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Rutherford investigated atoms by firing small, positively charged particles at a thin sheet of gold foil. What results would he expect to see if he believed Thomson’s model of the atom to be correct?

All of the particles would bounce back from the front of the foil because the atom was a dense, solid ball of matter.
Most of the particles would pass straight through the foil because the atom was mostly the empty space in the electron cloud.
Most of the particles would pass through at a small angle because the atom is mostly empty space, but with a massive, dense, positively charged center.
Most of the particles would pass through with a few moving at small angles because the atom was a low-density, positive material with electrons in it.

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Most of the particles would pass through with a few moving at small angles because the atom was a low-density, positive material with electrons in it.

Answer: The correct statement is all of the particles would bounce back from the front of the foil because the atom was a dense, solid ball of matter.

Explanation:

J.J. Thomson gave a model which is known as Plum pudding model. In this model, he stated that the electrons are embedded in the pool of positive charge just like the plums are embedded in a pudding.

Rutherford, then took an experiment known as Gold foil experiment. In his experiment, he took a gold foil and then he bombarded it with alpha particles which carry positive charge of +2 units. He first thought that many of the particles will bounce back from their path because a dense, solid ball of positive charge is present in an atom.

Hence, the correct statement is all of the particles would bounce back from the front of the foil because the atom was a dense, solid ball of matter.

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