Question

multiple choice question
what question did bohrs quantum model of the atom seem able to answer, for the first time?
where are the positive and negative charges in an atom located?
what is the charge on an electron?
why is energy quantized?
why are atomic emission spectra discontinuous?

Explanation:

Bohr's quantum model of the atom proposed that electrons exist in discrete energy levels. When electrons transition between these levels, they emit or absorb specific amounts of energy (photons). This leads to atomic emission spectra being discontinuous (composed of distinct lines) because only specific energy differences (corresponding to the allowed electron transitions between energy levels) are possible.

• The question "Where are the positive and negative charges in an atom located?" was addressed by earlier models like the Rutherford model (positive charge in a small nucleus, negative - charged electrons outside).
• The charge on an electron was determined through experiments like the Millikan oil - drop experiment, not by Bohr's model.
• While Bohr's model was based on the concept of quantized energy (electrons in quantized energy levels), the more fundamental "why" of energy quantization (in a more general sense beyond the atomic model context of his work) was a broader quantum - mechanical concept that had more to do with the nature of the quantum world at large, and Bohr's model was more focused on applying it to the atom. But his model was the first to successfully explain the discontinuous atomic emission spectra in terms of electron transitions between quantized energy levels in an atom.

Answer:

Why are atomic emission spectra discontinuous?