Absolute isotopic abundance ratio and atomic weight of terrestrial rubidium

Catanzaro, E.J.; Murphy, Thomas J.; Garner, E. L.; Shields, William R.

doi:10.6028/jres.073a.041

Cited by 70 publications

(38 citation statements)

References 3 publications

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“…Previous elements studied include silver [1] ,1 chlorine [2], copper [3], bromine [4], chromium [5], magnesium [6], lead _ [7], boron [8], and rubidium [9]. The present work extends the study to rhenium.…”

Section: Introductionmentioning

confidence: 72%

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Absolute isotopic abundance ratio and atomic weight of a reference sample of rhenium

Gramlich¹,

Murphy²,

Garner³

et al. 1973

J. RES. NATL. BUR. STAN. SECT. A.

127

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,An absolute value has been obtained for the isotopic abundance ratio of a reference sample of rhenium, using surface emission mass spectrometry. Samples of known isotopic composition , prepared from nearly isotopically pure se parat ed rhenium isotopes , were used to calibrate the mass spectrometers. The resulting absolute '85 Re/'·7 Re ratio is 0.59738 ± 0.00039, which yields atom per· cents of ' 8s Re=37 .398±0.016 and '87Re=62.602±0.016. The atomi c weight calculated from this isotopi c c omposition is 186.20679 ± 0.00031. The indi cated uncertainties are overall limits of e rror based on 95 perce nt confidence limits for th e mean and allowances for the effe cts of known sources of possible systematic error.

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Section: Introductionmentioning

confidence: 72%

“…That a single bias correction is valid for the single stage instrument over the range of isotopic compositions measured has been established previously through the measurement of synthetic isotopic mixtures of boron [8], chromium [5], magnesium [6], and rubidium [9].…”

Section: Mass Spectrometrymentioning

confidence: 98%

Absolute isotopic abundance ratio and atomic weight of a reference sample of rhenium

Gramlich¹,

Murphy²,

Garner³

et al. 1973

J. RES. NATL. BUR. STAN. SECT. A.

127

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“…In this study, an error due to isobaric interferences of 84 Kr and 86 Kr signals was corrected using an "on-peak" baseline-subtraction method. In the case of isobaric interference of 87 19 ) and C is a correction factor (discussed later). 85 Rbmeas is the measured intensity, and 87 Rbcalc denotes the calculated 87 Rb value, respectively.…”

Section: Correction Of Isobaric Interferencesmentioning

confidence: 99%

Simultaneous Determination of Mass-dependent Isotopic Fractionation and Radiogenic Isotope Variation of Strontium in Geochemical Samples by Multiple Collector-ICP-Mass Spectrometry

2007

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“…In 1969, CAWIA [4] recommended the current value of A r (Rb) = 85.4678(3) based on the "absolute" isotope-abundance measurement by Catanzaro et al [145], who reported a mole fraction of 85 Rb = 0.72165 (13), plus the work of Shields et al [363], who found no isotopic variations in terrestrial samples, and the atomic masses of Wapstra and Gove [48]. 87 Rb is β -active with a half-life of 4.88(5) × 10 10 a, which leaves A r (Rb) unaffected at the currently given precision of about 3 × 10 -6 in up to 10 6 a.…”

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confidence: 99%

Atomic weights of the elements. Review 2000 (IUPAC Technical Report)

Laeter¹,

Böhlke²,

Bièvre³

et al. 2003

Pure and Applied Chemistry

910

554

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Republication or reproduction of this report or its storage and/or dissemination by electronic means is permitted without the need for formal IUPAC permission on condition that an acknowledgmentAbstract: A consistent set of internationally accepted atomic weights has long been an essential aim of the scientific community because of the relevance of these values to science and technology, as well as to trade and commerce subject to ethical, legal, and international standards. The standard atomic weights of the elements are regularly evaluated, recommended, and published in updated tables by the Commission on Atomic Weights and Isotopic Abundances (CAWIA) of the International Union of Pure and Applied Chemistry (IUPAC). These values are invariably associated with carefully evaluated uncertainties. Atomic weights were originally determined by mass ratio measurements coupled with an understanding of chemical stoichiometry, but are now based almost exclusively on knowledge of the isotopic composition (derived from isotope-abundance ratio measurements) and the atomic masses of the isotopes of the elements. Atomic weights and atomic masses are now scaled to a numerical value of exactly 12 for the mass of the carbon isotope of mass number 12. Technological advances in mass spectrometry and nuclear-reaction energies have enabled atomic masses to be determined with a relative uncertainty of better than 1 × 10 -7 . Isotope abundances for an increasing number of elements can be measured to better than 1 × 10 -3 . The excellent precision of such measurements led to the discovery that many elements, in different specimens, display significant variations in their isotope-abundance ratios, caused by a variety of natural and industrial physicochemical processes. While such variations increasingly place a constraint on the uncertainties with which some standard atomic weights can be stated, they provide numerous opportunities for investigating a range of important phenomena in physical, chemical, cosmological, biological, and industrial processes. This review reflects the current and increasing interest of science in the measured differences between source-specific and even sample-specific atomic weights. These relative comparisons can often be made with a smaller uncertainty than is achieved in the best calibrated "absolute" (= SI-traceable) atomic-weight determinations. Accurate determinations of the atomic weights of certain elements also influence the values of fundamental constants such as the Avogadro, Faraday, and universal gas constants. This review is in two parts: the first summarizes the development of the science of atomic-weight determinations during the 20 th century; the second summarizes the changes and variations that have been recognized in the values and uncertainties of atomic weights, on an element-by-element basis, in the latter part of the 20 th century.J. R. de LAETER et al.

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Absolute isotopic abundance ratio and atomic weight of terrestrial rubidium

Cited by 70 publications

References 3 publications

Absolute isotopic abundance ratio and atomic weight of a reference sample of rhenium

Absolute isotopic abundance ratio and atomic weight of a reference sample of rhenium

Simultaneous Determination of Mass-dependent Isotopic Fractionation and Radiogenic Isotope Variation of Strontium in Geochemical Samples by Multiple Collector-ICP-Mass Spectrometry

Atomic weights of the elements. Review 2000 (IUPAC Technical Report)

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