Bohrium

Bohrium,  ₁₀₇Bh

General properties
Name, symbol	bohrium, Bh
Pronunciation	i/ˈbɔəriəm/
Bohrium in the periodic table
Re ↑ Bh ↓ (Uhu) seaborgium ← bohrium → hassium
Atomic number (Z)	107
Group, block	group 7, d-block
Period	period 7
Element category	transition metal
Standard atomic weight (Ar)	[270]
Electron configuration	[Rn] 5f14 6d5 7s2 [1][2]
per shell	2, 8, 18, 32, 32, 13, 2
Physical properties
Phase	solid (predicted)[3]
Density near r.t.	37.1 g/cm3 (predicted)[2][4]
Atomic properties
Oxidation states	7, (5), (4), (3)[2][4] ​(parenthesized oxidation states are predictions)
Ionization energies	1st: 742.9 kJ/mol 2nd: 1688.5 kJ/mol 3rd: 2566.5 kJ/mol (more) (all but first estimated)[2]
Atomic radius	empirical: 128 pm (predicted)[2]
Covalent radius	141 pm (estimated)[5]
Miscellanea
Crystal structure	​hexagonal close-packed (hcp) (predicted)[3]
CAS Number	54037-14-8
History
Naming	after Niels Bohr
Discovery	Gesellschaft für Schwerionenforschung (1981)
Most stable isotopes of bohrium
iso NA half-life DM DE (MeV) DP 274Bh syn ~54 s[6] α 8.8 270Db 272Bh syn 9.8 s α 9.02 268Db 271Bh syn 1.2 s[7] α 9.35[7] 267Db 270Bh syn 61 s α 8.93 266Db 267Bh syn 17 s α 8.83 263Db

Bohrium is a chemical element with symbol Bh and atomic number 107. It is named after Danish physicist Niels Bohr. It is a synthetic element (an element that can be created in a laboratory but is not found in nature) and radioactive; the most stable known isotope, ²⁷⁰Bh, has a half-life of approximately 61 seconds.

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 7 elements as the fifth member of the 6d series of transition metals. Chemistry experiments have confirmed that bohrium behaves as the heavier homologue to rhenium in group 7. The chemical properties of bohrium are characterized only partly, but they compare well with the chemistry of the other group 7 elements.

History

Element 107 was originally proposed to be named after Niels Bohr, a Danish nuclear physicist, with the name nielsbohrium (Ns). This name was later changed by IUPAC to bohrium (Bh).

Discovery

Two groups claimed discovery of the element. Evidence of bohrium was first reported in 1976 by a Russian research team led by Yuri Oganessian, in which targets of bismuth-209 and lead-208 were bombarded with accelerated nuclei of chromium-54 and manganese-58 respectively.^[8] Two activities, one with a half-life of one to two milliseconds, and the other with an approximately five-second half-life, were seen. Since the ratio of the intensities of these two activities was constant throughout the experiment, it was proposed that the first was from the isotope bohrium-261 and that the second was from its daughter dubnium-257. Later, the dubnium isotope was corrected to dubnium-258, which indeed has a five-second half-life (dubnium-257 has a one-second half-life); however, the half-life observed for its parent is much shorter than the half-lives later observed in the definitive discovery of bohrium at Darmstadt in 1981. The IUPAC/IUPAP Transfermium Working Group (TWG) concluded that while dubnium-258 was probably seen in this experiment, the evidence for the production of its parent bohrium-262 was not convincing enough.^[9]

In 1981, a German research team led by Peter Armbruster and Gottfried Münzenberg at the GSI Helmholtz Centre for Heavy Ion Research (GSI Helmholtzzentrum für Schwerionenforschung) in Darmstadt bombarded a target of bismuth-209 with accelerated nuclei of chromium-54 to produce 5 atoms of the isotope bohrium-262:^[10]

209
83Bi
+ 54
24Cr
→ 262
107Bh
+
n

This discovery was further substantiated by their detailed measurements of the alpha decay chain of the produced bohrium atoms to previously known isotopes of fermium and californium. The IUPAC/IUPAP Transfermium Working Group (TWG) recognised the GSI collaboration as official discoverers in their 1992 report.^[9]

