explain Rutherford atomic model
Answers
Why the Plum-Pudding Model Failed
The plum-pudding model of an atom was unable to explain the findings of Rutherfords experiment while studying radioactivity.
In an experiment with gold foil, Rutherford bombarded the gold foil withalpha particles. With Thomsons model as the basis, Rutherford expected small deviations; however, his findings were different from what was expected.
As we go further into this lesson, we will learn more about Rutherfords gold-foil experiment, his observations and his conclusions. We will also learn about the atomic model that he came up with on the basis of his conclusions.
Set up for Rutherfords experiment:
A thin gold foil, approximately 1000 atoms thick, was taken. Gold was chosen for its high ductility.
A detector screen with a small slit (for emission of radiation from the atom) was placed around the foil.
A source of alpha particles was kept in front of the foil.
The foil was bombarded with fast-moving alpha particles.
The set-up for Rutherfords gold-foil experiment is shown in the figure.
Rutherfords Expectations and Observations
What Rutherford expected?
Rutherford expected that the alpha particles would pass straight through the foil and only a small fraction of alpha particles would be deflected. This expectation was in compliance with Thomsons atomic model.
What Rutherford observed?
Rutherfords findings were contrary to his expectation. He observed that:
1. Most of the fast-moving alpha particles passed straight through the gold foil.
2. Some particles were deflected through the foil by small angles.
3. One out of every 12000 particles rebounded, i.e., they got deflected by an angle of 180.
What Rutherford Concluded from His Observations
Rutherford then carefully studied his observations and made the following conclusions.
Most alpha particles passed through the gold foil without any deflection. This indicates that most of the space inside an atom is empty.
Very few particles suffered a deflection from their path. This means that positive charge occupies very little space inside an atom.
Only a small fraction of particles underwent a180 deflection. This shows that the entire positive charge and mass of an atom are present within a very small volume inside the atom.
In many ways, the Rutherford model of the atom is the classic model of the atom, even though it's no longer considered an accurate representation. Rutherford's model shows that an atom is mostly empty space, with electrons orbiting a fixed, positively charged nucleus in set, predictable paths
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