In the case of an atom of Cesium ejecting an electron, it would lose one electron from the 6s orbital. The 6s orbital is very high in energy and similarly so would the electron that is ejected from it, right? So if there was a Nitrogen atom as well, how would it be possible that the Nitrogen accepts this electron of such high energy when its highest ground state sublevel is 2p. I would assume the electron loses energy in the transfer process but how exactly? The electron affinity in terms of enthalpy change for Nitrogen is positive, so I would assume energy is put in, but how can the energy change from a 6s orbital to 2p actually be calculated to determine if the necessary amount of energy was lost in this process? Also, is it wrong to assume that an electron ejected from a 6s orbital still has high energy? Or does the energy of the electron change completely once it is out of the atom? Any comments on where the electron's energy went and how an electron from the 6s orbital in Cesium (or higher from other atoms) can be contained in a Nitrogen atom would be greatly appreciated!