J.J. Thomson’s model, also known as the “plum pudding” model, had several key limitations. It failed to explain the stability of the atom, didn’t account for the presence of a nucleus, and couldn’t explain the results of Rutherford’s alpha-particle scattering experiment.
Here’s a more detailed look at the limitations:
Inability to explain atomic stability:
The model proposed that negatively charged electrons were embedded within a positively charged sphere, but it didn’t explain how these charges could remain together or how the atom could be stable.
Absence of a nucleus:
Thomson’s model did not include the concept of a central nucleus containing protons and neutrons, which was later established by Rutherford.
Failure to account for Rutherford’s experiment:
The model couldn’t explain why alpha particles, directed at a thin metal foil, would be deflected, rather than passing straight through, as predicted by Thomson’s model.
Lack of experimental evidence:
While Thomson’s model was based on the discovery of the electron, it lacked direct experimental support for its structure of the atom as a whole.