Hydrogen, deuterium, and tritium are isotopes of the element hydrogen, each with a different number of neutrons in their nucleus while maintaining the same number of protons (which defines the element). Here's a breakdown of each:
1. **Hydrogen-1 (H-1)**:
- This is the most common form of hydrogen found in nature.
- It consists of one proton and zero neutrons in its nucleus.
- It is symbolized as ¹H.
2. **Deuterium (H-2)**:
- Deuterium is an isotope of hydrogen.
- It has one proton and one neutron in its nucleus.
- Deuterium is symbolized as ²H.
- Deuterium is commonly used in nuclear reactions and as a tracer in chemical reactions.
3. **Tritium (H-3)**:
- Tritium is another isotope of hydrogen.
- It contains one proton and two neutrons in its nucleus.
- Tritium is symbolized as ³H.
- Tritium is radioactive and used in luminous paints, as well as in nuclear fusion research.
In summary, the main difference between these isotopes lies in the number of neutrons present in their nuclei. While all three isotopes have one proton (which defines them as hydrogen), deuterium has one neutron, tritium has two neutrons, and ordinary hydrogen has no neutrons.
