Bohr Model and Its Limitations

The radii of the first Bohr orbit of $\mathrm{H}\left({\mathrm{r}}_{\mathrm{H}}\right), {\mathrm{He}}^{+}\left({{\mathrm{r}}_{\mathrm{He}}}^{+}\right)$ and ${\mathrm{Li}}^{2+}\left({{\mathrm{r}}_{\mathrm{Li}}}^{2+}\right)$ are in the order

The electron in hydrogen atom is in the first Bohr orbit $\left(\mathrm{n}=1\right)$. The ratio of transition energies, $\mathrm{E}\left(\mathrm{n}=1\to \mathrm{n}=3\right)$ to $\mathrm{E}\left(\mathrm{n}=1\to \mathrm{n}=2\right)$, is:

The wavelength of a spectral line for an electronic transition is inversely proportional to:

If the value of ${\mathrm{E}}_{\mathrm{n}}=-78.4 \mathrm{k} \mathrm{cal}/\mathrm{mole},$ the order of the orbit in hydrogen atom is:

Which is the correct relationship?

According to Bohr's theory, the energy required for the transition of electron in $\mathrm{H}$-atom from $\mathrm{n}=6$ to $\mathrm{n}=8$ state is

In Bohr's orbit, what is the ratio of the total kinetic energy and the total energy of the electron?

In the hydrogen atom, the energy of the first excited state is $-3.4\mathrm{eV}$. Then, find out the $\mathrm{KE}$ of the same orbit of the hydrogen atom.

The ionisation energy of ${\mathrm{He}}^{+}$ is $19.6\times {10}^{-18} \mathrm{J}$ ${\mathrm{atom}}^{-1}$. The energy of the first stationary state $(\mathrm{n}=1)$ of ${\mathrm{Li}}^{2+}$ is

The energy of an electron in ${\mathrm{n}}^{\text{th }}$ Bohr orbit of the hydrogen atom is

The energy of an electron in the first Bohr orbit of $\mathrm{H}-$atom is $-13.6\mathrm{eV}$. The possible energy value(s) of the excited state(s) for electrons in Bohr orbits of hydrogen is (are)

In Bohr theory, if ${\mathrm{E}}_{{\mathrm{n}}^{\text{'}}}{\mathrm{K}}_{{\mathrm{n}}^{\text{'}}}{\mathrm{V}}_{\mathrm{n}}$ and ${\mathrm{r}}_{\mathrm{n}}$ denotes total energy, kinetic energy, potential energy and radius of ${\mathrm{n}}^{\mathrm{th}}$ orbit respectively, which of the following is (are) correct?

The energy of the second Bohr orbit of the hydrogen atom is $-3.41 \mathrm{eV}$. The energy of the third Bohr orbit of the ${\mathrm{He}}^{+}$ ion will be

Which hydrogen-like species will have the same radius as that of the first Bohr's orbit of the hydrogen atom?

Which is larger, an ${\mathrm{He}}^{+}$ ion with an electron in an orbit with $\mathrm{n}=3$ or a${\mathrm{Li}}^{+2}$ ion with an electron in an orbit with $\mathrm{n}=5$?

What is the ratio of the difference in energy between the first and the second Bohr's orbits to that between the second and the third Bohr's orbits for the $\mathrm{H}-$atom?

(Atomic number of $\mathrm{H}-$atom $=1$)

What is the ratio of the radii of the first three Bohr's orbits in the $\mathrm{H}-$atom? 

The energy of the second Bohr's orbit in the hydrogen atom is $-3.41 \mathrm{eV}$. What would be the energy of the second Bohr's orbit of ${\mathrm{He}}^{+}$ ion?

The ionisation potential of a hydrogen atom is $13.6 \mathrm{eV}$. What is the energy required to remove an electron in the $\mathrm{n}=2$ state of the hydrogen atom?

The electronic velocity in the fourth Bohr's orbit of hydrogen is $\mathrm{v}$. What will be the velocity of the electron in the first orbit?