The energy of an electron in the $n^{\text{th}}$ Bohr orbit of an $H$-atom is given by:
- A$\frac{-13.6}{n^2} \text{ eV}$
- B$\frac{-13.6}{n} \text{ eV}$
- C$\frac{-13.6}{n^4} \text{ eV}$
- D$\frac{-13.6}{n^3} \text{ eV}$
Explore More
Similar Questions
The ratio of energy of a hydrogen atom for the first and second excited states is ......
Medium
View SolutionIn which orbit of the Bohr model of the hydrogen atom is the speed of the electron maximum?
Easy
View SolutionThe ionization energy of $He^+$ is $19.6 \times 10^{-18} \ J \ atom^{-1}$. What is the energy of the first stationary state $(n = 1)$ of $Li^{2+}$?
Medium
View Solution$A$ single-electron species has a nuclear charge of $+Ze$,where $Z$ is a constant. The energy required to excite an electron from the $2^{nd}$ Bohr orbit to the $3^{rd}$ Bohr orbit is $47.2 \ eV$. Calculate the value of $Z$.
Medium
View SolutionWhich of the following electronic transitions in a hydrogen atom will require the largest amount of energy?
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