Physics:Isotopes of carbon

Short description: Carbon with different numbers of neutrons

Main isotopes of Chemistry:carbon (₆C)

Iso­tope Decay abun­dance half-life (t1/2) mode pro­duct 11C syn 20 min β+ 11B 12C 98.9% stable 13C 1.1% stable 14C 1 ppt 5730 y β− 14N
Standard atomic weight Ar, standard(C)	[12.0096, 12.0116] Conventional: 12.011

Carbon (₆C) has 15 known isotopes, from to , of which and are stable. The longest-lived radioisotope is , with a half-life of 5.70(3)×10³ years. This is also the only carbon radioisotope found in nature, as trace quantities are formed cosmogenically by the reaction + n → + . The most stable artificial radioisotope is , which has a half-life of 20.3402(53) min. All other radioisotopes have half-lives under 20 seconds, most less than 200 milliseconds. The least stable isotope is , with a half-life of 3.5(1.4)×10⁻²¹ s. Light isotopes tend to decay into isotopes of boron and heavy ones tend to decay into isotopes of nitrogen.

List of isotopes

Nuclide	Z	N	Isotopic mass (u)	Half-life [resonance width]	Decay mode	Daughter isotope	Spin and parity	Physics:Natural abundance (mole fraction)
								Normal proportion	Range of variation
	6	2	8.037643(20)	3.5(1.4) zs [230(50) keV]	2p		0+
	6	3	9.0310372(23)	126.5(9) ms	β+ (54.1(1.7)%)		3/2−
					β+α (38.4(1.6)%)
					β+p (7.5(6)%)
	6	4	10.01685322(8)	19.3011(15) s	β+		0+
	6	5	11.01143260(6)	20.3402(53) min	β+		3/2−
	12160(40) keV				p ?	?	1/2+
	6	6	12 exactly	Stable			0+	[0.9884, 0.9904]
	6	7	13.003354835336(252)	Stable			1/2−	[0.0096, 0.0116]
	6	8	14.003241989(4)	5.70(3)×103 y	β−		0+	Trace	< 10−12
	22100(100) keV				IT		(2−)
	6	9	15.0105993(9)	2.449(5) s	β−		1/2+
	6	10	16.014701(4)	750(6) ms	β−n (99.0(3)%)		0+
					β− (1.0(3)%)
	6	11	17.022579(19)	193(6) ms	β− (71.6(1.3)%)		3/2+
					β−n (28.4(1.3)%)
					β−2n ?	?
	6	12	18.02675(3)	92(2) ms	β− (68.5(1.5)%)		0+
					β−n (31.5(1.5)%)
					β−2n ?	?
	6	13	19.03480(11)	46.2(2.3) ms	β−n (47(3)%)		1/2+
					β− (46.0(4.2)%)
					β−2n (7(3)%)
	6	14	20.04026(25)	16(3) ms	β−n (70(11)%)		0+
					β−2n (< 18.6%)
					β− (> 11.4%)
?	6	15	21.04900(64)#	< 30 ns	n ?	?	1/2+#
	6	16	22.05755(25)	6.2(1.3) ms	β−n (61(14)%)		0+
					β−2n (< 37%)
					β− (> 2%)
?	6	17	23.06889(107)#		n ?	?	3/2+#

Carbon-11

Carbon-11 or 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. It has a half-life of 20.3402(53) min.

→ + positron + Electron neutrino + 0.96 MeV

+ e⁻ → + ν_e + 1.98 MeV

It is produced from nitrogen in a cyclotron by the reaction

+ proton → +

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 [[Chemistry:DASB|[[[Category:Pages with incorrect nuclide templates use]]]DASB]] and [[Chemistry:25I-NBOMe|[[[Category:Pages with incorrect nuclide templates use]]]Cimbi-5]].

Natural isotopes

Main articles: Physics:Carbon-12, Physics:Carbon-13, and Physics:Carbon-14

There are three naturally occurring isotopes of carbon: 12, 13, and 14. and are stable, occurring in a natural proportion of approximately 93:1. 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, constitutes a negligible part; but, since it is radioactive with a half-life of 5.70(3)×10³ years, it is radiometrically detectable. Since dead tissue does not absorb , the amount of is one of the methods used within the field of archeology for radiometric dating of biological material.

Paleoclimate

and 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). Plants find it easier to use the lighter isotopes () when they convert sunlight and carbon dioxide into food. So, for example, large blooms of plankton (free-floating organisms) absorb large amounts of from the oceans. Originally, the 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 from the surface, leaving the surface layers relatively rich in . Where cold waters well up from the depths (such as in the North Atlantic), the water carries back up with it. So, when the ocean was less stratified than today, there was much more in the skeletons of surface-dwelling species. Other indicators of past climate include the presence of tropical species, coral growths rings, etc.

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 = δ) is expressed as parts per thousand (‰):

$\delta {\phantom{A}}_{\phantom{}}^{\phantom{13}}{\phantom{A}}_{\phantom{2}}^{\phantom{2}13}\mathrm{C}=(\frac{{\left(\frac{{\phantom{A}}_{\phantom{}}^{\phantom{13}}{\phantom{A}}_{\phantom{2}}^{\phantom{2}13}\mathrm{C}}{{\phantom{A}}_{\phantom{}}^{\phantom{12}}{\phantom{A}}_{\phantom{2}}^{\phantom{2}12}\mathrm{C}}\right)}_{\text{sample}}}{{\left(\frac{{\phantom{A}}_{\phantom{}}^{\phantom{13}}{\phantom{A}}_{\phantom{2}}^{\phantom{2}13}\mathrm{C}}{{\phantom{A}}_{\phantom{}}^{\phantom{12}}{\phantom{A}}_{\phantom{2}}^{\phantom{2}12}\mathrm{C}}\right)}_{\text{standard}}}-1)\times 1000$ ‰

Stable carbon isotopes in carbon dioxide are utilized differentially by plants during photosynthesis. Grasses in temperate climates (barley, rice, wheat, rye, and oats, plus sunflower, potato, tomatoes, peanuts, cotton, sugar beet, and most trees and their nuts or fruits, roses, and Kentucky bluegrass) follow a C3 photosynthetic pathway that will yield δ¹³C values averaging about −26.5‰. 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‰.

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.

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).

See also

• Cosmogenic isotopes
• Environmental isotopes
• Isotopic signature
• Radiocarbon dating