Question

At one time, it was thought that positive charge was spread throughout the atom. This was the plum-pudding model. Rutherford's experiment to test this theory involved shooting positively charged particles toward the atom. Describe what the results of this experiment would have been if the plum-pudding model were correct.

Answer 1

The 2 positively charged particles would repel each other.

Answer 2

1) All the alpha particles must have deviated at some angle from their initial path.

2) None of the alpha particle will go out undeviating

Step-by-step explanation:

In Rutherford's experiment he bombarded alpha particles on the nucleus of gold atom and then he observed that most of the alpha particles moves out undeviating while few of them shows small deflection.

But the most shocking part of experiment was that he saw that one out of 10,000 alpha particles are such which retrace their initial path i.e. those alpha particles are deviated nearly 180 degree angle.

Now these all observations will concluded as

1. Most of the part of atom is vacant and hence atom is not made up of positively charged.

2. Electrons revolves around the nucleus in circular orbits

3. The positive charge of the nucleus is concentrated at the nucleus of of atom which is a very small and dense volume of atom.

So these results are totally opposite of plum pudding model because as per plum pudding model the atom is a positively charged sphere and electrons are randomly placed in it.

If this model is assumed to be correct then in that case the observations must be like following

1) All the alpha particles must have deviated at some angle from their initial path.

2) None of the alpha particle will go out undeviating