Final answer:
Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons, influencing their mass. Chemical behavior is generally unchanged, but their nuclear properties may differ, enabling nuclear scientists to distinguish them with advanced technology. Electron distribution in shells contributes to atomic stability.
Step-by-step explanation:
Definition of Isotopes
Isotopes are atoms of the same element that have the same number of protons but differ in the number of neutrons. They have the same atomic number (Z) but different mass numbers (A). A classic example of isotopes is carbon-12 and carbon-14; both have 6 protons, but carbon-12 has 6 neutrons whereas carbon-14 has 8 neutrons, making their mass numbers 12 and 14, respectively.
Key Distinction
The key distinction between isotopes of the same element is their different number of neutrons. This difference does not affect their chemical behavior significantly, as they occupy the same position on the periodic table, but it can affect their mass and nuclear properties. Nuclear scientists utilize sophisticated technology to distinguish and separate these isotopes, which is beyond what is typically available in chemical laboratories.
Electrons and Atomic Stability
Electrons occupy energy levels or electron shells around the nucleus of an atom. The distribution of electrons in these shells contributes to an atom's relative stability. Atoms strive to have filled outer electron shells, which generally leads to more stability.