Answer and Explanation:
Isotopes of an element differ in two main ways:
1. Atomic Mass:
Isotopes have different atomic masses. An isotope is identified by the total number of protons and neutrons in its nucleus. While the number of protons determines the element's identity, the number of neutrons can vary, resulting in different isotopes of that element. For example, carbon has three naturally occurring isotopes: carbon-12, carbon-13, and carbon-14. Carbon-12 has 6 protons and 6 neutrons, carbon-13 has 6 protons and 7 neutrons, and carbon-14 has 6 protons and 8 neutrons. The differing number of neutrons leads to different atomic masses for each isotope.
2. Stability and Radioactivity:
Isotopes can differ in their stability and radioactivity. Some isotopes are stable, meaning their nuclei do not undergo spontaneous changes over time. Other isotopes are radioactive and undergo radioactive decay, which involves the spontaneous breakdown of the atomic nucleus, emitting particles and energy. The stability or radioactivity of an isotope depends on the balance between the number of protons and neutrons in its nucleus. For example, carbon-12 and carbon-13 are stable isotopes, while carbon-14 is radioactive and undergoes radioactive decay.
These two ways of differing isotopes highlight the importance of understanding atomic structure and the composition of an element's nucleus. Isotopes play a significant role in various fields, including chemistry, biology, and archaeology, where their distinct properties are utilized for different purposes.