Limitations of Rutherford Atomic Model

Ernest Rutherford (and his students Hans Geiger and Ernest Marsden) performed an experiment popularly known as the alpha ray scattering experiment to study atoms. Before him, a scientist named Thomson had experimented to study atoms and their characteristics known as Thomson’s model. He reached many conclusions regarding the structure and position of electrons, neutrons, and protons in an atom. Rutherford, however, falsified some of Thomson’s conclusions and derived new conclusions from his experiment. 

Let us take a look at the Rutherford atomic model experiment, the conclusions reached, and the limitations involved. 

Rutherford’s Gold Foil Experiment

Rutherford conducted his famous alpha scattering experiment by blowing up a gold foil with alpha particles and then studied the path made by these particles after their first point of contact with the gold sheet. He placed a fluorescent screen of zinc sulphide around the gold sheet to observe the change in the paths of the alpha particles. When the alpha particles came in contact with the gold sheet, a spark was observed at that point.

• It has been assumed that the dispersing of a ray of alpha beams through a thin gold plate is the consequence of a large number of scatterings made by the molecules of the alpha particles.
• Some of the particles passed through zero-degree deviation and some by 90 degrees and a few by exactly an angle of 180 degrees.
• It appears to be sensible to assume that the deflexion through an enormous point is because of a solitary nuclear experience.

Conclusions Drawn from the Experiment

Rutherford’s alpha scattering experiment concludes that:

• A huge piece of the alpha particles passed by the gold leaf goes through it without deviation, which is the reason why the majority of the nuclear space is empty.

• In the Rutherford scattering experiment, some of the alpha particles were filtered by the gold sheet at small points, which is the actual reason why a positively charged atom can be commenced similarly. Great nuclear charging is centred around tiny spaces. There are not many alpha particles, for example, a couple of particles with a 1800deviation point. A few particles deviated by a little angle and 1 in 2000 returned.
• The particles which are charged and the atomic mass were focused in an entirely small volume. Which is then called the nucleus.
• His model recommended that electrons were negatively charged around the nucleus of an atom.
• Rutherford’s model recommended that electrons were negatively charged around the centre of an atom.  Electrons are ineffectively charged and the centre is a huge mass with charged particles called electrons surrounded and kept by a strong attractive field.

Contradictions with Thomson’s atomic model

• A large portion of the space in the atom is unfilled as the majority of the alpha-particles went through the foil undeflected. This contradicts Thomson’s statement that a mass is equally spread all around the atom concept.
•  A few positively charged alpha–particles got deviated from its path. The redirection should be because of tremendous ghastly power showing that the positive charge of the molecule isn’t spread all through the atom as Thomson had expressed.
•  The positive charge must be moved in a tiny volume that repulses and avoids the charged alpha-particles.
• Estimates by Rutherford showed that the volume occupied by the nucleus is very small compared with the total volume of the atom.

Drawbacks of Rutherford atomic model

The major limitations of the rutherford atomic model are:

• Rutherford stated that electrons move around the core centre in paths called orbits. Maxwell, a researcher after Rutherford had taken up this idea and played out a test utilising the idea of electro-attractive radiation.
• According to Maxwell, fastly moving particles induce electromagnetic radiation and to that end, the electrons around the centre should flow electromagnetic radiation. 
• This radiation will convey power from the electron advancement as a method for coming to the disadvantage of the decline of the radiation. Bits of knowledge have shown that as demonstrated by employing Rutherford’s model, the electron will tumble to the centre in less than 10-8 seconds. 
• Rutherford’s model changed eventually in a battle with Maxwell’s theory and couldn’t sort out atomic insurance.
• One of the demerits of Rutherford’s model is that he referenced nothing concerning the arrangement of electrons in iota that made his review separate.
• Another negative of Rutherford’s model is that he did not mention anything regarding the plan of electrons in atoms that made his study divided. 
• Also to explain further, The electron orbital is not expected to stabilize. Rutherford’s version could not make the experience of the steadiness of the molecule. Rutherford’s model didn’t make sense of the plan of the electron debris which made his speculation deficient. As indicated through Rutherford’s model, electrons might lose electricity as they go off their circle. These are considered as the major limitations of the Rutherford atomic model.
• Although early atomic kinds have been erroneous and failed to explain certain experimental consequences, they were the idea for destiny traits inside the world of quantum mechanics. Similarly, a few of the Rutherford conclusions were also drawn.

Conclusion

Rutherford’s contribution to modern science is great. He paved the way for the next generation of scientists to reach greater heights in scientific discoveries. Though there are several drawbacks of his experiment, still many of his observations and statements are of much value for modern science. The results of his experiment helped Maxwell to come up with further conclusions. However, the major drawback of his model is that he was not able to explain the stability of atoms and failed to throw light on the arrangement of atoms.