Seaborgium

\( \require{mhchem} \)

Seaborgium is a synthetic chemical element; it has symbol Sg and atomic number 106. It is named after the American nuclear chemist Glenn T. Seaborg. As a synthetic element, it can be created in a laboratory but is not found in nature. It is also radioactive; the most stable known isotope, 269Sg, has a half-life of approximately 14 minutes.[9]

Seaborgium, ₁₀₆Sg

Seaborgium
Pronunciation	/siːˈbɔːrɡiəm/ ⓘ ​(see-BOR-ghee-əm)
Mass number	[269]
Seaborgium in the periodic table
Atomic number (Z)	106
Group	group 6
Period	period 7
Block	d-block
Electron configuration	[Rn] 5f14 6d4 7s2[1]
Electrons per shell	2, 8, 18, 32, 32, 12, 2
Physical properties
Phase at STP	solid (predicted)[2]
Density (near r.t.)	23–24 g/cm3 (predicted)[3][4]
Atomic properties
Oxidation states	0, (+3), (+4), (+5), +6[1][5] (parenthesized: prediction)
Ionization energies	1st: 757 kJ/mol 2nd: 1733 kJ/mol 3rd: 2484 kJ/mol (more) (all but first estimated)[1]
Atomic radius	empirical: 132 pm (predicted)[1]
Covalent radius	143 pm (estimated)[6]
Other properties
Natural occurrence	synthetic
Crystal structure	​body-centered cubic (bcc) (predicted)[2]
CAS Number	54038-81-2
History
Naming	after Glenn T. Seaborg
Discovery	Lawrence Berkeley National Laboratory (1974)
Isotopes of seaborgium
Main isotopes[7] Decay abun­dance half-life (t1/2) mode pro­duct 265Sg synth 8.5 s α 261Rf 265mSg synth 14.4 s α 261mRf 267Sg synth 80 s α17% 263Rf SF83% – 268Sg synth 13 s[8] SF 269Sg synth 14 min[9] α 265Rf 271Sg synth 31 s[10] α73% 267Rf SF27%

In the periodic table of the elements, it is a d-block transactinide element. It is a member of the 7th period and belongs to the group 6 elements as the fourth member of the 6d series of transition metals. Chemistry experiments have confirmed that seaborgium behaves as the heavier homologue to tungsten in group 6. The chemical properties of seaborgium are characterized only partly, but they compare well with the chemistry of the other group 6 elements.

In 1974, a few atoms of seaborgium were produced in laboratories in the Soviet Union and in the United States. The priority of the discovery and therefore the naming of the element was disputed between Soviet and American scientists, and it was not until 1997 that the International Union of Pure and Applied Chemistry (IUPAC) established seaborgium as the official name for the element. It is one of only two elements named after a living person at the time of naming, the other being oganesson, element 118.[a]

Introduction

The heaviest[b] atomic nuclei are created in nuclear reactions that combine two other nuclei of unequal size[c] into one; roughly, the more unequal the two nuclei in terms of mass, the greater the possibility that the two react.[18] The material made of the heavier nuclei is made into a target, which is then bombarded by the beam of lighter nuclei. Two nuclei can fuse into one only if they approach each other closely enough; normally, nuclei (all positively charged) repel each other due to electrostatic repulsion. The strong interaction can overcome this repulsion but only within a very short distance from a nucleus; beam nuclei are thus greatly accelerated in order to make such repulsion insignificant compared to the velocity of the beam nucleus.[19] Coming close alone is not enough for two nuclei to fuse: when two nuclei approach each other, they usually remain together for approximately 10−20 seconds and then part ways (not necessarily in the same composition as before the reaction) rather than form a single nucleus.[19][20] If fusion does occur, the temporary merger—termed a compound nucleus—is an excited state. To lose its excitation energy and reach a more stable state, a compound nucleus either fissions or ejects one or several neutrons,[d] which carry away the energy. This occurs in approximately 10−16 seconds after the initial collision.[21][e]

