Work required to pull an electron from helium atom is 40 eV. Then the work required to pull both the electrons from the helium atom is

Which of the following statements is INCORRECT regarding the absorption spectrum of hydrogen?

(A) It consists of dark lines against a continuous background.

(B) The lines correspond to photons absorbed by the electron transitioning to higher energy levels.

(C) The wavelengths of the absorbed photons are identical to the wavelengths of the emitted photons in the emission spectrum.

(D) The absorption spectrum can be used to identify the presence of hydrogen in a sample.

Electron in hydrogen atom first jumps from third excited state to second excited state and then from second excited to the first excited state. The ratio of the wavelengths ${\lambda _1}:{\lambda _2}$ emitted in the two cases is

In a hydrogen atom, if $\lambda_B$ represents the wavelength of the last line of the Balmer series and $\lambda_L$ represents the wavelength of the last line of the Lyman series, then $\lambda_B$ is how many times $\lambda_L$?

Imagine an atom made up of a proton and a hypothetical particle of double the mass of the electron but having the same charge as the electron. Apply the Bohr’s atom model and consider all possible transitions of this hypothetical particle to the first excited level. The longest wavelength photon that will be emitted has wavelength $\lambda$ (given in terms of the Rydberg constant $R$ for the hydrogen atom) is equal to

If ${\lambda _{\max }}$ is $6563\,\,{A^0}$, then wavelength of second line for Balmer series will be

Maximum wavelength in Balmer series of hydrogen spectrum is (R : Rydberg constant)

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)

The energy of the highest energy photon of Balmer series of hydrogen spectrum is close to

Why does the emission spectrum of an element provide insights into its atomic structure?

Electrons in a certain energy level $n = {n_1}$, can emit ${\rm{3}}\,{\rm{ spectral}}\,{\rm{ lines}}$. When they are in another energy level, $n = {n_2}$. They can emit ${\rm{6}}\,{\rm{ spectral}}\,{\rm{ lines}}$. The orbital speed of the electrons in the two orbits are in the ratio