Classical Physics and the Bohr Model of Hydrogen Atom

[jstrike]

Homework Statement

Classical physics applied to the bohr model of the hydrogen atom would predict that light could be emitted continuously, rather than in discrete chunks of energy. Transitions between what kinds of energy levels would come close to the classical viewpoint?

A. Only levels having small quantum numbers.
B. Only when at least one of the levels has a very large quantum number.
C. Only levels of moderate quantum numbers.
D. There are no such levels.

The Attempt at a Solution

Have no idea what it is

 

[Jolb]

Think of it like this: a blackbody spectrum is what you get when there are a bunch of different energy transitions that could be made.

A hydrogen atom in the n=2 (princple q#) state has (basically) only one transition with only one possible energy, the Lyman-alpha line. Clearly this one line isn't a nice smooth blackbody spectrum. For a blackbody spectrum, you want a system that isn't constrained to only one or a few transitions, you want something with possible transitions of all different energies.

 

[kerimek]

asking

I can provide some clarification on the concepts of classical physics and the Bohr model of the hydrogen atom. Classical physics is a theory that describes the behavior of macroscopic objects, such as those we can see and interact with in our everyday lives. It is based on the laws of mechanics, such as Newton's laws of motion, and does not take into account the principles of quantum mechanics.

On the other hand, the Bohr model of the hydrogen atom is a quantum mechanical model that describes the behavior of electrons in the hydrogen atom. It was proposed by Niels Bohr in 1913 and is based on the idea that electrons can only exist in certain discrete energy levels around the nucleus of the atom.

Now, to answer the question, the Bohr model of the hydrogen atom deviates from classical physics in the sense that it predicts that electrons can only transition between energy levels in discrete steps, rather than continuously. This means that there are no intermediate energy levels that an electron can occupy, and therefore, the answer to the question is option D - there are no levels that come close to the classical viewpoint.

In other words, classical physics predicts that electrons should be able to transition between energy levels continuously, but the Bohr model shows that this is not the case for the hydrogen atom. Only transitions between specific energy levels are allowed, and these correspond to specific wavelengths of light being emitted or absorbed. This is in line with the principles of quantum mechanics, which state that energy is not continuous, but rather, it is quantized.

In conclusion, while classical physics and the Bohr model of the hydrogen atom may have some similarities, they also have significant differences, particularly in the way they explain the behavior of electrons in the atom. It is important to understand and recognize these differences in order to have a more complete understanding of the physical world around us.