Question

how did rutherford’s atomic model fix the shortcomings of thomson’s atomic model?

rutherford’s model showed that electrons orbit the nucleus with distinct radii.
rutherford’s model showed that the positive charge is concentrated in a small area.
rutherford’s model proved that electrons are dispersed in a cloud of positive charge.
rutherford’s model showed that electrons behave according to the wave theory.
rutherford’s model proved that much of the atom consists mostly of empty space.

Explanation:

1. Recall Thomson's "plum - pudding" model: It proposed that electrons are embedded in a positively charged "soup" (or cloud), and the atom is a uniform sphere of positive charge with electrons scattered within.
2. Analyze Rutherford's model (from his gold - foil experiment):

• When alpha particles were fired at gold foil, most passed through (showing that most of the atom is empty space), some were deflected at small angles, and a few were deflected at large angles (showing a small, dense, positively charged nucleus at the center).
• Option 1: Electrons orbiting with distinct radii was part of Bohr's model, not Rutherford's. So this is incorrect.
• Option 2: Rutherford's model showed that the positive charge is concentrated in a small area (the nucleus), while Thomson's model had positive charge spread out. This is correct.
• Option 3: This describes Thomson's model, not Rutherford's. So this is incorrect.
• Option 4: The wave theory of electrons is related to quantum mechanics (de Broglie, Schrödinger, etc.), not Rutherford's model. So this is incorrect.
• Option 5: Rutherford's gold - foil experiment showed that most alpha particles passed through the gold foil, meaning much of the atom consists mostly of empty space. Thomson's model did not account for this empty space. This is correct.

Answer:

B. Rutherford’s model showed that the positive charge is concentrated in a small area.
E. Rutherford’s model proved that much of the atom consists mostly of empty space.