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Both. The reason the electrons are quantized in their orbits around the nucleus is because of their wavelike properties (remember how in lecture, Lavelle showed how if the electron was in the wrong position, it would be cancelled out by its own wave). However, as an electron "drops" from a higher energy to a lower energy, it is better to think of it as a particle dropping down a hill. Though I think the dropping could be thought of as a wave, the particle model was used to describe it in lecture.
Atomic spectra are associated more with the quantum model. This is due to the fact that the spectral lines occur because the electrons can only exist at certain (quantized) distances from the nucleus.
In general, associate the photoelectric effect with electrons being treated as particles (because the intensity of the electron doesn't change its energy, which is counterintuitive when thinking about a wave) and the three fundamental equations we learned (deBroglie's, Heisenberg's Uncertainty Equation, and Schrodinger's Wave Function Equation) are associated with electrons treated as waves.
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