Describe Rutherford gold foil experiment
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Rutherford's Gold Foil Experiment-
This experiment lead to the discovery of the atomic particles.
The experiment setup was as follows-
A gold foil of very small thickness {approx. 8.6*10^(-6)cm.}. The gold foil was made to strike with the alpha- beam. Around the gold foil there was a fluorescent sheet.
Observations--
Each particle should have gone directly through the foil if the plum pudding model was correct (meaning that an atom was a vast amount of empty space and could easily be passed through by any particle). For the most part, the alpha particles corresponded with this hypothesis and passed straight through the gold foil. There were, however, a small hand full of particles that deflected slightly from the straight path by about one or two degrees. But the biggest discovery was made when 1 in 20,000 particles would deflect approximately 90 degrees or more from the parent beam. In fact, an occasional particle even fired right back at the experimenter.
Conclusions---
1. An atom was much more than just empty space and scattered electrons
2. An atom must have a positively charged center that contains most of its mass (which Rutherford termed as the nucleus). Since alpha particles are relatively heavy, positively charged particles, the fact that the occasional particle would be deflected by either a small or large margin proved that a portion of an atom was both positively charged (particles of identical charges repel one another while particles of opposite charges attract one another) and relatively heavy by atomic standards.
Since only a small number of alpha particles veered slightly when passed through the foil and since even fewer bounced back at the experiment, Rutherford reasoned that this positively charged center was relatively small in reference to the total size of the atom.
Hope this helps u :)
This experiment lead to the discovery of the atomic particles.
The experiment setup was as follows-
A gold foil of very small thickness {approx. 8.6*10^(-6)cm.}. The gold foil was made to strike with the alpha- beam. Around the gold foil there was a fluorescent sheet.
Observations--
Each particle should have gone directly through the foil if the plum pudding model was correct (meaning that an atom was a vast amount of empty space and could easily be passed through by any particle). For the most part, the alpha particles corresponded with this hypothesis and passed straight through the gold foil. There were, however, a small hand full of particles that deflected slightly from the straight path by about one or two degrees. But the biggest discovery was made when 1 in 20,000 particles would deflect approximately 90 degrees or more from the parent beam. In fact, an occasional particle even fired right back at the experimenter.
Conclusions---
1. An atom was much more than just empty space and scattered electrons
2. An atom must have a positively charged center that contains most of its mass (which Rutherford termed as the nucleus). Since alpha particles are relatively heavy, positively charged particles, the fact that the occasional particle would be deflected by either a small or large margin proved that a portion of an atom was both positively charged (particles of identical charges repel one another while particles of opposite charges attract one another) and relatively heavy by atomic standards.
Since only a small number of alpha particles veered slightly when passed through the foil and since even fewer bounced back at the experiment, Rutherford reasoned that this positively charged center was relatively small in reference to the total size of the atom.
Hope this helps u :)
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Rutherford designed an experiment.IN this experiment , fast moving α - particles(alpha particles)were made to fall on a thin golf foil.
Observations:
1. Most of the α - particles passed straight through the gold foil.
2. Some of the α - particles were deflected by small angles by the gold foil.
3. Surprisingly , one out of every 12,000 particles appeared to rebound.
Conclusions :
1.Most of the space inside the atom is empty because most of the α-particles passed through the gold foil without getting deflected.
2.Very few particles were deflected from their path, indicating that the positive charge of the atom occupies very little space.
3.A very small fraction of α - particles were deflected by very large angles, indicating that all the positive charge and mass of the gold atom were concentrated in a very small volume within the atom.
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Rutherford's Nuclear Model Of Atom :
1.There is a positively charged center in an atom called the nucleus. Nearly all the mass of an atom resides in the nucleus.
2.The electrons revolve around the nucleus in well-defined orbits.
3.The size of the nucleus is very small as compared to the size of the atom.
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Observations:
1. Most of the α - particles passed straight through the gold foil.
2. Some of the α - particles were deflected by small angles by the gold foil.
3. Surprisingly , one out of every 12,000 particles appeared to rebound.
Conclusions :
1.Most of the space inside the atom is empty because most of the α-particles passed through the gold foil without getting deflected.
2.Very few particles were deflected from their path, indicating that the positive charge of the atom occupies very little space.
3.A very small fraction of α - particles were deflected by very large angles, indicating that all the positive charge and mass of the gold atom were concentrated in a very small volume within the atom.
---------------------------------------------------------------------------------------------
Rutherford's Nuclear Model Of Atom :
1.There is a positively charged center in an atom called the nucleus. Nearly all the mass of an atom resides in the nucleus.
2.The electrons revolve around the nucleus in well-defined orbits.
3.The size of the nucleus is very small as compared to the size of the atom.
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