In 1910, Ernest Rutherford performed a set of experiments that helped scientists better understand the structure of atoms. He directed a beam of α particles (small, positively charged particles) at a very thin sheet of gold foil. He made several observations from the experiments.
How did Rutherford interpret the fact that most of the α particles seemed to pass right through the foil?
The foil was so thin that the α particles were able to pass in between the tiny, solid gold atoms.
Gold is malleable so the gold atoms moved out of the way of the α particles and allowed them to pass through.
Most of the volume of an atom is empty space so the α particles passed unobstructed through the electron clouds of the atoms.
How did Rutherford interpret the fact that a few of the α particles were deflected at very large angles?
The α particles were striking the small, positively charged nucleus of the gold atoms.
The α particles were striking the neutrally charged neutrons in the gold atoms.
The α particles were striking the negatively charged electrons in the gold atoms.
What differences would Rutherford have observed if he used aluminum foil instead of gold foil?
Less of the α particles would have passed through the aluminum foil unobstructed, and more would have been deflected at a large angle.
None of the α particles would have passed through the aluminum foil, and all of them would have deflected at a large angle.
More of the α particles would have passed through the aluminum foil unobstructed, and less would have been deflected at a large angle.
All of the α particles would have passed through the aluminum foil unobstructed, and no particles would have deflected at a large angle.