Isotopes of carbon

Summary

Main isotopes of carbon (6C)
Iso­tope Decay
abun­dance half-life (t1/2) mode pro­duct
11C syn 20.3402(53) min β+ 11B
12C [0.98840.9904] stable
13C [0.00960.0116] stable
14C 1 ppt 5.70(3)×103 y β 14N
Standard atomic weight Ar, standard(C)[12.009612.0116] conventional: 12.011[1][2]

Carbon (6C) has 15 known isotopes, from 8
C
to 22
C
, of which 12
C
and 13
C
are stable. The longest-lived radioisotope is 14
C
, with a half-life of (5.70±0.03)×103 years. This is also the only carbon radioisotope found in nature—trace quantities are formed cosmogenically by the reaction 14
N
+
n
14
C
+ 1
H
. The most stable artificial radioisotope is 11
C
, which has a half-life of 20.3402±0.0053 min. All other radioisotopes have half-lives under 20 seconds, most less than 200 milliseconds. The least stable isotope is 8
C
, with a half-life of (3.5±1.4)×10−21 s.

List of isotopes

Nuclide[3]
Z N Isotopic mass (Da)[4]
[n 1]
Half-life

[resonance width]
Decay
mode

[n 2]
Daughter
isotope

[n 3]
Spin and
parity
[n 4][n 5]
Natural abundance (mole fraction)
Normal proportion Range of variation
8
C
6 2 8.037643(20) 3.5(14) zs
[230(50) keV]
2p 6
Be
[n 6]
0+
9
C
6 3 9.0310372(23) 126.5(9) ms β+, p (61.6%) 8
Be
[n 7]
3/2−
β+, α (38.4%) 5
Li
[n 8]
10
C
6 4 10.01685322(8) 19.3011(15) s β+ 10
B
0+
11
C
[n 9]
6 5 11.01143260(6) 20.3402(53) min β+ (99.79%) 11
B
3/2−
EC (0.21%)[5][6] 11
B
11m
C
12160(40) keV p 10
B
1/2+
12
C
6 6 12 exactly[n 10] Stable 0+ [0.9984, 0.9904][7]
13
C
[n 11]
6 7 13.00335483534(25) Stable 1/2− [0.0096, 0.0116][8]
14
C
[n 12]
6 8 14.0032419890(4) 5.70(3)×103 y β 14
N
0+ Trace[n 13] <10−12
14m
C
22100(100) keV IT 14
C
(2−)
15
C
6 9 15.0105993(9) 2.449(5) s β 15
N
1/2+
16
C
6 10 16.014701(4) 750(6) ms β, n (99.0%) 15
N
0+
β (1.0%) 16
N
17
C
6 11 17.022579(19) 193(6) ms β (71.6%) 17
N
3/2+
β, n (28.4%) 16
N
18
C
6 12 18.02675(3) 92(2) ms β (68.5%) 18
N
0+
β, n (31.5%) 17
N
19
C
[n 14]
6 13 19.03480(11) 46.2(23) ms β, n (47%) 18
N
1/2+
β (46%) 19
N
β, 2n (7%) 17
N
20
C
6 14 20.04026(25) 16(3) ms β, n (70%) 19
N
0+
β, 2n (<18.6%) 18
N
β (>11.4%) 20
N
21
C
6 15 21.04900(64)# <30 ns n 20
C
1/2+#
22
C
[n 15]
6 16 22.05755(25) 6.2(13) ms β, n (61%) 21
N
0+
β, 2n (<37%) 20
N
β (>2%) 22
N
This table header & footer:
  1. ^ ( ) – Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
  2. ^ Modes of decay:
    EC: Electron capture


