Rutherford's Atomic Model And Limitations MCQ - Practice Questions with Answers

Rutherford's model of atom (I)

J.J Thomson's model - J. J. Thomson, who discovered the electron in 1897, proposed the plum pudding model of the atom in 1904 before the discovery of the atomic nucleus in order to include the electron in the atomic model. In Thomson’s model, the atom is composed of electrons surrounded by a soup of positive charge to balance the electrons’ negative charges, like negatively charged “plums” surrounded by positively charged “pudding”. 

The Rutherford Model (Gold Foil Experiment ) : 

Rutherford and his collegues Geiger and Marsden  bombarded a thin gold foil of thickness approximately $8.6\times {10}^{-6}\mathrm{cm}$ with a beam of alpha particles in vacuum. They used gold since it is highly malleable, producing sheets that can be only a few atoms thick, thereby ensuring smooth passage of the alpha particles. A circular screen coated with zinc sulphide surrounded the foil. Since the positively charged alpha particles possess mass and move very fast, it was hypothesized that they would penetrate the thin gold foil and land themselves on the screen, producing fluoro-scence in the part they struck.

In line with the plum pudding model, since the positive charge of atoms was evenly distributed and too small as compared to that of the alpha particles, the deflection of the particulate matter, if any, was predicted to be less than a small fraction of a degree.

Observations : 

•  Most of the alpha particles behaved as expected, there was a noticeable fraction of particles that got scattered by angles greater than 90 degrees.
• In fact, there were about 1 in every 2000 particles that got scattered by a full 180 degree, that is, they simply retraced their path after hitting the gold foil.

Conclusion:  A highly concentrated positive charge at the center of an atom that caused an electrostatic repulsion of the particles strong enough to bounce them back to their source. The particles that got deflected by huge angles passed close to the said concentrated mass. Most of the particles passed undeviated as there was no obstruction to their path, proving that the majority of an atom is empty.  Rutherford drew the conclusion that since the dense alpha particles could be deflected by the central core, it shows that almost the entire mass of the atom is concentrated there. Rutherford named it the “nucleaus” after performing the experiment in various gases.

Rutherford's model of atom (II) 

Distance of closest approach :  

The minimum distance from the nucleus up to which the $\alpha$ - particle approach, is called the distance of closest approach $\left(r_0\right)$. At this distance the entire initial kinetic energy has been converted into potential energy so

$$\frac{1}{2}m{v}^2=\frac{1}{4\pi {\epsilon }_0}\cdot \frac{(Ze)2e}{r_0}$$

$$r_0=\frac{Z{e}^2}{m{v}^2\pi {\epsilon }_0}=\frac{4kZ{e}^2}{m{v}^2}$$
 

Impact parameter:  It is defined as the perpendicular distance of the velocity of the alpha-particle from the centre of the nucleaus, when it is far away from the atom. The shape of the trajectory of the scattered alpha-particle depends on the impact parameter 'b' and the nature of the potential field. Rutherford deduced the following relationship between the impact parameter 'b' and the

scattering angle $\theta$. It is given as

$$\begin{array}{rl}b& =\frac{Z{e}^2\cot (\theta /2)}{4\pi {\epsilon }_0\left(\frac{1}{2}m{v}^2\right)}\\ \Rightarrow b& \propto \cot (\theta /2)\end{array}$$
 

Conclusion and drawback of Rutherford model:

Conclusion:  

1. A highly concentrated positive charge at the center of an atom that caused an electrostatic repulsion of the particles strong enough to bounce them back to their source.
2. The particles that got deflected by huge angles passed close to the said concentrated mass ( nearly 99.95 % ). Most of the particles passed undeviated as there was no obstruction to their path, proving that the majority of an atom is empty. 
3.  Rutherford drew the conclusion that since the dense alpha particles could be deflected by the central core, it shows that almost the entire mass of the atom is concentrated there. Rutherford named it the “nucleaus” after performing the experiment in various gases.

Limitations of Rutherford model: 

1. It could not explain stability of an atom because this model does not obey Maxwell law of electrodynamics. According to Maxwell electron should continuous emit radiation and thus and gradually lose energy , so its distance from nucleaus should become shorter and finally it should fall into the nucleus. 
2. It could not explain line spectra of atom. According to this model the spectrum of atom must be continuous whereas practically it is a line spectrum. 
3. It did not explain the distribution of electrons outside the nucleaus.