Proposed names

The German group suggested the name nielsbohrium with symbol Ns to honor the Danish physicist Niels Bohr. The Soviet scientists at the Joint Institute for Nuclear Research in Dubna, Russia had suggested this name be given to element 105 (which was finally called dubnium) and the German team wished to recognise both Bohr and the fact that the Dubna team had been the first to propose the cold fusion reaction to solve the controversial problem of the naming of element 105. The Dubna team agreed with the German group's naming proposal for element 107.^[11]

There was an element naming controversy as to what the elements from 104 to 106 were to be called; the IUPAC adopted unnilseptium (symbol Uns) as a temporary, systematic element name for this element.^[12] In 1994 a committee of IUPAC recommended that element 107 be named bohrium, not nielsbohrium, since there was no precedence for using a scientist's complete name in the naming of an element.^[12][13] This was opposed by the discoverers as there was some concern that the name might be confused with boron and in particular the distinguishing of the names of their respective oxyanions, bohrate and borate. The matter was handed to the Danish branch of IUPAC which, despite this, voted in favour of the name bohrium, and thus the name bohrium for element 107 was recognized internationally in 1997.^[12]

Isotopes

Bohrium 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. Eleven different isotopes of bohrium have been reported with atomic masses 260–262, 264–267, 270–272, and 274, one of which, bohrium-262, has a known metastable state. All of these decay only through alpha decay, although some unknown bohrium isotopes are predicted to undergo spontaneous fission.^[14]

The lighter isotopes usually have shorter half-lives; half-lives of under 100 ms for ²⁶⁰Bh, ²⁶¹Bh, ²⁶²Bh, and ^262mBh were observed. ²⁶⁴Bh, ²⁶⁵Bh, ²⁶⁶Bh, and ²⁷¹Bh are more stable at around 1 s, and ²⁶⁷Bh and ²⁷²Bh have half-lives of about 10 s. The heaviest isotopes are the most stable, with ²⁷⁰Bh and ²⁷⁴Bh having measured half-lives of about 61 s and 54 s respectively. The unknown isotopes ²⁷³Bh and ²⁷⁵Bh are predicted to have even longer half-lives of around 90 minutes and 40 minutes respectively. Before its discovery, ²⁷⁴Bh was also predicted to have a long half-life of 90 minutes, but it was found to have a shorter half-life of only about 54 seconds.^[14]

The proton-rich isotopes with masses 260, 261, and 262 were directly produced by cold fusion, those with mass 262 and 264 were reported in the decay chains of meitnerium and roentgenium, while the neutron-rich isotopes with masses 265, 266, 267 were created in irradiations of actinide targets. The four most neutron-rich ones with masses 270, 271, 272, and 274 appear in the decay chains of ²⁸²Nh, ²⁸⁷Mc, ²⁸⁸Mc, and ²⁹⁴Ts respectively. These eleven isotopes have half-lives ranging from about ten milliseconds for ^262mBh to about one minute for ²⁷⁰Bh and ²⁷⁴Bh.^[22]

Predicted properties

Chemical

Bohrium is the fifth member of the 6d series of transition metals and the heaviest member of group 7 in the Periodic Table, below manganese, technetium and rhenium. All the members of the group readily portray their group oxidation state of +7 and the state becomes more stable as the group is descended. Thus bohrium is expected to form a stable +7 state. Technetium also shows a stable +4 state whilst rhenium exhibits stable +4 and +3 states. Bohrium may therefore show these lower states as well.^[4] The higher +7 oxidation state is more likely to exist in oxyanions, such as perbohrate, BhO−
4, analogous to the lighter permanganate, pertechnetate, and perrhenate. Nevertheless, bohrium(VII) is likely to be unstable in aqueous solution, and would probably be easily reduced to the more stable bohrium(IV).^[2]

