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

According to Bohr theory, the electronic energy of a hydrogen atom in the ${\mathrm{n}}^{\mathrm{th}}$ Bohr atom is given by ${\mathrm{E}}_{\mathrm{n}}=\frac{21.76\times {10}^{-19}}{{\mathrm{n}}^2}\mathrm{J}$. Calculate the longest wavelength of light that will be needed to remove and electron from the third Bohr orbit of the ${\mathrm{He}}^{+}$ ion (If the wavelength is $x\times {10}^{-7}$(in meter) and $x$ is an integer. Report '$x$')

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?

The excited state is the most stable state for an electron in an atom.

What do you mean by excited state in an atom?

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?