which result of Rutherford's alpha particle scattering experiment nullifies the idea of uniform distribution of positive and negative charges in atom ?
Answers
Rutherford's alpha particle scattering experiment changed the way we think of atoms.
Before the experiment the best model of the atom was known as the Thomson or "plum pudding" model. The atom was believed to consist of a positive material "pudding" with negative "plums" distributed throughout.
Rutherford directed beams of alpha particles (which are the nuclei of helium atoms and hence positively charged) at thin gold foil to test this model and noted how the alpha particles scattered from the foil.
Rutherford made 3 observations:
Most of the fast, highly charged alpha particles went whizzing straight through undeflected. This was the expected result for all of the particles if the plum pudding model was correct.
Some of the alpha particles were deflected back through large angles. This was not expected.
A very small number of alpha particles were deflected backwards! This was definitely not as expected. Rutherford later remarked "It was as incredible as if you fired a 15-inch shell at a piece of tissue paper and it came back at you!"
Rutherford's alpha-particle scattering experiment nullifies the idea of uniform distribution of positive and negative charges in atom in which they get bombarded with very small angles.
Explanation:
- Alpha particles when scattered will give the following observations.
- A major part of the alpha particles while passing through the gold sheet will not deflect at all.
- Some alpha particles will be deflected with few angles and thus positive charge is not uniformly distributed.
- The Positive charge will be concentrated on a small volume.
- Then few particles will be deflected back by certain angles
- The angle of deflection will be 180 degree.