H- atoms in ground state (13.6eV) are excited by monochromatic radiations of photon of energy 12.1eV. Find the number of spectral lines emitted in H-atom.

Ionisation potential of hydrogen atom is 13.6 eV. Hydrogen atom in ground state is excited by monochromatic light of energy 12.1 eV. The spectral lines emitted by hydrogen according to Bohr's theory will be-

Ionisation potential of hydrogen atom is 13.6 eV. Hydrogen atom is ground state is excited by monochromatic light of energy 12.1 eV. The spectral lines emitted by hydrogen according to bohr's theory will be-

Hydrogen atom in ground state is excited by a monochromatic radiation of lambda=975"Å" . Number of spectral lines in the resulting spectrum emitted will be

Hydrogen atoms in the ground state are excited by means of radiation of wavelength 1026 Å. Find out the wavelength of radiation that this excited atoms can emit when they come back to ground state. Given, h=6.625xx10^(-34)J*s,c=3xx10^(8)m*s^(-1), 1 eV =1.6xx10^(-19)J ionisation energy of hydrogen = 13.62 eV.

Hydrogen atom in its ground state, is excited by means of monochromatic radiation of wavelength 975 Å . How many different lines are possible in the resulting spectrum ? Calculate the longest wavelength amongst them. Given, ionisation energy of hydrogen atom is 13.6 eV.

A hydrogen atom in the ground state is excited by monochromatic radiation of wavelength lambda overset@ . The resulting spectrum consists of maximum 15 different lines. What is the wavelength lamda ?

The ionisation potential of hydrogen atom is 13.6 eV . An electron in the ground state of hydrogen atom absorbs a photon of energy 12.75 eV. How many different spectral lines can one expect when the electron makes a downward transition ?

The ground state energy of hydrogen atom is -13.6 eV . If an electron makes a transition from an energy level -0.85 eV to -3.4 eV, calculate the wavelength of the spectral line emitted . To which series of hydrogen spectrum does this wavelength belong ?

The ground state energy of hydrogen atom is -13.6 eV . If an electron makes a transition from an energy level -1.51 eV to -3.4 eV, calculate the wavelength of the spectrum line emitted and name the series of hydrogen spectrum to which it belongs.

The electron in a hydrogen atom has been excited to the n -th state. What is the maximum number of spectral lines that may be emitted by the atom when the electron transits to the ground state ?