Editing Seaborgium (section)

==Experimental chemistry==
Experimental chemical investigation of seaborgium has been hampered due to the need to produce it one atom at a time, its short half-life, and the resulting necessary harshness of the experimental conditions.<ref name="carbonyl">{{Cite journal | doi = 10.1126/science.1255720| pmid = 25237098| title = Synthesis and detection of a seaborgium carbonyl complex| journal = Science| volume = 345| issue = 6203| pages = 1491–3| year = 2014| last1 = Even | first1 = J.| last2 = Yakushev | first2 = A.| last3 = Dullmann | first3 = C. E.| last4 = Haba | first4 = H.| last5 = Asai | first5 = M.| last6 = Sato | first6 = T. K.| last7 = Brand | first7 = H.| last8 = Di Nitto | first8 = A.| last9 = Eichler | first9 = R.| last10 = Fan | first10 = F. L.| last11 = Hartmann | first11 = W.| last12 = Huang | first12 = M.| last13 = Jager | first13 = E.| last14 = Kaji | first14 = D.| last15 = Kanaya | first15 = J.| last16 = Kaneya | first16 = Y.| last17 = Khuyagbaatar | first17 = J.| last18 = Kindler | first18 = B.| last19 = Kratz | first19 = J. V.| last20 = Krier | first20 = J.| last21 = Kudou | first21 = Y.| last22 = Kurz | first22 = N.| last23 = Lommel | first23 = B.| last24 = Miyashita | first24 = S.| last25 = Morimoto | first25 = K.| last26 = Morita | first26 = K.| last27 = Murakami | first27 = M.| last28 = Nagame | first28 = Y.| last29 = Nitsche | first29 = H.| last30 = Ooe | first30 = K.| display-authors = 29| bibcode = 2014Sci...345.1491E| s2cid = 206558746}} {{subscription required}}</ref> The isotope <sup>265</sup>Sg and its isomer <sup>265m</sup>Sg are advantageous for radiochemistry: they are produced in the <sup>248</sup>Cm(<sup>22</sup>Ne,5n) reaction.<ref name="Moody">{{cite book |chapter=Synthesis of Superheavy Elements |last1=Moody |first1=Ken |editor1-first=Matthias |editor1-last=Schädel |editor2-first=Dawn |editor2-last=Shaughnessy |title=The Chemistry of Superheavy Elements |publisher=Springer Science & Business Media |edition=2nd |pages=24–8 |isbn=9783642374661|date=2013-11-30 }}</ref>

In the first experimental chemical studies of seaborgium in 1995 and 1996, seaborgium atoms were produced in the reaction <sup>248</sup>Cm(<sup>22</sup>Ne,4n)<sup>266</sup>Sg, thermalised, and reacted with an O<sub>2</sub>/HCl mixture. The adsorption properties of the resulting oxychloride were measured and compared with those of molybdenum and tungsten compounds. The results indicated that seaborgium formed a volatile oxychloride akin to those of the other group 6 elements, and confirmed the decreasing trend of oxychloride volatility down group 6:

:Sg + {{chem|O|2}} + 2 HCl → {{chem|SgO|2|Cl|2}} + {{chem|H|2}}

In 2001, a team continued the study of the gas phase chemistry of seaborgium by reacting the element with O<sub>2</sub> in a H<sub>2</sub>O environment. In a manner similar to the formation of the oxychloride, the results of the experiment indicated the formation of seaborgium oxide hydroxide, a reaction well known among the lighter group 6 homologues as well as the pseudohomologue [[uranium]].<ref>{{cite journal
|url=http://www-w2k.gsi.de/kernchemie/images/pdf_Artikel/Radiochim_Acta_89_737_2001.pdf 
|title=Physico-chemical characterization of seaborgium as oxide hydroxide 
|journal=Radiochim. Acta 
|volume=89 
|pages=737–741 
|date=2001 
|doi=10.1524/ract.2001.89.11-12.737 
|display-authors=8 
|last1=Huebener 
|first1=S. 
|last2=Taut 
|first2=S. 
|last3=Vahle 
|first3=A. 
|last4=Dressler 
|first4=R. 
|last5=Eichler 
|first5=B. 
|last6=Gäggeler 
|first6=H. W. 
|last7=Jost 
|first7=D. T. 
|last8=Piguet 
|first8=D. 
|last9=Türler 
|first9=A. 
|last10=Brüchle 
|first10=W. 
|issue=11–12_2001 
|s2cid=98583998 
|url-status=bot: unknown 
|archive-url=https://web.archive.org/web/20141025201143/http://www-w2k.gsi.de/kernchemie/images/pdf_Artikel/Radiochim_Acta_89_737_2001.pdf 
|archive-date=2014-10-25 
}}</ref>

:2 Sg + 3 {{chem|O|2}} → 2 {{chem|SgO|3}}
:{{chem|SgO|3}} + {{chem|H|2|O}} → {{chem|SgO|2|(OH)|2}}

Predictions on the aqueous chemistry of seaborgium have largely been confirmed. In experiments conducted in 1997 and 1998, seaborgium was eluted from cation-exchange resin using a HNO<sub>3</sub>/HF solution, most likely as neutral SgO<sub>2</sub>F<sub>2</sub> or the anionic complex ion [SgO<sub>2</sub>F<sub>3</sub>]<sup>−</sup> rather than {{chem|SgO|4|2-}}. In contrast, in 0.1 M [[nitric acid]], seaborgium does not elute, unlike molybdenum and tungsten, indicating that the hydrolysis of [Sg(H<sub>2</sub>O)<sub>6</sub>]<sup>6+</sup> only proceeds as far as the cationic complex [Sg(OH)<sub>4</sub>(H<sub>2</sub>O)]<sup>2+</sup> or [SgO(OH)<sub>3</sub>(H<sub>2</sub>O)<sub>2</sub>]<sup>+</sup>, while that of molybdenum and tungsten proceed to neutral [MO<sub>2</sub>(OH)<sub>2</sub>].<ref name="Haire" />

The only other oxidation state known for seaborgium other than the group oxidation state of +6 is the zero oxidation state. Similarly to its three lighter congeners, forming [[chromium hexacarbonyl]], [[molybdenum hexacarbonyl]], and [[tungsten hexacarbonyl]], seaborgium has been shown in 2014 to also form [[seaborgium hexacarbonyl]], Sg(CO)<sub>6</sub>. Like its molybdenum and tungsten homologues, seaborgium hexacarbonyl is a volatile compound that reacts readily with [[silicon dioxide]].<ref name="carbonyl" />