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((short description|Ratio of the electrical charge to the radius of an ion))
((Refimprove|date=August 2017))
'''Ionic  potential''' is the [[ratio]] of the [[electric charge|electrical charge]] (''z'') to the [[ionic radius|radius]] (''r'') of an [[ion]].<ref>((Cite web| title = Ionic potential| url = http://www.encyclopedia.com/science/dictionaries-thesauruses-pictures-and-press-releases/ionic-potential| access-date = 17 April 2017))</ref>

<math display="block">\text{Ionic potential} = \frac{\text{electrical charge)){\text{ionic radius)) = \frac{z}{r}</math>

As such, this ratio is a measure of the [[charge density]] at the surface of the ion; usually the denser the charge, the stronger the [[ionic bond|bond]] formed by the ion with ions of opposite charge.<ref>((Cite web| first=Bruce |last=Railsback| title = Ionic potential| url=http://railsback.org/Fundamentals/IonicPotential04P.pdf|access-date = 16 July 2020|url-status=))</ref>

The ionic potential gives an indication of how strongly, or weakly, the ion will be electrostatically attracted by ions of opposite charge; and to what extent the ion will be repelled by ions of the same charge. 

[[Victor Moritz Goldschmidt]], the father of modern [[geochemistry]] found that the behavior of an element in its environment could be predicted from its ionic potential and illustrated this with a diagram (plot of the bare [[ionic radius]] as a function of the ionic charge).<ref name="Kauffman1997">((cite journal|last1=Kauffman|first1=George B.|title=Victor Moritz Goldschmidt (1888 – 1947): A tribute to the founder of modern geochemistry on the fiftieth anniversary of his death|journal=The Chemical Educator|volume=2|issue=5|year=1997|pages=1–26|issn=1430-4171|doi=10.1007/s00897970143a|s2cid=101664962))</ref> For instance, the [[solubility]] of dissolved iron is highly dependent on its redox state. ((chem|Fe|2+)) with a lower ionic potential than ((chem|Fe|3+)) is much more soluble because it exerts a weaker interaction force with ((chem|OH|-)) ion present in water and exhibits a less pronounced trend to [[hydrolysis]] and [[Precipitation (chemistry)|precipitation]]. Under reducing conditions Fe(II) can be present at relatively high concentration in [[Anoxic waters|anoxic water]], similar to these encountered for other divalent species such as ((chem|Ca|2+)) and ((chem|Mg|2+)). However, once anoxic ground water is pumped from a deep well and is discharged to the surface, it enters in contact with atmospheric oxygen. Then ((chem|Fe|2+)) is easily oxidized to ((chem|Fe|3+)) and this latter rapidly hydrolyzes and precipitates because of its lower solubility due to a higher z/r ratio. 

Millot (1970) also illustrated the importance of the ionic potential of cations to explain the high, or the low, [[solubility]] of minerals and the expansive behaviour (swelling/shrinking) of [[clay minerals|clay materials]].<ref name="Millot1970">((cite book|last1=Millot|first1=Georges|year=1970|title=Geology of clays: weathering – sedimentology – geochemistry|publisher=Springer Science & Business Media|doi=10.1007/978-3-662-41609-9|isbn=978-3-662-41611-2))</ref>

The ionic potential of the different cations (((chem|Na|+)), ((chem|K|+)), ((chem|Mg|2+)) and ((chem|Ca|2+))) present in the interlayer of clay minerals also contribute to explain their swelling/shrinking properties.<ref name="DelvilleLaszlo1990">((cite journal|last1=Delville|first1=Alfred|last2=Laszlo|first2=Pierre|title=The origin of the swelling of clays by water|journal=Langmuir|volume=6|issue=7|year=1990|pages=1289–1294|issn=0743-7463|doi=10.1021/la00097a017))</ref> The more hydrated cations such as ((chem|Na|+)) and ((chem|Mg|2+)) are responsible for the swelling of [[smectite]] while the less hydrated ((chem|K|+)) and ((chem|Ca|2+)) cause the collapse of the interlayer. In [[illite]], the interlayer is totally collapsed because of the presence of the poorly hydrated ((chem|K|+)). 

Ionic potential is also a measure of the [[Polarizability|polarising power]] of a [[cation]].

Ionic potential could be used as a general criterion for the selection of efficient [[adsorption|adsorbents]] for [[Toxic heavy metal|toxic elements]].<ref name="LiYang2014">((cite journal|last1=Li|first1=Ronghui|last2=Yang|first2=Weiyi|last3=Su|first3=Yu|last4=Li|first4=Qi|last5=Gao|first5=Shian|last6=Shang|first6=Jian Ku|title=Ionic potential: A general material criterion for the selection of highly efficient arsenic adsorbents|journal=Journal of Materials Science & Technology|volume=30|issue=10|year=2014|pages=949–953|issn=10050302|doi=10.1016/j.jmst.2014.08.010))</ref>

==See also==

* [[Ionization energy]]
* [[Metal ions in aqueous solution]]
* [[Surface charge]]

==References==
<references />

((DEFAULTSORT:Ionic Potential))
[[Category:Binding energy]]
[[Category:Chemical properties]]
[[Category:Ions]]
[[Category:Physical chemistry]]
[[Category:Electrochemical potentials]]
[[Category:Atomic radius]]


((Electrochem-stub))

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