A singly ionized Helium atom emits a photon of wavelength 164 nm. If the final state of the electron is n=3, what was the initial state?

The first line in the Lyman series has wavelength $\lambda$. The wavelength of the first line in Balmer series is

Which of the following is true for number of spectral lines in going from Lyman series to $P$-fund series

The shortest wavelength in the Lyman series of hydrogen spectrum is 912\mathop {\rm{A}}\limits^ \circ   corresponding to a photon energy of $13.6\,\,eV$. The shortest wavelength in the Balmer series is about

The largest wavelength in the ultraviolet region of the hydrogen spectrum is ${\rm{122 }}\,{\rm{nm}}$. The smallest wavelength in the infrared region of the hydrogen spectrum (to the nearest integer is)

In Bohr’s model of hydrogen atom, which of the following represents the variation of nth orbit radius with n?

The ratio of the wavelengths of the first line of the Lyman series and the first line of the Balmer series in the hydrogen spectrum is:

An Electron is revolving around nucleus of charge Ze, if 40.8 eV of energy needed to excite an electron from n=1 to n=2 state. What is value of Z?

Which of the following is NOT a characteristic of line spectra of atoms?

If $R$ is the Rydberg’s constant for hydrogen the wave number of the first line in the Lyman series will be

The wavelength of radiation emitted is ${\lambda _0}$ when an electron jumps from the third to second orbit of hydrogen atom. For the electron jump from fourth to the second orbit of the hydrogen atom, the wavelength of radiation emitted will be