Editing Fajans' rules

{{Short description|Explains the covalent character in molecules}}
In [[inorganic chemistry]], '''Fajans' rules''', formulated by [[Kazimierz Fajans]] in 1923,<ref>{{cite journal|last= Fajans|first=K.|authorlink=Kazimierz Fajans|year = 1923|title=Struktur und Deformation der Elektronenhüllen in ihrer Bedeutung für die chemischen und optischen Eigenschaften anorganischer Verbindungen|journal = [[Die Naturwissenschaften]]|volume=11|issue = 10|pages=165–72|doi= 10.1007/BF01552365|bibcode = 1923NW.....11..165F }}</ref><ref>{{cite journal|last = Fajans|first = K.|author2=Joos, G|year=1924|title=Molrefraktion von Ionen und Molekülen im Lichte der Atomstruktur |journal = [[Zeitschrift für Physik]]|volume=23|pages = 1–46|doi= 10.1007/BF01327574|bibcode = 1924ZPhy...23....1F }}</ref><ref>{{cite journal | url=http://www.degruyter.com/view/j/zkri.1924.61.issue-1/zkri.1924.61.1.18/zkri.1924.61.1.18.xml | title=II. Die Eigenschaften salzartiger Verbindungen und Atombau | author=Fajans, K. | journal=Zeitschrift für Kristallographie - Crystalline Materials| year=1924 | volume=61 | issue=1 | pages=18-48 | doi=10.1524/zkri.1924.61.1.18| url-access=subscription }}</ref> are used to predict whether a [[chemical bond]] will be [[covalent bond|covalent]] or [[ionic bond|ionic]], and depend on the charge on the [[cation]] and the relative sizes of the cation and [[anion]]. They can be summarized in the following table: 

[[Image:Atomic_vs_Ionic_Radius.png|thumb|right|600px|Chart illustrating the relationship between atomic and ionic radius]]

:{| class="wikitable"
!Ionic Character
!Covalent Character
|-
|Low positive charge
|High positive charge
|-
|Large cation
|Small cation
|-
|Small anion
|Large anion
|}
Although the bond in a compound like X+Y- may be considered to be 100% ionic, it will always have some degree of covalent character. When two oppositely charged ions (X+ and Y-) approach each other, the cation attracts electrons in the outermost shell of the anion but repels the positively charged nucleus. This results in a distortion, deformation or polarization of the anion. If the degree of polarization is quite small, an ionic bond is formed, while if the degree of polarization is large, a covalent bond results.<ref>{{Cite web |date=2015-11-27 |title=Polarizability |url=https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Physical_Properties_of_Matter/Atomic_and_Molecular_Properties/Polarizability |access-date=2024-12-30 |website=Chemistry LibreTexts |language=en}}</ref>[[File:Covalent and ionic bonds.jpg|thumb|right|Non-polar covalent bond (left), polar covalent bond (center), ionic bond(right)]]

Thus [[sodium chloride]] (with a low positive charge (+1), a fairly large cation (~1&nbsp;Å) and relatively small anion (~2&nbsp;Å) is ionic; but [[aluminium iodide]] (AlI<sub>3</sub>) (with a high positive charge (+3) and a large anion) is covalent.

Polarization will be increased by:
* High charge and small size of the cation, due to [[ionic potential]] Å Z+/r+ (= polarizing power)
*High charge and large size of the anion, due to polarizability which is related to the deformability of its electron cloud (i.e. its "softness")
*An incomplete valence shell electron configuration, due to the noble gas configuration of the cation producing better shielding and less polarizing power, for example Hg<sup>2+</sup> (r+ = 102 pm) is more polarizing than Ca<sup>2+</sup> (r+ = 100 pm)

The "size" of the charge in an ionic bond depends on the number of electrons transferred. An aluminum atom, for example, with a +3 charge has a relatively large positive charge. That positive charge then exerts an attractive force on the electron cloud of the other ion, which has accepted the electrons from the aluminum (or other) positive ion.

Two contrasting examples can illustrate the variation in effects. In the case of aluminum iodide an ionic bond with much covalent character is present. In the AlI<sub>3</sub> bonding, the aluminum gains a +3 charge. The large charge pulls on the electron cloud of the iodine. Now, if we consider the iodine atom, we see that it is relatively large and thus the outer shell electrons are relatively well shielded from the nuclear charge. In this case, the aluminum ion's charge will "tug" on the electron cloud of iodine, drawing it closer to itself. As the electron cloud of the iodine nears the aluminum atom, the negative charge of the electron cloud "cancels" out the positive charge of the aluminum cation. This produces an ionic bond with covalent character. A cation having inert gas like configuration has less polarizing power in comparison to cation having pseudo-inert gas like configuration.

[[File:Ionic character vs electronegativity 01.jpg|thumb|Graph of percentage ionic character]]

The situation is different in the case of [[aluminum fluoride]], AlF<sub>3</sub>. In this case, iodine is replaced by fluorine, a relatively small highly electronegative atom. The fluorine's electron cloud is less shielded from the nuclear charge and will thus be less polarizable. Thus, we get an ionic compound (metal bonded to a nonmetal) with a slight covalent character.

== References ==
<references />

==External links==
* {{cite web | author = Adrian Faiers | publisher = chembook.co.uk | title = Chapter 4: Chemical Bonding | work = Chemistry in Perspective | url = http://www.chembook.co.uk/chap4.htm}}

[[Category:Eponymous chemical rules]]
[[Category:Inorganic chemistry]]