Successive ionization energies (work functions?) for metals

Are there tables for successive ionization energies for metals (like for gases)? All I can find are work functions to remove one electron from the surface of a metal into vacuum (and to keep it there). However, I guess it gets harder to remove electrons the more electrons already have been removed, right? 


Maybe there's a way to relate that energy to the average degree of ionization of the material. Is it possible at all?


Finally, is it harder to ionize a metal gas or a metal solid? Although most work functions are a little bit smaller than the (1st) ionization-energies of the same material in gaseous state but I still think ionization of solids is harder. Am I correct?




In an infinite metal solid, there are an infinite number of electrons, so ***each one*** removed will be at the exactly identical work function with no change in energy.


Intuitively, this may seem a bit strange because .. well, it should be harder to remove an electron once positive charges start to accumulate.


If I have even a micron-sized piece of metal, that's [~$10^{13}$ atoms](http://www.chemteam.info/Liquids&Solids/WS-unit-cell-AP.html). So you really have to do a *lot* of ionization before you're even going to get 0.1% of the metal ions.


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Here is the link to the exact page you want: [Ionization energy of elements (Data Page)](https://en.wikipedia.org/wiki/Ionization_energies_of_the_elements_(data_page))


For a good measure, here is the one for electron affinities too: [Electron affinity (Data Page)](https://en.wikipedia.org/wiki/Electron_affinity_(data_page))




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Wikipedia defines ionization energy as:



> 
> The ionization energy is qualitatively defined as the amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated gaseous atom to form a cation.
> 
> 
> 


This means we cannot really talk about the ionization energy for solid metals. The closest interpretation we can get for solid metals is the work function, but i suspect they depend on the metal's crystal structure too, as i have written below.




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I would say that metal solids are harder to ionize because at low temperatures, the average energy of metal atoms is low and so thermal collisions generally may not have enough energy to knock an electron of a metal atom. A more important reason is that electrons are locked away in metallic bonds with other atoms (for solid metals), so you have to provide sufficient energy to the electron to not only break the metallic bonds, but also release the electron from the atomic nucleus. (Please correct me if i'm wrong.)


Also, check out this [ionization energy page](https://en.wikipedia.org/wiki/Ionization_energy) on Wikipedia for more information.


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