Energy of an eletron in hydrogen atom is given by `E=(13.6)/n^(2)` eV. If n is changed from 1 to 4 then energy 1 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?

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

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

Energy of an electron in a hydrogen atom is calculated as E_n=(-13.6)/n^2 eV. Is it possible for an electron in hydrogen atom to have energy of 2.8 eV

The total energy of the electron in an hydrogen atom is En = -13.6/n^2 eV What is the significance of the negative sign?

The energy of electron in hydrogen atom is E_n=(-13.6)/(n^(2)) eV , Where n=1, 2,3,......Show that (i) the electron in hydrogen atom cannot have an energy of -6.8eV. (ii) spacing between the lines (consecutive energy levels) within the given set of observed hydrogen spectrum decreases as n increases.

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

Energy of electron in its nth orbit is given by (E_n=-(13.6)/n^2 xxz)ev . Consider a hydrogen atom , find the amount of energy needed to transfer electron from 1st orbit to 3rd orbit: