Which hypothesis of thomson's atomic model was later found to be not true by niels bohr and why?
Answer is: the electrons are embedded in the positive charge.
J. J. Thomson discovered the electron in 1897.
Thomson suggested "plum pudding" model in 1904.
According to the Bohr model of the atom:
1. Electrons orbit the nucleus in orbits that have a set size and energy.
2. Energy levels of electrons are discrete (certain discrete values of energy).
3. Electrons can jump from one energy level to another, absorbing or emitting electromagnetic radiation with a frequency ν (energy difference of the levels).
J.J. Thompson hypothesized the atom in the form a positively charged sphere with negatively charged electrons floating the positively charged sphere. This was referred to as the Plum-pudding model. This assumption about the atom was shown to be incorrect by the next set of scientists Rutherford (planetary model) and Neils Bohr as the mass of the atom is localized at the center in the positively charged nucleus around which the negatively charged electrons orbited in specific paths. Bohr proposed that the energy levels or orbits in which the electrons revolve round the nucleus are quantized.
The "plum pudding" atomic model
J.J. Thomson suggested the "plum pudding" model in which the electrons and protons are uniformly mixed throughout the atom.
Rutherford discarded Thomson's hypothesis through the results he obtained in his "gold foil" experiment. According to Rutherford, if Thomson's model was correct, then the mass of the atom must extend throughout the atom, so if it triggered high-speed alpha particles to an atom, there would be very little room to deflect the particles. However, when he shot these particles at a thin film of gold atoms he observed that most of them went through the plate, but to their surprise, some alpha particles bounced almost directly backwards.
These deviations were not consistent with Thomson's model, so Rutherford was forced to discard Plum Pudding's model and reasoned that the only way alpha particles could deviate backward was if most of the mass in a atom was concentrated in a nucleus.
he proposed that the atom was mostly empty space . the electrons revolve in curcular orbits about the massive positive charge at the centre his model explained how most of the a particles passed straight through the foil .the small particle nucleus would deflect the few particles that came close ..
: hope this helped you
The Idea that Electrons are spread evenly throughout the atom. Rutherford disproved this by aiming charged alpha particles through a piece of gold foil. The result allowed for scientists to realize that there was a cloud of electrons surrounding the nucleus, rather than being evenly distributed throughout it.
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Thomson described the atom using the "plum pudding" model, wherein there is uniform distribution of protons and electrons throughout the atom.
Rutherford tested the plum pudding model by executing the "gold foil" experiment. Rutherford that most of the alpha particles went right through the gold foil, which was in according to the plum pudding model. However, he noticed that a few alpha particles rebounded almost directly backwards.
This was the critical observation which caused Rutherford to discard Thomson’s atomic model and he reasoned that most of the mass in an atom was concentrated in a nucleus. Rutherford thus established the planetary model of the atom, in which all positively charged protons resided in the nucleus and the electrons orbited around the nucleus like planets around the sun.