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ChatGPT
Jun 23
Enthalpy of atomisation is the amount of energy required to completely separate the atoms in one mole of a substance in the gaseous state into individual atoms. It is a measure of the strength of the bonds holding the atoms together in a molecule.
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Google Gemini AI
Jun 23
Enthalpy of Atomisation:
The enthalpy of atomisation is the amount of energy required to break all the chemical bonds in a molecule and separate it into its constituent atoms in the gaseous state. It is a measure of the stability of a molecule and represents the energy change when a mole of a substance in its standard state (usually at 298 K and 1 atm) is converted into its constituent atoms in the gaseous state.
Mathematically, the enthalpy of atomisation (∆H°ₐₜᵒₘ) can be expressed as:
∆H°ₐₜᵒₘ = Σ ∆H(bonds broken) - Σ ∆H(bonds formed)
where:
- Σ ∆H(bonds broken) is the sum of the bond energies of all the bonds broken during atomisation
- Σ ∆H(bonds formed) is the sum of the bond energies of all the bonds formed during the formation of the constituent atoms
The enthalpy of atomisation is typically a positive value, indicating that energy is required to break the bonds and separate the atoms. It provides insights into the strength and stability of the chemical bonds within a molecule. A higher enthalpy of atomisation indicates stronger bonds and a more stable molecule, while a lower enthalpy of atomisation suggests weaker bonds and a less stable molecule.
The enthalpy of atomisation is the amount of energy required to break all the chemical bonds in a molecule and separate it into its constituent atoms in the gaseous state. It is a measure of the stability of a molecule and represents the energy change when a mole of a substance in its standard state (usually at 298 K and 1 atm) is converted into its constituent atoms in the gaseous state.
Mathematically, the enthalpy of atomisation (∆H°ₐₜᵒₘ) can be expressed as:
∆H°ₐₜᵒₘ = Σ ∆H(bonds broken) - Σ ∆H(bonds formed)
where:
- Σ ∆H(bonds broken) is the sum of the bond energies of all the bonds broken during atomisation
- Σ ∆H(bonds formed) is the sum of the bond energies of all the bonds formed during the formation of the constituent atoms
The enthalpy of atomisation is typically a positive value, indicating that energy is required to break the bonds and separate the atoms. It provides insights into the strength and stability of the chemical bonds within a molecule. A higher enthalpy of atomisation indicates stronger bonds and a more stable molecule, while a lower enthalpy of atomisation suggests weaker bonds and a less stable molecule.
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