Bohr model

The radius of the second Bohr orbit for hydrogen atom is :

(Planck's Const. $h=6.6262\times10^{-34}$ Js; mass of electron $=9.1091\times10^{-31}$ kg; charge of electron $e=1.60210\times10^{-19}$ C; permittivity of vacuum $\epsilon_0=8.854185\times10^{-12}$ kg$^{-1}$m$^{-3}$A$^2$)

If the shortest wavelength in Lyman series of hydrogen atom is A, then the longest wavelength in Paschen series of $\ce{He+}$ is :

The electron in the hydrogen atom undergoes transition from higher orbitals to orbital of radius 211.6 pm. This transition is associated with :

Which of the following is the energy of a possible excited state of hydrogen ?

The energy of an electron in first Bohr orbit of H - atom is $-13.6$ eV. The energy value of electron in the excited state of $\ce{Li^2+}$ is :

Based on the equation :
$$\Delta E=-2.0\times10^{-18}\text{ J}\left(\frac1{n_2^2}-\frac1{n_1^2}\right)$$
the wavelength of the light that must be absorbed to excite hydrogen electron from level $n=1$ to level $n=2$ will be : ($h=6.625\times10^{-34}$ Js, $C=3\times10^8$ ms$^{-1}$)

If m and e are the mass and charge of the revolving electron in the orbit of radius r for hydrogen atom, the total energy of the revolving electron will be :

The kinetic energy of an electron in the second Bohr orbit of a hydrogen atom is [$a_0$ is Bohr radius]

Energy of the state $S_1$ in units of the hydrogen atom ground state energy is

The orbital angular momentum quantum number of the state $S_2$ is