Bohr's Atomic Model and its Limitations

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  $0.53 \mathrm{\AA }.$  What is the radius of  ${\mathrm{Li}}^{2+}$  ion (Atomic number $=3$) in a similar state?

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

Zeeman and Stark effects can be explained by _________________.

Stark and Zeeman effects can be explained by _________________.

The theoretical and experimental values of Rydberg constant are different.

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 ${\mathrm{He}}^{+}$?

Why the theoretical and experimental values of Rydberg constant are different?

The velocity of the electron in the third orbit of hydrogen atom will be

The velocity of electron in first orbit of $\mathrm{H}$-atoms as compared to the velocity of light is $\frac{1}{100}\mathrm{th}$.

The velocity of electron in first orbit of $\mathrm{H}$-atoms as compared to the velocity of light is

Calculate velocity of electron in first Bohr orbit of hydrogen atom $($Given, $\mathrm{r}={\mathrm{a}}_0)$.

Which of the following is not a hydrogen like species?

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 formula is used for calculating effective nuclear charge?