# How can I interpret the colour of flames in terms of spectral series?

I saw different colors of fire burning different metals. But how does this work? The Balmer series requires electrons to drop back down to n = 2. But, not all alkali metals have empty space in their second principle energy level. Does one electron, from the second principle energy level, just jump to somewhere of energy and come back down.

My description is kinda confusing, but all I'm saying is, where does that space in the second energy level come from?

But if you are speaking about the Hydrogen, for instance you also have the Paschen serie for electron down to the $n = 3$ level.
So it's the same for other elements, there is no special need for an electron to jump down on the precise level $n = 2$ to produce a photon within the visible spectra during its desexcitation.
• Well, I don't know about Pache serie. But it's true that Paschen Serie does not, althought it was just to illustrate the fact an electron has no vital need to jump down to the $n = 2$ energy level to produce a photon during the desexcitation. Dec 4 '14 at 12:25