Question

Explain how Rutherford's α-scattering experiment suggested that the nucleus of an atom is very small, very dense and positively charged.​

Answer 1

Answer:

Conclusion of Rutherford's scattering experiment:

Most of the space inside the atom is empty because most of the α-particles passed through the gold foil without getting deflected. Very few particles were deflected from their path, indicating that the positive charge of the atom occupies very little space

Explanation:

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Answer 2

Concept:

α-Particle scattering experiment, Rutherford's Atomic Model

Answer and explanation:

In 1911, Rutherford explained successfully the large-angle scattering by proposing the structure of the atom based on his α-Particle scattering experiment. The following observations confirm that nucleus of an atom is very small, very dense and positively charged :

i) Some α-particles were deflected at small angles and their angular distribution was definite. Now, since α-particles are positively charged, the part of the atom deflecting them must also be positive. On this basis, Rutherford concluded that the whole of the positive charge of atome must be in a very small space.

ii) Very few of the α-particles were scattered at angles greater than 90° from their initial path and returned back. From this it is evident that when high-speed α-particles pass through the atoms of the gold foil, then a few of them experience such a strong repulsive force so as to return back. On this basis, Rutherford concluded that the positive charge in the atom is concentrated in an extremely small space at the centre of the atom. This space is called the 'nucleus'.

Hence, these observations suggested that the nucleus of an atom is very small, very dense and positively charged.

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