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<span>Oxygen compounds</span> </div> </a> <ul id="toc-Oxygen_compounds-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Boranes" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Boranes"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Boranes</span> </div> </a> <ul id="toc-Boranes-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Nitrides" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Nitrides"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Nitrides</span> </div> </a> <ul id="toc-Nitrides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organoboron_chemistry" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Organoboron_chemistry"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Organoboron chemistry</span> </div> </a> <ul id="toc-Organoboron_chemistry-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Compounds_of_B(I)_and_B(II)" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Compounds_of_B(I)_and_B(II)"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>Compounds of B(I) and B(II)</span> </div> </a> <ul id="toc-Compounds_of_B(I)_and_B(II)-sublist" class="vector-toc-list"> </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"> <span class="vector-toc-numb">7</span> <span>See also</span> </div> </a> <ul id="toc-See_also-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#References"> <div 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id="mw-content-subtitle"></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Boron-trifluoride-pi-bonding-2D.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Boron-trifluoride-pi-bonding-2D.png/110px-Boron-trifluoride-pi-bonding-2D.png" decoding="async" width="110" height="135" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Boron-trifluoride-pi-bonding-2D.png/165px-Boron-trifluoride-pi-bonding-2D.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Boron-trifluoride-pi-bonding-2D.png/220px-Boron-trifluoride-pi-bonding-2D.png 2x" data-file-width="893" data-file-height="1100" /></a><figcaption><a href="/wiki/Boron_trifluoride" title="Boron trifluoride">Boron (III) trifluoride</a> structure, showing "empty" boron p orbital in pi-type <a href="/wiki/Coordinate_covalent_bond" title="Coordinate covalent bond">coordinate covalent bonds</a></figcaption></figure> <p><b>Boron compounds</b> are compounds containing the element <a href="/wiki/Boron" title="Boron">boron</a>. In the most familiar compounds, boron has the formal oxidation state +3. These include oxides, sulfides, nitrides, and halides.<sup id="cite_ref-HollemanAF_1-0" class="reference"><a href="#cite_note-HollemanAF-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Halides">Halides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Boron_compounds&action=edit&section=1" title="Edit section: Halides"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The trihalides adopt a planar trigonal structure. These compounds are <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acids</a> in that they readily form <a href="/wiki/Adduct" title="Adduct">adducts</a> with electron-pair donors, which are called <a href="/wiki/Lewis_base" class="mw-redirect" title="Lewis base">Lewis bases</a>. For example, fluoride (F<sup>−</sup>) and <a href="/wiki/Boron_trifluoride" title="Boron trifluoride">boron trifluoride</a> (BF<sub>3</sub>) combined to give the <a href="/wiki/Tetrafluoroborate" title="Tetrafluoroborate">tetrafluoroborate</a> anion, BF<sub>4</sub><sup>−</sup>. Boron trifluoride is used in the petrochemical industry as a catalyst. The halides react with water to form <a href="/wiki/Boric_acid" title="Boric acid">boric acid</a>.