Bismuthine

<h2 id="preparation-and-properties">Preparation and properties</h2>
<p>BiH3 is prepared by the redistribution of methylbismuthine (BiH2Me):<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a>
</p>
3 BiH2Me →  2 BiH3  +  BiMe3
<p>The required BiH2Me, which is also thermally unstable, is generated by reduction of <a href="/facts/Methylbismuth_dichloride/QSCyvWUJ">methylbismuth dichloride</a>, BiCl2Me with <a href="/facts/Lithium_aluminium_hydride/QMMhdqEy">LiAlH4</a>.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a>
</p><p>As suggested by the behavior of <a href="/facts/Stibine/8QlRphHB">SbH3</a>, BiH3 is unstable and decomposes to its constituent elements according to the following equation:
</p>
2 BiH3   →  3 H2  +  2 Bi  (Δ<i>H</i>of(gas) = −278 kJ/mol)
<p>The methodology used for detection of <a href="/facts/Arsenic/k1c4f44D">arsenic</a> ("<a href="/facts/Marsh_test/utnS7NEh">Marsh test</a>") can also be used to detect BiH3.  This test relies on the <a href="/facts/Thermal_decomposition/Qqx9RqkW">thermal decomposition</a> of these trihydrides to the metallic mirrors of reduced As, Sb, and Bi.  These deposits can be further distinguished by their distinctive solubility characteristics: arsenic dissolves in <a href="/facts/Sodium_hypochlorite/sp99uHHQ">NaOCl</a>, antimony dissolves in <a href="/facts/Polysulfide/PpfaUlw4">ammonium polysulfide</a>, and bismuth resists both reagents.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a>
</p>
<h2 id="uses-and-safety-considerations">Uses and safety considerations</h2>
<p>The low stability of BiH3 precludes significant health effects, it decomposes rapidly well below room temperature.
</p>

<h2 id="references">References</h2>

<ol>
<li id="fn:1"><p>W. Jerzembeck; H. Bürger; L. Constantin; L. Margulès; J. Demaison; J. Breidung; W. Thiel (2002). "Bismuthine BiH3: Fact or Fiction? High-Resolution Infrared, Millimeter-Wave, and Ab Initio Studies". Angew. Chem. Int. Ed. 41 (14): 2550–2552. doi:10.1002/1521-3773(20020715)41:14<2550::AID-ANIE2550>3.0.CO;2-B. PMID 12203530. Archived from the original on 2013-01-05. <a href="https://archive.today/20130105102945/http://www3.interscience.wiley.com/journal/96516335/abstract" target="_blank">https://archive.today/20130105102945/http://www3.interscience.wiley.com/journal/96516335/abstract</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li>
<li id="fn:2"><p>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001.ISBN 0-12-352651-5. <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li>
<li id="fn:3"><p>W. Jerzembeck; H. Bürger; L. Constantin; L. Margulès; J. Demaison; J. Breidung; W. Thiel (2002). "Bismuthine BiH3: Fact or Fiction? High-Resolution Infrared, Millimeter-Wave, and Ab Initio Studies". Angew. Chem. Int. Ed. 41 (14): 2550–2552. doi:10.1002/1521-3773(20020715)41:14<2550::AID-ANIE2550>3.0.CO;2-B. PMID 12203530. Archived from the original on 2013-01-05. <a href="https://archive.today/20130105102945/http://www3.interscience.wiley.com/journal/96516335/abstract" target="_blank">https://archive.today/20130105102945/http://www3.interscience.wiley.com/journal/96516335/abstract</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li>
<li id="fn:4"><p>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001.ISBN 0-12-352651-5. <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li>
</ol>

Bismuthine open-in-new

Bismuthine