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Inchemistry, theenthalpy of atomization (alsoatomisation in British English) is theenthalpy change that accompanies the total separation of allatoms in a chemical substance either anelement or acompound.[1] This is often represented by the symbol or All bonds in the compound are broken in atomization and none are formed, so enthalpies of atomization are always positive. The associatedstandard enthalpy is known as thestandard enthalpy of atomization,ΔatH⊖/(kJ mol−1), at 298.15 K (or 25 degrees Celsius) and 100 kPa.
Enthalpy of atomization is the amount of enthalpy change when bonds of the compound are broken and the component atoms are separated into single atoms ( or monoatom).
Enthalpy of atomization is denoted by the symbol ΔHat. The enthalpy change of atomization of gaseousH2O is, for example, the sum of the HO–H and H–OHbond dissociation enthalpies.
The enthalpy of atomization of an elemental solid is exactly the same as theenthalpy of sublimation for any elemental solid that becomes amonatomic gas uponevaporation.
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.
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