Question

In Rutherford's experiment, generally the thin foil of heavy atoms like gold, platinum etc. have been used to be bombarded by the α-particles. If the thin foil of light atoms like aluminium etc. is used, what difference would be observed from the above results?

Answer 1

As we know that the Rutherford model was concocted by the New Zealand-conceived physicist Ernest Rutherford to depict a molecule. Rutherford coordinated the Geiger–Marsden try in $1909$ , which recommended, upon Rutherford's $1911$ examination, that J. J. Thomson's plum pudding model of the iota was erroneous. Rutherford's new model for the particle, in view of the test results, contained new highlights of a moderately high focal charge gathered into a little volume in contrast with the remainder of the molecule and with this focal volume additionally containing the heft of the nuclear mass of the iota. This area would be known as the "core" of the particle.

Complete answer:
Significant ends from the Rutherford try were drawn from the number and point of impression of the helium particles from the occurrence point. Returning back around one out of $20,000$ occurrence alpha particles because of aversion affirmed the presence of a weighty and enormous positive charge in the gold iota ($Z = 79$ ).
A foil of little molecules like aluminum, having a less number of positive charges ($Z = 13$ ) won't rebuff a quick alpha molecule to return. At the most extreme it might divert them at little points.
Thus, the arrival of alpha particles would not have been noticed and the foundation of a core would not have been made.

Note:
We need to know that after Rutherford's revelation, researchers began to understand that the molecule isn't conclusively a solitary molecule, however it consists of far more modest subatomic particles. Ensuing examination determined the specific nuclear construction which prompted Rutherford's gold foil test. Researchers in the long run found that molecules have an emphatically charged core (with an accurate nuclear number of charges) in the middle, with a range of about $1.2 \times meters \times \left[\text{atomic mass number}\right]$ . Electrons were discovered to be considerably more modest.
Afterward, researchers tracked down the normal number of electrons (equivalent to the nuclear number) in an iota by utilizing X-beams. At the point when an X-beam goes through a molecule, some of it is dispersed, while the rest goes through the iota. Since the X-beam loses its power basically because of dissipating at electrons, by noticing the pace of abatement in X-beam force, the quantity of electrons contained in a particle can be precisely assessed.