Question

1. what was the most surprising observation from rutherfords gold foil experiment that contradicted the plum pudding model?
2. rutherfords gold foil experiment led to the development of the nuclear model of the atom. what is the central feature of this model?
3. how did rutherfords model of the atom differ most significantly from thomsons model?

a) rutherford proposed that atoms were indivisible. b) rutherford placed the positive charge in a concentrated central region. c) thomsons model included neutrons in the nucleus. d) thomsons model suggested that electrons orbited a central nucleus.

1. consider the progression of atomic models. how did

Explanation:

1. In Rutherford's gold - foil experiment, the most surprising was that a small fraction of alpha particles were deflected at large angles, which contradicted the plum - pudding model's idea of a uniform distribution of positive charge.
2. The central feature of Rutherford's nuclear model is that the atom has a small, dense, positively - charged nucleus at its center, with electrons orbiting around it.
3. Rutherford placed the positive charge in a concentrated central region, while Thomson's plum - pudding model had positive charge uniformly distributed. Thomson's model did not have a distinct nucleus and did not include neutrons in the nucleus, and electrons were not orbiting a central nucleus in his model. So the answer is b.

Answer:

1. A small fraction of alpha particles were deflected at large angles.
2. A small, dense, positively - charged nucleus at the center with electrons orbiting around it.
3. b. Rutherford placed the positive charge in a concentrated central region.