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

Energy of an electron in the nth orbit hydrogen atom is given by E_n = - (13.6)/(n^2) eV How much energy is required to take an electron from the ground state to the first excited state?

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 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 remove an electron in the n = 2 state of the hydrogen atom is

The energy of an electron in the nth orbit of hydrogen atom is (-13.6 eV)/n^2) . The energy required to raise an electron form the 1st Bohr orbit to the 2nd orbit in eV is