Isotopes of an element are variants of the same element that have different numbers of neutrons in their atomic nuclei. This difference in neutron number gives each isotope a unique atomic mass. While the number of protons determines the element's identity, isotopes of an element have varying numbers of neutrons while retaining the same number of protons.
For example, let's consider the element carbon (C). Carbon typically has 6 protons in its nucleus, but it can have different numbers of neutrons, leading to different isotopes. The three most common isotopes of carbon are carbon-12 (12C), carbon-13 (13C), and carbon-14 (14C).
- Carbon-12 (12C) has 6 neutrons along with its 6 protons, resulting in an atomic mass of 12 atomic mass units (amu).
- Carbon-13 (13C) has 7 neutrons and 6 protons, giving it an atomic mass of 13 amu.
- Carbon-14 (14C) has 8 neutrons and 6 protons, leading to an atomic mass of 14 amu.
These isotopes of carbon have the same number of protons (6) but differ in their neutron numbers and atomic masses.
Isotopes exist for many elements, and some elements may have numerous isotopes. Each isotope has its own specific properties, such as stability, radioactivity, and abundance in nature, which can have significant implications in various scientific and practical applications.