Question:

A particle of mass $m$ moves in circular orbits with potential energy $V(r)= Fr$, where $F$ is a positive constant and $r$ is its distance from the origin. Its energies are calculated using the Bohr model. If the radius of the particle's orbit is denoted by $R$ and its speed and energy are denoted by $v$ and $E$, respectively, then for the $n ^{\text {th }}$ orbit (here $h$ is the Planck's constant)

Updated On: Jul 13, 2024
  • $R \propto n ^{\frac{1 }{ 3}}$ and $v \propto n ^{\frac{2 }{ 3}}$

  • $R \propto n ^{\frac{2 }{ 3}}$ and $v \propto n ^{\frac{1 }{ 3}}$

  • $E=\frac{3}{2}\left(\frac{n^{2} h^{2} F^{2}}{4 \pi^{2} m}\right)^{\frac{1 }{ 3}}$

  • $E=2\left(\frac{n^{2} h^{2} F^{2}}{4 \pi^{2} m}\right)^{\frac{1 }{3}}$
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The Correct Option is B, C

Solution and Explanation

The Correct Option is (B) and(C):

$R \propto n ^{\frac{2 }{ 3}}$ and $v \propto n ^{\frac{1 }{ 3}}$
 \(E=\frac{3}{2}\left(\frac{n^{2} h^{2} F^{2}}{4 \pi^{2} m}\right)^{\frac{1 }{ 3}}\)

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Concepts Used:

Atomic Spectra

The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation emitted due to an electron making a transition from a high energy state to a lower energy state. The photon energy of the emitted photon is equal to the energy difference between the two states.

Read More: Atomic Spectra

Spectral Series of Hydrogen Atom

Rydberg Formula:

The Rydberg formula is the mathematical formula to compute the wavelength of light.

\[\frac{1}{\lambda} = RZ^2(\frac{1}{n_1^2}-\frac{1}{n_2^2})\]

Where,

R is the Rydberg constant (1.09737*107 m-1)

Z is the atomic number

n is the upper energy level

n’ is the lower energy level

λ is the wavelength of light

Spectral series of single-electron atoms like hydrogen have Z = 1.

Uses of Atomic Spectroscopy:

  • It is used for identifying the spectral lines of materials used in metallurgy.
  • It is used in pharmaceutical industries to find the traces of materials used.
  • It can be used to study multidimensional elements.