cite_ref-4">^</a></b></span> <span class="reference-text">Greenwood & Earnshaw, p. 996.</span> </li> <li id="cite_note-Nakamoto-5"><span class="mw-cite-backlink"><b><a href="#cite_ref-Nakamoto_5-0">^</a></b></span> <span class="reference-text">K. Nakamoto <i>Infrared and Raman spectra of inorganic and coordination compounds</i>, 5th. edition, Part A, Wiley, 1997 <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><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-471-19406-9" title="Special:BookSources/0-471-19406-9">0-471-19406-9</a>, Tables II-4c, II-6g, II-6h, II-7b, II-8c</span> </li> <li id="cite_note-6"><span class="mw-cite-backlink"><b><a href="#cite_ref-6">^</a></b></span> <span class="reference-text">Shriver & Atkins, Figure 13.8, p. 447</span> </li> <li id="cite_note-7"><span class="mw-cite-backlink"><b><a href="#cite_ref-7">^</a></b></span> <span class="reference-text">Shriver & Atkins, p. 358</span> </li> <li id="cite_note-8"><span class="mw-cite-backlink"><b><a href="#cite_ref-8">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMargraveSharpWilson1969" class="citation journal cs1">Margrave, J. L.; Sharp, K. G.; Wilson, P. W. (9 September 1969). "Silicon-Fluorine Chemistry IX: The Reactions of Silicon Difluoride and Silicon Tetrafluoride with Water and Some Reactions of Tetrafluorodisiloxane". <i>Journal of the American Chemical Society</i>. <b>92</b> (6) (published 25 March 1970). <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1021%2Fja00709a015">10.1021/ja00709a015</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+of+the+American+Chemical+Society&rft.atitle=Silicon-Fluorine+Chemistry+IX%3A+The+Reactions+of+Silicon+Difluoride+and+Silicon+Tetrafluoride+with+Water+and+Some+Reactions+of+Tetrafluorodisiloxane&rft.volume=92&rft.issue=6&rft.date=1969-09-09&rft_id=info%3Adoi%2F10.1021%2Fja00709a015&rft.aulast=Margrave&rft.aufirst=J.+L.&rft.au=Sharp%2C+K.+G.&rft.au=Wilson%2C+P.+W.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-9"><span class="mw-cite-backlink"><b><a href="#cite_ref-9">^</a></b></span> <span class="reference-text">Housecroft & Sharpe, pp. 329–330</span> </li> <li id="cite_note-10"><span class="mw-cite-backlink"><b><a href="#cite_ref-10">^</a></b></span> <span class="reference-text">Housecroft & Sharpe, pp. 365–367</span> </li> <li id="cite_note-s397-11"><span class="mw-cite-backlink">^ <a href="#cite_ref-s397_11-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-s397_11-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text">Shriver & Atkins, p. 397</span> </li> <li id="cite_note-r3-12"><span class="mw-cite-backlink"><b><a href="#cite_ref-r3_12-0">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFOberhammerSeppelt1978" class="citation journal cs1">Oberhammer, Heinz; Seppelt, Konrad (1978). "Molecular Structure of F<sub>5</sub>SOSF<sub>5</sub>, F<sub>5</sub>SeOSeF<sub>5</sub>, and F<sub>5</sub>TeOTeF<sub>5</sub>: d-Orbital Participation in Bonds between Main Group Elements". <i>Angewandte Chemie International Edition</i>. <b>17</b> (1): 69–70. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2Fanie.197800691">10.1002/anie.197800691</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Angewandte+Chemie+International+Edition&rft.atitle=Molecular+Structure+of+F%3Csub%3E5%3C%2Fsub%3ESOSF%3Csub%3E5%3C%2Fsub%3E%2C+F%3Csub%3E5%3C%2Fsub%3ESeOSeF%3Csub%3E5%3C%2Fsub%3E%2C+and+F%3Csub%3E5%3C%2Fsub%3ETeOTeF%3Csub%3E5%3C%2Fsub%3E%3A+d-Orbital+Participation+in+Bonds+between+Main+Group+Elements&rft.volume=17&rft.issue=1&rft.pages=69-70&rft.date=1978&rft_id=info%3Adoi%2F10.1002%2Fanie.197800691&rft.aulast=Oberhammer&rft.aufirst=Heinz&rft.au=Seppelt%2C+Konrad&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-13"><span class="mw-cite-backlink"><b><a href="#cite_ref-13">^</a></b></span> <span class="reference-text">Housecroft & Sharpe, p. 395</span> </li> <li id="cite_note-14"><span class="mw-cite-backlink"><b><a href="#cite_ref-14">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFFouratiChaabouniBelinCharbonnel1986" class="citation journal cs1">Fourati, Mohieddine; Chaabouni, Moncef; Belin, Claude Henri; Charbonnel, Monique; Pascal, Jean Louis; Potier, Jacqueline (1986). "A strongly chelating bidentate CLO4. New synthesis route and crystal structure determination of Ti(CLO4)". <i>Inorg. Chem</i>. <b>25</b> (9): 1386–1390. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1021%2Fic00229a019">10.1021/ic00229a019</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Inorg.+Chem.&rft.atitle=A+strongly+chelating+bidentate+CLO4.+New+synthesis+route+and+crystal+structure+determination+of+Ti%28CLO4%29&rft.volume=25&rft.issue=9&rft.pages=1386-1390&rft.date=1986&rft_id=info%3Adoi%2F10.1021%2Fic00229a019&rft.aulast=Fourati&rft.aufirst=Mohieddine&rft.au=Chaabouni%2C+Moncef&rft.au=Belin%2C+Claude+Henri&rft.au=Charbonnel%2C+Monique&rft.au=Pascal%2C+Jean+Louis&rft.au=Potier%2C+Jacqueline&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-15"><span class="mw-cite-backlink"><b><a href="#cite_ref-15">^</a></b></span> <span class="reference-text">Greenwood & Earnshaw, Chapters 22–25, section halides and oxohalides</span> </li> <li id="cite_note-16"><span class="mw-cite-backlink"><b><a href="#cite_ref-16">^</a></b></span> <span class="reference-text">Greenwood & Earnshaw p. 993.</span> </li> <li id="cite_note-r2-17"><span class="mw-cite-backlink">^ <a href="#cite_ref-r2_17-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-r2_17-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFStraussNoirotAnderson1985" class="citation journal cs1">Strauss, Steven H.; Noirot, Mark D.; Anderson, Oren P. (1985). "Preparation and characterization of silver(I) teflate complexes: bridging OTeF<sub>5</sub> groups in the solid state and in solution". <i>Inorg. Chem</i>. <b>24</b> (25): 4307–4311. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1021%2Fic00219a022">10.1021/ic00219a022</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Inorg.+Chem.&rft.atitle=Preparation+and+characterization+of+silver%28I%29+teflate+complexes%3A+bridging+OTeF%3Csub%3E5%3C%2Fsub%3E+groups+in+the+solid+state+and+in+solution&rft.volume=24&rft.issue=25&rft.pages=4307-4311&rft.date=1985&rft_id=info%3Adoi%2F10.1021%2Fic00219a022&rft.aulast=Strauss&rft.aufirst=Steven+H.&rft.au=Noirot%2C+Mark+D.&rft.au=Anderson%2C+Oren+P.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-18"><span class="mw-cite-backlink"><b><a href="#cite_ref-18">^</a></b></span> <span class="reference-text">Housectroft & Sharpe, Chapters 21 and 22 illustrate many structures, including M-O and M-Cl bond lengths.</span> </li> <li id="cite_note-19"><span class="mw-cite-backlink"><b><a href="#cite_ref-19">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFDewanEdwards,_Anthony_J.;_Calves,_Jean_Y.;_Guerchais,_Jacques_E.1997" class="citation journal cs1">Dewan, John. C.; Edwards, Anthony J.; Calves, Jean Y.; Guerchais, Jacques E. (1997). "Fluoride crystal structures. Part 28. Bis(tetraethylammonium)μ-oxo-bis[pentafluorotantalate(V)]". <i>J. Chem. Soc., Dalton Trans.</i> (10): 978–980. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1039%2FDT9770000978">10.1039/DT9770000978</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J.