Final answer:
The energy gaps between successive electron energy levels in an atom decrease as the principal quantum number n increases. This describes the quantized nature of electronic energies within an atom, with higher n levels being closer in energy.
Step-by-step explanation:
The question asks about how the energy gaps between successive electron energy levels in an atom change as the principal quantum number n increases. In an atom, electrons exist in discrete energy levels characterized by an n value. As the value of n increases, the energy gap between successive levels actually decreases. So, as an electron moves to higher energy levels (further away from the nucleus), these levels are closer in energy compared to the spacing between lower energy levels. When an electron transitions from a higher energy level to a lower one, it releases energy, often observed as light, leading to the discrete spectra characteristic of different elements.
When describing energy levels, we are discussing the quantized nature of electronic energies, with n corresponding to different 'shells' or energy levels around the nucleus. The principal quantum number increases with distance from the nucleus, and higher energy levels are associated with higher values of n. The relationship between n and energy dictates that transitions for electrons between these quantum states lead to the unique spectral lines for each element.