Bohr's Model for the Hydrogen Atom

According to the Bohr Theory, among the following, which transition in the hydrogen atom will give rise to the least energetic photon?

The energy of the second Bohr orbit of the hydrogen atom is $-328 \mathrm{kJ} {\mathrm{mol}}^{-1}$. Hence, the energy of the fourth Bohr orbit would be

The Bohr orbit radius for the hydrogen atom (n = 1) is approximately  $0.530\AA .$  The radius for the first excited state (n = 2) orbit is  $(in\AA )$

The radius of hydrogen atom in the ground state is  $0.53\mathrm{\AA }.$  The radius of  ${\mathrm{Li}}^{2+}$ ion (Atomic number = $3$) in first orbit is

Among the  ${\mathrm{He}}^{+}$ ion with an electron in an orbit with $\mathrm{n}=3$ and a${\mathrm{Li}}^{+2}$ ion with an electron in an orbit with $\mathrm{n}=5$, the largest ion is

Calculate the possible change in angular momentum of an electron in Balmer transition inside a hydrogen atom.

Which of the following species have the same energy as that of the first Bohr's orbit of the hydrogen atom?

In the Balmer series of atomic spectra of hydrogen, there is spectral line having wavelength $434.4 \mathrm{nm}$. Calculate the number of higher orbit from which the electron drops to generate this line. $\left(\mathrm{R}=10.97\times {10}^6 {\mathrm{m}}^{-1}\right)$

${\mathrm{E}}_{\mathrm{n}} = -\frac{313.6}{{\mathrm{n}}^2}$, if the value of ${\mathrm{E}}_1 = -34.84$ to which value $\text{'}\mathrm{n}\text{'}$ corresponds?

If the series limit to the wavelength of the Lyman series of the hydrogen atom is $912 \mathrm{\AA }$, then the series limit to the wavelength for the Balmer series of the hydrogen atom is

In a hydrogen atom, if the energy of an electron in the ground state is  $\text{–13.6 eV}$, then that in the $\text{2nd}$ excited state is

Which of the following is the correct value of most probable radius for locating the electron in ${\mathrm{He}}^{+}$?

Which of the following is not a hydrogen like species?

Assertion : The spectrum of ${\mathrm{He}}^{+}$ is expected to be similar to that of hydrogen.

Reason : ${\mathrm{He}}^{+}$ is also one electron system.

An energy of $40.8 \mathrm{eV}$ is required to excite a Hydrogen-like species from $1^{\mathrm{st} }$ Bohr orbit to second. Which is/are correct statement(s):

Which of the following is the value of the Rydberg constant for hydrogen?

Among the following, which transition in the Hydrogen spectrum would have the same wavelength as Balmer transition, $\mathrm{n}=4$ to $\mathrm{n}=2$ in ${\mathrm{He}}^{+}$ spectrum?

If the wavelength of the first line in Balmer series is $656 \mathrm{nm}$, then the wavelengths of its second line and limiting line respectively are