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((short description|Enthalpy change needed to separate all atoms in a substance))
((More citations needed|date=February 2019))

In [[chemistry]], the '''enthalpy of atomization''' (also '''atomisation''' in British English) is the [[enthalpy]] change that accompanies the total separation of all [[atoms]] in a chemical substance (either an [[chemical element|element]] or a [[chemical compound|compound]]).<ref>((cite web|url=http://chemistry.about.com/od/chemistryglossary/g/Enthalpy-Of-Atomization-Definition.htm|title=Enthalpy of Atomization Definition|last=Helmenstine|first=Anne Marie|publisher=[[About.com]]|accessdate=11 August 2014|archive-date=10 August 2014|archive-url=https://web.archive.org/web/20140810034558/http://chemistry.about.com/od/chemistryglossary/g/Enthalpy-Of-Atomization-Definition.htm|url-status=dead))</ref> This is often represented by the symbol ((tmath|\Delta_{at}H)) or ((tmath|\Delta H_{at}.)) All bonds in the compound are broken in atomization and none are formed, so enthalpies of atomization are always positive. The associated [[standard enthalpy]] is known as the '''standard enthalpy of atomization''', ((math|Δ((sub|at))''H''((sup|⊖))))/([[Joule|kJ]]&thinsp;[[mole (unit)|mol]]<sup>−1</sup>), at 298.15&nbsp;[[Kelvin|K]] (or 25 degrees Celsius) and 100&nbsp;[[Pascal (unit)|kPa]].

==Definition==
Enthalpy of atomization is the amount of enthalpy change when a compound's bonds are broken and the component atoms are separated into single atoms ( or monoatom).

Enthalpy of atomization is denoted by the symbol ΔH<sub>at</sub>. The enthalpy change of atomization of gaseous [[water (molecule)|H<sub>2</sub>O]] is, for example, the sum of the HO–H and H–OH [[bond-dissociation energy|bond dissociation enthalpies]].

The enthalpy of atomization of an elemental solid is exactly the same as the [[enthalpy of sublimation]] for any elemental solid that becomes a [[monatomic]] gas upon [[evaporation]].

When a diatomic element is converted to gaseous atoms, only half a mole of molecules will be needed, as the standard enthalpy change is based purely on the production of one mole of gaseous atoms. When the atoms in the molecule are different isotopes of the same element the calculation becomes non-trivial.

==See also==
* [[Ionization energy]]
* [[Electron gain enthalpy]]

==References==
((reflist))

((DEFAULTSORT:Enthalpy Change Of Atomization))
[[Category:Enthalpy]]


((thermodynamics-stub))
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