Define isotope
An isotope is a variant of an atom that has the same number of protons, but a different number of neutrons. This leads to variations in the mass number of the atom, resulting in different isotopes of the same element. Isotopes of an element have similar chemical properties but may have different physical properties, such as different nuclear stability and radioactive decay rates.
An isotope refers to any of two or more forms of an element that have the same atomic number but different atomic masses. In other words, isotopes are variants of an element with the same number of protons in the nucleus but different numbers of neutrons. This variation in neutron number leads to differences in atomic mass for isotopes of the same element. Isotopes can be either stable or unstable (radioactive), depending on the balance between the number of protons and neutrons in their nuclei.
An isotope is a variant of an element with the same number of protons but a different number of neutrons in its nucleus. This means that isotopes of the same element have the same atomic number (number of protons) but different mass numbers (sum of protons and neutrons). For example, carbon-12, carbon-13, and carbon-14 are three isotopes of carbon, with 6 protons but 6, 7, and 8 neutrons, respectively.
To determine if two atoms are isotopes of the same element, you need to compare the number of protons they have. This information is readily available on the periodic table, which lists the atomic number for each element (usually located above the element's symbol).
Isotopes play a crucial role in various fields such as archaeology, medicine, and nuclear energy, as their distinct properties allow scientists to study and track the behavior of different forms of elements in a variety of applications.