What Makes an Isotope ‘Stable’?
Stable isotopes have a balanced ratio of neutrons and protons, giving them a unique atomic mass (weight) and providing the stability that ensures they don’t decay or emit radiation.
Unstable isotopes, or radioisotopes, have an imbalanced ratio of neutrons to protons in their nucleus. This imbalance makes their nucleus energetically unstable, causing them to undergo radioactive decay to reach a more stable state.
How Do Stable Isotopes Work?
When we introduce a specific stable isotope into a system – be it the human body, an ecosystem, or a manufacturing process – we can use specialized equipment to precisely track its journey and how it’s used, simply by looking for its unique “weight signature.” This means stable isotopes can act as natural, harmless tags or labels that we can follow to see where they go, how they are processed, and where they accumulate, all without using radioactivity.
How are Stable Isotopes Used?
As substances for direct use in non-radioactive end products
Stable isotopes possess unique atomic mass signatures (weights), allowing them to be distinguished and traced. They’re used across diverse scientific disciplines for research and analysis, and are ideal for detailed chemical analysis (e.g., mass spectrometry) and safe medical diagnostic tests (e.g., breath tests).
As essential starting materials for creating radioisotopes
Stable isotopes serve as precursor materials that are transformed into radioactive isotopes utilised by the medical and industrial sectors. They are critical for applications like medical imaging (e.g., PET/SPECT scans), targeted cancer therapies, and industrial gauging.
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