how is bohr's atomic model different from rutherfords model
Answers
Answer:
Bohr thought that electrons orbited the nucleus in quantised orbits. ... In Rutherford's model most of the atom's mass is concentrated into the centre (what we now call the nucleus) and electrons surround the positive mass in something like a cloud. Bohr's most significant contribution was the quantization of the model
Rutherford proposed that most of the atom was empty space with the mass and positive charge concentrated in a tiny nucleus. Electrons would orbit the nucleus similar to how planets orbit the sun.
However, Rutherford's model did not explain why the negative orbiting electron did not lose energy and be pulled into the positive nucleus.
Bohr proposed an atomic model based on quantum theory where electrons moved around the nucleus in definite orbits.
If the electron absorbs a quantum of energy, it moves to an orbit with a higher energy level. It then becomes excited and emits energy to return to its stable orbit.
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Answer:
Rutherford depicted the particle as comprising of a little certain mass encompassed by a haze of negative electrons. Bohr felt that electrons circled the core in quantised circles.
Bohr based upon Rutherford's model of the particle. In Rutherford's model a large portion of the particle's mass is moved into the middle (what we currently call the core) and electrons encompass the positive mass in something like a cloud.
Bohr's most critical commitment was the quantisation of the model. He accepted that electrons moved around the core in roundabout circles with quantised potential and motor energies. So it was impractical for electrons to involve only any energy level.
On a fundamental level the quantisation part of the model is as yet accepted to be right. The primary issue lies in the possibility of electrons in round circles. This doesn't fulfill the Heisenberg vulnerability standard, which is that it is beyond the realm of possibilities to expect to know the position and energy of a molecule at the same time.
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