If the Thompson model of the atom was correct, then the result of Rutherford's gold foil experiment would have been :
Show Hint
Rutherford's gold foil experiment was a pivotal moment in atomic theory. The key observation was the large-angle scattering of a few alpha particles, which was completely unexpected based on Thomson's model and implied a small, dense, positively charged nucleus.
All of the $\alpha$-particles pass through the gold foil without decrease in speed.
$\alpha$-Particles pass through the gold foil deflected by small angles and with reduced speed.
$\alpha$-Particles are deflected over a wide range of angles.
All $\alpha$-particles get bounced back by 180$^\circ$.
Hide Solution
Verified By Collegedunia
The Correct Option isA
Solution and Explanation
The Thompson model, also known as the "plum pudding" model, described the atom as a sphere of uniformly distributed positive charge with negatively charged electrons embedded within it.
In this model, the mass and positive charge are spread out over the entire volume of the atom.
If $\alpha$-particles (which are positively charged) were fired at such an atom, they would not encounter any concentrated region of positive charge or mass.
The electrostatic repulsive forces from the diffuse positive charge would be too weak to cause any significant deflection.
Therefore, according to the Thompson model, the $\alpha$-particles were expected to pass straight through the gold foil with little to no deflection.
Option (A) best represents this expected outcome, simplifying "little to no deflection" to an ideal case of no deflection or change in speed. Option (C) and (D) describe the actual observations that disproved the Thompson model and led to the Rutherford nuclear model.
