(D) In Bohr's model,the time period of revolution $T$ is given by the relation $T \propto \frac{n^3}{Z^2}$.For $T_{1,2}$,$n = 1$ and $Z = 2$,so $T_{1,

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(D) In Bohr's model,the time period of revolution $T$ is given by the relation $T \propto \frac{n^3}{Z^2}$.For $T_{1,2}$,$n = 1$ and $Z = 2$,so $T_{1,2} \propto \frac{1^3}{2^2} = \frac{1}{4}$.For $T_{2,1}$,$n = 2$ and $Z = 1$,so $T_{2,1} \propto \frac{2^3}{1^2} = \frac{8}{1} = 8$.Therefore,the ratio $T_{1,2} : T_{2,1} = \frac{1}{4} : 8 = 1 : 32$.

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

Medium

If in Bohr's model,for a unielectronic atom,the time period of revolution is represented as $T_{n,Z}$ where $n$ represents the shell number and $Z$ represents the atomic number,then the value of $T_{1,2} : T_{2,1}$ will be

A
$8 : 1$
B
$1 : 8$
C
$1 : 1$
D
$1 : 32$

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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 frequency of radiation emitted when the electron falls from $n = 4$ to $n = 1$ in a hydrogen atom will be (Given ionization energy of $H = 2.18 \times 10^{-18} \ J \ atom^{-1}$ and $h = 6.625 \times 10^{-34} \ Js$)

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Calculate the wavelength for the emission transition if it starts from the orbit having radius $1.3225 \, nm$ and ends at $211.6 \, pm$. Name the series to which this transition belongs and the region of the spectrum.

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Find the energy of a photon having a wavelength of $6000 \ \mathring{A}$. (Given: $h = 6.62 \times 10^{-27} \ erg \cdot s$)

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The difference in wavelength of first and second spectral lines of Lyman series in $Li^{2+}$ ion spectrum is ................ $\mathring{A}$

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If the potential energy of an electron in the second orbit of $He^+$ is $-27.2 \, eV$,then calculate the double value of the energy of the first excited state of a hydrogen atom in $eV$.

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If in Bohr's model,for a unielectronic atom,the time period of revolution is represented as $T_{n,Z}$ where $n$ represents the shell number and $Z$ represents the atomic number,then the value of $T_{1,2} : T_{2,1}$ will be

Similar Questions

The frequency of radiation emitted when the electron falls from $n = 4$ to $n = 1$ in a hydrogen atom will be (Given ionization energy of $H = 2.18 \times 10^{-18} \ J \ atom^{-1}$ and $h = 6.625 \times 10^{-34} \ Js$)

Calculate the wavelength for the emission transition if it starts from the orbit having radius $1.3225 \, nm$ and ends at $211.6 \, pm$. Name the series to which this transition belongs and the region of the spectrum.

Find the energy of a photon having a wavelength of $6000 \ \mathring{A}$. (Given: $h = 6.62 \times 10^{-27} \ erg \cdot s$)

The difference in wavelength of first and second spectral lines of Lyman series in $Li^{2+}$ ion spectrum is ................ $\mathring{A}$

If the potential energy of an electron in the second orbit of $He^+$ is $-27.2 \, eV$,then calculate the double value of the energy of the first excited state of a hydrogen atom in $eV$.

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