Gallium(III) sulfide

<h2 id="structure">Structure</h2>
There are four <a href="/facts/Polymorphism_(materials_science)/bu2tqsB9">polymorphs</a>, α (hexagonal), α' (monoclinic), β(hexagonal) and γ(cubic). The alpha form is yellow. The crystal structures are related to those of <a href="/facts/Zinc_sulfide/K8l5AF3K">ZnS</a> with gallium in tetrahedral positions.<a class="footnote-ref" id="fnref:1" href="#fn:1">1</a><a class="footnote-ref" id="fnref:2" href="#fn:2">2</a><a class="footnote-ref" id="fnref:3" href="#fn:3">3</a> The alpha and beta forms are isostructural with their aluminium analogues.<a class="footnote-ref" id="fnref:4" href="#fn:4">4</a> The similarity in crystal form of gamma- with <a href="/facts/Sphalerite/5NumvnzR">sphalerite</a> (zinc blende), <a href="/facts/Zinc_sulfide/K8l5AF3K">ZnS</a> is believed to explain the enrichment of gallium in <a href="/facts/Sphalerite/5NumvnzR">sphalerite</a> ores.<a class="footnote-ref" id="fnref:5" href="#fn:5">5</a>

<h2 id="preparation-and-chemical-properties">Preparation and chemical properties</h2>
Ga2S3 can prepared by reacting the elements at high temperature or as a white solid by heating Ga in a stream of <a href="/facts/Hydrogen_sulfide/UbCqjMMk">H2S</a> at high temperature (950 °C).<a class="footnote-ref" id="fnref:6" href="#fn:6">6</a>
It may also prepared by a solid state reaction of <a href="/facts/Gallium_trichloride/gMs76FbG">GaCl3</a> and <a href="/facts/Sodium_sulfide/DKu0s158">Na2S</a>.<a class="footnote-ref" id="fnref:7" href="#fn:7">7</a>
The method of production can determine the polymorphic form produced, the reaction of <a href="/facts/Gallium_hydroxide/kmXTFHQq">Ga(OH)3</a> with <a href="/facts/Hydrogen_sulfide/UbCqjMMk">H2S</a> at different temperatures is reported to produce a different polymorph depending on the temperature, α- 1020 K, β- 820 K and γ- above 873 K <a class="footnote-ref" id="fnref:8" href="#fn:8">8</a>
Ga2S3 decomposes at high temperature forming the <a href="/facts/Non-stoichiometric_compound/DAssoN0e">non-stoichiometric</a> sulfide, Ga4Sx (4.8 < x < 5.2).<a class="footnote-ref" id="fnref:9" href="#fn:9">9</a>
Ga2S3 dissolves in aqueous acids and decomposes slowly in moist air forming <a href="/facts/Hydrogen_sulfide/UbCqjMMk">H2S</a>.<a class="footnote-ref" id="fnref:10" href="#fn:10">10</a>
Ga2S3 dissolves in aqueous solutions of <a href="/facts/Potassium_sulfide/fpNzYwkX">potassium sulfide</a>, K2S to form K8Ga4S10 containing the (Ga4S10)8− anion which has an <a href="/facts/Adamantane/tlvgCxYf">adamantane</a>, <a href="/facts/Phosphorus_pentoxide/GKTSUNqS">molecular P4O10</a> structure.<a class="footnote-ref" id="fnref:11" href="#fn:11">11</a>
Ternary sulfides MIGaS2, MIIGa2S4 and MIIIGaS3 respectively have been of interest due to their unusual electrical properties and some of these can be prepared by reactions of Ga2S3 with metal sulfides e.g. CdGa2S4:-<a class="footnote-ref" id="fnref:12" href="#fn:12">12</a>

Ga2S3 + <a href="/facts/Cadmium_sulfide/lsYV3Gum">CdS</a> → CdGa2S4
Although by itself Ga2S3 is not a glass former it can be reacted with rare earth sulfides to form glasses e.g. the reaction with lanthanum sulfide, La2S3, forms <a href="/facts/Gallium_lanthanum_sulfide_glass/Kp3EEeYa">gallium lanthanum sulfide glass</a> which has interesting optical properties and is a semiconductor.<a class="footnote-ref" id="fnref:13" href="#fn:13">13</a>

