College Physics II – Mechanics, Sound, Oscillations, and Waves
Definition
Rutherford scattering describes the deflection of particles off a target nucleus observed by Ernest Rutherford. It provided key insights into the structure of the atom, specifically the existence of a small, dense nucleus.
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Rutherford's experiment involved alpha particles and gold foil.
Most particles passed through the foil with little to no deflection, indicating atoms are mostly empty space.
A small fraction of particles were deflected at large angles, suggesting a dense, positively charged nucleus.
The discovery led to the nuclear model of the atom, replacing the plum pudding model.
Rutherford scattering equations can be derived using principles of conservation of momentum and energy.
Review Questions
What was significant about the large-angle deflections observed in Rutherford's experiment?
How did Rutherford's findings contradict the plum pudding model?
What key principle is used to derive equations for Rutherford scattering?
Related terms
Alpha Particles: Positively charged particles consisting of two protons and two neutrons, emitted during radioactive decay.
Nuclear Model: The atomic model proposing that atoms have a small, dense nucleus surrounded by electrons.
Conservation of Momentum: $\text{A fundamental principle stating that the total linear momentum in a closed system remains constant if no external forces act on it.}$