I actually first worked on this table to explain speciaton of cations in solution, as shown above. Here we're working across the same part of the new table, with ionic potential increasing from left to right:
>>>>>>>>Cations of low ionic potential, at the left, attract the negative (O2-) ends of water molecules, and are thus hydrated in solution.
>>>>>>>>Cations of a little higher ionic potential have enough positive charge to repel some of the H+ ions of potential hydrating water molecules. They thus instead have OH-s around them - they form hydroxocomplexes.
>>>>>>>> Moving farther to the right, you encounter cations of still higher ionic potential, so that their positive charge repels still more H+ ions, stripping some oxygens of both H+ ions. They thus form oxohydroxo complexes.
>>>>>>>> Farthest to the right, cations of highest ionic potential repel all H+ ions and thus have nothing but O2-s around them, and so they form oxocomplexes like the familiar nitrate of N5+ and sulfate of S6+. On the other hand, we don't talk about "calciates" and the like because of the much lower ionic potential of Ca2+.

        This pattern shows up on the full table . . . .


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Railsback's main page about the Earth Scientist's Periodic Table of the Elements and Their Ions
e-mail to Bruce Railsback (rlsbk@gly.uga.edu)
Railsback's main web page
UGA Geology Department web page

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