Rutherfordium

Rutherfordium,  ₁₀₄Rf

General properties
Name, symbol	rutherfordium, Rf
Pronunciation	^i/ˌrʌðərˈfɔːrdiəm/ RUDH-ər-FOR-dee-əm
Rutherfordium in the periodic table
Hf ↑ Rf ↓ (Uph) lawrencium ← rutherfordium → dubnium
Atomic number (Z)	104
Group, block	group 4, d-block
Period	period 7
Element category	transition metal
Standard atomic weight (Ar)	[267]
Electron configuration	[Rn] 5f^14 6d^2 7s^2[1][2]
per shell	2, 8, 18, 32, 32, 10, 2
Physical properties
Phase	solid (predicted)[1][2]
Melting point	2400 K ​(2100 °C, ​3800 °F) (predicted)[1][2]
Boiling point	5800 K ​(5500 °C, ​9900 °F) (predicted)[1][2]
Density near r.t.	23.2 g/cm^3 (predicted)[1][2][3]
Atomic properties
Oxidation states	4,[1] (3), (2)[2][3] ​(parenthesized numbers are predictions)
Ionization energies	1st: 579.9 kJ/mol 2nd: 1389.4 kJ/mol 3rd: 2296.4 kJ/mol (more) (all estimated)[2]
Atomic radius	empirical: 150 pm (estimated)[2]
Covalent radius	157 pm (estimated)[1]
Miscellanea
Crystal structure	​hexagonal close-packed (hcp) (predicted)[4]
CAS Number	53850-36-5
History
Naming	after Ernest Rutherford
Discovery	Joint Institute for Nuclear Research (1964)
Most stable isotopes of rutherfordium
iso NA half-life DM DE (MeV) DP ^261Rf syn 70 s[5] >80% α 8.28 ^257No <15% ε ^261Lr <10% SF ^263Rf syn 15 min[5] <100% SF ~30% α 7.90 ? ^259No ^265Rf syn 1.0+1.2 −0.3 min​[6][7][8] SF ^266Rf? syn 10? h SF?/α? ^267Rf syn 1.3 h[5] SF ^268Rf? syn 6? h SF?/α?

Rutherfordium is a chemical element with symbol Rf and atomic number 104, named in honor of physicist Ernest Rutherford. 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, ²⁶⁷Rf, has a half-life of approximately 1.3 hours.

In the periodic table of the elements, it is a d-block element and the second of the fourth-row transition elements. It is a member of the 7th period and belongs to the group 4 elements. Chemistry experiments have confirmed that rutherfordium behaves as the heavier homologue to hafnium in group 4. The chemical properties of rutherfordium are characterized only partly. They compare well with the chemistry of the other group 4 elements, even though some calculations had indicated that the element might show significantly different properties due to relativistic effects.

In the 1960s, small amounts of rutherfordium were produced in laboratories in the former Soviet Union and in California. 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 International Union of Pure and Applied Chemistry (IUPAC) established rutherfordium as the official name for the element.

History

Discovery

Rutherfordium was reportedly first detected in 1964 at the Joint Institute of Nuclear Research at Dubna (then in the Soviet Union). Researchers there bombarded a plutonium-242 target with neon-22 ions and separated the reaction products by gradient thermochromatography after conversion to chlorides by interaction with ZrCl₄. The team identified spontaneous fission activity contained within a volatile chloride portraying eka-hafnium properties. Although a half-life was not accurately determined, later calculations indicated that the product was most likely rutherfordium-259 (abbreviated as ²⁵⁹Rf in standard notation):^[9]

242
94Pu + 22
10Ne → 264−x
104Rf → 264−x
104RfCl₄

In 1969, researchers at the University of California, Berkeley conclusively synthesized the element by bombarding a californium-249 target with carbon-12 ions and measured the alpha decay of ²⁵⁷Rf, correlated with the daughter decay of nobelium-253:^[10]

249
98Cf + 12
6C → 257
104Rf + 4 n

The American synthesis was independently confirmed in 1973 and secured the identification of rutherfordium as the parent by the observation of K-alpha X-rays in the elemental signature of the ²⁵⁷Rf decay product, nobelium-253.^[11]

