When an electron drops from a higher energy level to a low energy level, then

According to Bohr.s theory, when ever the electron drops from a higher energy level to a lower energy level, the frequency of radiation emitted is related to the energy change as

According to Bohr.s theory, when ever the electron drops from a higher energy level to a lower energy level, the frequency of radiation emitted is related to the energy change as

Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" The energy required to promote the ground state electron of H-atom to the first excited state is: When an electron returns from a higher energy level to a lower energy level, energy is given out in the form of UV//Visible radiation.

Assertion : Energy is released in the form of light, when electron drops from a higher energy level to lower energy level Reason : A spectral lines can be seen for 3d_(z)^(2)" to "3dx^(2)-y^(2) transition

When electron transist from higher energy level to lower energy level then …..

When an electron falls from a higher energy to a lower energy level, the difference in the energies appears in the forms of electromagnetic radiation. Why cannot it be emitted as other forms of energy?

When an electron falls from a higher energy to a lower energy level, the difference in the energies appears in the forms of electromagnetic radiation. Why cannot it be emitted as other forms of energy?