isotóppal

Isotopes are variants of a particular chemical element which differ in neutron number, and consequently in nucleon number. All isotopes of an element have the same number of protons in each atom. The number of protons determines the chemical element. For example, all atoms with 6 protons are carbon atoms, and all of them are isotopes of carbon. A typical carbon atom has 6 neutrons as well, making its mass number 12 (6 protons + 6 neutrons). This isotope is called carbon-12. However, carbon atoms can also have 7 neutrons (carbon-13) or 8 neutrons (carbon-14). Carbon-13 and carbon-14 are isotopes of carbon.

The word isotope is derived from Greek, meaning "same place," because isotopes occupy the same position in the periodic table. The number of neutrons in the nucleus of an atom does not affect its chemical properties, which are determined by the number of electrons, and thus the number of protons. Therefore, isotopes of an element behave very similarly in chemical reactions. However, they can have different physical properties, such as mass, density, and boiling point. Isotopes also differ in their nuclear properties. Some isotopes are stable, meaning their nuclei do not spontaneously decay. Others are radioactive, meaning their nuclei undergo radioactive decay, emitting particles and energy.

Radioactive isotopes, also known as radioisotopes, have various applications in science, medicine, and industry. For instance, carbon-14 is used in radiocarbon dating to determine the age of ancient artifacts. Medical imaging techniques often utilize radioisotopes to diagnose and treat diseases. In industry, radioisotopes can be used for sterilization, thickness gauging, and tracing the flow of materials. The study of isotopes is a fundamental part of nuclear chemistry and physics.