How does Rutherford's Atomic Model explain energy loss in revolving electrons?

In summary, the conversation discusses the unsatisfactory aspects of Rutherford's Atomic Model, specifically the idea that electrons would lose energy in their revolving motion due to the emission of electromagnetic radiation. This is not in line with classical mechanics, but can be explained through classical electrodynamics.
  • #1
moatasim23
78
0
I studied it in a book that Rutherfords Atomic Model was Unsatisfactory bcz the revolving electrons in his model would lose energy.How would they lose energy as far as I know they are kept in rotation by the centripetal force and work done by centripetal force is 0.NO work done no energy loss.Then how would the revolution cause the electron to lose energy?
 
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  • #2
Charged particles undergoing acceleration emit electromagnetic radiation. That radiation has energy. So an electron orbiting the nucleus of an atom would continuously emit electromagnetic radiation and spiral into the nucleus. This is why Rutherford's model is not satisfactory.

This isn't what you expect if you consider classical mechanics since orbiting bodies (such as planets) do not emit radiation.
 
  • #3
Pengwuino said:
Charged particles undergoing acceleration emit electromagnetic radiation. That radiation has energy. So an electron orbiting the nucleus of an atom would continuously emit electromagnetic radiation and spiral into the nucleus. This is why Rutherford's model is not satisfactory.

This isn't what you expect if you consider classical mechanics since orbiting bodies (such as planets) do not emit radiation.

DO we know what causes the electron to emit radiations?
 
  • #4
For the classical electrodynamics explanation, see the derivation of Larmor's radiation formula. (Try a Google search on that phrase.)
 

What is Rutherford's Atomic Model?

Rutherford's Atomic Model, also known as the Planetary Model, was proposed by Ernest Rutherford in 1911. It explained the structure of an atom as a small, dense, positively charged nucleus surrounded by orbiting negatively charged electrons.

What was the key discovery made by Rutherford in his atomic model?

The key discovery made by Rutherford in his atomic model was that the atom has a small, positively charged nucleus at its center. This discovery was made through the famous gold foil experiment, where he observed that most of the alpha particles passed through the foil, but some were deflected at large angles, indicating the presence of a small, positively charged nucleus.

How did Rutherford's Atomic Model differ from previous models?

Rutherford's Atomic Model differed from previous models, such as the Thomson's Plum Pudding Model, by proposing that the positive charge of an atom is concentrated in a small, dense nucleus, rather than being spread out throughout the atom. It also accounted for the existence of empty space within an atom.

What were the limitations of Rutherford's Atomic Model?

One of the limitations of Rutherford's Atomic Model was that it could not explain the stability of atoms, as according to classical electromagnetic theory, orbiting electrons would eventually lose energy and fall into the nucleus. It also could not explain the emission spectra of different elements.

How did Rutherford's Atomic Model contribute to the development of modern atomic theory?

Rutherford's Atomic Model contributed greatly to the development of modern atomic theory by providing a foundation for further scientific research and experiments. It also led to the discovery of subatomic particles, such as protons and neutrons, and the development of the Bohr Model, which further explained the structure of atoms.

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