Advantages and disadvantages of rutherford atomic model
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Rutherford concluded from the α-particle scattering experiment that:
(i)Most of the space inside the atom is empty because most of the α-particles passed through the gold foil without getting deflected.(ii)Very few particles were deflected from their path, indicating that the positive charge of the atom occupies very little space.(iii)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.
(i)Most of the space inside the atom is empty because most of the α-particles passed through the gold foil without getting deflected.(ii)Very few particles were deflected from their path, indicating that the positive charge of the atom occupies very little space.(iii)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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It could not explain the stability of electrons in the orbits.
The electrons revolving in orbits are accelerating charged particles which will emit electromagnetic radiations which carry energy.
Due to continuous loss of energy the electron will revolve in a spiral path and finally will fall into nucleus. In this way, electrons can't exist outside the nucleus.
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