Isotopes are variants of a particular chemical element which differ in neutron number and consequently in nucleon number.

Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This results in a difference in the atomic mass of the isotopes. Isotopes can be naturally occurring or artificially created through nuclear reactions.

Naturally Occurring Isotopes
- Some elements have naturally occurring isotopes, such as carbon, which has three isotopes: carbon-12, carbon-13, and carbon-14.
- Carbon-12 is the most abundant isotope, making up about 99% of all carbon atoms. Carbon-13 makes up about 1% of carbon atoms, and carbon-14 is a rare isotope that makes up only a tiny fraction of a percent of carbon atoms.

Artificially Created Isotopes
- Isotopes can also be artificially created through nuclear reactions, such as bombarding atoms with particles or exposing them to radiation.
- These isotopes can be used in a variety of ways, such as in medical imaging and cancer treatment, as well as in research and industry.

Uses of Isotopes
- Isotopes have a variety of uses in different fields, such as:
- Medical: Isotopes can be used in medical imaging techniques such as PET scans and MRI scans.
- Agriculture: Isotopes can be used to study plant growth and nutrient uptake.
- Archaeology: Isotopes can be used to determine the age of artifacts and fossils.
- Energy: Isotopes can be used as a source of energy in nuclear power plants.

Conclusion
- Isotopes are atoms of the same element that have different numbers of neutrons, resulting in a difference in atomic mass.
- Isotopes can be naturally occurring or artificially created.
- Isotopes have a variety of uses in different fields, such as medicine, agriculture, archaeology, and energy.