Radioactive Decay is the spontaneous process by which an unstable atomic nucleus loses energy by emitting radiation. This transformation results in the nucleus changing into a different nuclide or a lower energy state. The rate of decay is characterized by the Half-Life—the time required for half of the radioactive atoms in a sample to decay.
N(t) = N₀ × e^(-λt)
Where:
• N(t) = Remaining Quantity
• N₀ = Initial Quantity
• λ (Lambda) = Decay Constant (ln(2) / Half-life)
• t = Time Elapsed
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Nuclei with too many neutrons or protons are unstable. Decay is the natural method of seeking a "Valley of Stability."
Gamma rays from isotopes like Cobalt-60 are used to sterilize medical equipment and preserve food by killing bacteria.
PET scans use Positron Emission (Beta Plus decay) to create detailed 3D images of internal organs and metabolic processes.
| Isotope | Decay Type | Half-Life | Primary Use |
|---|---|---|---|
| Carbon-14 | Beta Minus | 5,730 Years | Organic Dating |
| Uranium-235 | Alpha | 704 Million Years | Fission Fuel |
| Cobalt-60 | Gamma | 5.27 Years | Cancer Therapy |
| Tritium (H-3) | Beta Minus | 12.3 Years | Exit Signs/Research |
| Technetium-99m | Gamma | 6 Hours | Diagnostic Imaging |
| Radon-222 | Alpha | 3.8 Days | Mining Safety Geoproxy |
In modern research, radioactive decay is used as a "Tracer." For example, in Environmental Science, scientists measure the decay of isotopes in groundwater to track the speed of underground currents. In Cosmology, the decay of Aluminum-26 in meteorites provides evidence of supernova explosions that occurred before our solar system was even formed.