In Rutherford's golf foil experiment, no α-particles stuck to the atom. If α-particles had stuck to the atom, what might you have deduced about the atom's structure?

Rutherford concluded that most of the atom was empty space because of the large number of alpha particles that passed through the gold foil without being deviated.

The deflected particles must have hit the positive core of the atom where most of its mass was concentrated.

From our idea of electricity, positive and negative charges attract each other. If the atom was largely filled with electrons, then the positively charged alpha particle will stick to the electrons due to Coulumbic attraction. This would have been Rutherford's conclusion if the alpha particles had stuck to the atom.

batolisis batolisis · Answer 2 · 2021-11-28T12:08:02+01:00

what can be deduced about the atom's structure if α-particles had stuck to the atom is :

The atom is filled with electrons which are negatively charged

The alpha particles passed through the gold foil used in Rutherford's experiment without been deviated and Rutherford deduced that most of the atoms were empty while some particle were deviated most passed through freely.

If the alpha particles stick to the atom we can deduce that the atom is filled with electrons which are negatively charged particles and this is because in magnetism and electricity unlike poles and unlike charges attract each other while like charges repel one another.

Hence we can conclude that The atom is filled electrons which are negatively charged.

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