Isotoopi

Isotoopi, known in English as isotopes, are variants of a chemical element that share the same number of protons but differ in the number of neutrons. This difference in neutron count gives each isotope a distinct atomic mass while preserving most chemical properties, so isotopes of the same element behave similarly in chemical reactions but can have different nuclear properties.

Each isotope is identified by its mass number A and atomic number Z. For example, carbon-12 and carbon-14 are isotopes of carbon; both have Z = 6, but A = 12 and A = 14. Isotopes may be stable or unstable; radioactive isotopes decay over time into other elements, characterized by a half-life.

Natural occurrence varies by element. Some elements have several stable isotopes and occur naturally in multiple forms, while others may have few or no stable isotopes. Unstable isotopes can be produced naturally (in trace amounts) or artificially in laboratories and reactors.

Applications of isotopes are diverse. Radiometric dating uses radiocarbon (carbon-14) and other isotopes to determine ages of rocks and fossils. In medicine, radioactive isotopes such as technetium-99m and iodine-131 are used for diagnostics and therapy. Isotopes also serve as tracers in biology, environmental science, and industry, helping to track processes without significantly altering them.

Production and measurement involve nuclear reactors, particle accelerators, or neutron capture for creating specific isotopes. Detection and analysis are performed with techniques such as mass spectrometry and various spectroscopic methods to determine isotopic composition and abundance.