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What happened to the alpha particles in Rutherford's experiment?
Wiki User
∙ 8y ago
The source used in the Rutherford experiments was purifed radium contained in a thin-walled 1-mm diameter glass tube. The source strength was about 0.1 Curie, or about 4 billion nuclear decays per second. The alpha particles were allowed to pass through a small diaphragm and were directed toward a thin foil target. The detector was a small (10-6 m2) zinc sulfide screen mounted a few centimeters away from the target. (Rohlf) answer above posted by strawberry
Wiki User
∙ 16y ago
Wiki User
∙ 12y agoi think but i am not sure.............
So I think the reason why he chose to use alpha particles was because they are positively charged (since they do not have any electrons), hence upons close proximity to the positively charged nucleus of the atom, these particles will be repelled and thus scattered, as like charges repel.
hope it's right............
Wiki User
∙ 11y agoHe didn't discover them but he did give them the name and he showed that alpha and beta radiation were different, proving that the former were helium ions.
This work was part of his work that resulted in his Nobel prize.
He later used them in his famous experiment where he discovered the nucleus.
The "how" part of the question is most relevant to the work done with Royds.
Alpha particles were well known as a certain type of radiation, but not really identified. In 1907 Ernest Rutherford and Thomas Royds collected alpha particles in an evacuated tube. They passed electrical sparks through the tube and, as the alphas accumulated, they eventually observed the spectrum of helium gas proving that alphas were ionized helium atoms.
Wiki User
∙ 8y agoMost of them passed through the single atom thick gold foil, as expected.
However a small number were deflected 180 degrees back toward the source, this was impossible if the Thomson "Plum Pudding" model of the atom was correct.
This forced Rutherford to develop his model of the atom containing a small nucleus at the center surrounded with orbiting electrons, to explain these results.
Wiki User
∙ 11y agothey were ejected out of radium atoms during nuclear decay. So basically he couldn't be bothered - he let nature do the work for him.
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In Rutherfords gold foil experiment particles in dense atomic nuclei caused some alpha particles to bounce straight back from the gold foil.?
positive
Do the alpha particles in Rutherford's experiment contain electrons?
Alpha particles are helium-4 nuclei; they do not contain electrons.
Why did Rutherford use alpha particles rather than electrons for his scattering experenment?
Because the alpha particles are positively charged. In order for the experiment to work, the positive alpha particles must be attracted to the negatively charged gold foil.
Who said atoms were made up of subatomic particles?
Rutherford proved it it from his alpha-particle scattering experiment.
Who provided evidence for the exsitist of an atomic nucleus?
This is the well known gold foil experiment: alpha particles are scattered by the atomic nucleus.
What was rutherfords experiment?
he shot tiny alpha particles throug a piece of gold foil. -Apex
What was ernest rutherfords's experiment?
he shot tiny alpha particles throug a piece of gold foil.
In Rutherfords gold foil experiment particles in dense atomic nuclei caused some alpha particles to bounce straight back from the gold foil.?
positive
What feature of rutherfords gold foil experiment was most surprising to those who carried out the experiment?
Some alpha particles deflected, some went straight through and come were deflected.
In Rutherfords gold foil experiment shown in Figure 4-1 alpha particles that bounce straight back from the foil have struck in the gold atoms?
No, they struck the nucleus of the atom. Since the alpha particles are positively charged and nucleus is positively charged as well, they repelled each other and alpha particles are repelled back
Rutherfords alpha scattering experiment showed that the charge on the nucleus of the atom must be?
positive
What caused the deflection of the alpha particles in Rutherfords gold foil experiment?
A zinc sulfide coated screen surrounding the gold foil produced a flash of light whenever it was struck by an alpha particle. By noting where the flash occurred, the scientists could determine if the atoms in the gold foil deflected the alpha particles.
How did Rutherford's alpha scattering experiment show that Thomson's plum pudding model of the atom incorrect?
Rutherfords experiment proved the existence of a nucleus as some alpha particles "bounced back" from the gold foil sample . Thomson model did not involve a nucleus and predicted just a slight deflection or none at all.
Do the alpha particles in Rutherford's experiment contain electrons?
Alpha particles are helium-4 nuclei; they do not contain electrons.
What conclusion about the atom came from Ernest Rutherfords famous gold foil experiment?
The conclusions were that the nucleus in an atom must:- (1) Be positive as it repelled the positive alpha-particles (2) Have a high mass, as the deflections were massive (3) Be very small as only a few of the particles were deflected
When Rutherford performed his metal foil experiment did the alpha particles pass straight through the foil or bounce back?
The alpha particles beam is scattered.
What scientific inquiry skill was Rutherford using in selecting Thomson's model for investigation?
Thomsons model is sometimes called the plum pudding model. Rutherfords results that while most alpha particles were undeflected some alpha particles bounced back
