Drawbacks of Rutherford's model of an atom...
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RUTHERFORD DIDN'T EXPLAIN STABILITY OF AN ATOM WHICH MEANS THAT THE DRAWBACK WAS HE Didn't PROVE THAT IF THE ELECTRON IS REVOLVING AROUND THE NUCLEUS IT MUST HAVE SOME ACCELERATION AND IT SHOULD LOOSE ENERGY AND FALL INTO THE NUCLEUS BUT THIS DOES NOT HAPPEN IN REAL LIFE
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The comparison of electrons with planeta in the solar system is the main drawback of Rutherford's atomic model. According to the classical laws of mechanics and electrodynamics, if an electrically charged particle is in motion, it inevitably radiates energy. Thus, an electron, when moving around the nucleus continually, should radiate energy,i.e. loses energy. As a result, it should be gradually pulled towards the nucleus and end up colliding with it. This should result in the total collapse of the atom. If it was so, the atom should exist in the form that we know. However, we know that an atom is structurally stable. Thus Rutherford's model failed to explain the stability of an atom.
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