In chemistry, the enthalpy of atomization (also atomisation in British English) is the

enthalpy Enthalpy , a property of a thermodynamic system, is the sum of the system's internal energy and the product of its pressure and volume. It is a state function used in many measurements in chemical, biological, and physical systems at a constant ...

change that accompanies the total separation of all atoms in a chemical substance (either an element or a

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). 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 associated standard enthalpy is known as the standard enthalpy of atomization, /( kJ mol⁻¹), at 298.15 K (or 25 degrees Celsius) and 100

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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 Δ_at''H''. The enthalpy change of atomization of gaseous H₂O is, for example, the sum of the HO–H and H–OH bond dissociation enthalpies. The enthalpy of atomization of an elemental solid is exactly the same as the

enthalpy of sublimation In thermodynamics, the enthalpy of sublimation, or heat of sublimation, is the heat required to sublimate (change from solid to gas) one mole of a substance at a given combination of temperature and pressure, usually standard temperature and p ...

for any elemental solid that becomes a

monatomic In physics and chemistry, "monatomic" is a combination of the words "mono" and "atomic", and means "single atom". It is usually applied to gases: a monatomic gas is a gas in which atoms are not bound to each other. Examples at standard conditions ...

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.

References

Enthalpy {{Chem-stub

Definition

See also

References