<sup id="cite_ref-HollemanAF_1-1" class="reference"><a href="#cite_note-HollemanAF-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Oxygen_compounds">Oxygen compounds</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Boron_compounds&action=edit&section=2" title="Edit section: Oxygen compounds"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Boron is found in nature on Earth almost entirely as various oxides of B(III), often associated with other elements. More than one hundred <a href="/wiki/Borate_mineral" title="Borate mineral">borate minerals</a> contain boron in oxidation state +3. These minerals resemble <a href="/wiki/Silicate" title="Silicate">silicates</a> in some respect, although boron is often found not only in a tetrahedral coordination with oxygen, but also in a trigonal planar configuration. Unlike silicates, boron minerals never contain boron with coordination number greater than four. A typical motif is exemplified by the tetraborate anions of the common mineral <a href="/wiki/Borax" title="Borax">borax</a>, shown at left. The formal negative charge of the tetrahedral borate center is balanced by metal cations in the minerals, such as the sodium (Na<sup>+</sup>) in <a href="/wiki/Borax" title="Borax">borax</a>.<sup id="cite_ref-HollemanAF_1-2" class="reference"><a href="#cite_note-HollemanAF-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> The <a href="/w/index.php?title=Tourmaline_group&action=edit&redlink=1" class="new" title="Tourmaline group (page does not exist)">tourmaline group</a> of borate-silicates is also a very important boron-bearing mineral group, and a number of <a href="/wiki/Borosilicate" class="mw-redirect" title="Borosilicate">borosilicates</a> are also known to exist naturally.<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> <div class="mw-heading mw-heading2"><h2 id="Boranes">Boranes</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Boron_compounds&action=edit&section=3" title="Edit section: Boranes"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Boranes" title="Boranes">Boranes</a></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Deltahedral-borane-cluster-array-numbered-3D-bs-17.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Deltahedral-borane-cluster-array-numbered-3D-bs-17.png/220px-Deltahedral-borane-cluster-array-numbered-3D-bs-17.png" decoding="async" width="220" height="503" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Deltahedral-borane-cluster-array-numbered-3D-bs-17.png/330px-Deltahedral-borane-cluster-array-numbered-3D-bs-17.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Deltahedral-borane-cluster-array-numbered-3D-bs-17.png/440px-Deltahedral-borane-cluster-array-numbered-3D-bs-17.png 2x" data-file-width="3478" data-file-height="7958" /></a><figcaption><a href="/wiki/Ball-and-stick_model" title="Ball-and-stick model">Ball-and-stick models</a> showing the structures of the boron skeletons of <a href="/wiki/Boranes" title="Boranes">borane</a> <a href="/wiki/Atom_cluster" class="mw-redirect" title="Atom cluster">clusters</a>. The structures can be rationalised by <a href="/wiki/Polyhedral_skeletal_electron_pair_theory" title="Polyhedral skeletal electron pair theory">polyhedral skeletal electron pair theory</a>.<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></figcaption></figure> <p>Boranes are chemical compounds of boron and hydrogen, with the generic formula of B<sub>x</sub>H<sub>y</sub>. These compounds do not occur in nature. Many of the boranes readily oxidise on contact with air, some violently. The parent member BH<sub>3</sub> is called <a href="/wiki/Borane" title="Borane">borane</a>, but it is known only in the gaseous state, and <a href="/wiki/Dimer_(chemistry)" class="mw-redirect" title="Dimer (chemistry)">dimerises</a> to form <a href="/wiki/Diborane" title="Diborane">diborane</a>, B<sub>2</sub>H<sub>6</sub>. The larger boranes all consist of boron clusters that are polyhedral, some of which exist as isomers. For example, isomers of B<sub>20</sub>H<sub>26</sub> are based on the fusion of two 10-atom clusters. </p><p>The most important boranes are diborane B<sub>2</sub>H<sub>6</sub> and two of its <a href="/w/index.php?title=Pyrolysis_product&action=edit&redlink=1" class="new" title="Pyrolysis product (page does not exist)">pyrolysis products</a>, <a href="/wiki/Pentaborane" title="Pentaborane">pentaborane</a> B<sub>5</sub>H<sub>9</sub> and <a href="/wiki/Decaborane" title="Decaborane">decaborane</a> B<sub>10</sub>H<sub>14</sub>. A large number of anionic boron hydrides are known, e.g. [B<sub>12</sub>H<sub>12</sub>]<sup>2−</sup>. </p><p>The formal <a href="/wiki/Oxidation_number" class="mw-redirect" title="Oxidation number">oxidation number</a> in boranes is positive, and