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Carbon-14

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Carbon-14, 14C
General
Symbol14C
Namescarbon-14, 14C, C-14,
radiocarbon
Protons (Z)6
Neutrons (N)8
Nuclide data
Natural abundance1 part per trillion
Half-life (t1/2)5,730
Isotope mass14.003241 Da
Spin0+
Decay modes
Decay modeDecay energy (MeV)
Beta0.156476[1]
Isotopes of carbon
Complete table of nuclides

Carbon-14, 14C, or radiocarbon, is a radioactive isotope of carbon with a nucleus containing 6 protons and 8 neutrons. Its presence in organic materials is the basis of the radiocarbon dating method to date archaeological, geological, and hydrogeological samples. Carbon-14 was discovered on 27 February 1940, by Martin Kamen and Sam Ruben at the University of California Radiation Laboratory in Berkeley, although its existence had been suggested by Franz Kurie in 1934.[2]

There are three naturally occurring isotopes of carbon on Earth: 99% of the carbon is carbon-12, 1% is carbon-13, and carbon-14 occurs in trace amounts, e.g. making up as much as 1 part per trillion (0.0000000001%) of the carbon in the atmosphere. The half-life of carbon-14 is 5,730±40 years. It decays into nitrogen-14 through beta decay.[3] The activity of the modern radiocarbon standard[4] is about 14 disintegrations per minute (dpm) per gram carbon.[5]

The atomic mass of carbon-14 is about 14.003241 amu. The different isotopes of carbon do not differ appreciably in their chemical properties. This is used in chemical research in a technique called carbon labeling: some carbon-12 atoms of a given compound are replaced with carbon-14 atoms (or some carbon-13 atoms) in order to trace them along chemical reactions involving the given compound.

Origin and radioactive decay

Carbon-14 is produced in the upper layers of the troposphere and the stratosphere by thermal neutrons absorbed by nitrogen atoms. When cosmic rays enter the atmosphere, they undergo various transformations, including the production of neutrons. The resulting neutrons (1n) participate in the following reaction:

1n + 14N → 14C + 1H

The highest rate of carbon-14 production takes place at altitudes of 9 to 15 km (30,000 to 50,000 ft) and at high geomagnetic latitudes, but the carbon-14 readily mixes and becomes evenly distributed throughout the atmosphere and reacts with oxygen to form radioactive carbon dioxide. Carbon dioxide also dissolves in water and thus permeates the oceans. Carbon-14 can also be produced in ice by fast neutrons causing spallation reactions in oxygen.

Carbon-14 then goes through radioactive beta decay.

By emitting an electron and an anti-neutrino, carbon-14 (half life of 5730 years) decays into the stable (non-radioactive) isotope nitrogen-14.

The inventory of carbon-14 in Earth's biosphere is about 300 million Curies, of which most is in the oceans.[6]

Radiocarbon dating

Main article: Radiocarbon dating

Radiocarbon dating is a radiometric dating method that uses (14C) to determine the age of carbonaceous materials up to about 60,000 years old. The technique was developed by Willard Libby and his colleagues in 1949[7] during his tenure as a professor at the University of Chicago. Libby estimated that the radioactivity of exchangeable carbon-14 would be about 14 disintegrations per minute (dpm) per gram. In 1960, he was awarded the Nobel Prize in chemistry for this work. One of the frequent uses of the technique is to date organic remains from archaeological sites. Plants fix atmospheric carbon during photosynthesis, so the level of 14C in plants and animals when they die approximately equals the level of 14C in the atmosphere at that time. However, it decreases thereafter from radioactive decay, allowing the date of death or fixation to be estimated. The initial 14C level for the calculation can either be estimated, or else directly compared with known year-by-year data from tree-ring data (dendrochronology) to 10,000 years ago, or from cave deposits (speleothems), to about 45,000 years of age. A calculation or (more accurately) a direct comparison with tree ring or cave-deposit carbon-14 levels, gives the wood or animal sample age-from-formation. The technique has limitations within the modern industrial era, due to fossil fuel carbon (which has little carbon-14) being released into the atmosphere in large quantities, in the past few centuries.

Formation during nuclear tests

Atmospheric 14C, New Zealand[8] and Austria[9]. The New Zealand curve is representative for the Southern Hemisphere, the Austrian curve is representative for the Northern Hemisphere. Atmospheric nuclear weapon tests almost doubled the concentration of 14C in the Northern Hemisphere [10].

The above-ground nuclear tests that occurred in several countries between 1955 and 1963 dramatically increased the amount of carbon-14 in the atmosphere and subsequently in the biosphere; after the tests ended the atmospheric concentration of the isotope began to decrease.

One side effect of the change in atmospheric carbon-14 is that this enables the determination of the birth year of an individual: the amount of carbon-14 in tooth enamel is measured with accelerator mass spectrometry and compared to records of past atmospheric carbon-14 concentrations. Since teeth are formed at a specific age and do not exchange carbon thereafter, this method allows age to be determined to within 1.6 years. This method only works for individuals born after 1943,[11][12] and it must be known whether the individual was born in the Northern or the Southern Hemisphere.

