What is the primary function of electrons in an atom?

Electrons play a crucial role in defining the properties of an atom, particularly in terms of charge and bonding capabilities. The primary function of electrons is to determine how an atom interacts with others, which is essential for chemical bonding.

Electrons reside in different energy levels or shells around the nucleus of an atom, and their arrangement influences how the atom can bond with others to form molecules. The number of electrons in the outermost shell, known as valence electrons, dictates an atom's reactivity and the types of bonds it can form—whether ionic, covalent, or metallic. The presence of electrons also determines the overall charge of the atom; for instance, if an atom gains or loses electrons, it becomes an ion (positively or negatively charged).

In contrast, while the stability of the nucleus is primarily maintained by protons and neutrons through the strong nuclear force, it is the electrons that facilitate interactions between atoms. Electrons do not contribute significantly to the mass of an atom compared to protons and neutrons; thus, they are not responsible for increasing mass. Isotopes refer to variations of elements that have different numbers of neutrons, which is unrelated to the function of electrons. Therefore, the role of electrons in determining charge