Naming controversy

Element 104 was eventually named after Ernest Rutherford

The Russian scientists proposed the name kurchatovium and the American scientists suggested the name rutherfordium for the new element.^[12] In 1992, the IUPAC/IUPAP Transfermium Working Group (TWG) assessed the claims of discovery and concluded that both teams provided contemporaneous evidence to the synthesis of element 104 and that credit should be shared between the two groups.^[9]

The American group wrote a scathing response to the findings of the TWG, stating that they had given too much emphasis on the results from the Dubna group. In particular they pointed out that the Russian group had altered the details of their claims several times over a period of 20 years, a fact that the Russian team does not deny. They also stressed that the TWG had given too much credence to the chemistry experiments performed by the Russians and accused the TWG of not having appropriately qualified personnel on the committee. The TWG responded by saying that this was not the case and having assessed each point raised by the American group said that they found no reason to alter their conclusion regarding priority of discovery.^[13] The IUPAC finally used the name suggested by the American team (rutherfordium) which may in some way reflect a change of opinion.^[14]

As a consequence of the initial competing claims of discovery, an element naming controversy arose. Since the Soviets claimed to have first detected the new element they suggested the name kurchatovium, Ku, in honor of Igor Kurchatov (1903–1960), former head of Soviet nuclear research. This name had been used in books of the Soviet Bloc as the official name of the element. The Americans, however, proposed rutherfordium (Rf) for the new element to honor Ernest Rutherford, who is known as the "father" of nuclear physics. The International Union of Pure and Applied Chemistry (IUPAC) adopted unnilquadium, Unq, as a temporary, systematic element name, derived from the Latin names for digits 1, 0, and 4. In 1994, IUPAC suggested the name dubnium to be used since rutherfordium was suggested for element 106 and IUPAC felt that the Dubna team should be rightly recognized for their contributions. However, there was still a dispute over the names of elements 104–107. In 1997 the teams involved resolved the dispute and adopted the current name rutherfordium. The name dubnium was given to element 105 at the same time.^[14]

Isotopes

Isotope half-lives and discovery years

Isotope	Half-life [5]	Decay mode[5]	Discovery year	Reaction
^253Rf	48 μs	α, SF	1994	^204Pb(^50Ti,n)[15]
^254Rf	23 μs	SF	1994	^206Pb(^50Ti,2n)[15]
^255Rf	2.3 s	ε?, α, SF	1974	^207Pb(^50Ti,2n)[16]
^256Rf	6.4 ms	α, SF	1974	^208Pb(^50Ti,2n)[16]
^257Rf	4.7 s	ε, α, SF	1969	^249Cf(^12C,4n)[10]
^257mRf	4.1 s	ε, α, SF	1969	^249Cf(^12C,4n)[10]
^258Rf	14.7 ms	α, SF	1969	^249Cf(^13C,4n)[10]
^259Rf	3.2 s	α, SF	1969	^249Cf(^13C,3n)[10]
^259mRf	2.5 s	ε	1969	^249Cf(^13C,3n)[10]
^260Rf	21 ms	α, SF	1969	^248Cm(^16O,4n)[9]
^261Rf	78 s	α, SF	1970	^248Cm(^18O,5n)[17]
^261mRf	4 s	ε, α, SF	2001	^244Pu(^22Ne,5n)[18]
^262Rf	2.3 s	α, SF	1996	^244Pu(^22Ne,4n)[19]
^263Rf	15 min	α, SF	1999	^263Db(e−,ν e)[20]
^263mRf ?	8 s	α, SF	1999	^263Db(e−,ν e)[20]
^264Rf	1? h	α ?	unknown	—
^265Rf	1.0 min[7][8]	SF	2010	^269Sg(—,α)[6]
^266Rf	23 s?	α, SF ?	2007?	^266Db(e−,ν e)?[21][22]
^267Rf	1.3 h	SF	2004	^271Sg(—,α)[23]
^268Rf	1.5 s?	α, SF ?	2004?	^268Db(e−,ν e)?[22][24]

