Isotopes

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Isotopes

Isotopes (/ˈaɪsətoʊps/) are variants of a particular chemical element which differ in neutron number, and consequently in nucleon number. All isotopes of a given element have the same number of protons but different numbers of neutrons in each atom.

Etymology

The term "isotope", a portmanteau of the Greek words isos (ἴσος "equal") and topos (τόπος "place"), was introduced by the British chemist Frederick Soddy in 1913.

Types of Isotopes

There are two types of isotopes: stable isotopes and radioactive isotopes. Stable isotopes do not decay into other elements. In contrast, radioactive isotopes (also known as radioisotopes) decay over time.

Stable Isotopes

Stable isotopes have a stable combination of protons and neutrons, so they have a stable nucleus and do not undergo radioactive decay. Examples include Carbon-12 and Oxygen-16.

Radioactive Isotopes

Radioactive isotopes have an unstable combination of protons and neutrons, so they have an unstable nucleus that undergoes radioactive decay. Examples include Carbon-14 and Uranium-235.

Applications of Isotopes

Isotopes have many applications in various fields such as medicine, archaeology, and physics. For instance, in medicine, radioactive isotopes are used in both diagnosis and treatment of diseases. In archaeology, isotopes are used in dating artifacts and fossils.

See Also

References

External links

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