Question

Limitations of rutherfords model of an atom

Answer 1

Limitations of Rutherford Model
Although Rutherford’s atomic model was based on experimental observations it failed to explain certain things.

Rutherford proposed that the electrons revolve around the nucleus in fixed paths called orbits. According to Maxwell, accelerated charged particles emit electromagnetic radiations and hence an electron revolving around the nucleus should emit electromagnetic radiation. This radiation would carry energy from the motion of the electron which would come at the cost of shrinking of orbits. Ultimately the electrons would collapse in the nucleus. Calculations have shown that as per Rutherford’s model an electron would collapse in the nucleus in less than 10-8 seconds. So Rutherford’s model was not in accordance with Maxwell’s theory and could not explain the stability of an atom.
One of the drawbacks of Rutherford’s model was also that he did not say anything about the arrangement of electrons in an atom which made his theory incomplete.
Although the early atomic models were inaccurate and failed to explain certain experimental results, they were the base for future developments in the world of quantum mechanics. Visit Byju’s YouTube Channel to learn more.

Answer 2

The revolution of an electron in a circular orbit is not expected to be stable. any particle in a circular orbit would undergo acceleration.
during acceleration, charged particles would radiate energy. thus , the revolving electron would lose energy and finally fall into the nucleus.if this were so, the atom should be highly stable and hence matter would not exist in the form that we know, as we know that atom are quite stable.