The beam passes through the target and reaches the next chamber, the separator; if a new nucleus is produced, it is carried with this beam.[24] In the separator, the newly produced nucleus is separated from other nuclides (that of the original beam and any other reaction products)[f] and transferred to a surface-barrier detector, which stops the nucleus. The exact location of the upcoming impact on the detector is marked; also marked are its energy and the time of the arrival.[24] The transfer takes about 10−6 seconds; in order to be detected, the nucleus must survive this long.[27] The nucleus is recorded again once its decay is registered, and the location, the energy, and the time of the decay are measured.[24]

Stability of a nucleus is provided by the strong interaction. However, its range is very short; as nuclei become larger, their influence on the outermost nucleons (protons and neutrons) weakens. At the same time, the nucleus is torn apart by electrostatic repulsion between protons, as it has unlimited range.[28] Nuclei of the heaviest elements are thus theoretically predicted[29] and have so far been observed[30] to primarily decay via decay modes that are caused by such repulsion: alpha decay and spontaneous fission;[g] these modes are predominant for nuclei of superheavy elements. Alpha decays are registered by the emitted alpha particles, and the decay products are easy to determine before the actual decay; if such a decay or a series of consecutive decays produces a known nucleus, the original product of a reaction can be determined arithmetically.[h] Spontaneous fission, however, produces various nuclei as products, so the original nuclide cannot be determined from its daughters.[i]

The information available to physicists aiming to synthesize one of the heaviest elements is thus the information collected at the detectors: location, energy, and time of arrival of a particle to the detector, and those of its decay. The physicists analyze this data and seek to conclude that it was indeed caused by a new element and could not have been caused by a different nuclide than the one claimed. Often, provided data is insufficient for a conclusion that a new element was definitely created and there is no other explanation for the observed effects; errors in interpreting data have been made.[j]

History

Following claims of the observation of elements 104 and 105 in 1970 by Albert Ghiorso et al. at the Lawrence Livermore National Laboratory, a search for element 106 using oxygen-18 projectiles and the previously used californium-249 target was conducted.[42] Several 9.1 MeV alpha decays were reported and are now thought to originate from element 106, though this was not confirmed at the time. In 1972, the HILAC accelerator received equipment upgrades, preventing the team from repeating the experiment, and data analysis was not done during the shutdown.[42] This reaction was tried again several years later, in 1974, and the Berkeley team realized that their new data agreed with their 1971 data, to the astonishment of Ghiorso. Hence, element 106 could have actually been discovered in 1971 if the original data was analyzed more carefully.[42]

Two groups claimed discovery of the element. Unambiguous evidence of element 106 was first reported in 1974 by a Russian research team in Dubna led by Yuri Oganessian, in which targets of lead-208 and lead-207 were bombarded with accelerated ions of chromium-54. In total, fifty-one spontaneous fission events were observed with a half-life between four and ten milliseconds. After having ruled out nucleon transfer reactions as a cause for these activities, the team concluded that the most likely cause of the activities was the spontaneous fission of isotopes of element 106. The isotope in question was first suggested to be seaborgium-259, but was later corrected to seaborgium-260.[43]

²⁰⁸₈₂Pb+ ⁵⁴₂₄Cr→ ²⁶⁰₁₀₆Sg+ 2 n

²⁰⁷₈₂Pb+ ⁵⁴₂₄Cr→ ²⁶⁰₁₀₆Sg+ n

A few months later in 1974, researchers including Glenn T. Seaborg, Carol Alonso and Albert Ghiorso at the University of California, Berkeley, and E. Kenneth Hulet from the Lawrence Livermore National Laboratory, also synthesized the element[44] by bombarding a californium-249 target with oxygen-18 ions, using equipment similar to that which had been used for the synthesis of element 104 five years earlier, observing at least seventy alpha decays, seemingly from the isotope seaborgium-263m with a half-life of 0.9±0.2 seconds. The alpha daughter rutherfordium-259 and granddaughter nobelium-255 had previously been synthesised and the properties observed here matched with those previously known, as did the intensity of their production. The cross-section of the reaction observed, 0.3 nanobarns, also agreed well with theoretical predictions. These bolstered the assignment of the alpha decay events to seaborgium-263m.[43]

