Ar Atomic Mass

Isotope	Atomic mass (Da)	Isotopic abundance (amount fraction)
³⁶Ar	35.967 5451(2)	[0.0000, 0.0207]
³⁸Ar	37.962 732(2)	[0.000, 0.043]
⁴⁰Ar	39.962 383 12(2)	[0.936, 1.000]

Atomic Mass Vs Atomic Number
Element Ar
Ar Atomic Number
Element Ar Atomic Mass
Ar Atomic Mass In Kg
Ar Relative Atomic Mass

There is a difference between the meanings of the chemistry terms atomic mass and mass number.One is the average weight of an element and the other is the total number of nucleons in the atom's nucleus. Atomic Mass of Argon Atomic mass of Argon is 39.948 u.

The most abundant isotope of argon in the universe is argon-36, which is made when stars with a mass about 11 times greater than the Sun are in their silicon-burning phase. In this phase, an alpha particle (helium nucleus) is added to a silicon-32 nucleus to make sulfur-34, which adds an alpha particle to become argon-36.
Ar I Ground State 1s 2 2s 2 2p 6 3s 2 3p 6 1 S 0 Ionization energy 127109.842 cm-1 (15.759610 eV) Ref. VHU99 Ar II Ground State 1s 2 2s 2 2p 6 3s 2 3p 5 2 P° 3 / 2 Ionization energy 222848.3 cm-1 (27.62966 eV) Ref.
Atomic mass of Argon is 39.948 u. The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a.

The atomic weight of argon is based on analyses of argon separated from air. In 1961, the Commissionchanged the recommended value of A_r(Ar) from 39.944, based on gas density measurements, to 39.948,based on the calibrated mass-spectrometric measurements reported by Nier.In 1979, the Commission examined the available literature and recommended A_r(Ar) = 39.948(1). This value of A_r(Ar) was one of the critical parameters to determinethe value of the universal gas constant R by acoustic methods.

In 2007, the Commission recommended value for the isotope-amount ratio of n(⁴⁰Ar)/n(³⁶Ar) in air, which isof importance in geochronology and geochemistry, as 298.56(31).

The isotopic composition and atomic weight of argon are variable in terrestrial materials. Those variations are a source of uncertainty in the assignment of standard properties for argon, but they provide useful information in many areas of science. Variations in the stable isotopic composition and atomic weight of argon are caused by several different processes, including
(1) isotope production from other elements by radioactive decay (radiogenic isotopes) or other nuclear transformations (e.g., nucleogenic isotopes), and
(2) isotopic fractionation by physical-chemical processes such as diffusion or phase equilibria.
Physical-chemical processes cause correlated mass-dependent variations in the argon isotope-amount ratios (⁴⁰Ar/³⁶Ar and ³⁸Ar/³⁶Ar), whereas nuclear transformation processes cause mass-independent variations. While atmospheric argon can serve as an abundant and homogeneous isotopic reference, deviations from the atmospheric isotopic ratios in other argon occurrences limit the precision with which a standard atomic weight can be given for argon. Published data indicate variation of argon atomic weights in normal terrestrial materials between 39.792 and 39.963. The upper bound of this interval is given by the atomic mass of ⁴⁰Ar, as some samples contain almost pure radiogenic argon-40. The lower bound is derived from analyses of pitchblende (uranium mineral) containing large amounts of nucleogenic ³⁶Ar and ³⁸Ar. Within this interval, measurements of different isotope ratios (⁴⁰Ar/³⁶Ar or ³⁸Ar/³⁶Ar) at various levels of precision are widely used for studies in geochronology, water–rock interaction, atmospheric evolution, and other fields.

