Editing Intermolecular force (section)

===Ion–dipole and ion–induced dipole forces===

Ion–dipole and ion–induced dipole forces are similar to dipole–dipole and dipole–induced dipole interactions but involve ions, instead of only polar and non-polar molecules. Ion–dipole and ion–induced dipole forces are stronger than dipole–dipole interactions because the charge of any ion is much greater than the charge of a dipole moment. Ion–dipole bonding is stronger than hydrogen bonding.<ref>{{Cite book|title=Chemistry: A Molecular Approach| vauthors = Tro N |publisher=Pearson Education Inc|year=2011|isbn=978-0-321-65178-5|location=United States|pages=466}}</ref>

An ion–dipole force consists of an ion and a polar molecule interacting. They align so that the positive and negative groups are next to one another, allowing maximum attraction. An important example of this interaction is hydration of ions in water which give rise to [[Hydration energy|hydration enthalpy]]. The polar water molecules surround themselves around ions in water and the energy released during the process is known as hydration enthalpy. The interaction has its immense importance in justifying the stability of various ions (like Cu<sup>2+</sup>) in water.

An ion–induced dipole force consists of an ion and a non-polar molecule interacting. Like a dipole–induced dipole force, the charge of the ion causes distortion of the electron cloud on the non-polar molecule.<ref name=Michael-Blaber-1996>{{cite web | vauthors = Blaber M | date = 1996 | url = http://www.mikeblaber.org/oldwine/chm1045/notes/Forces/Intermol/Forces02.htm | title = Intermolecular Forces | work = mikeblaber.org | access-date = 2011-11-17 | archive-date = 2020-08-01 | archive-url = https://web.archive.org/web/20200801205131/http://www.mikeblaber.org/oldwine/chm1045/notes/Forces/Intermol/Forces02.htm | url-status = usurped }}</ref>