As far as I've understood, the color of an object depends on which wavelenghts from the more or less "white" sun light it reflects and absorbs.
I think that an atom can only absorb the light that has exactly the right wavelenght to exite an electron to a higher energy level. All light that doesn't is reflected and determines the color of the atom (or, more precisely, of a very big group of atoms as individual ones are way to small to be seen by the naked eye).
Is this right? And how does it compare to emission lines which are basically the wavelenghts being absorbed and then re-emitted? Wouldn't it be kind of the same thing?
However, that doesn't make a lot of sense since oxygen, for example is invisible but has emission lines in the visible spectrum.
Thanks in advance