![]() ![]() This model could not explain atomic stability. Limitation & drawback of Rutherford Model ![]() This model is used for determining the closest distance of approach between positively charged particles and stationary nucleus. Nucleus are positively charged & placed at the center of atom were conformed. Read also: Bohr's atomic model Success of Rutherford Atomic Model The highly dense region with positive charge were called nucleus.Since a very few of these particles are deflected back to its source, he concluded that small highly dense concentrated region exists at the center of atom. A very few α-particles were deflected back towards the source.Deflection of few particles at angle less than 90? concluded that negative(-ve) charge particles are revolving around the circular path, known as electrons.Majority of α-particles passed straight through the gold foil, Rutherford concluded that large part of an atom is empty or hollow.A very few alpha(α) particles turned back towards the source after striking the foil i.e.A few α-particles striking the gold foil were deflected through certain angles i.e.Rutherford observe that majority of α-particles passed straight through the foil without deviation.With the help of microscope, fluorescent screens were studied. The fluorescent screens were adjusted in such a way that deviated rays falls on it. On hitting the foil, alpha particles were deviated in different directions. The α-particles emitting from radioactive source were allowed to passed through the slit of the lead screen which hits the thin gold foil. Radium was placed in a lead shield with a small opening to prevent from radiations during the experimental procedures. The source of α-particles was Radium(Ra), a radioactive substances. The fluorescent screens were used to detect the deflection of α-particles on striking the gold foil. ![]() The α-particles emitting from radioactive source were allowed to pass through a sheet of thin gold foil.
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