QuestionJune 20, 2025

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? Since some alpha particles were deflected, the atom must contain a small region with a strong electric charge. Since most of the alpha particles were not deflected, the atom's positive charges must be spread thinly across a large region. Since some of the alpha particles were deflected, the atom's negative charges must not be attracted to the alpha particles. Since most of the alpha particles were not deflected, the atom's negative charges must exist in a thin cloud around the atom.

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? Since some alpha particles were deflected, the atom must contain a small region with a strong electric charge. Since most of the alpha particles were not deflected, the atom's positive charges must be spread thinly across a large region. Since some of the alpha particles were deflected, the atom's negative charges must not be attracted to the alpha particles. Since most of the alpha particles were not deflected, the atom's negative charges must exist in a thin cloud around the atom.
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? Since some alpha particles were deflected, the atom must contain a small region with a strong electric charge. Since most of the alpha particles were not deflected, the atom's positive charges must be spread thinly across a large region. Since some of the alpha particles were deflected, the atom's negative charges must not be attracted to the alpha particles. Since most of the alpha particles were not deflected, the atom's negative charges must exist in a thin cloud around the atom.

Solution
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Answer

The Plum Pudding Model cannot explain Rutherford's results because it lacks a concentrated nucleus to cause significant deflection of alpha particles. Explanation 1. Analyze the Plum Pudding Model The Plum Pudding Model suggests that positive charges are spread uniformly throughout the atom, with electrons embedded within it. 2. Compare with Rutherford's Observations Rutherford observed that most alpha particles passed through the foil, but some were deflected at large angles, indicating a concentrated positive charge. 3. Explain Deflection of Alpha Particles The deflection implies a small, dense region of positive charge (nucleus), which contradicts the uniform distribution in the Plum Pudding Model. 4. Conclusion on Charge Distribution Since most alpha particles were not deflected, positive charges cannot be spread thinly; they must be concentrated in a nucleus.

Explanation

1. Analyze the Plum Pudding Model<br /> The Plum Pudding Model suggests that positive charges are spread uniformly throughout the atom, with electrons embedded within it.<br /><br />2. Compare with Rutherford's Observations<br /> Rutherford observed that most alpha particles passed through the foil, but some were deflected at large angles, indicating a concentrated positive charge.<br /><br />3. Explain Deflection of Alpha Particles<br /> The deflection implies a small, dense region of positive charge (nucleus), which contradicts the uniform distribution in the Plum Pudding Model.<br /><br />4. Conclusion on Charge Distribution<br /> Since most alpha particles were not deflected, positive charges cannot be spread thinly; they must be concentrated in a nucleus.
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