Final answer:
Electrons in an atom cannot exist between energy levels; they can only occupy discrete energy levels indexed by the principal quantum number. These levels are quantized, and transitions involve absorbing or releasing energy, often observed as light.
Step-by-step explanation:
The statement that electrons in an atom can exist between energy levels is false. In an atom, electrons are arranged in various energy levels, which are indexed by the principal quantum number, denoted as 'n'. These energy levels are akin to the steps of a staircase; an electron can be on one step or another, but not in between the steps, which means the energy of electrons is quantized. Within each energy level, electrons reside in specific regions known as orbitals, each of which can hold up to two electrons.
When electrons gain or lose energy, they jump from one energy level to another, corresponding to a change of one or more 'steps' on the energy staircase. This can result in the absorption or emission of light, particularly if an electron moves to a lower energy state, releasing energy.
Furthermore, larger principal quantum numbers correlate with higher energy levels and greater average distances from the nucleus. This concept is a fundamental part of atomic structure and quantum mechanics, as well as the behavior of atoms and molecules in various states.