Radiogenic ⁴⁰Ar is produced (along with ⁴⁰Ca) by decay of a minor isotope of potassium (⁴⁰K), whichhas a total half-life of 1.26(1) Ga. This radioactivity results in many geological samples havinganomalous amounts of ⁴⁰Ar and is the basis of the K-Ar and Ar-Ar dating methods used in geochronology.Samples containing only minor components of noble gases from non-radiogenic sources may have A_r(Ar) values approachingthat of pure ⁴⁰Ar. Owing to the wide distribution of potassium, even major sources of Ar suchas some natural gas deposits and geothermal reservoirs can have sufficiently high ⁴⁰Ar concentrations.

In contrast, it is much less common for natural samples to have n(⁴⁰Ar)/n(³⁶Ar) ratios significantly less than that of air. Radiogenic ³⁶Ar can accumulate by decay of ³⁶Cl (half-life = 0.301(2) Ma), which in turn is produced from ³⁵Cl by neutron capture associated with cosmic-ray interactions in the atmosphere and with U and Th decayin the solid earth. Similarly, ³⁸Ar may accumulate as a result of reactions such as ³⁷Cl(n,γ)³⁸Cl or ³⁵Cl(α,p)³⁸Cl. Some samples of argon extracted from microscopic Cl-bearing inclusions in minerals have beenreported to have anomalously high concentrations of ³⁶Ar and ³⁸Ar that may be attributable to nucleogenesis.

Radioactive ³⁷Ar and ³⁹Ar are formed continuously in the atmosphere as products of cosmic-rayreactions, and they are components of cosmic dust entering the earth's atmosphere. Both isotopes alsoare formed by nuclear reactions on and beneath the earth's surface. At the present time, most of the new³⁹Ar introduced to the atmosphere each year is from nuclear reactors. ³⁹Ar decays to ³⁹K with a half-lifeof 269 a; while ³⁷Ar decays to ³⁷Cl with a half-life of 35 days. The amounts of ³⁷Ar and ³⁹Ar innormal samples are variable and may be useful in environmental studies, but they are several orders ofmagnitude too small to affect the standard atomic weight of argon at its current level of reported uncertainty.

SOURCESAtomic weights of the elements: Review 2000 by John R de Laeter et al. Pure Appl. Chem. 2003 (75) 683-800
Variation in the terrestrial isotopic composition and atomic weight of argon by J.K. Böhlke. Pure Appl. Chem. 2014 (86) 1421-1432

CIAAW

Atomic Mass Vs Atomic Number

Argon
A_r(Ar) = [39.792, 39.963] since 2017
The name derives from the Greek argos for 'lazy' or 'inactive' because it does not combine with otherelements. It was discovered in 1894 by the Scottish chemist William Ramsay and the English physicistRobert John Strutt (Lord Rayleigh) in liquefied air. Rayleigh's initial interest derived from a problemposed by the English physicist Henry Cavendish in 1785, i.e., when oxygen and nitrogen were removedfrom air, there was an unknown residual gas remaining.

Element Ar

Natural variations of argon isotopic composition

For more information about the natural variations of the atomic weight of argon please read IUPAC Technical Report Variation in the terrestrial isotopic composition and atomic weight of argon by J.K. Böhlke. Pure Appl. Chem.86, 1421-1432 (2014).

Formula: Ar
Molecular weight: 39.948
IUPAC Standard InChI:
InChI=1S/Ar
Download the identifier in a file.
IUPAC Standard InChIKey:XKRFYHLGVUSROY-UHFFFAOYSA-N
CAS Registry Number: 7440-37-1
Chemical structure:
This structure is also available as a 2d Mol file
Other names:Ar;UN 1006;UN 1951;argon atom
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Mass spectrum (electron ionization)

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Ar Atomic Number

Data compiled by:NIST Mass Spectrometry Data Center, William E. Wallace, director

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Element Ar Atomic Mass

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Origin	DOW CHEMICAL COMPANY / ASTM E14-UNCERTIFIED SPECTRUM 1
NIST MS number	34321

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References

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No reference data available.

Notes

Ar Atomic Mass In Kg

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Ar Relative Atomic Mass

Data from NIST Standard Reference Database 69:NIST Chemistry WebBook
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