What Are the Key Differences Between Bohr's Atomic Model and Classical Physics?

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Homework Help Overview

The discussion revolves around the differences between Bohr's atomic model and classical physics, specifically addressing questions about the nature of atomic structure, electron behavior, and the implications of quantized energy levels on atomic spectra.

Discussion Character

  • Exploratory, Conceptual clarification, Assumption checking

Approaches and Questions Raised

  • Participants explore the Bohr model's description and its contrast with classical physics, particularly regarding electron stability and energy levels. Questions arise about the implications of continuous versus quantized energy levels on atomic spectra and the validity of classical principles in atomic contexts.

Discussion Status

Some participants have provided insights into the nature of atomic spectra and the stability of electrons in the Bohr model, while others question the applicability of classical physics principles to atomic behavior. Multiple interpretations of the implications of these principles are being explored.

Contextual Notes

Participants note the relevance of textbook readings for understanding the Bohr model and its foundational postulates. There is an acknowledgment of the distinction between macroscopic and subatomic physics principles in the discussion.

Omid
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I need help with these 3 questions:
1. Describe the Bohr model of the atom. How does it differ from a planetary model based on classical physics?
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2. In terms of the Bohr theory why is that electrons don't spiral into the nucleus?
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3. If atomic energy levels were not quantized, but could vary within certain limits, what colud atomic spectra look like?
 
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In principle questions 1 and 3 would be automatically answered as you read the relevant portions from your physics textbook. For question 2 you need to know a Bohr postulate which explained it. The electron wouldn't spiral into the nucleus unless it lost kinetic energy. So the only we could have a stable rotational condition if the kinetic energy would be constant through the uniformly circular trajectory. This was explained with the help of Stationary Orbits...in which the electron would rotate without radiating energy. You might think this has something to do with standing waves on a stretched string and you would be right...but I'll leave the reading to you.
 
I re-read question 3 and I have the following short answer, if you mean that the energy levels are continuous. The spectra would be continuous too as energy wouldn't be quantized and so the wavelengths would be continuous functions as well. So you wouldn't be able to recognize discontinuities corresponding to different energy levels in the spectra.
 
Surely I have done the reading, these are the quetions of that chapter.
I don't get what happened to the classical physics principle, the one that said: a charged mass radiates when it accelerates.

Did Bohr model reject that principle? Or we still believe in it?

P.S I'm studing chemistry :)
 
That principle is totally inaccurate in the atomic (subatomic) world...It's in the realm of MACROSCOPIC PHYSICS,namely classical electrodynamics...

Daniel.
 
Thank you
 
dextercioby said:
That principle is totally inaccurate in the atomic (subatomic) world...It's in the realm of MACROSCOPIC PHYSICS,namely classical electrodynamics...

Omid said:
P.S I'm studing chemistry :)

Thats why.....
 

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