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Related Concept Videos

Mass Spectrometry: Isotope Effect01:13

Mass Spectrometry: Isotope Effect

2.5K
Most elements exist in nature as a mixture of isotopes. The isotopes differ in weight due to their respective number of neutrons. The molecular weight of a molecule is different depending on the specific isotope of its elements involved. As a result, the mass spectrum of the molecule exhibits peaks from the same fragment at multiple positions. The positions of these mass signals depend on the difference between the molecular mass. Furthermore, the intensity of these signals is dependent on the...
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Isotopes01:12

Isotopes

60.0K
Elements have a set number of protons that determines their atomic number (Z). For example, all atoms with eight protons are oxygen; however, the number of neutrons can vary for atoms of the same element. The sum of the number of protons and the number of neutrons is the mass number (A). Atoms with the same atomic number but different mass numbers are called isotopes. Elements can have multiple isotopes, for example, carbon-12, carbon-13, and carbon-14.
An element's atomic mass, or weight,...
60.0K
Isotopes and Radioisotopes01:28

Isotopes and Radioisotopes

10.1K
In the early 1900s, English chemist Frederick Soddy realized that an element could have atoms with different masses that were chemically indistinguishable. These different types are called isotopes — atoms of the same element that differ in mass. Isotopes differ in mass because they have different numbers of neutrons but are chemically identical because they have the same number of protons. Soddy was awarded the Nobel Prize in Chemistry in 1921 for this discovery.
An isotope containing...
10.1K
Nuclear Stability03:18

Nuclear Stability

19.9K
Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10−15 meters, a nucleus is quite small compared to the radius of the entire atom, which is about 10−10 meters. Nuclei are extremely dense compared to bulk matter, averaging 1.8 × 1014 grams per cubic centimeter. If the earth’s density were equal to the average nuclear density, the earth’s radius would be only about 200 meters.
To hold positively charged protons together...
19.9K
Radioactive Decay and Radiometric Dating02:48

Radioactive Decay and Radiometric Dating

34.9K
Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. The number of disintegrations per unit time is called the activity (A), which is directly proportional to the number of nuclei in the sample. The decay constant (λ) is an average probability of decay per nucleus in unit time.
34.9K
¹³C NMR: ¹H–¹³C Decoupling01:04

¹³C NMR: ¹H–¹³C Decoupling

1.2K
The probability of having two carbon-13 atoms next to each other is negligible because of the low natural abundance of carbon-13. Consequently, peak splitting due to carbon-carbon spin-spin coupling is not observed in spectra. However, protons up to three sigma bonds away split the carbon signal according to the n+1 rule, resulting in complicated spectra.
A broadband decoupling technique is used to simplify these complex, sometimes overlapping, signals. Broadband decoupling relies on a...
1.2K

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Updated: Sep 12, 2025

Fatty Acid 13C Isotopologue Profiling Provides Insight into Trophic Carbon Transfer and Lipid Metabolism of Invertebrate Consumers
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Stable Isotope Abundance Patterns as Potential Biosignatures.

David J Des Marais1, Tristan Caro2, Rajani Dhingra3

  • 1NASA, Ames Research Center, Moffett Field, California, USA.

Astrobiology
|August 6, 2025
PubMed
Summary
This summary is machine-generated.

Stable isotope patterns offer clues to a substance's origin and history. However, distinguishing biological from non-biological origins requires careful analysis and context for reliable life detection.

Keywords:
Biosignatures—Stable isotopes—Prevalence—Signal strength—Carbon—Sulfur

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Area of Science:

  • Geochemistry
  • Astrobiology
  • Biogeochemistry

Background:

  • Stable isotope abundance and distribution reveal substance source, synthesis, and environmental history.
  • Isotopic discrimination during chemical reactions offers insights into specific pathways and conditions.
  • Biosynthetic pathways can generate distinct isotopic patterns compared to abiotic processes, though not universally.

Discussion:

  • Isotope patterns serve as chemical reaction signatures, necessitating additional context for use as biosignatures.
  • The Life Detection Knowledge Base framework evaluates arguments for and against using isotopic patterns in life detection.
  • Carbon and sulfur isotopic patterns in organic matter and minerals illustrate the application of 'prevalence' and 'signal strength' criteria.

Key Insights:

  • Isotopic patterns are valuable indicators but require careful interpretation to avoid false positives in life detection.
  • The 'prevalence' and 'signal strength' criteria can be applied to isotopic data for assessing potential biosignatures.
  • Distinguishing biotic from abiotic origins of isotopic patterns is crucial for robust life detection.

Outlook:

  • Further characterization of abiotic processes is needed to mitigate false-positive life detection claims.
  • Expanding research to diverse microbial communities, taxa, biomolecules, and elements will enhance isotopic biosignature discovery.
  • Investigating isotopic patterns in sedimentary macromolecular organic matter is crucial for deeper insights.