Explain how the lines seen in the spectroscope relate to the position of electrons in the metal atoms.?

Answer 1

Every line in the emission spectrum of any atom (not just metals) represents the energy difference between two energy levels between which an electron has moved. The energy levels are characteristic of the element, so the spectrum lines can be used to uniquely identify it. In order to emit a photon of some particular wavelength, an electron must have been knocked out of its original orbital into a higher energy orbital by some event: absorption of a photon, impact of another electron in an electric arc, or other cause. Presently the electron will fall (in one or more steps) back to its original level, emitting photon(s) as it does so.

Answer 2

Electron falling from higher energy levels to the 1 st energy shell produces ultaviolet light...those falling to the 2nd energy level produces visible light.....Higher levels produce infrared light.