Physics:Quantum atoms/isotopes of hydrogen
Hydrogen isotopes are a Book II topic in the Quantum Collection. They are atoms with one proton in the nucleus and different numbers of neutrons: protium, deuterium, and tritium. Isotopic mass changes the reduced mass of the electron-nucleus system, producing measurable isotope shifts in atomic spectra. Nuclear spin also affects hyperfine structure and molecular behavior. Hydrogen isotopes are important in precision spectroscopy, isotope chemistry, fusion research, nuclear physics, cosmology, and tests of simple quantum systems.
Main isotopes
| Isotope | Symbol | Nucleus | Stability | Notes |
|---|---|---|---|---|
| Protium | one proton | stable | Most common hydrogen isotope; no neutron. | |
| Deuterium | or D | one proton and one neutron | stable | Used in heavy water, isotope labeling, and precision spectroscopy. |
| Tritium | or T | one proton and two neutrons | radioactive | Beta emitter with a half-life of about 12.3 years; used in tracing and fusion research. |
Quantum effects
Different hydrogen isotopes have slightly different atomic energy levels because the nuclear mass changes the reduced mass of the electron-nucleus system. These isotope shifts are measured in high-precision spectroscopy.[1]
The nuclear spin also affects hyperfine splitting. Ordinary hydrogen and deuterium have different nuclear spin values, so their hyperfine spectra differ. Tritium is radioactive, but it is still useful in nuclear and atomic physics contexts.
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References
- ↑ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A. (2022). "Standard atomic weights of the elements 2021". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603.
