Question

Choose the correct option from the following options given below:

• A. In the ground state of Rutherford's model electrons are in stable equilibrium. While in Thomson's model electrons always experience a net force.
• B. An atom has a nearly continuous mass distribution in Rutherford's model but has a highly non uniform mass distribution in Thomson's model.
• C. A classical atom based on Rutherford's model is doomed to collapse.
• D. The positively charged part of the atom possesses most of the mass in Rutherford's model but not in Thomson's model.

Hint:

Rutherford's model assumes electrons in stable orbits, but classical electrodynamics predicts the electron will lose energy and spiral inward, making the atom unstable. This led to the development of Bohr's model, where electrons exist in quantized orbits to avoid collapse.

Answer 1

The Correct Option is C

Step 1: Understanding Rutherford's Model 
In Rutherford's model, electrons revolve around the positively charged nucleus, but this system is unstable. Due to the continuous acceleration of electrons, electromagnetic radiation is emitted, causing the electrons to spiral inward, leading to collapse. 
Step 2: Understanding Thomson's Model 
In Thomson's model, the electrons are embedded in a uniform positive charge distribution (often referred to as the "plum pudding model"). This model assumes the atom as electrically neutral and stable without the collapsing problem seen in Rutherford’s model. 
Step 3: The Correct Answer 
Option (c) is correct because, according to classical electrodynamics, an electron moving in a circular orbit under the influence of Coulomb force would continuously radiate energy and spiral inward, leading to the atom's collapse. This is the key flaw in Rutherford’s model. 
Final Answer: A classical atom based on Rutherford's model is doomed to collapse.