is based on the assumption that hydrogen is counted as −1 as in active metal hydrides. The mean oxidation number for the boron atoms is then simply the ratio of hydrogen to boron in the molecule. For example, in diborane B<sub>2</sub>H<sub>6</sub>, the boron oxidation state is +3, but in decaborane B<sub>10</sub>H<sub>14</sub>, it is <sup>7</sup>/<sub>5</sub> or +1.4. In these compounds the oxidation state of boron is often not a whole number. </p> <div class="mw-heading mw-heading2"><h2 id="Nitrides">Nitrides</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Boron_compounds&action=edit&section=4" title="Edit section: Nitrides"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></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/Boron_nitride" title="Boron nitride">Boron nitride</a></div> <p>The <a href="/wiki/Boron_nitride" title="Boron nitride">boron nitrides</a> are notable for the variety of structures that they adopt. They exhibit structures analogous to various <a href="/wiki/Allotropes_of_carbon" title="Allotropes of carbon">allotropes of carbon</a>, including graphite, diamond, and nanotubes. In the diamond-like structure, called cubic boron nitride (tradename <a href="/wiki/Borazon" title="Borazon">Borazon</a>), boron atoms exist in the tetrahedral structure of carbon atoms in diamond, but one in every four B-N bonds can be viewed as a <a href="/wiki/Coordinate_covalent_bond" title="Coordinate covalent bond">coordinate covalent bond</a>, wherein two electrons are donated by the nitrogen atom which acts as the <a href="/wiki/Lewis_base" class="mw-redirect" title="Lewis base">Lewis base</a> to a bond to the <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acidic</a> boron(III) centre. Cubic boron nitride, among other applications, is used as an abrasive, as it has a hardness comparable with diamond (the two substances are able to produce scratches on each other). In the BN compound analogue of graphite, hexagonal boron nitride (h-BN), the positively charged boron and negatively charged nitrogen atoms in each plane lie adjacent to the oppositely charged atom in the next plane. Consequently, graphite and h-BN have very different properties, although both are lubricants, as these planes slip past each other easily. However, h-BN is a relatively poor electrical and thermal conductor in the planar directions.<sup id="cite_ref-dkg_4-0" class="reference"><a href="#cite_note-dkg-4"><span class="cite-bracket">[</span>4<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-b1_5-0" class="reference"><a href="#cite_note-b1-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Organoboron_chemistry">Organoboron chemistry</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Boron_compounds&action=edit&section=5" title="Edit section: Organoboron chemistry"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></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/Organoboron_chemistry" title="Organoboron chemistry">Organoboron chemistry</a></div> <p>A large number of organoboron compounds are known and many are useful in <a href="/wiki/Organic_synthesis" title="Organic synthesis">organic synthesis</a>. Many are produced from <a href="/wiki/Hydroboration%E2%80%93oxidation_reaction" title="Hydroboration–oxidation reaction">hydroboration</a>, which employs <a href="/wiki/Diborane" title="Diborane">diborane</a>, B<sub>2</sub>H<sub>6</sub>, a simple <a href="/wiki/Borane" title="Borane">borane</a> chemical. Organoboron(III) compounds are usually tetrahedral or trigonal planar, for example, <a href="/wiki/Tetraphenylborate" title="Tetraphenylborate">tetraphenylborate</a>, [B(C<sub>6</sub>H<sub>5</sub>)<sub>4</sub>]<sup>−</sup> vs. <a href="/wiki/Triphenylborane" title="Triphenylborane">triphenylborane</a>, B(C<sub>6</sub>H<sub>5</sub>)<sub>3</sub>. However, multiple boron atoms reacting with each other have a tendency to form novel dodecahedral (12-sided) and icosahedral (20-sided) structures composed completely of boron atoms, or with varying numbers of carbon heteroatoms. </p><p>Organoboron chemicals have been employed in uses as diverse as <a href="/wiki/Boron_carbide" title="Boron carbide">boron carbide</a> (see below), a complex very hard ceramic