²⁴⁹₉₈Cf+ ¹⁸₈O→ ^263m₁₀₆Sg+ 4 ¹₀n→ ²⁵⁹₁₀₄Rf+ α→ ²⁵⁵₁₀₂No+ α

A dispute thus arose from the initial competing claims of discovery, though unlike the case of the synthetic elements up to element 105, neither team of discoverers chose to announce proposed names for the new elements, thus averting an element naming controversy temporarily. The dispute on discovery, however, dragged on until 1992, when the IUPAC/IUPAP Transfermium Working Group (TWG), formed to put an end to the controversy by making conclusions regarding discovery claims for elements 101 to 112, concluded that the Soviet synthesis of seaborgium-260 was not convincing enough, "lacking as it is in yield curves and angular selection results", whereas the American synthesis of seaborgium-263 was convincing due to its being firmly anchored to known daughter nuclei. As such, the TWG recognised the Berkeley team as official discoverers in their 1993 report.[43]
Element 106 was named after Glenn T. Seaborg, a pioneer in the discovery of synthetic elements, with the name seaborgium (Sg).
Seaborg pointing to the element named after him on the periodic table

Seaborg had previously suggested to the TWG that if Berkeley was recognised as the official discoverer of elements 104 and 105, they might propose the name kurchatovium (symbol Kt) for element 106 to honour the Dubna team, which had proposed this name for element 104 after Igor Kurchatov, the former head of the Soviet nuclear research programme. However, due to the worsening relations between the competing teams after the publication of the TWG report (because the Berkeley team vehemently disagreed with the TWG's conclusions, especially regarding element 104), this proposal was dropped from consideration by the Berkeley team.[45] After being recognized as official discoverers, the Berkeley team started deciding on a name in earnest:

...we were given credit for the discovery and the accompanying right to name the new element. The eight members of the Ghiorso group suggested a wide range of names honoring Isaac Newton, Thomas Edison, Leonardo da Vinci, Ferdinand Magellan, the mythical Ulysses, George Washington, and Finland, the native land of a member of the team. There was no focus and no front-runner for a long period.
Then one day Al [Ghiorso] walked into my office and asked what I thought of naming element 106 "seaborgium." I was floored.[46]
— Glenn Seaborg

Seaborg's son Eric remembered the naming process as follows:[47]

With eight scientists involved in the discovery suggesting so many good possibilities, Ghiorso despaired of reaching consensus, until he awoke one night with an idea. He approached the team members one by one, until seven of them had agreed. He then told his friend and colleague of 50 years: "We have seven votes in favor of naming element 106 seaborgium. Will you give your consent?" My father was flabbergasted, and, after consulting my mother, agreed.[47]
— Eric Seaborg

Glenn T. Seaborg

The name seaborgium and symbol Sg were announced at the 207th national meeting of the American Chemical Society in March 1994 by Kenneth Hulet, one of the co-discovers.[46] However, IUPAC resolved in August 1994 that an element could not be named after a living person, and Seaborg was still alive at the time. Thus, in September 1994, IUPAC recommended a set of names in which the names proposed by the three laboratories (the third being the GSI Helmholtz Centre for Heavy Ion Research in Darmstadt, Germany) with competing claims to the discovery for elements 104 to 109 were shifted to various other elements, in which rutherfordium (Rf), the Berkeley proposal for element 104, was shifted to element 106, with seaborgium being dropped entirely as a name.[45]

Summary of element naming proposals and final decisions for elements 101–112 (those covered in the TWG report)^[45]

