Question

Describe what Rutherford would have seen in his gold foil experiment if J.J Thompson's Plum Pudding model was completly accurate

Answer 1

If the plum-pudding model were correct, alpha particles should travel straight through the atoms that make up the gold. If the plum-pudding model were correct, all of the alpha particles should hit the screen almost directly opposite the particle source. However, that is not what they observed. Most of the alpha particles passed right though the foil, as expected. However, some of them were deflected at very large angels. Rutherford's results showed that the plum-pudding model could not be correct. Instead, an atom must actually contain mostly empty space. All of the positive charge is concentrated in a tiny, dense nucleus. Electrons surround the nucleus.

Step-by-step explanation:

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Answer 2

Answer is: Rutherford demonstrate that J.J Thompson's Plum Pudding model was not accurate.

Rutherford theorized that atoms have their charge concentrated in a very small nucleus.
This was famous Rutherford's Gold Foil Experiment: he bombarded thin foil of gold with positive alpha particles (helium atom particles, consist of two protons and two neutrons).
Rutherford observed the deflection of alpha particles on the photographic film and notice that most of alpha particles passed straight through foil.
That is different from Plum Pudding model, because it shows that most of the atom is empty space.