+Chem.+Soc.%2C+Dalton+Trans.&rft.atitle=Fluoride+crystal+structures.+Part+28.+Bis%28tetraethylammonium%29%CE%BC-oxo-bis%5Bpentafluorotantalate%28V%29%5D&rft.issue=10&rft.pages=978-980&rft.date=1997&rft_id=info%3Adoi%2F10.1039%2FDT9770000978&rft.aulast=Dewan&rft.aufirst=John.+C.&rft.au=Edwards%2C+Anthony+J.%3B+Calves%2C+Jean+Y.%3B+Guerchais%2C+Jacques+E.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span><span class="cs1-maint citation-comment"><code class="cs1-code">{{<a href="/wiki/Template:Cite_journal" title="Template:Cite journal">cite journal</a>}}</code>: CS1 maint: multiple names: authors list (<a href="/wiki/Category:CS1_maint:_multiple_names:_authors_list" title="Category:CS1 maint: multiple names: authors list">link</a>)</span>. The structure is illustrated in Housectroft & Sharpe, Figure 22.5.</span> </li> <li id="cite_note-20"><span class="mw-cite-backlink"><b><a href="#cite_ref-20">^</a></b></span> <span class="reference-text">Housectroft & Sharpe, Figure 22.15.</span> </li> <li id="cite_note-r1-21"><span class="mw-cite-backlink"><b><a href="#cite_ref-r1_21-0">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFCrossmanHopeSaunders1996" class="citation journal cs1">Crossman, Martin C.; Hope, Eric G.; Saunders, Graham C. (1996). "Cyclopentadienyl metal teflate (OTeF<sub>5</sub>) complexes". <i>J. Chem. Soc., Dalton Trans.</i> (4): 509–511. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1039%2FDT9960000509">10.1039/DT9960000509</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J.+Chem.+Soc.%2C+Dalton+Trans.&rft.atitle=Cyclopentadienyl+metal+teflate+%28OTeF%3Csub%3E5%3C%2Fsub%3E%29+complexes&rft.issue=4&rft.pages=509-511&rft.date=1996&rft_id=info%3Adoi%2F10.1039%2FDT9960000509&rft.aulast=Crossman&rft.aufirst=Martin+C.&rft.au=Hope%2C+Eric+G.&rft.au=Saunders%2C+Graham+C.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-handbook-22"><span class="mw-cite-backlink"><b><a href="#cite_ref-handbook_22-0">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFAnthony,_John_W.Bideaux,_Richard_A.Bladh,_Kenneth_W.Nichols,_Monte_C." class="citation book cs1 cs1-prop-long-vol">Anthony, John W.; Bideaux, Richard A.; Bladh, Kenneth W.; Nichols, Monte C. (eds.). "Bismoclite". <a rel="nofollow" class="external text" href="http://rruff.geo.arizona.edu/doclib/hom/bismoclite.pdf"><i>Handbook of Mineralogy</i></a> <span class="cs1-format">(PDF)</span>. Vol. III (Halides, Hydroxides, Oxides). Chantilly, VA: Mineralogical Society of America. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-9622097-2-4" title="Special:BookSources/0-9622097-2-4"><bdi>0-9622097-2-4</bdi></a><span class="reference-accessdate">. Retrieved <span class="nowrap">December 5,</span> 2011</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Bismoclite&rft.btitle=Handbook+of+Mineralogy&rft.place=Chantilly%2C+VA&rft.pub=Mineralogical+Society+of+America&rft.isbn=0-9622097-2-4&rft_id=http%3A%2F%2Frruff.geo.arizona.edu%2Fdoclib%2Fhom%2Fbismoclite.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-23"><span class="mw-cite-backlink"><b><a href="#cite_ref-23">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFHillebrandW._T._Schaller1907" class="citation journal cs1 cs1-prop-long-vol">Hillebrand, W. F.; W. T. Schaller (1907). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=qRTSAAAAMAAJ&pg=PA259">"Art. XXVI. <i>The Mercury Minerals from Terlingua, Texas: Kleinite, Terlinguaite, Eglestonite, Montroydite, Calomel, Mercury</i>"</a>. <i>The American Journal of Science</i>. s4-24 (139): 259–274. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.2475%2Fajs.s4-24.141.259">10.2475/ajs.s4-24.141.259</a><span class="reference-accessdate">. Retrieved <span class="nowrap">2009-05-21</span></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=The+American+Journal+of+Science&rft.atitle=Art.+XXVI.+The+Mercury+Minerals+from+Terlingua%2C+Texas%3A+Kleinite%2C+Terlinguaite%2C+Eglestonite%2C+Montroydite%2C+Calomel%2C+Mercury&rft.volume=s4-24&rft.issue=139&rft.pages=259-274&rft.date=1907&rft_id=info%3Adoi%2F10.2475%2Fajs.s4-24.141.259&rft.aulast=Hillebrand&rft.aufirst=W.+F.&rft.au=W.+T.+Schaller&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DqRTSAAAAMAAJ%26pg%3DPA259&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span></span> </li> <li id="cite_note-24"><span class="mw-cite-backlink"><b><a href="#cite_ref-24">^</a></b></span> <span class="reference-text">Wells, pp. 390–392</span> </li> </ol></div> <div class="mw-heading mw-heading2"><h2 id="Bibliography">Bibliography</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Oxohalide&action=edit&section=13" title="Edit section: Bibliography"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1235681985">.mw-parser-output .side-box{margin:4px 0;box-sizing:border-box;border:1px solid #aaa;font-size:88%;line-height:1.25em;background-color:var(--background-color-interactive-subtle,#f8f9fa);display:flow-root}.mw-parser-output .side-box-abovebelow,.mw-parser-output .side-box-text{padding:0.25em 0.9em}.mw-parser-output .side-box-image{padding:2px 0 2px 0.9em;text-align:center}.mw-parser-output .side-box-imageright{padding:2px 0.9em 2px 0;text-align:center}@media(min-width:500px){.mw-parser-output .side-box-flex{display:flex;align-items:center}.mw-parser-output .side-box-text{flex:1;min-width:0}}@media(min-width:720px){.mw-parser-output .side-box{width:238px}.mw-parser-output .side-box-right{clear:right;float:right;margin-left:1em}.mw-parser-output .side-box-left{margin-right:1em}}</style><style data-mw-deduplicate="TemplateStyles:r1237033735">@media print{body.ns-0 .mw-parser-output .sistersitebox{display:none!important}}@media screen{html.skin-theme-clientpref-night .mw-parser-output .sistersitebox img[src*="Wiktionary-logo-en-v2.svg"]{background-color:white}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .sistersitebox img[src*="Wiktionary-logo-en-v2.svg"]{background-color:white}}</style><div class="side-box side-box-right plainlinks sistersitebox"><style data-mw-deduplicate="TemplateStyles:r1126788409">.mw-parser-output .plainlist ol,.mw-parser-output .plainlist ul{line-height:inherit;list-style:none;margin:0;padding:0}.mw-parser-output .plainlist ol li,.mw-parser-output .plainlist ul li{margin-bottom:0}</style> <div class="side-box-flex"> <div class="side-box-image"><span class="noviewer" typeof="mw:File"><span><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/30px-Commons-logo.svg.png" decoding="async" width="30" height="40" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/45px-Commons-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/59px-Commons-logo.svg.png 2x" data-file-width="1024" data-file-height="1376" /></span></span></div> <div class="side-box-text plainlist">Wikimedia Commons has media related to <span style="font-weight: bold; font-style: italic;"><a href="https://commons.wikimedia.org/wiki/Category:Oxohalides" class="extiw" title="commons:Category:Oxohalides">Oxohalides</a></span>.</div></div> </div> <ul><li><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). <i>Chemistry of the Elements</i> (2nd ed.). <a href="/wiki/Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. <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.