In Ernest Rutherfords gold foil experiment, most positively charged particles passed through the foil, but a few particles were deflected strongly. What did this result cause Rutherford to infer?

That electrons have almost no mass.

That an atoms positive charge must be clustered in a tiny region in its center, called the nucleus.

That an atom consists of negative charges scattered throughout a ball of positive charge something like raisins or berries in a muffin.

That electrons move in specific orbits around the nucleus of an atom.

Question

In Ernest Rutherfords gold foil experiment, most positively charged particles passed through the foil, but a few particles were deflected strongly. What did this result cause Rutherford to infer?
 	
	That electrons have almost no mass.

That an atoms positive charge must be clustered in a tiny region in its center, called the nucleus.

That an atom consists of negative charges scattered throughout a ball of positive charge something like raisins or berries in a muffin.

That electrons move in specific orbits around the nucleus of an atom.

anonymous · Answer

That an atoms positive charge must be clustered in a tiny region in its center, called the nucleus.

anonymous · Answer

coulomb's law states that opposite charges attract and like charges repel. And that guy is wrong. The electrons were deflected randomly because they were repelling off of the golds electrons. So the final choice is the correct one.

ookawaiioo · Answer

Ya both wrong....

Its....

That an atom consists of negative charges scattered throughout a ball of positive charge something like raisins or berries in a muffin.

ookawaiioo · Answer

Wait, actually, the first guy, 2cool, is correct.

vincent-lyon.fr · Answer

The second answer is the right one.