(A) In Bohr's atomic model,the radius of the $n^{th}$ orbit is given by $r_n = \frac{n^2 h^2 \epsilon_0}{\pi m Z e^2}$,which implies $r \propto n^2$.

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$E \propto -1/n^2, r \propto n^2$

(A) In Bohr's atomic model,the radius of the $n^{th}$ orbit is given by $r_n = \frac{n^2 h^2 \epsilon_0}{\pi m Z e^2}$,which implies $r \propto n^2$. The total energy of an electron in the $n^{th}$ orbit is $E_n = -\frac{m Z^2 e^4}{8 \epsilon_0^2 h^2 n^2}$,which implies $E \propto -1/n^2$. Considering the magnitude of energy,the relationship is $r \propto n^2$ and $E \propto 1/n^2$.

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

Medium

In Bohr's atomic model,the radius $(r)$ and energy $(E)$ of an orbit $(n)$ are related as:

A
$E \propto -1/n^2, r \propto n^2$
B
$r \propto 1/n^2, E \propto n^2$
C
$r \propto 1/n, E \propto n$
D
$r \propto n^2, E \propto 1/n^2$

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Class 11

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Structure of Atom

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Atomic models and Planck's quantum theory

The figure shows six spectral lines in an emission spectrum arising from energy level transitions. Which of the following spectral lines does not appear in the absorption spectrum?

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The $Bohr$ model of an atom could not account for:

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Which of the following statements is $NOT$ correct regarding the Bohr model?

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Calculate the energy required for the process $He_{(g)}^{+} \rightarrow He_{(g)}^{2+} + e^{-}$. The ionization energy for the $H$ atom in the ground state is $2.18 \times 10^{-18} \, J \, atom^{-1}$.

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When the electron passes from the energy state nearest to the nucleus to the third energy level,it will:

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In Bohr's atomic model,the radius $(r)$ and energy $(E)$ of an orbit $(n)$ are related as:

Similar Questions

The figure shows six spectral lines in an emission spectrum arising from energy level transitions. Which of the following spectral lines does not appear in the absorption spectrum?

The $Bohr$ model of an atom could not account for:

Which of the following statements is $NOT$ correct regarding the Bohr model?

Calculate the energy required for the process $He_{(g)}^{+} \rightarrow He_{(g)}^{2+} + e^{-}$. The ionization energy for the $H$ atom in the ground state is $2.18 \times 10^{-18} \, J \, atom^{-1}$.

When the electron passes from the energy state nearest to the nucleus to the third energy level,it will:

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