    n: Neutron emission
    p: Proton emission
  3. ^ Bold symbol as daughter – Daughter product is stable.
  4. ^ ( ) spin value – Indicates spin with weak assignment arguments.
  5. ^ # – Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
  6. ^ Subsequently decays by double proton emission to 4
    He
    for a net reaction of 8
    C
    4
    He
    + 41
    H
  7. ^ Immediately decays into two 4
    He
    atoms for a net reaction of 9
    C
    → 2 4
    He
    + 1
    H
    +
    e
  8. ^ Immediately decays by proton emission to 4
    He
    for a net reaction of 9
    C
    → 2 4
    He
    + 1
    H
    +
    e
  9. ^ Used for labeling molecules in PET scans
  10. ^ The unified atomic mass unit is defined as 1/12 the mass of an unbound atom of carbon-12 at ground state
  11. ^ Ratio of 12C to 13C used to measure biological productivity in ancient times and differing types of photosynthesis
  12. ^ Has an important use in radiodating (see carbon dating)
  13. ^ Primarily cosmogenic, produced by neutrons striking atoms of 14
    N
    (14
    N
    +
    n
    14
    C
    + 1
    H
    )
  14. ^ Has 1 halo neutron
  15. ^ Has 2 halo neutrons

Carbon-11

Carbon-11 or 11
C
is a radioactive isotope of carbon that decays to boron-11. This decay mainly occurs due to positron emission, with around 0.19–0.23% of decays instead occurring by electron capture.[5][6] It has a half-life of 20.364 minutes.

11
C
11
B
+
e+
+
ν
e
+ 0.96 MeV
11
C
+
e
11
B
+
ν
e
+ 1.98 MeV

It is produced from nitrogen in a cyclotron by the reaction

14
N
+
p
11
C
+ 4
He

Carbon-11 is commonly used as a radioisotope for the radioactive labeling of molecules in positron emission tomography. Among the many molecules used in this context are the radioligands [11
C
]DASB
and [11
C
]Cimbi-5
.

Natural isotopes

There are three naturally occurring isotopes of carbon: 12, 13, and 14. 12
C
and 13
C
are stable, occurring in a natural proportion of approximately 93:1. 14
C
is produced by thermal neutrons from cosmic radiation in the upper atmosphere, and is transported down to earth to be absorbed by living biological material. Isotopically, 14
C
constitutes a negligible part; but, since it is radioactive with a half-life of (5.70±0.03)×103 years, it is radiometrically detectable. Since dead tissue does not absorb 14
C
, the amount of 14
C
is one of the methods used within the field of archeology for radiometric dating of biological material.

Paleoclimate

12
C
and 13
C
are measured as the isotope ratio δ13C in benthic foraminifera and used as a proxy for nutrient cycling and the temperature dependent air-sea exchange of CO2 (ventilation) (Lynch-Stieglitz et al., 1995). Plants find it easier to use the lighter isotopes (12
C
) when they convert sunlight and carbon dioxide into food. So, for example, large blooms of plankton (free-floating organisms) absorb large amounts of 12
C
from the oceans. Originally, the 12
C
was mostly incorporated into the seawater from the atmosphere. If the oceans that the plankton live in are stratified (meaning that there are layers of warm water near the top, and colder water deeper down), then the surface water does not mix very much with the deeper waters, so that when the plankton dies, it sinks and takes away 12
C
from the surface, leaving the surface layers relatively rich in 13
C
. Where cold waters well up from the depths (such as in the North Atlantic), the water carries 12
C
back up with it. So, when the ocean was less stratified than today, there was much more 12
C
in the skeletons of surface-dwelling species. Other indicators of past climate include the presence of tropical species, coral growths rings, etc.[9]

Tracing food sources and diets

The quantities of the different isotopes can be measured by mass spectrometry and compared to a standard; the result (e.g. the delta of the 13
C
= δ13
C
) is expressed as parts per thousand (‰):[10]

