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Protium is the most abundant isotope of hydrogen. It accounts for more than 99.98% of the hydrogen found in nature. Protium consists of just one proton and one electron. It has no neutrons.

• Symbol: \(^1_1H\)
• Atomic mass: approximately 1 amu (atomic mass unit)

Protium plays a key role in many chemical processes. Due to its simplicity, it is often used in introductory chemistry to illustrate fundamental concepts about atoms and elements. Since it lacks neutrons, it has the simplest atomic structure among all hydrogen isotopes.

Deuterium, often represented by the symbol \(^2_1H\) or simply \(D\), is another stable isotope of hydrogen. Unlike protium, deuterium contains one proton and one neutron in its nucleus. This addition of a neutron doubles its atomic mass compared to protium.

• Symbol: \(^2_1H\) or \(D\)
• Atomic mass: approximately 2 amu

Deuterium occurs naturally in trace amounts, making up about 0.0156% of hydrogen found in Earth's oceans. It is useful in various scientific applications, such as nuclear fusion research, where it serves as a potential fuel source.

Tritium is a rare and radioactive isotope of hydrogen, symbolized by \(^3_1H\) or \(T\). It consists of one proton, two neutrons, and one electron, resulting in a higher atomic mass.

• Symbol: \(^3_1H\) or \(T\)
• Atomic mass: approximately 3 amu

Being radioactive, tritium can decay over time, releasing radiation. This property is leveraged in applications such as glow-in-the-dark materials, where tritium's decay produces light, and in controlled nuclear fusion research. Tritium is naturally found in very small quantities in the environment, primarily created by cosmic rays interacting with the atmosphere.

Radioactive isotopes are nuclides that are unstable. They undergo radioactive decay, emitting energy in the form of particles or electromagnetic waves to reach a stable state. In the case of hydrogen, tritium is the radioactive isotope. Its instability is due to the two extra neutrons in its nucleus, which results in decay processes such as beta decay. This property makes radioactive isotopes useful, as well as hazardous, depending on context. Some common uses of radioactive isotopes include medical imaging and treatment, radiocarbon dating in archaeology, and energy production in nuclear reactors. Safety precautions are important when handling radioactive materials to prevent radiation exposure, which can be harmful to living organisms.