Sulfidisotooppien

Sulfidisotooppien refers to the different stable and radioactive isotopes of sulfur. Sulfur, a chemical element with the symbol S and atomic number 16, has four stable isotopes: sulfur-32 (³²S), sulfur-33 (³³S), sulfur-34 (³⁴S), and sulfur-36 (³⁶S). Sulfur-32 is the most abundant, making up over 94% of natural sulfur.

Isotopes of an element have the same number of protons but different numbers of neutrons. This difference in neutron count affects their mass and, for unstable isotopes, their radioactivity. While the stable isotopes of sulfur are crucial for understanding geological and biological processes, radioactive isotopes of sulfur have various applications. For example, sulfur-35 (³⁵S) is a commonly used radioisotope in biological research due to its relatively short half-life and its ability to be incorporated into biomolecules.

The relative abundance of sulfur isotopes in natural samples can vary depending on the origin and formation processes. This variation, known as sulfur isotope fractionation, is a valuable tool in fields like geochemistry, paleoclimatology, and environmental science. By analyzing the ratios of different sulfur isotopes (e.g., the δ³⁴S value), scientists can trace the sources of sulfur in the atmosphere, water, and rocks, and reconstruct past environmental conditions. Stable isotope analysis provides a powerful, non-destructive method for tracking elemental cycling and understanding complex earth systems.