Explain how the existence of electron energy levels in atoms give rise to line spectra, which may be emission?

Question

Explain how the existence of electron energy levels in atoms give rise to line spectra, which may be emission or absorption spectra?

Why is there dark lines in the spectrum?

Please explain the difference between absorption, emission and continuous spectrum.

What leads to continuous and line spectra?

Answer 1

Because of the energy levels having definite energies, transitions from one to another are always the same energy. This means there are some energies that there are no transitions corresponding to them, thus there are colors that are not possible to emit from a given element. Keep in mind that the element can absorb or emit these definite energies--so when a continuous spectrum--that's ALL colors passes through a given gas, ONLY these energies are absorbed, thus there are black bands which correspond exactly to the emission spectra . . . the absorbtion and emmission spectra are identical, except for the first you are absorbing the given colors and in the second emitting the colors. Continuous spectra usually come from hot things, black body radiation, whereas line spectra come from the electron energy transitions already discussed.

Answer 2

whilst the atoms of the pattern a heated they benefit ability and shift from floor state to existed state. in this state they are risky and that they fall returned to their preliminary state wth emmision of sunshine of distinctive frequencies. because of the fact those electrons are of distinctive atoms they dont posses the comparable floor state ability and neither do they after absorption of ability. this suggests that they dont bring about one very final ability point as a result they emit easy of distinctive frequencies, its this distinction in emmision that evidences the version in ability point ability as a result proving the existence of ability stages in atoms