A charged particle travelling in a circular path would constantly lose energy and collapse into the nucleus.According to Rutherford’s Model, electrons will circle the positively charged nucleus, which is not expected to be stable.Because only a tiny fraction of α-particles entirely rebounded, it suggested that the atom’s mass and positive charge are concentrated in a limited volume and are not evenly distributed.Only a few α-particles deviated from their path, implying that the atom’s positive charge occupies a small amount of space.Because a vast number of the α-particles directed towards the gold sheet pass through it without deflection, the bulk of the space in an atom is empty.Only a few α-particles were redirected (by 180 degrees).Some of the α-particles were deflected by the foil at relatively small angles.The vast majority of the fast-moving α-particles passed right through the gold foil.Rutherford discovered the following as a result of his α-particle scattering experiment: However, the experiment yielded utterly unexpected outcomes.Rutherford did not expect to see substantial deflections since the alpha-particles were much heavier than the protons.The notion was that the subatomic particles in gold atoms would deflect alpha particles.Alpha-particles are double-charged helium ions because they have a mass of around 4 amu, rapidly moving alpha-particles contain a lot of energy.The gold foil had a thickness of roughly 1000 atoms.He used the gold foil to provide an exceedingly thin coating.A thin sheet of gold was bombarded with rapidly moving alpha -particles.Rutherford organised the Alpha particle Scattering Experiment to investigate how electrons are grouped in an atom. After striking the foil, the path of the particles can be traced by flashes produced on the photographic plate. In Rutherford’s alpha scattering experiment, fast-moving alpha particles are emitted from the source, which is directed towards gold foil. Rutherford organised the Alpha Particle Scattering Experiment to find out the arrangement of electrons in an atom. Rutherford’s models of an atom include the nuclear model and the planetary model. The Rutherford model improved on the Thomson model, but it still could not explain the stability of the atom or how the electron does not sink into the nucleus. For instance, the model asserts that most of an atom is empty, with the nucleus containing the majority of the atomic mass. Depending on the outcomes of the alpha-particle scattering experiment, Rutherford’s atomic model provides information about the configuration of an atom. Ernest Rutherford conducted the alpha particle scattering experiment to understand the positioning of subatomic particles inside an atom.
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