Bohrs Model#!#Wavelength of energy emiited upon transition to lower energy level #!#Practice Problems

Bohr Model Practice

An electron in hydrogen atom is in the n=4 energy level. When it makes a transition to some lower energy level, to which series the wavelength of emitted photon belong?

An electron in an excited hydrogen atom acquired an energy of 12.1 eV. To what energy level did it jump? How many spectral lines may be emitted in the course of the transition to lower energy level? Calculate the corresponding wavelengths.

Bohr's Model(energy of electron in an orbit)

Bohr Model (Practice)

Question on Bohr model||Debrogile concept||Problems

The wavelength of radiation emitted due to transition of electron from energy level E to zero is equal to lamda . The wavelength of radiation (lamda_(1)) emitted when electronjumpsfrom energy level (3E)/(2) to zero will be :

Bohr's Model(Energy Level of H atoms)

If nuclecus in an excited state fall to a lower energy level, energy is emitted as :