# Carbon-14

Carbon-14
General
Neutrons 8
Protons 6
Nuclide data
Natural abundance 1 part per trillion
Half-life 5,730 ± 40 years
Isotope mass 14.003241 u
Decay mode Decay energy
Beta .156476[1] MeV

Carbon-14, 14C, or radiocarbon, is a radioactive isotope of carbon discovered on February 27, 1940, by Martin Kamen and Sam Ruben at the University of California Radiation Laboratory in Berkeley. Its nucleus contains 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.

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, making up as much as 1 part per trillion (0.0000000001%) of the carbon on the Earth. The half-life of carbon-14 is 5,730±40 years. It decays into nitrogen-14 through beta-decay.[2] The activity of the modern radiocarbon standard[3]is about 14 disintegrations per minute (dpm) per gram carbon [4].

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 of carbon-14

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 feet) 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.

${\displaystyle \mathrm {~_{6}^{14}C} \rightarrow \mathrm {~_{7}^{14}N} +e^{-}+{\bar {\nu }}_{e}}$

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.[5]

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[6] during his tenure as a professor at the University of Chicago. Libby estimated that the steady state radioactivity concentration 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 at the time wood is laid down, or in animals at the time they die, 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 several centuries.

## Carbon-14 and fossil fuels

Most man-made chemicals are made of fossil fuels, such as petroleum or coal, in which the carbon-14 has long since decayed. However, oil 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).[citation needed] This may indicate possible contamination by small amounts of bacteria, underground sources of radiation (such as uranium decay, although reported measured amounts of 14C/U in uranium-bearing ores imply an unlikely (improbably large) quantity of uranium involved, roughly half as much as the carbon in the deposits, to match the 10-15 14C/C measured[7]), or other unknown secondary sources of carbon-14 production. Presence of carbon-14 in the isotopic signature of a sample of carbonaceous material indicates its possible contamination by biogenic sources or the decay of radioactive material in surrounding geologic strata.

## Carbon-14 and 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 a deceased 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 crystallines" 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 within three days after death before it decays too much, and the individual cannot have subsisted primarily on seafood[13].

## Carbon-14 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 approx 1 mrem/year (.01 mSv /year) to each person's dose of ionizing radiation.[14] This is small compared to the doses from potassium-40 (0.39 mSv/year) and radon (which vary).

Carbon-14 can be used as a radioactive tracer in medicine. In the urea breath test, a diagnostic test for Helicobacter pylori, urea labeled with approx 1 μCi (37kBq) 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.[15]

## References

1. A.H Waptstra, G. Audi, and C. Thibault. "AME atomic mass evaluation 2003". Retrieved 2007-06-03.
2. "What is carbon dating?". National Ocean Sciences Accelerator Mass Spectrometry Facility. Retrieved 2007-06-11.
3. "Carbon 14:age calculation". C14dating.com. Retrieved 2007-06-11.
4. "Class notes for Isotope Hydrology EESC W 4886: Radiocarbon 14C". Martin Stute's homepage at Columbia. Retrieved 2007-06-11.
5. "Human Health Fact Sheet - Carbon 14" (PDF). Argonne National Laboratory, EVS. August 2005.
6. Arnold, J. R. and Libby, W. F. (1949). "Age Determinations by Radiocarbon Content: Checks with Samples of Known Age,". Science. 110: 678–680. doi:10.1126/science.110.2869.678. PMID 15407879.
7. Jull, A.J.T. (1985). "Carbon-14 Abundances in Uranium Ores and Possible Spontaneous Exotic Emission from U-Series Nuclides". Meteorics. 20: 676. Unknown parameter |coauthors= ignored (help); Unknown parameter |month= ignored (help) (abstract)
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). 14C record from Vermunt". Trends: A Compendium of Data on Global Change. Carbon Dioxide Information Analysis Center.
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: 333-4. doi:10.1038/437333a. PMID 16163340.