Rutherfordium 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. Fifteen different isotopes have been reported with atomic masses from 253 to 268 (with the exception of 264). Most of these decay predominantly through spontaneous fission pathways.^[5][25]

Life-times

Out of isotopes whose half-lives are known, the lighter isotopes usually have shorter half-lives; half-lives of under 50 μs for ²⁵³Rf and ²⁵⁴Rf were observed. ²⁵⁶Rf, ²⁵⁸Rf, ²⁶⁰Rf are more stable at around 10 ms, ²⁵⁵Rf, ²⁵⁷Rf, ²⁵⁹Rf, and ²⁶²Rf live between 1 and 5 seconds, and ²⁶¹Rf, ²⁶⁵Rf, and ²⁶³Rf are more stable, at around 1, 1.5, and 10 min respectively. The heaviest isotopes are the most stable, with ²⁶⁷Rf having a measured half-life of about 1.3 h.^[5] Half-lives for ²⁶⁹Rf and higher are not known.

The lightest isotopes were synthesized by direct fusion between two lighter nuclei and as decay products. The heaviest isotope produced by direct fusion is ²⁶²Rf; heavier isotopes have only been observed as decay products of elements with larger atomic numbers, of which only ²⁶⁷Rf has been confirmed. The isotopes ²⁶⁶Rf and ²⁶⁸Rf may have also been observed as decay products, but have short half-lives to spontaneous fission. While the isotope ²⁶⁴Rf has yet to be observed, it is predicted to have a long half-life of 1 h.^[5] Before its discovery, ²⁶⁵Rf was predicted to have an even longer half-life of 13 h,^[5] but it has a half-life of only 2.5 min.^[6]

In 1999, American scientists at the University of California, Berkeley, announced that they had succeeded in synthesizing three atoms of ²⁹³118.^[26] These parent nuclei were reported to have successively emitted seven alpha particles to form ²⁶⁵Rf nuclei, but their claim was retracted in 2001.^[27]

Predicted properties

Chemical

Rutherfordium is the first transactinide element and the first member of the 6d series of transition metals. Calculations on its ionization potentials, atomic radius, as well as radii, orbital energies, and ground levels of its ionized states are similar to that of hafnium and very different from that of lead. Therefore, it was concluded that rutherfordium's basic properties will resemble those of other group 4 elements, below titanium, zirconium, and hafnium.^[20][28] Some of its properties were determined by gas-phase experiments and aqueous chemistry. The oxidation state +4 is the only stable state for the latter two elements and therefore rutherfordium should also exhibit a stable +4 state.^[28] In addition, rutherfordium is also expected to be able to form a less stable +3 state.^[2]

The chemical properties of rutherfordium were based on calculation which indicated that the relativistic effects on the electron shell might be strong enough that the p orbitals have a lower energy level than the d orbitals, giving it a valence electron configuration of 6d¹ 7s² 7p¹ or even 7s² 7p², therefore making the element behave more like lead than hafnium. With better calculation methods and studies of the chemical properties of rutherfordium compounds it could be shown that rutherfordium behaves according to the rest of the group 4 elements.^[28][2]

In an analogous manner to zirconium and hafnium, rutherfordium is projected to form a very stable, high melting point oxide, RfO₂. It reacts with halogens to form tetrahalides, RfX₄, which hydrolyze on contact with water to form oxyhalides RfOX₂. The tetrahalides are volatile solids existing as monomeric tetrahedral molecules in the vapor phase.^[28]

In the aqueous phase, the Rf⁴⁺ ion hydrolyzes less than titanium(IV) and to a similar extent as zirconium and hafnium, thus resulting in the RfO²⁺ ion. Treatment of the halides with halide ions promotes the formation of complex ions. The use of chloride and bromide ions produces the hexahalide complexes RfCl2−
6 and RfBr2−
6. For the fluoride complexes, zirconium and hafnium tend to form hepta- and octa- complexes. Thus, for the larger rutherfordium ion, the complexes RfF2−
6, RfF3−
7 and RfF4−
8 are possible.^[28]

