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Neutrons are subatomic particles found in the nucleus of an atom. They, along with protons, make up the atomic nucleus. Unlike protons, which carry a positive charge, neutrons are neutral, meaning they have no charge. The number of neutrons in an atom can vary without affecting the atomic element. This variance leads to the formation of isotopes. Isotopes are versions of elements that have the same number of protons but different numbers of neutrons. This difference in neutron count results in different atomic masses for the isotopes, but they still remain classified as the same element. For example, carbon, which typically has 6 neutrons, can have isotopes like carbon-13, with 7 neutrons. Despite these differences in neutron count, isotopes of an element will still exhibit very similar chemical behavior, primarily because they have the same number of protons and electrons.

The atomic number of an element is a fundamental property that defines an element. It is equal to the number of protons present in an atom's nucleus. Each element on the periodic table is uniquely identified by its atomic number. For instance, hydrogen, with an atomic number of 1, has one proton, while helium, with an atomic number of 2, has two protons.
The atomic number not only determines the identity of an element but also its placement on the periodic table. Since isotopes of the same element all have the same number of protons, they all share the same atomic number. Thus, even if the number of neutrons changes, resulting in different isotopes, the atomic number—and therefore the elemental identity—remains constant.

Electrons are the subatomic particles that orbit an atom's nucleus. They carry a negative charge, which balances the positive charge from protons in a neutral atom. In a neutral atom, the number of electrons is equal to the number of protons. This balance ensures that the atom has no overall electrical charge.
Electrons play a critical role in the chemical properties of an element. They are involved in forming chemical bonds and reactions. In isotopes, the number of electrons remains constant, even though the number of neutrons might change. This constancy ensures that isotopes of a particular element will typically engage in similar chemical interactions. Understanding the behavior and arrangement of electrons helps in predicting how atoms will react and form compounds.