The spectral series formed when electrons of excited hydrogen atoms return to the third orbit from higher energy orbits is

According to Bohr's model,the energy of an electron is given by $E = -\frac{2.176 \times 10^{-18}}{n^2} \, J \, atom^{-1}$. Calculate the minimum energy required to remove an electron from the $3^{rd}$ orbit of a $He^{+}$ ion,and also calculate the corresponding wavelength of the photon.

The radius of the first Bohr orbit of the hydrogen atom is the same as that of the orbit $(n)$ of a hydrogen-like species $X$. The values of $(n)$ and $X$ respectively are:

If the energy of a photon is $14 \, eV$ and it interacts with a hydrogen atom,which of the following is correct?

When an electron with energy $10.8 \,eV$ collides with a hydrogen $(H)$ atom,what will happen?

For a $H$ atom,the energy transition from $n = 1$ to $n = 2$ is $10.2 \ eV$. What will be the energy for the same transition in $Be^{3+}$ ion?