Atomic number	Systematic	American	Russian	German	Compromise 92	IUPAC 94	ACS 94	IUPAC 95	IUPAC 97	Present
101	unnilunium	mendelevium	—	—	mendelevium	mendelevium	mendelevium	mendelevium	mendelevium	mendelevium
102	unnilbium	nobelium	joliotium	—	joliotium	nobelium	nobelium	flerovium	nobelium	nobelium
103	unniltrium	lawrencium	rutherfordium	—	lawrencium	lawrencium	lawrencium	lawrencium	lawrencium	lawrencium
104	unnilquadium	rutherfordium	kurchatovium	—	meitnerium	dubnium	rutherfordium	dubnium	rutherfordium	rutherfordium
105	unnilpentium	hahnium	nielsbohrium	—	kurchatovium	joliotium	hahnium	joliotium	dubnium	dubnium
106	unnilhexium	seaborgium	—	—	rutherfordium	rutherfordium	seaborgium	seaborgium	seaborgium	seaborgium
107	unnilseptium	—	—	nielsbohrium	nielsbohrium	bohrium	nielsbohrium	nielsbohrium	bohrium	bohrium
108	unniloctium	—	—	hassium	hassium	hahnium	hassium	hahnium	hassium	hassium
109	unnilennium	—	—	meitnerium	hahnium	meitnerium	meitnerium	meitnerium	meitnerium	meitnerium
110	ununnilium	hahnium	becquerelium	darmstadtium	—	—	—	—	—	darmstadtium
111	unununium	—	—	roentgenium	—	—	—	—	—	roentgenium
112	ununbium	—	—	copernicium	—	—	—	—	—	copernicium

This decision ignited a firestorm of worldwide protest for disregarding the historic discoverer's right to name new elements, and against the new retroactive rule against naming elements after living persons; the American Chemical Society stood firmly behind the name seaborgium for element 106, together with all the other American and German naming proposals for elements 104 to 109, approving these names for its journals in defiance of IUPAC.[45] At first, IUPAC defended itself, with an American member of its committee writing: "Discoverers don't have a right to name an element. They have a right to suggest a name. And, of course, we didn't infringe on that at all." However, Seaborg responded:

This would be the first time in history that the acknowledged and uncontested discoverers of an element are denied the privilege of naming it.[46]
— Glenn Seaborg

Bowing to public pressure, IUPAC proposed a different compromise in August 1995, in which the name seaborgium was reinstated for element 106 in exchange for the removal of all but one of the other American proposals, which met an even worse response. Finally, IUPAC rescinded these previous compromises and made a final, new recommendation in August 1997, in which the American and German proposals for elements 104 to 109 were all adopted, including seaborgium for element 106, with the single exception of element 105, named dubnium to recognise the contributions of the Dubna team to the experimental procedures of transactinide synthesis. This list was finally accepted by the American Chemical Society, which wrote:[45]

In the interest of international harmony, the Committee reluctantly accepted the name 'dubnium' for element 105 in place of 'hahnium' [the American proposal], which has had long-standing use in literature. We are pleased to note that 'seaborgium' is now the internationally approved name for element 106.[45]
— American Chemical Society

Seaborg commented regarding the naming:

I am, needless to say, proud that U.S. chemists recommended that element 106, which is placed under tungsten (74), be called 'seaborgium.' I was looking forward to the day when chemical investigators will refer to such compounds as seaborgous chloride, seaborgic nitrate, and perhaps, sodium seaborgate.
This is the greatest honor ever bestowed upon me—even better, I think, than winning the Nobel Prize.[k] Future students of chemistry, in learning about the periodic table, may have reason to ask why the element was named for me, and thereby learn more about my work.[46]
— Glenn Seaborg

Seaborg died a year and a half later, on 25 February 1999, at the age of 86.[46]
Isotopes
Main article: Isotopes of seaborgium

