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yes it is
Vincent Hilpert
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∙ 13y agoAlpha particles have twice the charge of beta particles, so they will tend to interact with an electric field more than beta. Also, they have mass approximately 7,300 times more than beta, so they will also tend to interact with matter more than beta.
Wiki User
∙ 7y agoThe conclusion was that alpha particles met another particles with positive charge.
Wiki User
∙ 12y agoyes it is
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What is the difference between the angle of deviation of the alpha particles closer to the nucleus and that of those that are farther away?
Angle of deviation closer to the nucleus is greater that father from nucleus. These deviations are caused by repulsion of like charges, that is the proton and the alpha particle. Most of the alpha particles pass through, not deviated by large angles, and few rebound back. :D
What did Rutherford gold foil experiment suggest about the structure of an atom?
1) Atoms were mostly empty space (because most alpha particles went straight through the gold foil) 2) Atoms had a dense nucleus (because few alpha particles bounced straight back from the atoms) 3) The nucleus of atoms were positively charged (some alpha particles were deflected at large angles)
Why is proton more effective than in electron in deflecting alpha particles?
Alpha particles, which are helium nuclei consisting of two protons and two neutrons, are large and positively charged. Electrons have almost no mass and are negatively charged. They would be attracted to alpha particles, not deflected. Protons are approximately 2000 times larger than electrons and are positively charged, therefore they would be much more effective in deflecting alpha particles. Remember that like charges repel.
Are alpha particles big or small?
Absolutely small ... they're the nucleus of a helium atom (2protons & 2 neutrons) - But they are gigantic as compared to a beta particle ... which is just a free electron. - Note that gamma rays don't have any (rest) mass ... they're just radiation.
How did Rutherford infer that the nucleus was very small?
In conclusion... Rutherford's experiment involved a radioactive source emitting alpha particles (2 protons and 2 neutrons). The radioactive source was aimed at a thin sheet of gold. The main observation made was that a few alpha particles were repelled back the way they had come, and this was not expected. This was because the positively charged alpha particles (2 protons), by the laws of electrostatic repulsion, were repelled by the positively charged nucleus of the atoms in the gold. He then made the final conclusion of that the small nucleus of an atom is central, has a large mass and positive charge. So yes, the nucleus is small compared to the size of an atom, however it was mainly the fact that there is one concentration of positive charge (nucleus) in the atom that repelled the alpha particles that helped Rutherford to show the structure of an atom.
Why weren't all the alpha particles deflected in Rutherford experiment?
While most alpha particles passed straight through the foil. A small % of them were deflected at very large angles, some even backscattered. Because alpha particles have about 8000x the mass of an electron and impacted the foil at very high velocitiesIn order for the alpha particles to be deflected by significant amounts, they must pass close to one or more nuclei in the foil. Since nuclei occupy only a very small fraction of the the volume of an atom, and the foil was very thin so it was not very many atoms thick, the likelihood of such close encounters was small and only a small fraction of the alpha particles were deflected by large angles.
What is the difference between the angle of deviation of the alpha particles closer to the nucleus and that of those that are farther away?
Angle of deviation closer to the nucleus is greater that father from nucleus. These deviations are caused by repulsion of like charges, that is the proton and the alpha particle. Most of the alpha particles pass through, not deviated by large angles, and few rebound back. :D
If Rutherford had seen a large number of alpha particles reflected what view of the atom would we accept today?
that the nucleus of the atom was a lot larger than we now believe but the charge was not as spread out as you would expect.
Why does paper stop alpha from traveling?
The alpha particles are too large to fit through the gaps between the particles of the paper.
Why did the path of only some alpha particles deviate in Rutherford experiment?
Alpha particles are positively charged helium nuclei. As such, they are repelled by other positively-charged nuclei. In Rutherford's experiment, he used gold foil. Since gold atoms have large, massive nuclei, the alpha particles were easily repelled by the large gold atom nuclei, and they were scattered in different directions.
Which observations helped Rutherford determine that atoms have tiny dense positively charged nuclei?
