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Asked by Riddhi Last Modified
Answer Rutherford's α-particle scattering experiment provided significant insights into the structure of the atom. Let's analyze each option:
(a) Most of the space in the atom is empty. - This conclusion could be derived from Rutherford's experiment. The fact that most α-particles passed through the atom undeflected indicated that the majority of the atom is empty space.
(b) The radius of the atom is about 10−1010−10 m while that of the nucleus is 10−1510−15. - This conclusion could be derived from Rutherford's experiment. The scattering pattern of α-particles suggested that the nucleus, where most of the atom's mass is concentrated, is very small compared to the overall size of the atom.
(c) Electrons move in a circular path of fixed energy called orbits. - This conclusion could not be directly derived from Rutherford's experiment. Rutherford's experiment focused on the nucleus of the atom and did not provide direct evidence for the existence of electron orbits. This concept was later proposed by Niels Bohr based on the quantization of angular momentum in the hydrogen atom.
(d) Electrons and the nucleus are held together by electrostatic forces of attraction. - This conclusion could be derived from Rutherford's experiment. The fact that some α-particles were deflected suggested the presence of a positively charged nucleus that interacted with the negatively charged electrons, leading to the conclusion that electrons and the nucleus are held together by electrostatic forces of attraction.
Therefore, the conclusion that could not be directly derived from Rutherford's α-particle scattering experiment is:
(c) Electrons move in a circular path of fixed energy called orbits.
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