composed of boron-carbon cluster anions and cations, to <a href="/wiki/Carborane" title="Carborane">carboranes</a>, carbon-boron <a href="/wiki/Cluster_chemistry" class="mw-redirect" title="Cluster chemistry">cluster chemistry</a> compounds that can be halogenated to form reactive structures including <a href="/wiki/Carborane_acid" title="Carborane acid">carborane acid</a>, a <a href="/wiki/Superacid" title="Superacid">superacid</a>. As one example, carboranes form useful molecular moieties that add considerable amounts of boron to other biochemicals in order to synthesize boron-containing compounds for <a href="/wiki/Boron_neutron_capture_therapy" class="mw-redirect" title="Boron neutron capture therapy">boron neutron capture therapy</a> for cancer. </p> <div class="mw-heading mw-heading2"><h2 id="Compounds_of_B(I)_and_B(II)"><span id="Compounds_of_B.28I.29_and_B.28II.29"></span>Compounds of B(I) and B(II)</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Boron_compounds&action=edit&section=6" title="Edit section: Compounds of B(I) and B(II)"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>As anticipated by its <a href="/wiki/Boron_hydride" class="mw-redirect" title="Boron hydride">hydride clusters</a>, boron forms a variety of stable compounds with formal oxidation state less than three. <a href="/wiki/Diboron_tetrafluoride" title="Diboron tetrafluoride">B<sub>2</sub>F<sub>4</sub></a> and B<sub>4</sub>Cl<sub>4</sub> are well characterized.<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 class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Magnesium-diboride-3D-balls.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d2/Magnesium-diboride-3D-balls.png/220px-Magnesium-diboride-3D-balls.png" decoding="async" width="220" height="159" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d2/Magnesium-diboride-3D-balls.png/330px-Magnesium-diboride-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d2/Magnesium-diboride-3D-balls.png/440px-Magnesium-diboride-3D-balls.png 2x" data-file-width="1100" data-file-height="793" /></a><figcaption>Ball-and-stick model of superconductor magnesium diboride. Boron atoms lie in hexagonal aromatic graphite-like layers, with a charge of −1 on each boron atom. Magnesium(II) ions lie between layers</figcaption></figure> <p>Binary metal-boron compounds, the metal borides, contain boron in negative oxidation states. Illustrative is <a href="/wiki/Magnesium_diboride" title="Magnesium diboride">magnesium diboride</a> (MgB<sub>2</sub>). Each boron atom has a formal −1 charge and magnesium is assigned a formal charge of +2. In this material, the boron centers are trigonal planar with an extra double bond for each boron, forming sheets akin to the carbon in <a href="/wiki/Graphite" title="Graphite">graphite</a>. However, unlike hexagonal boron nitride, which lacks electrons in the plane of the covalent atoms, the delocalized electrons in magnesium diboride allow it to conduct electricity similar to isoelectronic graphite. In 2001, this material was found to be a high-temperature <a href="/wiki/Superconductor" class="mw-redirect" title="Superconductor">superconductor</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><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> It is a superconductor under active development. A project at <a href="/wiki/CERN" title="CERN">CERN</a> to make MgB<sub>2</sub> cables has resulted in superconducting test cables able to carry 20,000 amperes for extremely high current distribution applications, such as the contemplated high luminosity version of the <a href="/wiki/Large_hadron_collider" class="mw-redirect" title="Large hadron collider">large hadron collider</a>.<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><p>Certain other metal borides find specialized applications as hard materials for cutting tools.