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: Analysis of Rutherford's Atomic Model
Rutherford's model posits electrons orbiting a positive nucleus. However, this configuration is inherently unstable. Continuous electron acceleration results in the emission of electromagnetic radiation, causing electrons to spiral inwards and leading to atomic collapse.
Step 2: Analysis of Thomson's Atomic Model 
Thomson's model describes electrons embedded within a homogeneous distribution of positive charge, commonly known as the "plum pudding model." This model posits atomic electrical neutrality and stability, avoiding the collapse issue observed in Rutherford's model. 
Step 3: Determination of the Correct Option 
Option (c) is accurate. Classical electrodynamics dictates that an electron in circular orbit, under Coulombic attraction, would continuously emit energy and spiral inward, causing atomic collapse. This represents the fundamental deficiency in Rutherford's model. 
Conclusion: A classical atom structured according to Rutherford's model is inherently unstable and destined to collapse.