List of seaborgium isotopes

Isotope	Half-life[l]		Decay mode	Discovery year	Discovery reaction
	Value	ref
258Sg	2.7 ms	[7]	SF	1994	209Bi(51V,2n)
259Sg	402 ms	[7]	α	1985	207Pb(54Cr,2n)
259mSg	226 ms	[7]	α, SF	2015	206Pb(54Cr,n)[49]
260Sg	4.95 ms	[7]	SF, α	1985	208Pb(54Cr,2n)
261Sg	183 ms	[7]	α, β+, SF	1985	208Pb(54Cr,n)
261mSg	9.3 μs	[7]	IT	2009	208Pb(54Cr,n)
262Sg	10.3 ms	[7]	SF, α	2001	270Ds(—,2α)
263Sg	940 ms	[7]	α, SF	1994	271Ds(—,2α)
263mSg	420 ms	[7]	α	1974	249Cf(18O,4n)
264Sg	78 ms	[7]	SF	2006	238U(34Si,4n)
265Sg	9.2 s	[7]	α	1993	248Cm(22Ne,5n)
265mSg	16.4 s	[7]	α	1993	248Cm(22Ne,5n)
266Sg	390 ms	[7]	SF	2004	270Hs(—,α)
267Sg	1.8 min	[7]	SF, α	2004	271Hs(—,α)
268Sg	13 s	[8]	SF	2022	276Ds(—,2α)
269Sg	14 min	[9]	α	2010	285Fl(—,4α)
271Sg	31 s	[10]	α, SF	2003	287Fl(—,4α)

Superheavy elements such as seaborgium are produced by bombarding lighter elements in particle accelerators that induces fusion reactions. Whereas most of the isotopes of seaborgium can be synthesized directly this way, some heavier ones have only been observed as decay products of elements with higher atomic numbers.[50]

Depending on the energies involved, fusion reactions that generate superheavy elements are separated into "hot" and "cold". In hot fusion reactions, very light, high-energy projectiles are accelerated toward very heavy targets (actinides), giving rise to compound nuclei at high excitation energy (~40–50 MeV) that may either fission or evaporate several (3 to 5) neutrons.[50] In cold fusion reactions, the produced fused nuclei have a relatively low excitation energy (~10–20 MeV), which decreases the probability that these products will undergo fission reactions. As the fused nuclei cool to the ground state, they require emission of only one or two neutrons, and thus, allows for the generation of more neutron-rich products.[51] The latter is a distinct concept from that of where nuclear fusion claimed to be achieved at room temperature conditions (see cold fusion).[52]

Seaborgium has no stable or naturally occurring isotopes. Several radioactive isotopes have been synthesized in the laboratory, either by fusing two atoms or by observing the decay of heavier elements. Thirteen different isotopes of seaborgium have been reported with mass numbers 258–269 and 271, three of which, seaborgium-261, 263, and 265, have known metastable states. All of these decay only through alpha decay and spontaneous fission, with the single exception of seaborgium-261 that can also undergo electron capture to dubnium-261.[53]

There is a trend toward increasing half-lives for the heavier isotopes, though even–odd isotopes are generally more stable than their neighboring even–even isotopes, because the odd neutron leads to increased hindrance of spontaneous fission;^[54] among known seaborgium isotopes, alpha decay is the predominant decay mode in even–odd nuclei whereas fission dominates in even–even nuclei. Three of the heaviest known isotopes, ²⁶⁷Sg, ²⁶⁹Sg, and ²⁷¹Sg, are also the longest-lived, having half-lives on the order of 1 minute.^[53] Some other isotopes in this region are predicted to have comparable or even longer half-lives. Additionally, ²⁶³Sg, ²⁶⁵Sg, ^265mSg, and ²⁶⁸Sg^[8] have half-lives measured in seconds. All the remaining isotopes have half-lives measured in milliseconds, with the exception of the shortest-lived isotope, ^261mSg, with a half-life of only 92 microseconds.^[53]

The proton-rich isotopes from ²⁵⁸Sg to ²⁶¹Sg were directly produced by cold fusion; all heavier isotopes were produced from the repeated alpha decay of the heavier elements hassium, darmstadtium, and flerovium, with the exceptions of the isotopes ^263mSg, ²⁶⁴Sg, ²⁶⁵Sg, and ^265mSg, which were directly produced by hot fusion through irradiation of actinide targets. The twelve isotopes of seaborgium have half-lives ranging from 92 microseconds for ^261mSg to 14 minutes for ²⁶⁹Sg.^[9][53]

