In rutherfords gold foil experiment he concluded that the atom is mostly empty space with a small massive positively chargeed centrer because?

Answer 1

When the beam of electrons passed through the gold foil, some were deflected at odd angles. This indicated the presence of a more massive portion of the atom that could be explained by the raisin pudding model.

Answer 2

Under the prevailing plum pudding model of thomson, the alpha particles should all have been deflected by, at most, a few degrees; measuring the pattern of scattered particles was expected to provide information about the distribution of charge within the atom.

However it was observed that a very small percentage of particles were deflected through angles much larger than 90 degrees. This led them to conclude that most of the space in

an atom was empty and the charge is concentrated at very tiny space.

Answer 3

most of the alpha particles passed through the gold foil undeflected or with slight deflection, suggesting that the atom is mostly made up of empty space. The few alpha particles that were deflected back indicated the presence of a small, dense, positively charged nucleus at the center of the atom.

Answer 4

Because most of the particles passed straight through the foil, some were slightly deflected and a few were bounced back.