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When Rutherford ran his gold foil experiment, he expected to see results like those in the Plum Pudding Atom simulation. Instead, his experimental results were closer to those seen in the Rutherford Atom simulation.

Why can’t the plum pudding model of the atom explain Rutherford’s experimental results?

A. Since some alpha particles were deflected, the atom must contain a small region with a strong electric charge.

B. Since most of the alpha particles were not deflected, the atom’s positive charges must be spread thinly across a large region.

C. Since some of the alpha particles were deflected, the atom’s negative charges must not be attracted to the alpha particles.

D. Since most of the alpha particles were not deflected, the atom’s negative charges must exist in a thin cloud around the atom.

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Rutherford's result can not be explained on the basis of the plum pudding model because of the fact that, since some alpha particles were deflected, the atom must contain a small region with a strong electric charge.

The empirical study of the atom led to the emergence of several models of the atom. In the Plum - pudding model, the atom was regarded as a positively charged sphere with embedded negative charges.

This model can not interpret the Rutherford experiment since alpha particles were deflected. The deflection of alpha particles means that, the atom must contain a small region with a strong electric charge.

Learn more: https://brainly.com/question/730256

Answer:

A. Since some alpha particles were deflected, the atom must contain a small region with a strong electric charge.

Explanation:

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