Predicted properties

Very few properties of seaborgium or its compounds have been measured; this is due to its extremely limited and expensive production[18] and the fact that seaborgium (and its parents) decays very quickly. A few singular chemistry-related properties have been measured, but properties of seaborgium metal remain unknown and only predictions are available.
Physical

Seaborgium is expected to be a solid under normal conditions and assume a body-centered cubic crystal structure, similar to its lighter congener tungsten.[2] Early predictions estimated that it should be a very heavy metal with density around 35.0 g/cm3,[1] but calculations in 2011 and 2013 predicted a somewhat lower value of 23–24 g/cm3.[3][4]
Chemical

Seaborgium is the fourth member of the 6d series of transition metals and the heaviest member of group 6 in the periodic table, below chromium, molybdenum, and tungsten. All the members of the group form a diversity of oxoanions. They readily portray their group oxidation state of +6, although this is highly oxidising in the case of chromium, and this state becomes more and more stable to reduction as the group is descended: indeed, tungsten is the last of the 5d transition metals where all four 5d electrons participate in metallic bonding.[55] As such, seaborgium should have +6 as its most stable oxidation state, both in the gas phase and in aqueous solution, and this is the only oxidation state that is experimentally known for it; the +5 and +4 states should be less stable, and the +3 state, the most common for chromium, would be the least stable for seaborgium.[1]

This stabilisation of the highest oxidation state occurs in the early 6d elements because of the similarity between the energies of the 6d and 7s orbitals, since the 7s orbitals are relativistically stabilised and the 6d orbitals are relativistically destabilised. This effect is so large in the seventh period that seaborgium is expected to lose its 6d electrons before its 7s electrons (Sg, [Rn]5f¹⁴6d⁴7s²; Sg⁺, [Rn]5f¹⁴6d³7s²; Sg²⁺, [Rn]5f¹⁴6d³7s¹; Sg⁴⁺, [Rn]5f¹⁴6d²; Sg⁶⁺, [Rn]5f¹⁴). Because of the great destabilisation of the 7s orbital, Sg^IV should be even more unstable than W^IV and should be very readily oxidised to Sg^VI. The predicted ionic radius of the hexacoordinate Sg⁶⁺ ion is 65 pm, while the predicted atomic radius of seaborgium is 128 pm. Nevertheless, the stability of the highest oxidation state is still expected to decrease as Lr^III > Rf^IV > Db^V > Sg^VI. Some predicted standard reduction potentials for seaborgium ions in aqueous acidic solution are as follows:^[1]

2 SgO3 + 2 H+ + 2 e−	⇌ Sg2O5 + H2O	E0 = −0.046 V
Sg2O5 + 2 H+ + 2 e−	⇌ 2 SgO2 + H2O	E0 = +0.11 V
SgO2 + 4 H+ + e−	⇌ Sg3+ + 2 H2O	E0 = −1.34 V
Sg3+ + e−	⇌ Sg2+	E0 = −0.11 V
Sg3+ + 3 e−	⇌ Sg	E0 = +0.27 V

Seaborgium should form a very volatile hexafluoride (SgF₆) as well as a moderately volatile hexachloride (SgCl₆), pentachloride (SgCl₅), and oxychlorides SgO₂Cl₂ and SgOCl₄.^[5] SgO₂Cl₂ is expected to be the most stable of the seaborgium oxychlorides and to be the least volatile of the group 6 oxychlorides, with the sequence MoO₂Cl₂ > WO₂Cl₂ > SgO₂Cl₂.^[1] The volatile seaborgium(VI) compounds SgCl₆ and SgOCl₄ are expected to be unstable to decomposition to seaborgium(V) compounds at high temperatures, analogous to MoCl₆ and MoOCl₄; this should not happen for SgO₂Cl₂ due to the much higher energy gap between the highest occupied and lowest unoccupied molecular orbitals, despite the similar Sg–Cl bond strengths (similarly to molybdenum and tungsten).^[56]