Physical and atomic

Rutherfordium is expected to be a solid under normal conditions and assume a hexagonal close-packed crystal structure (^c/_a = 1.61), similar to its lighter congener hafnium.^[4] It should be a very heavy metal with a density of around 23.2 g/cm³; in comparison, the densest known element that has had its density measured, osmium, has a density of 22.61 g/cm³. This results from rutherfordium's high atomic weight, the lanthanide and actinide contractions, and relativistic effects, although production of enough rutherfordium to measure this quantity would be impractical, and the sample would quickly decay. The atomic radius for rutherfordium is expected to be around 150 pm. Due to the relativistic stabilization of the 7s orbital and destabilization of the 6d orbital, the Rf⁺ and Rf²⁺ ions are predicted to give up 6d electrons instead of 7s electrons, which is the opposite of the behavior of its lighter homologues.^[2]

Experimental chemistry

Summary of compounds and complex ions

Formula	Names
RfCl4	rutherfordium tetrachloride, rutherfordium(IV) chloride
RfBr4	rutherfordium tetrabromide, rutherfordium(IV) bromide
RfOCl2	rutherfordium oxychloride, rutherfordyl(IV) chloride, rutherfordium(IV) dichloride oxide
[RfCl6]^2−	hexachlororutherfordate(IV)
[RfF6]^2−	hexafluororutherfordate(IV)
K2[RfCl6]	potassium hexachlororutherfordate(IV)

Gas phase

The tetrahedral structure of the RfCl₄ molecule

Early work on the study of the chemistry of rutherfordium focused on gas thermochromatography and measurement of relative deposition temperature adsorption curves. The initial work was carried out at Dubna in an attempt to reaffirm their discovery of the element. Recent work is more reliable regarding the identification of the parent rutherfordium radioisotopes. The isotope ^261mRf has been used for these studies. The experiments relied on the expectation that rutherfordium would begin the new 6d series of elements and should therefore form a volatile tetrachloride due to the tetrahedral nature of the molecule.^[28][29][30] Rutherfordium(IV) chloride is more volatile than its lighter homologue hafnium(IV) chloride (HfCl₄) because its bonds are more covalent.^[2]

A series of experiments confirmed that rutherfordium behaves as a typical member of group 4, forming a tetravalent chloride (RfCl₄) and bromide (RfBr₄) as well as an oxychloride (RfOCl₂). A decreased volatility was observed for RfCl
4 when potassium chloride is provided as the solid phase instead of gas, highly indicative of the formation of nonvolatile K
2RfCl
6 mixed salt.^[20][28][31]

Aqueous phase

Rutherfordium is expected to have the electron configuration [Rn]5f¹⁴ 6d² 7s² and therefore behave as the heavier homologue of hafnium in group 4 of the periodic table. It should therefore readily form a hydrated Rf⁴⁺ ion in strong acid solution and should readily form complexes in hydrochloric acid, hydrobromic or hydrofluoric acid solutions.^[28]

The most conclusive aqueous chemistry studies of rutherfordium have been performed by the Japanese team at Japan Atomic Energy Research Institute using the radioisotope ^261mRf. Extraction experiments from hydrochloric acid solutions using isotopes of rutherfordium, hafnium, zirconium, and thorium have proved a non-actinide behavior for rutherfordium. A comparison with its lighter homologues placed rutherfordium firmly in group 4 and indicated the formation of a hexachlororutherfordate complex in chloride solutions, in a manner similar to hafnium and zirconium.^[28][32]

261m
Rf4+
+ 6 Cl−
→ [^261mRfCl
6]2−

Very similar results were observed in hydrofluoric acid solutions. Differences in the extraction curves were interpreted as a weaker affinity for fluoride ion and the formation of the hexafluororutherfordate ion, whereas hafnium and zirconium ions complex seven or eight fluoride ions at the concentrations used:^[28]

261m
Rf4+
+ 6 F−
→ [^261mRfF
6]2−

References

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External links

• Rutherfordium at The Periodic Table of Videos (University of Nottingham)
• WebElements.com – Rutherfordium