Boranes

<h2 id="history">History</h2>
<p>The development of the chemistry of boranes led to innovations in synthetic methods as well as structure and bonding. First, new synthetic techniques were required to handle diborane and many of its derivatives, which are both <a href="/facts/Pyrophoric/1b8Sl2AJ">pyrophoric</a> and volatile. <a href="/facts/Alfred_Stock/qeq9FG3G">Alfred Stock</a> invented the glass vacuum line for this purpose.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a> The structure of diborane was correctly predicted in 1943 many years after its discovery.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a> Interest in boranes increased during World War II due to the potential of <a href="/facts/Uranium_borohydride/n9aB4nhf">uranium borohydride</a> for enrichment of the uranium isotopes and as a source of hydrogen for inflating weather balloons. In the US, a team led by <a href="/facts/Hermann_Irving_Schlesinger/nAlvvLEy">Schlesinger</a> developed the basic chemistry of the anionic boron hydrides and the related aluminium hydrides. Schlesinger's work laid the foundation for a host of boron hydride <a href="/facts/Reagent/c3GLInCu">reagents</a> for <a href="/facts/Organic_synthesis/aprl6Iq7">organic synthesis</a>, most of which were developed by his student <a href="/facts/Herbert_C._Brown/gzHbbzR3">Herbert C. Brown</a>. Borane-based reagents are now widely used in organic synthesis. Brown was awarded the <a href="/facts/Nobel_Prize/3z1Y3oFL">Nobel Prize</a> in Chemistry in 1979 for this work.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a>
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<h2 id="synthesis">Synthesis</h2>
<p class="note">Main article: <a href="/facts/Organoboron_chemistry/r6NQHXYt">Organoboron chemistry</a></p>
<p>Most boranes are prepared directly or indirectly from <a href="/facts/Diborane/k7egwbPf">diborane</a>.  Diborane reacts with alkenes to give alkylboranes, a process known as <a href="/facts/Hydroboration/Wm7v7Inr">hydroboration</a>:
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B2H6  +  2 CH2=CHR   →   2 BH2(CH2CH2R)
B2H6  +  4 CH2=CHR   →   2 BH(CH2CH2R)2
B2H6  +  6 CH2=CHR   →   2 B(CH2CH2R)2
<p>Alkyl and aryl boranes can also be produced by <a href="/facts/Alkylation/1rd5SNbt">alkylation</a> of chloroboranes and <a href="/facts/Boronic_ester/BtN4s5B4">boronic esters</a>.
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<h2 id="classes-of-boranes">Classes of boranes</h2>

<h3>Binary boron hydrides</h3>
<p>The parent boranes are binary boron hydrides, starting with <a href="/facts/Borane/pHQMPw5r">borane</a> (BH3) and its dimer <a href="/facts/Diborane/k7egwbPf">diborane</a> (B2H6).  Pyrolysis of these species leads to higher boranes, such as <a href="/facts/Tetraborane/rN9fGKvs">tetraborane</a> and <a href="/facts/Pentaborane/coB2EDUm">pentaborane</a>.  These two are early members of the <a href="/facts/Boron_hydride_clusters/wu3RTzUS">boron hydride clusters</a>.
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<h3>Primary and secondary boranes</h3>
<p>This family of boron hydrides includes mono- and dialkylboranes.  The simplest members readily engage in <a href="/facts/Redistribution_reaction/pdbYLmRB">redistribution reactions</a>:
</p>
2 BH2(CH3)   →   BH(CH3)2 + 0.5 B2H6
<p>With bulky substituents, primary and secondary boranes are more readily isolable and even useful.  Examples include <a href="/facts/Thexylborane/lq6pISgn">thexylborane</a> and <a href="/facts/9-BBN/8TMvv7m5">9-BBN</a>.  Almost all primary and secondary boranes are dimeric with bridging hydrides.
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<h3>Tertiary boranes</h3>
<p>Most work focuses on trialkyl and triaryl boranes.  These are all monomers (in contrast to the corresponding trialkyl and triarylaluminium compounds). Their BC3 cores are planar. Well known examples are <a href="/facts/Trimethylboron/MhndDXHj">trimethylboron</a>, <a href="/facts/Triethylboron/qLlyzN2r">triethylboron</a>, and <a href="/facts/Triphenylboron/IEACoCmR">triphenylboron</a>. Many tertiary boranes are produced by <a href="/facts/Hydroboration/Wm7v7Inr">hydroboration</a>.
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<h2 id="reactivity-of-boranes">Reactivity of boranes</h2>
<p class="note">For reactions of diborane, see <a href="/facts/Diborane/k7egwbPf">diborane</a>.</p>
<p>The lowest borane, BH3 exists only transiently, <a href="/facts/Dimerization_(chemistry)/mU64PnEq">dimerizing</a> instantly to form diborane, B2H6. Its adduct <a href="/facts/Borane%E2%80%93tetrahydrofuran/XsAC5Yur">borane–tetrahydrofuran</a> and <a href="/facts/Borane%E2%80%93dimethylsulfide/2TvG1KpB">borane–dimethylsulfide</a> are useful in <a href="/facts/Hydroboration/Wm7v7Inr">hydroboration</a> reactions. 
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<h2 id="references">References</h2>

<ol>
<li id="fn:1"><p>Greenwood, Norman  N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. pp 151-195 <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li>
<li id="fn:2"><p>Stock, Alfred (1933). The Hydrides of Boron and Silicon. New York: Cornell University Press. <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li>
<li id="fn:3"><p>Longuet-Higgins, H. C.; Bell, R. P. (1943). "64. The Structure of the Boron Hydrides". Journal of the Chemical Society (Resumed). 1943: 250–255. doi:10.1039/JR9430000250. <a href="/wiki/H._Christopher_Longuet-Higgins" target="_blank">/wiki/H._Christopher_Longuet-Higgins</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li>
<li id="fn:4"><p>Brown, H. C. Organic Syntheses via Boranes John Wiley & Sons, Inc. New York: 1975. ISBN 0-471-11280-1. <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li>
</ol>

Boranes open-in-new

Boranes