An electron in the `n = 1` orbit of hydrogen atom is bound by `13.6 eV`. If a hydrogen atom I sin the `n = 3` state, how much energy is required to ionize it
An electron in the n = 1 orbit of hydrogen atom is bound by 13.6 eV energy is required to ionize it is
The ionization energy of the electron in the lowest orbit of hydrogen atom is 13.6 eV. The energies required in eV to remove an electron from three lowest energy orbits of hydrogen atom respectively are
The ionisation potential of hydrogen atom is 13.6 eV The energy required to remve as electron in the n = 2 state of the hydrogen atom is
The ionisation potential of hydrogen atom is 13.6 volt. The energy required to remove an electron in the n = 2 state of the hydrogen atom is
Assume that the charge of an electron is 1.6times10^(-19) coulomb and the energy of the first orbit of hydrogen atom is -13.6 eV. If the energy required to excite the ground state electron of hydrogen atom to the first excited state, is expressed as y times10^(-19)J per atom, what is the value of y ?
Energy of the electron in nth orbit of hydrogen atom is given by E_(n) =-(13.6)/(n^(2))eV . The amount of energy needed to transfer electron from first orbit to third orbit is
