(a.) The figure below representing the lowest energy levels of the electron in the hydrogen atom, gives the principal quantum number n associated with each, and the corresponding value of the energy, measured in joules. (i.) Calculate the wavelength of the lines arising from the transitions márk A, B, C, D on the figure. (ii.) Show that the other transitions that can occur give rise to lines which are in either the ultraviolet or the infrared regions of the spectrum. (iii.) The level n = 1 is the ground state of the excited hydrogen atom. Explain why hydrogen in its ground state is quite transparent to light emitted by the transition A, B, C, D and also what happens when 21.7 × 10-19 J of energy is supplied to a hydrogen atom in its ground state

(a.) The figure below representing the lowest energy levels of the electron in the hydrogen atom, gives the principal quantum number n associated with each, and the corresponding value of the energy, measured in joules.

(i.) Calculate the wavelength of the lines arising from the transitions márk A, B, C, D on the figure.
(ii.) Show that the other transitions that can occur give rise to lines which are in either the ultraviolet or the infrared regions of the spectrum.
(iii.) The level n = 1 is the ground state of the excited hydrogen atom. Explain why hydrogen in its ground state is quite transparent to light emitted by the transition A, B, C, D and also what happens when 21.7 × 10^-19 J of energy is supplied to a hydrogen atom in its ground state.