Question

Explain Rutherford’s α-particle scattering experiment and give its observation and conclusion drawn.

Answer 1

Answer:

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Explanation:

Rutherford reasoned that if positively charged mass present within the atom is thinly spread, then, any

positively charged particle moving with sufficient kinetic energy would easily penetrate through it. Thus,

if a thin gold foil is exposed to fast moving positively charged particles then the particles should pass

through the foil .These particles can be detected using a zinc sulphide screen, placed behind the gold

foil, when scintillations are produced on screen. Rutherford chose alpha particles (He 2+ ) obtained from

radium and then accelerated these particles. They were then condensed to a narrow beam by passing

them through positively charged parallel plates . They were finally directed against a very thin gold foil

placed at the centre of a circular zinc sulphide screen.

. Observation and Inference

1 Most of the fast moving particles

passed straight through the gold foil.

Most of the space inside the atoms is empty.

2 Some of the alpha particles deflected

by the foil through small or large

angles.

The positive charge of the atom occupies very little

space inside the atom.

3 One out of every 12000 alpha particles

appeared to rebound / recoil.

All the positive charge and mass of the atom are

concentrated in a very small volume within the

atom.

On the basis of his experiment Rutherford put forward his nuclear model of the atom.

i) There is a positively charged centre in the atom called the nucleus. Nearly all the mass of the

atom resides in the nucleus.

ii) The electrons revolve around the nucleus in well defined orbits.

iii) The size of the nucleus is very small as compared to the size of the atom.

Answer 2

Rutherford passed beams of alpha particles through a thin gold foil to observe the atom and noted how the alpha particles scattered from the foil.

Observations of Rutherford's alpha ray scattering experiment:
1.Most of the α-particles passed straight through the gold foil without any deviation.
2. Some of the α-particles were deflected by the foil by some angles.
3.Interestingly one out of every 12,000 alpha particles appeared to rebound

Conclusion of Rutherford's scattering experiment:
1.Most of the space inside the atom is empty because most of the α-particles passed through the gold foil without getting deflected.
2. Very few particles were deflected from their path, indicating that the positive charge of the atom occupies very little space.
3.A very small fraction of α-particles were deflected by very large angles, indicating that all the positive charge and mass of the gold atom were concentrated in a very small volume within the atom.