<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> Often the boron in borides has fractional oxidation states, such as −1/3 in <a href="/wiki/Calcium_hexaboride" title="Calcium hexaboride">calcium hexaboride</a> (CaB<sub>6</sub>). </p><p>From the structural perspective, the most distinctive chemical compounds of boron are the hydrides. Included in this series are the cluster compounds <a href="/wiki/Dodecaborate" title="Dodecaborate">dodecaborate</a> (<span class="chemf nowrap">B<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">12</sub></span></span>H<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">2−</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">12</sub></span></span></span>), <a href="/wiki/Decaborane" title="Decaborane">decaborane</a> (B<sub>10</sub>H<sub>14</sub>), and the <a href="/wiki/Carborane" title="Carborane">carboranes</a> such as C<sub>2</sub>B<sub>10</sub>H<sub>12</sub>. Characteristically such compounds contain boron with coordination numbers greater than four.<sup id="cite_ref-HollemanAF_1-3" class="reference"><a href="#cite_note-HollemanAF-1"><span class="cite-bracket">[</span>1<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=Boron_compounds&action=edit&section=7" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><a href="/wiki/Boranylium_ions" title="Boranylium ions">Boranylium ions</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=Boron_compounds&action=edit&section=8" 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"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-HollemanAF-1"><span class="mw-cite-backlink">^ <a href="#cite_ref-HollemanAF_1-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-HollemanAF_1-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-HollemanAF_1-2"><sup><i><b>c</b></i></sup></a> <a href="#cite_ref-HollemanAF_1-3"><sup><i><b>d</b></i></sup></a></span> <span class="reference-text"><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="CITEREFHollemanWibergWiberg1985" class="citation book cs1 cs1-prop-foreign-lang-source">Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). "Bor". <i>Lehrbuch der Anorganischen Chemie</i> (in German) (91–100 ed.). Walter de Gruyter. pp. 814–864. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3-11-007511-3" title="Special:BookSources/978-3-11-007511-3"><bdi>978-3-11-007511-3</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Bor&rft.btitle=Lehrbuch+der+Anorganischen+Chemie&rft.pages=814-864&rft.edition=91%E2%80%93100&rft.pub=Walter+de+Gruyter&rft.date=1985&rft.isbn=978-3-11-007511-3&rft.aulast=Holleman&rft.aufirst=Arnold+F.&rft.au=Wiberg%2C+Egon&rft.au=Wiberg%2C+Nils&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></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"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.mindat.org/">"Mindat.org - Mines, Minerals and More"</a>. <i>mindat.org</i>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20110422205859/http://www.mindat.org/">Archived</a> from the original on 22 April 2011<span class="reference-accessdate">. Retrieved <span class="nowrap">4 August</span> 2019</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=mindat.org&rft.atitle=Mindat.org+-+Mines%2C+Minerals+and+More&rft_id=https%3A%2F%2Fwww.mindat.org%2F&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></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"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWelch2013" class="citation journal cs1">Welch, Alan J. (2013). "The significance and impact of Wade's rules". <i>Chem. Commun</i>. <b>49</b> (35): 3615–3616. <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%2FC3CC00069A">10.1039/C3CC00069A</a>. <a href="/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/23535980">23535980</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chem.+Commun.&rft.atitle=The+significance+and+impact+of+Wade%27s+rules&rft.volume=49&rft.issue=35&rft.pages=3615-3616&rft.date=2013&rft_id=info%3Adoi%2F10.1039%2FC3CC00069A&rft_id=info%3Apmid%2F23535980&rft.aulast=Welch&rft.aufirst=Alan+J.