Noble gas configuration

Electron atomic and molecular orbitals

Noble gas configuration is the electron configuration of noble gases. The basis of all chemical reactions is the tendency of chemical elements to acquire stability. For some main group elements, chemical bond formation often results in a complete electronic configuration resembling a noble gas.[1]

## Kossel and Lewis approach

W. Kossel and Gilbert N. Lewis saw that noble gases did not have the tendency of taking part in chemical reactions under ordinary conditions. On the basis of this observation they concluded that atoms of noble gases are stable and on the basis of this conclusion they proposed a theory of valency known as "Electronic Theory of valency" in 1916:

> During the formation of a chemical bond, atoms combine together by gaining, losing or sharing electrons in such a way that they acquire nearest noble gas configuration.[2]

## Stable configuration

Every system has the tendency to acquire the state of stability or a state of minimum energy, and so chemical elements take part in chemical reactions to acquire a stable electronic configuration similar to that of its nearest noble gas. An example of this tendency is hydrogen'(H)s reaction with oxygen(O) to form water(H2O). Hydrogen in ground state has the Valency 1 and on formation of water it acquires a stable valency of 2, similar to that of its nearest noble gas helium. Nevertheless, a lot of chemical elements especially transition elements can achieve stability with other configurations.

## References

1. ↑ CliffsNotes 2007, p. 15
2. ↑ "The Atom and the Molecule. April 1916. - Published Papers and Official Documents - Linus Pauling and The Nature of the Chemical Bond: A Documentary History". Osulibrary.oregonstate.edu. Archived from the original on November 25, 2013. https://web.archive.org/web/20131125222947/http://osulibrary.oregonstate.edu/specialcollections/coll/pauling/bond/papers/corr216.3-lewispub-19160400.html. Retrieved 2014-01-03.

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Periodic table

Periodic table forms|

| Standard|

* 18-column
* 32-column

|

Alternative|

* Alternatives
* Janet's left step table

Extended|

* Extension beyond the 7th period
* Aufbau
* Fricke
* Pyykkö

Sets of elements|

| By periodic table structure|

| Groups|

* 1 (Alkali metals)
* 2 (Alkaline earth metals)
* 3
* 4
* 5
* 6
* 7
* 8
* 9
* 10
* 11
* 12
* 13
* 14
* 15 (Pnictogens)
* 16 (Chalcogens)
* 17 (Halogens)
* 18 (Noble gases)

|

Periods|

* 1
* 2
* 3
* 4
* 5
* 6
* 7
* 8+
* Aufbau
* Fricke
* Pyykkö

Blocks|

* s-block
* p-block
* d-block
* f-block
* g-block
* Aufbau principle

By metallicity|

| Metals|

* Alkali metals
* Alkaline earth metals
* Lanthanides
* Actinides
* Transition metals
* Post-transition metals

|

Metalloids|

* Lists of metalloids by source
* Dividing line

Nonmetals|

* Reactive nonmetals
* Noble gases

Other sets|

* Platinum-group metals (PGM)
* Rare-earth elements
* Refractory metals
* Precious metals
* Coinage metals
* Noble metal
* Heavy metals
* Native metals
* Transuranium elements
* Superheavy elements
* Major actinides
* Minor actinides

Elements|

| Lists|

* By: Abundance (in humans)
* Atomic properties
* Nuclear stability
* Production
* Symbol

|

Properties|

* Crystal structure
* Electron configuration
* Electronegativity
* Goldschmidt classification
* Term symbol

Data pages|

* Abundance
* Atomic radius
* Boiling point
* Critical point
* Density
* Elasticity
* Electrical resistivity
* Electron affinity
* Electron configuration
* Electronegativity
* Hardness
* Heat capacity
* Heat of fusion
* Heat of vaporization
* Ionization energy
* Melting point
* Oxidation state
* Speed of sound
* Thermal conductivity
* Thermal expansion coefficient
* Vapor pressure

History|

* Element discoveries
* Mendeleev's predictions
* Naming
* etymology
* controversies
* for places
* for people
* in East Asia

See also|

* IUPAC
* nomenclature
* systematic element name
* Trivial name
* Dmitri Mendeleev

* Book
* Category

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