Explain: "Rutherford's atomic model cannot explain the stability of an atom."
(N/A) Rutherford's nuclear model of an atom is analogous to a solar system where the nucleus acts as the sun and electrons act as planets.
According to classical electromagnetic theory,any charged particle moving in a circular orbit undergoes acceleration due to the continuous change in the direction of its velocity.
Maxwell's electromagnetic theory states that an accelerated charged particle must emit electromagnetic radiation.
As the electron emits radiation,it loses energy,causing its orbit to shrink continuously.
Calculations suggest that the electron should spiral into the nucleus within approximately $10^{-8} \ s$.
However,atoms are known to be stable,and electrons do not collapse into the nucleus.
Therefore,Rutherford's model fails to explain the stability of an atom.
According to classical electromagnetic theory,any charged particle moving in a circular orbit undergoes acceleration due to the continuous change in the direction of its velocity.
Maxwell's electromagnetic theory states that an accelerated charged particle must emit electromagnetic radiation.
As the electron emits radiation,it loses energy,causing its orbit to shrink continuously.
Calculations suggest that the electron should spiral into the nucleus within approximately $10^{-8} \ s$.
However,atoms are known to be stable,and electrons do not collapse into the nucleus.
Therefore,Rutherford's model fails to explain the stability of an atom.
Explore More
Similar Questions
What is the potential energy of the electron in the $L$ shell of the hydrogen atom? (in $eV$)
Medium
View SolutionSupposing the energy (in arbitrary units) of the energy levels in the hydrogen atom is given as under:
Energy level $K$ $(n=1)$ $L$ $(n=2)$ $M$ $(n=3)$ $N$ $(n=4...n=\infty)$ Energy $-864 \ a.u.$ $-216 \ a.u.$ $-96 \ a.u.$ $0 \ a.u.$
The excitation energy needed to raise the electron from $M$ level to $n = \infty$ would be:
| Energy level | $K$ $(n=1)$ | $L$ $(n=2)$ | $M$ $(n=3)$ | $N$ $(n=4...n=\infty)$ |
| Energy | $-864 \ a.u.$ | $-216 \ a.u.$ | $-96 \ a.u.$ | $0 \ a.u.$ |
The excitation energy needed to raise the electron from $M$ level to $n = \infty$ would be:
Medium
View SolutionThe series limit for the Balmer series of $H$ atom spectra is:
Easy
View SolutionIf the shortest wavelength of the hydrogen atom in the Lyman series is $x$, then the longest wavelength in the Balmer series of $He^+$ is:
DifficultJEE MAIN 2026
View SolutionFind the energy of $1$ mole of photons having a frequency of $5 \times 10^{10} \ s^{-1}$. $(h = 6.62 \times 10^{-34} \ J \ s)$
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo