Path of Scattered Alpha Particles in Rutherford's Experiment
The path of scattered alpha particles in Rutherford's experiment can be explained in detail as follows:

1. Setup of the Experiment:
- In Rutherford's famous gold foil experiment, alpha particles were emitted from a radioactive source towards a thin gold foil.
- The alpha particles were expected to pass through the gold foil with little to no deflection, according to the prevailing plum pudding model of the atom.

2. Observation of Scattering:
- Surprisingly, some alpha particles were deflected at large angles, while others even bounced back in the direction from which they came.
- This unexpected result led Rutherford to conclude that the positive charge of the atom must be concentrated in a small, dense nucleus at its center.

3. Explanation of Scattering Path:
- Most of the alpha particles passed straight through the gold foil, as they encountered no significant obstacles.
- Some alpha particles were deflected at small angles as they came close to the positively charged nucleus of the gold atoms.
- A few alpha particles, due to their close approach to the nucleus, experienced strong repulsion and were scattered at large angles or even bounced back.

4. Significance of the Experiment:
- Rutherford's experiment revolutionized the understanding of atomic structure, leading to the development of the nuclear model of the atom.
- The discovery of the atomic nucleus paved the way for further research into subatomic particles and the development of modern atomic theory.
In conclusion, the path of scattered alpha particles in Rutherford's experiment revealed the existence of a dense, positively charged nucleus at the center of the atom, challenging the prevailing model of the atom at that time.

About 99% remained indeflected 0.9% particles move making some angle and only about 0.1% alpha particles get completely reflected and move antiparallel to original direction. it proves small and highly densed nucleus located in an atom.