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></span> </li> <li id="cite_note-dkg-4"><span class="mw-cite-backlink"><b><a href="#cite_ref-dkg_4-0">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFEngler,_M.2007" class="citation journal cs1">Engler, M. (2007). <a rel="nofollow" class="external text" href="http://www.esk.com/uploads/tx_userjspresseveroeff/PR_0712_CFI_12-2007_Hexagonales-BN_e_01.pdf">"Hexagonal Boron Nitride (hBN) – Applications from Metallurgy to Cosmetics"</a> <span class="cs1-format">(PDF)</span>. <i>Cfi/Ber. DKG</i>. <b>84</b>: D25. <a href="/wiki/ISSN_(identifier)" class="mw-redirect" title="ISSN (identifier)">ISSN</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/issn/0173-9913">0173-9913</a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20130613174727/http://www.esk.com/uploads/tx_userjspresseveroeff/PR_0712_CFI_12-2007_Hexagonales-BN_e_01.pdf">Archived</a> <span class="cs1-format">(PDF)</span> from the original on 13 June 2013<span class="reference-accessdate">. Retrieved <span class="nowrap">8 January</span> 2012</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Cfi%2FBer.+DKG&rft.atitle=Hexagonal+Boron+Nitride+%28hBN%29+%E2%80%93+Applications+from+Metallurgy+to+Cosmetics&rft.volume=84&rft.pages=D25&rft.date=2007&rft.issn=0173-9913&rft.au=Engler%2C+M.&rft_id=http%3A%2F%2Fwww.esk.com%2Fuploads%2Ftx_userjspresseveroeff%2FPR_0712_CFI_12-2007_Hexagonales-BN_e_01.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></span> </li> <li id="cite_note-b1-5"><span class="mw-cite-backlink"><b><a href="#cite_ref-b1_5-0">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGreim,_JochenSchwetz,_Karl_A.2005" class="citation book cs1">Greim, Jochen & Schwetz, Karl A. (2005). "Boron Carbide, Boron Nitride, and Metal Borides". <i>Boron Carbide, Boron Nitride, and Metal Borides, in Ullmann's Encyclopedia of Industrial Chemistry</i>. Wiley-VCH: Weinheim. <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%2F14356007.a04_295.pub2">10.1002/14356007.a04_295.pub2</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3527306732" title="Special:BookSources/978-3527306732"><bdi>978-3527306732</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Boron+Carbide%2C+Boron+Nitride%2C+and+Metal+Borides&rft.btitle=Boron+Carbide%2C+Boron+Nitride%2C+and+Metal+Borides%2C+in+Ullmann%27s+Encyclopedia+of+Industrial+Chemistry&rft.pub=Wiley-VCH%3A+Weinheim&rft.date=2005&rft_id=info%3Adoi%2F10.1002%2F14356007.a04_295.pub2&rft.isbn=978-3527306732&rft.au=Greim%2C+Jochen&rft.au=Schwetz%2C+Karl+A.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></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"><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%3ABoron+compounds" class="Z3988"></span></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"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFJones,_Morton_E.Marsh,_Richard_E.1954" class="citation journal cs1">Jones, Morton E. & Marsh, Richard E. (1954). "The Preparation and Structure of Magnesium Boride, MgB<sub>2</sub>". <i>Journal of the American Chemical Society</i>. <b>76</b> (5): 1434–1436. <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%2Fja01634a089">10.1021/ja01634a089</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=The+Preparation+and+Structure+of+Magnesium+Boride%2C+MgB%3Csub%3E2%3C%2Fsub%3E&rft.volume=76&rft.issue=5&rft.pages=1434-1436&rft.date=1954&rft_id=info%3Adoi%2F10.1021%2Fja01634a089&rft.au=Jones%2C+Morton+E.&rft.au=Marsh%2C+Richard+E.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></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="CITEREFCanfieldCrabtree2003" class="citation journal cs1">Canfield, Paul C.; <a href="/wiki/George_Crabtree" title="George Crabtree">Crabtree, George W.</a> (2003). <a rel="nofollow" class="external text" href="http://cmp.physics.iastate.edu/canfield/pub/pt0303.pdf">"Magnesium Diboride: Better Late than Never"</a> <span class="cs1-format">(PDF)</span>. <i>Physics Today</i>. <b>56</b> (3): 34–40. <a href="/wiki/Bibcode_(identifier)" class="mw-redirect" title="Bibcode (identifier)">Bibcode</a>:<a rel="nofollow" class="external text" href="https://ui.adsabs.harvard.edu/abs/2003PhT....56c..34C">2003PhT....56c..34C</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1063%2F1.1570770">10.1063/1.1570770</a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20120226233637/http://cmp.physics.iastate.edu/canfield/pub/pt0303.pdf">Archived</a> <span class="cs1-format">(PDF)</span> from the original on 26 February 2012<span class="reference-accessdate">. Retrieved <span class="nowrap">8 January</span> 2012</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Physics+Today&rft.atitle=Magnesium+Diboride%3A+Better+Late+than+Never&rft.volume=56&rft.issue=3&rft.pages=34-40&rft.date=2003&rft_id=info%3Adoi%2F10.1063%2F1.1570770&rft_id=info%3Abibcode%2F2003PhT....56c..34C&rft.aulast=Canfield&rft.aufirst=Paul+C.