Rutherford’s accelerating electrons should radiate energy and collapse into the nucleus, causing atomic instability. Bohr resolved this by proposing that electrons revolve in discrete non-radiating orbits called stationary states, preventing atomic collapse.
Both Rutherford’s and Bohr’s models have electrons orbiting the nucleus. Why did Rutherford’s model fail to explain atomic stability, while Bohr’s model succeeded?
Share
According to classical physics, an electron in Rutherford’s model accelerates along a curved path and must continuously radiate energy, spiraling inward until it crashes into the nucleus. Bohr succeeded because he proposed that electrons revolve exclusively within discrete, fixed orbits termed stationary states or energy levels. Moving within these specific allowed shells, an electron does not emit radiation, ensuring complete atomic stability.
For more NCERT Solutions of Class 9 Science Exploration Chapter 8 Journey Inside the Atom Question Answer (2026-27)
https://www.tiwariacademy.com/ncert-solutions/class-9/science/exploration-chapter-8/