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

<ol>
<li id="fn:1">Pardo, M.P.; Guittard, M.; Chilouet, A.; Tomas, A. (1993). "Diagramme de phases gallium-soufre et études structurales des phases solides". Journal of Solid State Chemistry. 102 (2): 423–433. Bibcode:1993JSSCh.102..423P. doi:10.1006/jssc.1993.1054. ISSN 0022-4596. <a href="/wiki/Bibcode_(identifier)" target="_blank">/wiki/Bibcode_(identifier)</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></li>
<li id="fn:2">The Chemistry of Aluminium, Gallium, Indium and Thallium, Anthony John Downs, 1993, ISBN 075140103X , ISBN 978-0751401035 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></li>
<li id="fn:3">Peter Atkins; T.L. Overton; J.P. Rourke; M.T. Weller; F.A. Armstrong (2010). Inorganic Chemistry (Fifth ed.). New York: W. H. Freeman and Company. p. 346. ISBN 978-1429218207. <a href="978-1429218207" target="_blank">978-1429218207</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></li>
<li id="fn:4">Barron, Andrew R.; MacInnes, Andrew N. (1994). "Gallium: Inorganic chemistry". In King, R. Bruce (ed.). Encyclopedia of Inorganic Chemistry. John Wiley and Sons. pp. 100–110. ISBN 0-471-93620-0. <a href="0-471-93620-0" target="_blank">0-471-93620-0</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></li>
<li id="fn:5">Barron, Andrew R.; MacInnes, Andrew N. (1994). "Gallium: Inorganic chemistry". In King, R. Bruce (ed.). Encyclopedia of Inorganic Chemistry. John Wiley and Sons. pp. 100–110. ISBN 0-471-93620-0. <a href="0-471-93620-0" target="_blank">0-471-93620-0</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></li>
<li id="fn:6">The Chemistry of Aluminium, Gallium, Indium and Thallium, Anthony John Downs, 1993, ISBN 075140103X , ISBN 978-0751401035 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></li>
<li id="fn:7">Barron, Andrew R.; MacInnes, Andrew N. (1994). "Gallium: Inorganic chemistry". In King, R. Bruce (ed.). Encyclopedia of Inorganic Chemistry. John Wiley and Sons. pp. 100–110. ISBN 0-471-93620-0. <a href="0-471-93620-0" target="_blank">0-471-93620-0</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></li>
<li id="fn:8">Semiconductors: Data Handbook 3d Ed., Otfried Madelung, Springer, 2004, ISBN 978-3540404880 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></li>
<li id="fn:9">Barron, Andrew R.; MacInnes, Andrew N. (1994). "Gallium: Inorganic chemistry". In King, R. Bruce (ed.). Encyclopedia of Inorganic Chemistry. John Wiley and Sons. pp. 100–110. ISBN 0-471-93620-0. <a href="0-471-93620-0" target="_blank">0-471-93620-0</a> <a href="#fnref:9" class="footnote-back-ref">↩</a></li>
<li id="fn:10">The Chemistry of Aluminium, Gallium, Indium and Thallium, Anthony John Downs, 1993, ISBN 075140103X , ISBN 978-0751401035 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:10" class="footnote-back-ref">↩</a></li>
<li id="fn:11">Barron, Andrew R.; MacInnes, Andrew N. (1994). "Gallium: Inorganic chemistry". In King, R. Bruce (ed.). Encyclopedia of Inorganic Chemistry. John Wiley and Sons. pp. 100–110. ISBN 0-471-93620-0. <a href="0-471-93620-0" target="_blank">0-471-93620-0</a> <a href="#fnref:11" class="footnote-back-ref">↩</a></li>
<li id="fn:12">Barron, Andrew R.; MacInnes, Andrew N. (1994). "Gallium: Inorganic chemistry". In King, R. Bruce (ed.). Encyclopedia of Inorganic Chemistry. John Wiley and Sons. pp. 100–110. ISBN 0-471-93620-0. <a href="0-471-93620-0" target="_blank">0-471-93620-0</a> <a href="#fnref:12" class="footnote-back-ref">↩</a></li>
<li id="fn:13">Semiconducting Chalcogenide Glass III: Applications of Chalcogenide Glasses, Robert Fairman, Boris Ushkov, Elsevier, 2004, (ebook), ISBN 9780080541068 <a href="/wiki/ISBN_(identifier)" target="_blank">/wiki/ISBN_(identifier)</a> <a href="#fnref:13" class="footnote-back-ref">↩</a></li>
</ol>

Gallium(III) sulfide open-in-new

Gallium(III) sulfide