&rft.au=Crabtree%2C+George+W.&rft_id=http%3A%2F%2Fcmp.physics.iastate.edu%2Fcanfield%2Fpub%2Fpt0303.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" 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"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://cds.cern.ch/journal/CERNBulletin/2014/16/News+Articles/1693853">"Category "News+Articles" not found - CERN Document Server"</a>. <i>cds.cern.ch</i>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20220220075257/https://cds.cern.ch/journal/CERNBulletin/2014/16/News+Articles/1693853">Archived</a> from the original on 20 February 2022<span class="reference-accessdate">. Retrieved <span class="nowrap">9 October</span> 2020</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=cds.cern.ch&rft.atitle=Category+%22News%2BArticles%22+not+found+-+CERN+Document+Server&rft_id=https%3A%2F%2Fcds.cern.ch%2Fjournal%2FCERNBulletin%2F2014%2F16%2FNews%2BArticles%2F1693853&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></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"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFCardarelli,_François2008" class="citation book cs1">Cardarelli, François (2008). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=PvU-qbQJq7IC&pg=PA638">"Titanium Diboride"</a>. <i>Materials handbook: A concise desktop reference</i>. pp. 638–639. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-1-84628-668-1" title="Special:BookSources/978-1-84628-668-1"><bdi>978-1-84628-668-1</bdi></a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20170108051112/https://books.google.com/books?id=PvU-qbQJq7IC&pg=PA638">Archived</a> from the original on 8 January 2017<span class="reference-accessdate">. Retrieved <span class="nowrap">5 January</span> 2016</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Titanium+Diboride&rft.btitle=Materials+handbook%3A+A+concise+desktop+reference&rft.pages=638-639&rft.date=2008&rft.isbn=978-1-84628-668-1&rft.au=Cardarelli%2C+Fran%C3%A7ois&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DPvU-qbQJq7IC%26pg%3DPA638&rfr_id=info%3Asid%2Fen.wikipedia.org%3ABoron+compounds" class="Z3988"></span></span> </li> </ol></div></div> <div class="navbox-styles"><style data-mw-deduplicate="TemplateStyles:r1129693374">.mw-parser-output .hlist dl,.mw-parser-output .hlist ol,.mw-parser-output .hlist ul{margin:0;padding:0}.mw-parser-output .hlist dd,.mw-parser-output .hlist dt,.mw-parser-output .hlist li{margin:0;display:inline}.mw-parser-output .hlist.inline,.mw-parser-output .hlist.inline dl,.mw-parser-output .hlist.inline ol,.mw-parser-output .hlist.inline ul,.mw-parser-output .hlist dl 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.navbar li{word-spacing:-0.125em}.mw-parser-output .navbar a>span,.mw-parser-output .navbar a>abbr{text-decoration:inherit}.mw-parser-output .navbar-mini abbr{font-variant:small-caps;border-bottom:none;text-decoration:none;cursor:inherit}.mw-parser-output .navbar-ct-full{font-size:114%;margin:0 7em}.mw-parser-output .navbar-ct-mini{font-size:114%;margin:0 4em}html.skin-theme-clientpref-night .mw-parser-output .navbar li a abbr{color:var(--color-base)!important}@media(prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .navbar li a abbr{color:var(--color-base)!important}}@media print{.mw-parser-output .navbar{display:none!important}}</style><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Boron_compounds" title="Template:Boron compounds"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Boron_compounds" title="Template talk:Boron compounds"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Boron_compounds" title="Special:EditPage/Template:Boron compounds"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Boron_compounds" style="font-size:114%;margin:0 4em"><a class="mw-selflink selflink">Boron compounds</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">Boron pnictogenides</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Boron_arsenide" title="Boron arsenide">BAs</a></li> <li><a href="/wiki/Boron_nitride" title="Boron nitride">BN</a></li> <li><a