An alternative dating method relies on the lens of the eye; transparent proteins called "lens crystallins" produced during the first year of life are unchanged afterward, so measuring carbon-14 concentrations there can provide a record of the time of birth. The primary restrictions on the technology are that the person has to have been born after 1950, the lens must be removed while the subject is alive or within three days after death before it decays too much, and the individual cannot have subsisted primarily on seafood.[13]

Occurrence

In fossil fuels

Most man-made chemicals are made of fossil fuels, such as petroleum or coal, in which the carbon-14 should have long since decayed. However, such deposits often contain trace amounts of carbon-14 (varying significantly, but ranging from 1% the ratio found in living organisms to amounts comparable to an apparent age of 40,000 years for oils with the highest levels of carbon-14) [14]. This may indicate possible contamination by small amounts of bacteria, underground sources of radiation (such as uranium decay, although reported measured ratios of 14C/U in uranium-bearing ores[15] would imply roughly 1 uranium atom for each two carbon atoms in order to cause the 10−15 14C/12C measured), or other unknown secondary sources of carbon-14 production. Presence of carbon-14 in the isotopic signature of a sample of carbonaceous material possibly indicates its contamination by biogenic sources or the decay of radioactive material in surrounding geologic strata.

In the human body

Since essentially all sources of human food are derived from plants, the carbon that comprises our bodies contains carbon-14 at the same concentration as the atmosphere. The beta-decays from this internal radiocarbon contribute approximately 0.01 mSv/year (1 mrem/year)to each person's dose of ionizing radiation.[16] This is small compared to the doses from potassium-40 (0.39 mSv/year) and radon (variable).

Carbon-14 can be used as a radioactive tracer in medicine. In the initial variant of the urea breath test, a diagnostic test for Helicobacter pylori, urea labeled with approximately 37 kBq (1.0 μCi) carbon-14 is fed to a patient. In the event of a H. pylori infection, the bacterial urease enzyme breaks down the urea into ammonia and radioactively-labeled carbon dioxide, which can be detected by low-level counting of the patient's breath.[17] The 14-C urea breath test has been largely replaced by the 13-C urea breath test which has no radiation issues.

See also

References

  1. ^ A.H Waptstra, G. Audi, and C. Thibault. "AME atomic mass evaluation 2003". Retrieved 2007-06-03.{{cite web}}: CS1 maint: multiple names: authors list (link)
  2. ^ Kamen, Martin D. (1963). "Early History of Carbon-14: Discovery of this supremely important tracer was expected in the physical sense but not in the chemical sense". Science. 140 (3567): 584–590. doi:10.1126/science.140.3567.584. PMID 17737092. {{cite journal}}: Cite has empty unknown parameter: |month= (help)
  3. ^ "What is carbon dating?". National Ocean Sciences Accelerator Mass Spectrometry Facility. Retrieved 2007-06-11.
  4. ^ "Carbon 14:age calculation". C14dating.com. Retrieved 2007-06-11.
  5. ^ "Class notes for Isotope Hydrology EESC W 4886: Radiocarbon 14C". Martin Stute's homepage at Columbia. Retrieved 2007-06-11.
  6. ^ "Human Health Fact Sheet - Carbon 14" (PDF). Argonne National Laboratory, EVS. 2005. {{cite web}}: Unknown parameter |month= ignored (help)
  7. ^ Arnold, J. R. and Libby, W. F. (1949). "Age Determinations by Radiocarbon Content: Checks with Samples of Known Age,". Science. 110 (2869): 678–680. doi:10.1126/science.110.2869.678. PMID 15407879.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  8. ^ "Atmospheric δ14C record from Wellington". Trends: A Compendium of Data on Global Change. Carbon Dioxide Information Analysis Center. Oak Ridge National Laboratory. 1994. Retrieved 2007-06-11.
  9. ^ Levin, I.; et al. (1994). "δ14C record from Vermunt". Trends: A Compendium of Data on Global Change. Carbon Dioxide Information Analysis Center. {{cite journal}}: Explicit use of et al. in: |author= (help)
  10. ^ "Radiocarbon dating". University of Utrecht. Retrieved 2008-02-19.
  11. ^ "Radiation in Teeth Can Help Date, ID Bodies, Experts Say". National Geographic News. 2005-09-22.
  12. ^ Spalding KL, Buchholz BA, Bergman LE, Druid H, Frisen J. (2005-09-15). "Forensics: age written in teeth by nuclear tests". Nature. 437 (7057): 333–4. doi:10.1038/437333a. PMID 16163340.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  13. ^ http://www.plosone.org/article/info:doi/10.1371/journal.pone.0001529 Niels Lynnerup, et al., Radiocarbon Dating of the Human Eye Lens Crystallines Reveal Proteins without Carbon Turnover throughout Life, Public Library of Science
  14. ^ D.C. Lowe, "Problems Associated with the Use of Coal as a Source of 14C Free Background Material," Radiocarbon, 1989, 31:117-120
  15. ^ Jull, A.J.T. (1985). "Carbon-14 Abundances in Uranium Ores and Possible Spontaneous Exotic Emission from U-Series Nuclides". Meteorics. 20: 676. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help); Unknown parameter |month= ignored (help) (abstract)
  16. ^ NCRP Report No. 93 (1987). Ionizing Radiation Exposure of the Population of the United States. National Council on Radiation Protection and Measurements.{{cite book}}: CS1 maint: numeric names: authors list (link) (excerpt)
  17. ^ "Society of Nuclear Medicine Procedure Guideline for C-14 Urea Breath Test" (PDF). 2001-06-23. Retrieved 2007-07-04.

Further reading

  • Kamen, Martin D. (1985). Radiant Science, Dark Politics: A Memoir of the Nuclear Age. Berkeley: University of California Press. ISBN 0520049292. {{cite book}}: Cite has empty unknown parameter: |coauthors= (help)

External links


Lighter:
carbon-13 		Carbon-14 is an
isotope of carbon 		Heavier:
carbon-15
Decay product of:
boron-14, nitrogen-18 		Decay chain
of carbon-14 		Decays to:
nitrogen-14
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