Final answer:
In the Bohr model of the atom, the energy levels in each atom are indeed unique. Electrons can only occupy these quantized energy levels, which determines the specific wavelengths of light emitted during electronic transitions.
Step-by-step explanation:
The answer is true. According to the Bohr model, each atom has a set of unique, unchangeable energy levels. The energy levels, or orbits, that electrons inhabit around the nucleus are quantized. This means that electrons can only be at these specific energy levels and nowhere in between. When an electron jumps from a higher energy level to a lower one, it emits energy in the form of light, with a wavelength that directly corresponds to the energy difference between the two levels. This emission of light at specific wavelengths creates the characteristic emission spectra of an atom.
Bohr's model was successful in explaining the spectral lines of the hydrogen atom and why atoms absorbed or emitted light only at certain wavelengths. Each transition between energy levels results in a fixed and definite energy change, confirming the uniqueness of energy levels within atoms.