Hydrogen Spectrum

The ground state energy of the hydrogen atom is $–13.6 \mathrm{eV}$ . The kinetic and potential energies of electrons in this state are:

For a hydrogen atom the value of ionization energy is equal to:

A potential difference of $20 \mathrm{kV}$ is applied across an X-ray tube. The minimum wavelength of X-rays generated is

An electron in a hydrogen atom in its ground state absorbs energy equal to the ionisation energy of ${\mathrm{Li}}^{+2}$ . Calculate the wavelength of the emitted electron.

Which one of the following statements about $X$-rays is not true?

The minimum energy of an incident electron necessary for ionization of atom of hydrogen is equal to $W_0$. Find minimum initial energy $W (= a{W}_0)$ of singly ionized incident helium atom, necessary for ionization of stationary hydrogen atom.

In hydrogen spectrum, the shortest wavelength in the Balmer series is$\lambda$. The shortest wavelength in the Brackett series is :

The ratio of wavelength of spectral lines ${\mathrm{H}}_{\alpha }$ and ${\mathrm{H}}_{\beta }$ in the Balmer series is $\frac{x}{20}$. The value of $x$ is _____.

If $917 \mathrm{\AA }$  be the lowest wavelength of Lyman series then the lowest wavelength of Balmer series will be $\mathrm{\AA }$.

In a sample of hydrogen like atoms all of which are in ground state, a photon beam containing photons of various energies is passed. In absorption spectrum, five dark lines are observed. The number of bright lines in the emission spectrum will be (Assume that all transitions take place)
 

A glass container contains hydrogen atoms with all its atoms in their ground states. The container is irradiated with electromagnetic waves containing wavelengths corresponding to Lyman, Balmer and Paschen series. The electromagnetic waves exiting the glass container are found to have certain strong absorption spectral lines. Identify one or more series to which these absorption spectral lines would correspond to. Explain. Assume that once an electron absorbs a photon and jumps to a higher level, it does not absorb more photons to jump to even higher levels.

By what factor does kinetic and potential energy of an electron in a hydrogen atom change as it moves from $n=1$ to $n=3$?

Minimum wavelength of the spectral line obtained in the Paschen series in the spectrum of hydrogen atom is

The frequency of radiation emitted when the electron falls from $n=4$ to $n=1$ in a hydrogen atom will be (Given ionization energy of $H=2.18\times {10}^{18} \mathrm{J} {\mathrm{atom}}^{-1}$ and $h=6.625\times {10}^{-34}\mathrm{Js}$)
 

Which electronic transition in a hydrogen atom, starting from the orbit $n=7$, will produce infrared light of wavelength $2170\mathrm{nm}$? (Given : $R_H=1.09677\times {10}^7 {\mathrm{m}}^{-1}$)

If the series limit frequency of Balmer series is ${\nu }_{\mathrm{B}}$, then the series limit frequency of the Brackett series is

The ratio between shortest wavelength in Balmer series to shortest wavelength in Brackett series is

Energy of a stationary electron in the hydrogen atom is $E=-\frac{13.6}{n^2}\mathrm{eV}$ then the energies required to excite the electron in hydrogen atom to (a) its second excited state and (b) ionized state respectively

What are the frequency and wavelength in $\left(\mathrm{nm}\right)$ of a photon emitted during a transition from $n=5$ to $n=2$ in the Hydrogen atom.