A+ answer: A few of the alpha particles in his expeirment were deflected from the gold foil at large angles. Scattering pattern of alpha particles 'shot' at a thin gold foil. Most went straight thru showing the nucleus was very small. Analysis of the scattering showed electrical repulsion, not that the particles actually hit the nucleus and bounced off.
What is Rutherford's experiment with gold foil and alpha particles?
The initial discovery of "Rutherford Scattering" was made by Hans Geiger and Ernest Marsden in 1909 when they performed the gold foil experiment under the direction of Rutherford, in which they fired a beam of alpha particles (helium nuclei) at layers of gold leaf only a few atoms thick. The intriguing results showed that around 1 in 8000 alpha particles were deflected by very large angles (over 90°), while the rest passed straight through with little or no deflection. From this, Rutherford concluded that the majority of the mass was concentrated in a minute, positively charged region (the nucleus) surrounded by electrons. When a (positive) alpha particle approached sufficiently close to the nucleus, it was repelled strongly enough to rebound at high angles. The small size of the nucleus explained the small number of alpha particles that were repelled in this way.
What did Rutherford gold foil experiment suggest about the structure of an atom?
1) Atoms were mostly empty space (because most alpha particles went straight through the gold foil) 2) Atoms had a dense nucleus (because few alpha particles bounced straight back from the atoms) 3) The nucleus of atoms were positively charged (some alpha particles were deflected at large angles)
Why is proton more effective than in electron in deflecting alpha particles?
Alpha particles, which are helium nuclei consisting of two protons and two neutrons, are large and positively charged. Electrons have almost no mass and are negatively charged. They would be attracted to alpha particles, not deflected. Protons are approximately 2000 times larger than electrons and are positively charged, therefore they would be much more effective in deflecting alpha particles. Remember that like charges repel.
What caused the deflection of the alpha particles in Rutherford's gold foil experiment?
The alpha particles scatter from the atomic nuclei in the gold foil. The repulsive electrostatic force between the nucleus and the alpha particle (because both are positively charged and like charges repel) deflects the alpha particle. Because of the large mass and (relatively) large energy of the alpha particles in Rutherford scattering experiments, the alpha particles are largely unaffected by the electrons in the gold atoms. More accurately, the scattering of the alpha particles from the electrons produces small angular deflections.Because the nucleus is small -- approximately 1/10000th the size of the whole atom -- most of the time the alpha particles will pass through the atom with little or no deflection. But occasionally, the alpha particles will start on a trajectory that, without the electrostatic deflection, would take them very close to the nucleus. In such cases, the electrostatic force produces a large angular deflection and can even scatter the alpha particles backwards. If the positive charge in the atom were distributed over the entire size of the atom, the likelihood of having such a large-angle scattering would be much smaller than it was (is) observed to be. Thus, the original experiments demonstrated that the positive charge in atoms is confined to a small region at the very center of an atom. Indeed, the data also provided an estimate of the size of the nucleus. More advanced analyses of such scattering experiments with modern equipment but using electron beams have provided detailed measurements of nuclear diameters for a wide range of atomic nuclei.
How did Rutherford explain the results of his gold foil experiment?
Rutherford made the following conclusions:Since most of the alpha particles passed straight through the gold foil without any deflection, most of the space within the atoms is empty.Since some of the alpha particles (which are big in size) were deflected by large angles or bounced backwards, they must have approached some positively charged region responsible for the deflection. This positively charged region is now called the nucleus.As very few alpha particles undergone the deflection, it was concluded that the volume occupied by the central region ( nucleus ) is very small.Since alpha particles which are relatively denser, were deflected by the central volume of charge, it shows that almost the complete mass of the atom must be within the central volume.
What is the penetration ability of alpha?
Alpha particles have a large mass and are easily absorbed and thus can only travel a few inches from their sources in air and will easily be absorbed by clothing. That being said if the source is ingested alpha particles are the most damaging form of radiation having a strong ionizing effect on their surroundings due to their high charge.