Stable carbon isotopes in carbon dioxide are utilized differentially by plants during photosynthesis.[citation needed] Grasses in temperate climates (barley, rice, wheat, rye and oats, plus sunflower, potato, tomatoes, peanuts, cotton, sugar beet, and most trees and their nuts/fruits, roses and Kentucky bluegrass) follow a C3 photosynthetic pathway that will yield δ13C values averaging about −26.5‰.[citation needed] Grasses in hot arid climates (maize in particular, but also millet, sorghum, sugar cane and crabgrass) follow a C4 photosynthetic pathway that produces δ13C values averaging about −12.5‰.[11]

It follows that eating these different plants will affect the δ13C values in the consumer's body tissues. If an animal (or human) eats only C3 plants, their δ13C values will be from −18.5 to −22.0‰ in their bone collagen and −14.5‰ in the hydroxylapatite of their teeth and bones.[12]

In contrast, C4 feeders will have bone collagen with a value of −7.5‰ and hydroxylapatite value of −0.5‰.

In actual case studies, millet and maize eaters can easily be distinguished from rice and wheat eaters. Studying how these dietary preferences are distributed geographically through time can illuminate migration paths of people and dispersal paths of different agricultural crops. However, human groups have often mixed C3 and C4 plants (northern Chinese historically subsisted on wheat and millet), or mixed plant and animal groups together (for example, southeastern Chinese subsisting on rice and fish).[13]

See also

References

  1. ^ "Standard Atomic Weights: Carbon". CIAAW. 2009.
  2. ^ Meija, Juris; et al. (2016). "Atomic weights of the elements 2013 (IUPAC Technical Report)". Pure and Applied Chemistry. 88 (3): 265–91. doi:10.1515/pac-2015-0305.
  3. ^ Half-life, decay mode, nuclear spin, and isotopic composition is sourced in:
    Kondev, F.G.; Wang, M.; Huang, W.J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  4. ^ Wang, Meng; Huang, W.J.; Kondev, F.G.; Audi, G.; Naimi, S. (2021). "The AME 2020 atomic mass evaluation (II). Tables, graphs and references*". Chinese Physics C. 45 (3): 030003. doi:10.1088/1674-1137/abddaf.
  5. ^ a b Scobie, J.; Lewis, G. M. (1 September 1957). "K-capture in carbon 11". Philosophical Magazine. 2 (21): 1089–1099. Bibcode:1957PMag....2.1089S. doi:10.1080/14786435708242737.
  6. ^ a b Campbell, J. L.; Leiper, W.; Ledingham, K. W. D.; Drever, R. W. P. (1967-04-11). "The ratio of K-capture to positron emission in the decay of 11C". Nuclear Physics A. 96 (2): 279–287. Bibcode:1967NuPhA..96..279C. doi:10.1016/0375-9474(67)90712-9.
  7. ^ "Atomic Weight of Carbon". CIAAW.{{cite web}}: CS1 maint: url-status (link)
  8. ^ "Atomic Weight of Hydrogen". CIAAW. Retrieved 24 June 2021.{{cite web}}: CS1 maint: url-status (link)
  9. ^ Tim Flannery The weather makers: the history & future of climate change, The Text Publishing Company, Melbourne, Australia. ISBN 1-920885-84-6
  10. ^ Miller, Charles B.; Wheeler, Patricia (2012). Biological oceanography (2nd ed.). Chichester, West Sussex: John Wiley & Sons, Ltd. p. 186. ISBN 9781444333022. OCLC 794619582.
  11. ^ https://www.ldeo.columbia.edu/~polissar/OrgGeochem/oleary-1988-carbon-isotopes.pdf
  12. ^ Tycot, R. H. (2004). M. Martini; M. Milazzo; M. Piacentini (eds.). "Stable isotopes and diet: you are what you eat" (PDF). Proceedings of the International School of Physics "Enrico Fermi" Course CLIV.
  13. ^ Richard, Hedges (2006). "Where does our protein come from?". British Journal of Nutrition. 95 (6): 1031–2. doi:10.1079/bjn20061782. PMID 16768822.