Molybdenum and tungsten are very similar to each other and show important differences to the smaller chromium, and seaborgium is expected to follow the chemistry of tungsten and molybdenum quite closely, forming an even greater variety of oxoanions, the simplest among them being seaborgate, SgO²⁻
₄, which would form from the rapid hydrolysis of Sg(H
₂O)⁶⁺
₆, although this would take place less readily than with molybdenum and tungsten as expected from seaborgium's greater size. Seaborgium should hydrolyse less readily than tungsten in hydrofluoric acid at low concentrations, but more readily at high concentrations, also forming complexes such as SgO₃F⁻ and SgOF⁻
₅: complex formation competes with hydrolysis in hydrofluoric acid.^[1]

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.^[57] The isotope ²⁶⁵Sg and its isomer ^265mSg are advantageous for radiochemistry: they are produced in the ²⁴⁸Cm(²²Ne,5n) reaction.^[58]

In the first experimental chemical studies of seaborgium in 1995 and 1996, seaborgium atoms were produced in the reaction ²⁴⁸Cm(²²Ne,4n)²⁶⁶Sg, thermalised, and reacted with an O₂/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 + O₂ + 2 HCl → SgO₂Cl₂ + H₂

In 2001, a team continued the study of the gas phase chemistry of seaborgium by reacting the element with O₂ in a H₂O 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.^[59]

2 Sg + 3 O₂ → 2 SgO₃

SgO₃ + H₂O → SgO₂(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 HNO₃/HF solution, most likely as neutral SgO₂F₂ or the anionic complex ion [SgO₂F₃]⁻ rather than SgO²⁻₄. In contrast, in 0.1 M nitric acid, seaborgium does not elute, unlike molybdenum and tungsten, indicating that the hydrolysis of [Sg(H₂O)₆]⁶⁺ only proceeds as far as the cationic complex [Sg(OH)₄(H₂O)]²⁺ or [SgO(OH)₃(H₂O)₂]⁺, while that of molybdenum and tungsten proceed to neutral [MO₂(OH)₂].^[1]

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)₆. Like its molybdenum and tungsten homologues, seaborgium hexacarbonyl is a volatile compound that reacts readily with silicon dioxide.^[57]

Absence in nature
See also: Island of stability § Possible natural occurrence

Searches for long-lived primordial nuclides of seaborgium in nature have all yielded negative results. One 2022 study estimated the concentration of seaborgium atoms in natural tungsten (its chemical homolog) is less than 5.1×10−15 atom(Sg)/atom(W).[60]
Notes

