Isotopes
Isotopes are atoms of the same element that have different numbers of neutrons but the same number of protons and electrons. The difference in the number of neutrons between the various isotopes of an element means that the various isotopes have different masses. The superscript number to the left of the element abbreviation indicates the number of protons plus neutrons in the isotope. For example, among the hydrogen isotopes, deuterium (denoted as 2H or D) has one neutron and one proton. This is approximately twice the mass of protium (1H), whereas tritium (3H) has approximately three times the mass of protium
Related Conference of Isotopes
April 20-21, 2026
13th International Conference and Exhibition on Chromatography and Analytical Techniques
Rome, Italy
August 11-12, 2026
5th World Congress on Plasma Chemistry and Plasma Processing
Amsterdam, Netherlands
November 26-27, 2026
6th International Conference on Petrochemistry and Natural Gas
Amsterdam, Netherlands
Isotopes Conference Speakers
Recommended Sessions
- Nuclear Chemistry
- Radionuclide speciation
- Radionuclides in the environment, radioecology
- Advanced chemistry
- An Introduction to Nuclear Medicine
- Chemistry of actinide elements
- Chemistry of Trans actinide
- Coordination chemistry of the radioactive elements
- Environmental radiochemistry
- Environmental radioecology
- Industrial Application of Radioisotopes
- Isotopes
- Nuclear analytical methods
- Nuclear Energy Production
- Nuclear forensics
- Nuclear Reaction
- Physicochemical Application of Radiotracer Methods
- Production and application of radionuclides
- Radiation chemistry
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- Radioactive Decay
- Radiochemical analysis
- Radiopharmaceutical chemistry, labeled compounds
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