In Rutherford's famous experiment, he shot heavy, fast moving, positive alpha particles at a thin gold foil. Based on Thomson's plum pudding model of the atom, what did Rutherford expect to happen, and why? All the alpha particles would be deflected by the foil because of the even distribution of mass and charge throughout the atom. All the alpha particles would pass straight through the foil because of the even distribution of mass and charge throughout the atom. Most of the alpha particles would become embedded in the foil because they are attracted to the negative electrons in the atom. Some of the alpha particles would be deflected and some would pass through because of the negative charge of the electron cloud.

Rutherford expected alpha particle to travel almost straight through a target of gold foil. The results of his gold foil experiment did not supportGroup of answer choicesThomson’s plum pudding theoryMillikan’s oil drop experimentThe cathode ray phenomenonBohr’s atomic model

Explain Rutherford's gold foil experiment. What were its major findings and how did it contribute to our understanding of atomic structure?

In Rutherford experiment a small fraction of  α -particles are scattered at small angle becauseSelect an answerA α  -particles are attracted by a negatively charged particleB α  -particles are pushed towards the heavy nuclear regionC α  -particles are repelled by positively charges regionD α  -particles are attracted by positively charged region

Rutherford’s experiment established that

explain rutherford experiment with diagram