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%3AOxohalide" class="Z3988"></span></li> <li>Housecroft, C. E. and Sharpe, A. G. <i>Inorganic Chemistry</i>, 2nd ed., Pearson Prentice-Hall 2005. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-582-31080-6" title="Special:BookSources/0-582-31080-6">0-582-31080-6</a></li> <li>Shrivr, D. F. and Atkins, P. W. <i>Inorganic Chemistry</i>, 3rd edn. Oxford University Press, 1999. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-19-850330-X" title="Special:BookSources/0-19-850330-X">0-19-850330-X</a></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWells1962" class="citation book cs1">Wells, A. F. (1962). <i>Structural Inorganic Chemistry</i> (3rd ed.). Oxford: Clarendon Press. pp. 384–392. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-19-855125-8" title="Special:BookSources/0-19-855125-8"><bdi>0-19-855125-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Structural+Inorganic+Chemistry&rft.place=Oxford&rft.pages=384-392&rft.edition=3rd&rft.pub=Clarendon+Press&rft.date=1962&rft.isbn=0-19-855125-8&rft.aulast=Wells&rft.aufirst=A.+F.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AOxohalide" class="Z3988"></span>.</li></ul>    </div><noscript><img src="https://login.wikimedia.org/wiki/Special:CentralAutoLogin/start?type=1x1" alt="" width="1" height="1" style="border: none; position: absolute;"></noscript> <div class="printfooter" data-nosnippet="">Retrieved from "<a dir="ltr" href="https://en.wikipedia.org/w/index.php?title=Oxohalide&oldid=1246876379">https://en.wikipedia.org/w/index.php?title=Oxohalide&oldid=1246876379</a>"</div></div> <div id="catlinks" class="catlinks" data-mw="interface"><div id="mw-normal-catlinks" class="mw-normal-catlinks"><a href="/wiki/Help:Category" title="Help:Category">Category</a>: <ul><li><a href="/wiki/Category:Oxohalides" title="Category:Oxohalides">Oxohalides</a></li></ul></div><div id="mw-hidden-catlinks" class="mw-hidden-catlinks mw-hidden-cats-hidden">Hidden categories: <ul><li><a href="/wiki/Category:CS1_maint:_multiple_names:_authors_list" title="Category:CS1 maint: multiple names: authors list">CS1 maint: multiple names: authors list</a></li><li><a href="/wiki/Category:CS1:_long_volume_value" title="Category:CS1: long volume value">CS1: long volume value</a></li><li><a href="/wiki/Category:Articles_with_short_description" title="Category:Articles with short description">Articles with short description</a></li><li><a href="/wiki/Category:Short_description_is_different_from_Wikidata" title="Category:Short description is different from Wikidata">Short description is different from Wikidata</a></li><li><a href="/wiki/Category:Commons_category_link_is_on_Wikidata" title="Category:Commons category link is on Wikidata">Commons category link is on Wikidata</a></li></ul></div></div> </div> </main> </div> <div class="mw-footer-container"> <footer id="footer" class="mw-footer" > <ul id="footer-info"> <li id="footer-info-lastmod"> This page was last edited on 21 September 2024, at 16:12<span class="anonymous-show"> (UTC)</span>.</li> <li id="footer-info-copyright">Text is available under the <a href="/wiki/Wikipedia:Text_of_the_Creative_Commons_Attribution-ShareAlike_4.0_International_License" title="Wikipedia:Text of the Creative Commons Attribution-ShareAlike 4.0 International License">Creative Commons Attribution-ShareAlike 4.0 License</a>; additional terms may apply. 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