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Enthalpy of atomisation, often referred to as atomization energy, is a thermodynamic concept that represents the energy required to completely separate one mole of a substance into its individual atoms in the gas phase. This process involves breaking all the chemical bonds within the substance’s molecules and dispersing the resulting atoms.
Atomization energy is a crucial parameter in understanding the stability and reactivity of substances. It provides insights into the strength of the chemical bonds within a molecule and the energy needed to create individual, non-interacting atoms from it. This energy is typically measured in kilojoules per mole (kJ/mol) and is expressed as a positive value since energy is required for the process.
In simpler terms, enthalpy of atomization gives us an idea of the energy needed to break a substance down into its most fundamental components – individual atoms – which is essential in fields such as chemistry, material science, and thermodynamics.
What is the Enthalpy of Atomisation?
The enthalpy of atomization (ΔH) is the energy released when a mole of atoms is formed from the element in its gaseous state. The enthalpy of atomization a measure of the energy required to break the chemical bonds between the atoms in the molecule.
Atomisation for many elements is high, indicating that it takes a lot of energy to break chemical bonds between the atoms. This is because the atoms held together by strong covalent bonds. The enthalpy of atomisation for hydrogen is low, indicating that it takes very little energy to break the chemical bonds between the atoms. This is because hydrogen atoms held together by weak hydrogen bonds.
Changes in Response Enthalpy
- The enthalpy of a reaction the heat absorbed or released when the reaction takes place. Enthalpy state function, which means that enthalpy of reaction same regardless of path taken to get there.
- The enthalpy of reaction can changed by changing temperature of the reaction or by changing pressure of the reaction. When the temperature of the reaction changed, the enthalpy changed because the heat absorbed or released by the reaction changes. When the pressure of the reaction changed, the enthalpy changed because the work done by the reaction changes.
Also read: Important Topic of Chemistry: Atomization
Standard Enthalpy of Formation
Standard enthalpy of formation is enthalpy change that accompanies formation of one mole of substance from its component elements in their standard states. The standard enthalpy of formation usually expressed in kilojoules per mole (kJ/mol). Formation of compound determined experimentally by measuring enthalpy change accompanying formation of compound from its elements in their standard states.
Enthalpy of Sublimation
The enthalpy of sublimation is the amount of energy required to convert a solid into a gas. This energy used to overcome the attractions between the particles in the solid and the particles in the gas.
Enthalpy of Fusion
The enthalpy of fusion is the enthalpy change when one mole of a substance melts. The enthalpy of fusion for water is 6.02 kJ/mol.
Also read: Important Topic of Chemistry: Enthalpy
Frequently Asked Questions (FAQs) on Enthalpy of Atomisation
Enthalpy of atomization, also known as atomization energy, is the energy required to separate one mole of a substance into its individual atoms in the gas phase.
Enthalpy of atomization provides insights into the strength of chemical bonds within a molecule and helps understand the substance's stability and reactivity.
Enthalpy of atomization is measured in kilojoules per mole (kJ/mol) and represents the energy needed for atomization.
The enthalpy of atomization is a positive value since energy is required to break chemical bonds during atomization. What is enthalpy of atomization?
Why is enthalpy of atomization important?
How is enthalpy of atomization measured?
Is the enthalpy of atomization a positive or negative value?
