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Bohr's model:  
In  1913 Bohr proposed his quantized shell model of the atom to explain how electrons can have stable orbits around the nucleus. The motion of the electrons in the Rutherford model was unstable because, according to classical mechanics and electromagnetic theory, any charged particle moving on a curved path emits electromagnetic radiation; thus, the electrons would lose energy and spiral into the nucleus. To remedy the stability problem, Bohr modified the Rutherford model by requiring that the electrons move in orbits of fixed size and energy. The energy of an electron depends on the size of the orbit and is lower for smaller orbits. Radiation can occur only when the electron jumps from one orbit to another. The atom will be completely stable in the state with the smallest orbit, since there is no orbit of lower energy into which the electron can jump.
Rutherford model: 
By 1911 the components of the atom had been discovered. The atom consisted of subatomic particles called protons and electrons. However, it was not clear how these protons and electrons were arranged within the atom. J.J. Thomson suggested the"plum pudding" model. In this model the electrons and protons are uniformly mixed throughout the atom:
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Rutherford proposed that the atom consists of a nucleus composed of protons with electrons spinning around it.
However, this model was considered to be unstable because electrons would eventually lose energy and fall into the nucleus.
To remedy this problem, Bohr proposed a concept of 'discrete orbits', orbits having a specific angular momentum. These were the only orbits which could exist in an atom. Electrons in these orbits could neither radiate nor gain energy.
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Bohr's model :
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