If the electron jumps from $7.00 \ eV$ energy level to $5.0 \ eV$ energy level,it :

The ionization energy of a $H$ atom is $13.6 \, eV$. The energy required to excite the electron from the ground state $(n=1)$ to the first excited state $(n=2)$ is ... $eV$.

The radius ratio of Bohr's first orbit of hydrogen-like species $He^{+}$,$Li^{2+}$,and $Be^{3+}$ is:

Which of the following statements is $NOT$ true about the $Bohr$ atomic model?

Which transition in the hydrogen spectrum would have the same wavelength as the Balmer type transition from $n = 4$ to $n = 2$ of $He^+$ spectrum?

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.