In   1911,   Rutherford presented a model of atom called Rutherford's model,   according   to  which the mass of the  atom  and  its whole  positive   charge   are  concentrated at the centre of the atom in a nuclear radius.   Around   the nucleus are distributed electrons in a hollow sphere and the total negative charge of the electron is equal to the positive charge of the nucleus.  Rutherford  assumed  that the electrons in the atom are not stationary, but are revolving around the nucleus in different circular orbits and the necessary centripetal force is provided by the electrostatic force of attraction between the electron and the nucleus.

The Classical Theory of Rutherford Model: Path of Electrons

In the classical theory of the Rutherford atomic model, the path of an electron is described as a circular orbit around the nucleus. This model was proposed by physicist Ernest Rutherford in 1911 based on his famous gold foil experiment.

1. Rutherford's Gold Foil Experiment:
Rutherford conducted an experiment in which he fired alpha particles (positively charged) at a thin gold foil. According to the prevailing model at that time, the Thomson model, it was expected that the alpha particles would mostly pass through the gold foil with slight deflections due to the positive charge spread uniformly throughout the atom.

2. Unexpected Observations:
However, Rutherford observed some unexpected results during the experiment. Most of the alpha particles passed through the foil, but some were deflected at large angles, and a few even bounced back in the direction from which they came.

3. Rutherford's Conclusion:
Based on these observations, Rutherford proposed a new model of the atom, known as the Rutherford model or the planetary model. According to this model, the atom consists of a tiny, dense, positively charged nucleus at the center, surrounded by negatively charged electrons.

4. Electron Path:
In the Rutherford model, the path of an electron is described as a circular orbit around the nucleus. The electrons are attracted to the positively charged nucleus due to the electrostatic force of attraction. However, they are also in motion, creating a centrifugal force that opposes the attraction.

5. Balance of Forces:
The balance between the attractive force and the centrifugal force determines the path of the electron. If the attractive force is stronger, the electron will move closer to the nucleus, resulting in a smaller orbit. Conversely, if the centrifugal force is stronger, the electron will move farther from the nucleus, resulting in a larger orbit.

6. Limitations of the Rutherford Model:
While the Rutherford model provided significant insights into the structure of the atom, it had some limitations. According to classical physics, an electron in a circular orbit would continuously emit electromagnetic radiation, losing energy and eventually spiraling into the nucleus. However, this contradicts experimental observations.

7. Quantum Mechanical Model:
The limitations of the classical Rutherford model were overcome by the development of quantum mechanics. According to the quantum mechanical model, electrons do not follow specific paths but exist in electron clouds or orbitals with defined probabilities of being found in certain regions around the nucleus.

In conclusion, according to the classical theory of the Rutherford model, the path of an electron is described as a circular orbit around the nucleus. However, this model has its limitations and has been replaced by the quantum mechanical model, which provides a more accurate description of electron behavior in atoms.

Circular