Isotopes are different forms of the same element that have the same number of protons but different numbers of neutrons. This means that isotopes have the same atomic number but different mass numbers.

For example, carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. All three isotopes of carbon have six protons, but carbon-12 has six neutrons, carbon-13 has seven neutrons, and carbon-14 has eight neutrons.

The different isotopes of an element have different physical and chemical properties. For example, carbon-12 and carbon-13 are both stable isotopes, but carbon-14 is a radioactive isotope with a half-life of 5,730 years. This means that carbon-14 is constantly decaying into nitrogen-14.

The different isotopes of an element can be used for a variety of purposes. For example, carbon-14 is used for radiocarbon dating, which is a method of determining the age of organic materials. Carbon-13 is used in nuclear magnetic resonance (NMR) spectroscopy, which is a technique for studying the structure of molecules.

Overall, isotopes are important because they contribute to the diversity of elements and allow for a variety of applications in science and technology.