href="/wiki/Boron_phosphide" title="Boron phosphide">BP</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Boron halides</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Boron_tribromide" title="Boron tribromide">BBr<sub>3</sub></a></li> <li><a href="/wiki/Boron_trichloride" title="Boron trichloride">BCl<sub>3</sub></a></li> <li><a href="/wiki/Boron_monofluoride" title="Boron monofluoride">BF</a></li> <li><a href="/wiki/Boron_monofluoride_monoxide" title="Boron monofluoride monoxide">BFO</a></li> <li><a href="/wiki/Boron_trifluoride" title="Boron trifluoride">BF<sub>3</sub></a></li> <li><a href="/wiki/Boron_triiodide" title="Boron triiodide">BI<sub>3</sub></a></li> <li><a href="/wiki/Diboron_tetrafluoride" title="Diboron tetrafluoride">B<sub>2</sub>F<sub>4</sub></a></li> <li><a href="/wiki/Diboron_tetrachloride" title="Diboron tetrachloride">B<sub>2</sub>Cl<sub>4</sub></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Acids</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Tetranitratoborate" title="Tetranitratoborate">B(NO<sub>3</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Boric_acid" title="Boric acid">B(OH)<sub>3</sub></a></li> <li><a href="/wiki/Boron_phosphate" title="Boron phosphate">BPO<sub>4</sub></a></li> <li><a href="/wiki/Borinic_acid" title="Borinic acid">BH<sub>3</sub>O</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Boranes" title="Boranes">Boranes</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Borane" title="Borane">BH<sub>3</sub></a></li> <li><a href="/wiki/Diborane(4)" title="Diborane(4)">B<sub>2</sub>H<sub>4</sub></a></li> <li><a href="/wiki/Diborane" title="Diborane">B<sub>2</sub>H<sub>6</sub></a></li> <li><a href="/wiki/Ammonia_borane" title="Ammonia borane">BH<sub>3</sub>NH<sub>3</sub></a></li> <li><a href="/wiki/Tetraborane" title="Tetraborane">B<sub>4</sub>H<sub>10</sub></a></li> <li><a href="/wiki/Pentaborane(9)" title="Pentaborane(9)">B<sub>5</sub>H<sub>9</sub></a></li> <li><a href="/wiki/Pentaborane(11)" title="Pentaborane(11)">B<sub>5</sub>H<sub>11</sub></a></li> <li><a href="/wiki/Hexaborane(10)" title="Hexaborane(10)">B<sub>6</sub>H<sub>10</sub></a></li> <li><a href="/wiki/Hexaborane(12)" title="Hexaborane(12)">B<sub>6</sub>H<sub>12</sub></a></li> <li><a href="/wiki/Decaborane" title="Decaborane">B<sub>10</sub>H<sub>14</sub></a></li> <li><a href="/wiki/Octadecaborane" title="Octadecaborane">B<sub>18</sub>H<sub>22</sub></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Boron oxides and sulfides</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Boron_monoxide" title="Boron monoxide">B<sub>2</sub>O</a></li> <li><a href="/wiki/Boron_trioxide" title="Boron trioxide">B<sub>2</sub>O<sub>3</sub></a></li> <li><a href="/wiki/Boron_sulfide" title="Boron sulfide">B<sub>2</sub>S<sub>3</sub></a></li> <li><a href="/wiki/Boron_suboxide" title="Boron suboxide">B<sub>6</sub>O</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Carbides</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Boron_carbide" title="Boron carbide">B<sub>4</sub>C</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Organoboron_compounds" class="mw-redirect" title="Organoboron compounds">Organoboron compounds</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/1,2-Dimethyldiborane" title="1,2-Dimethyldiborane">(BH<sub>2</sub>Me)<sub>2</sub></a></li> <li><a href="/wiki/Trimethylborane" title="Trimethylborane">BMe<sub>3</sub></a></li> <li><a href="/wiki/Triethylborane" title="Triethylborane">BEt<sub>3</sub></a></li> <li><a href="/wiki/Tetraacetyl_diborate" title="Tetraacetyl diborate">Ac<sub>4</sub>(BO<sub>3</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Borane_carbonyl" title="Borane carbonyl">COBH<sub>3</sub></a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"><style data-mw-deduplicate="TemplateStyles:r1038841319">.mw-parser-output .tooltip-dotted{border-bottom:1px dotted;cursor:help}</style><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1038841319"></div><div role="navigation" class="navbox authority-control" aria-label="Navbox" style="padding:3px"><table class="nowraplinks hlist navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="row" class="navbox-group" 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