The names einsteinium and fermium for elements 99 and 100 were proposed when their namesakes (Albert Einstein and Enrico Fermi respectively) were still alive, but were not made official until Einstein and Fermi had died.[11]
In nuclear physics, an element is called heavy if its atomic number is high; lead (element 82) is one example of such a heavy element. The term "superheavy elements" typically refers to elements with atomic number greater than 103 (although there are other definitions, such as atomic number greater than 100[13] or 112;[14] sometimes, the term is presented an equivalent to the term "transactinide", which puts an upper limit before the beginning of the hypothetical superactinide series).[15] Terms "heavy isotopes" (of a given element) and "heavy nuclei" mean what could be understood in the common language—isotopes of high mass (for the given element) and nuclei of high mass, respectively.
In 2009, a team at JINR led by Oganessian published results of their attempt to create hassium in a symmetric 136Xe + 136Xe reaction. They failed to observe a single atom in such a reaction, putting the upper limit on the cross section, the measure of probability of a nuclear reaction, as 2.5 pb.[16] In comparison, the reaction that resulted in hassium discovery, 208Pb + 58Fe, had a cross section of ~20 pb (more specifically, 19+19
−11 pb), as estimated by the discoverers.[17]
The greater the excitation energy, the more neutrons are ejected. If the excitation energy is lower than energy binding each neutron to the rest of the nucleus, neutrons are not emitted; instead, the compound nucleus de-excites by emitting a gamma ray.[21]
The definition by the IUPAC/IUPAP Joint Working Party states that a chemical element can only be recognized as discovered if a nucleus of it has not decayed within 10−14 seconds. This value was chosen as an estimate of how long it takes a nucleus to acquire its outer electrons and thus display its chemical properties.[22] This figure also marks the generally accepted upper limit for lifetime of a compound nucleus.[23]
This separation is based on that the resulting nuclei move past the target more slowly then the unreacted beam nuclei. The separator contains electric and magnetic fields whose effects on a moving particle cancel out for a specific velocity of a particle.[25] Such separation can also be aided by a time-of-flight measurement and a recoil energy measurement; a combination of the two may allow to estimate the mass of a nucleus.[26]
Not all decay modes are caused by electrostatic repulsion. For example, beta decay is caused by the weak interaction.[31]
Since mass of a nucleus is not measured directly but is rather calculated from that of another nucleus, such measurement is called indirect. Direct measurements are also possible, but for the most part they have remained unavailable for heaviest nuclei.[32] The first direct measurement of mass of a superheavy nucleus was reported in 2018 at LBNL.[33] Mass was determined from the location of a nucleus after the transfer (the location helps determine its trajectory, which is linked to the mass-to-charge ratio of the nucleus, since the transfer was done in presence of a magnet).[34]
Spontaneous fission was discovered by Soviet physicist Georgy Flerov,[35] a leading scientist at JINR, and thus it was a "hobbyhorse" for the facility.[36] In contrast, the LBL scientists believed fission information was not sufficient for a claim of synthesis of an element. They believed spontaneous fission had not been studied enough to use it for identification of a new element, since there was a difficulty of establishing that a compound nucleus had only ejected neutrons and not charged particles like protons or alpha particles.[23] They thus preferred to link new isotopes to the already known ones by successive alpha decays.[35]
For instance, element 102 was mistakenly identified in 1957 at the Nobel Institute of Physics in Stockholm, Stockholm County, Sweden.[37] There were no earlier definitive claims of creation of this element, and the element was assigned a name by its Swedish, American, and British discoverers, nobelium. It was later shown that the identification was incorrect.[38] The following year, LBNL was unable to reproduce the Swedish results and announced instead their synthesis of the element; that claim was also disproved later.[38] JINR insisted that they were the first to create the element and suggested a name of their own for the new element, joliotium;[39] the Soviet name was also not accepted (JINR later referred to the naming of element 102 as "hasty").[40] The name "nobelium" remained unchanged on account of its widespread usage.[41]
Seaborg had in fact previously won the 1951 Nobel Prize in Chemistry together with Edwin McMillan for "their discoveries in the chemistry of the first transuranium elements".[48]

Different sources give different values for half-lives; the most recently published values are listed.

References

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Periodic table
H																															He
Li	Be																									B	C	N	O	F	Ne
Na	Mg																									Al	Si	P	S	Cl	Ar
K	Ca	Sc															Ti	V	Cr	Mn	Fe	Co	Ni	Cu	Zn	Ga	Ge	As	Se	Br	Kr
Rb	Sr	Y															Zr	Nb	Mo	Tc	Ru	Rh	Pd	Ag	Cd	In	Sn	Sb	Te	I	Xe
Cs	Ba	La	Ce	Pr	Nd	Pm	Sm	Eu	Gd	Tb	Dy	Ho	Er	Tm	Yb	Lu	Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg	Tl	Pb	Bi	Po	At	Rn
Fr	Ra	Ac	Th	Pa	U	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr	Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts	Og
Alkali metals Alkaline earth metals Lanthanoids Actinoids Transition metals Other metals Metalloids Other nonmetals Halogens Noble gases

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