Technetium and rhenium are known to form volatile heptoxides M₂O₇ (M = Tc, Re), so bohrium should also form the volatile oxide Bh₂O₇. The oxide should dissolve in water to form perbohric acid, HBhO₄. Rhenium and technetium form a range of oxyhalides from the halogenation of the oxide. The chlorination of the oxide forms the oxychlorides MO₃Cl, so BhO₃Cl should be formed in this reaction. Fluorination results in MO₃F and MO₂F₃ for the heavier elements in addition to the rhenium compounds ReOF₅ and ReF₇. Therefore, oxyfluoride formation for bohrium may help to indicate eka-rhenium properties.^[23] Since the oxychlorides are asymmetrical, and they should have increasingly large dipole moments going down the group, they should become less volatile in the order TcO₃Cl > ReO₃Cl > BhO₃Cl: this was experimentally confirmed in 2000 by measuring the enthalpies of adsorption of these three compounds. The values are for TcO₃Cl and ReO₃Cl are −51 kJ/mol and −61 kJ/mol respectively; the experimental value for BhO₃Cl is −77.8 kJ/mol, very close to the theoretically expected value of −78.5 kJ/mol.^[2]

Physical and atomic

Bohrium is expected to be a solid under normal conditions and assume a hexagonal close-packed crystal structure (^c/_a = 1.62), similar to its lighter congener rhenium.^[3] It should be a very heavy metal with a density of around 37.1 g/cm³, which would be the third-highest of any of the 118 known elements, lower than only meitnerium (37.4 g/cm³) and hassium (41 g/cm³), the two following elements in the periodic table. In comparison, the densest known element that has had its density measured, osmium, has a density of only 22.61 g/cm³. This results from bohrium's high atomic weight, the lanthanide and actinide contractions, and relativistic effects, although production of enough bohrium to measure this quantity would be impractical, and the sample would quickly decay.^[2]

The atomic radius of bohrium is expected to be around 128 pm.^[2] Due to the relativistic stabilization of the 7s orbital and destabilization of the 6d orbital, the Bh⁺ ion is predicted to have an electron configuration of [Rn] 5f¹⁴ 6d⁴ 7s², giving up a 6d electron instead of a 7s electron, which is the opposite of the behavior of its lighter homologues manganese and technetium. Rhenium, on the other hand, follows its heavier congener bohrium in giving up a 5d electron before a 6s electron, as relativistic effects have become significant by the sixth period, where they cause among other things the yellow color of gold and the low melting point of mercury. The Bh²⁺ ion is expected to have an electron configuration of [Rn] 5f¹⁴ 6d³ 7s²; in contrast, the Re²⁺ ion is expected to have a [Xe] 4f¹⁴ 5d⁵ configuration, this time analogous to manganese and technetium.^[2] The ionic radius of hexacoordinate heptavalent bohrium is expected to be 58 pm (heptavalent manganese, technetium, and rhenium having values of 46, 57, and 53 pm respectively). Pentavalent bohrium should have a larger ionic radius of 83 pm.^[2]

Experimental chemistry

In 1995, the first report on attempted isolation of the element was unsuccessful, prompting new theoretical studies to investigate how best to investigate bohrium (using its lighter homologs technetium and rhenium for comparison) and removing unwanted contaminating elements such as the trivalent actinides, the group 5 elements, and polonium.^[24]

In 2000, it was confirmed that although relativistic effects are important, bohrium behaves like a typical group 7 element.^[25] A team at the Paul Scherrer Institute (PSI) conducted a chemistry reaction using six atoms of ²⁶⁷Bh produced in the reaction between ²⁴⁹Bk and ²²Ne ions. The resulting atoms were thermalised and reacted with a HCl/O₂ mixture to form a volatile oxychloride. The reaction also produced isotopes of its lighter homologues, technetium (as ¹⁰⁸Tc) and rhenium (as ¹⁶⁹Re). The isothermal adsorption curves were measured and gave strong evidence for the formation of a volatile oxychloride with properties similar to that of rhenium oxychloride. This placed bohrium as a typical member of group 7.^[26] The adsorption enthalpies of the oxychlorides of technetium, rhenium, and bohrium were measured in this experiment, agreeing very well with the theoretical predictions and implying a sequence of decreasing oxychloride volatility down group 7 of TcO₃Cl > ReO₃Cl > BhO₃Cl.^[2]

2 Bh + 3 O
2 + 2 HCl → 2 BhO
3Cl + H
2

References

External links

• Bohrium at The Periodic Table of Videos (University of Nottingham)