Define bond dissociation enthalpy
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Bond dissociation enthalpy and bond dissociation energy is defined as the energy used or needed to break a bond or one mole of a bond.
It is used to calculate the breaking of bonds in gaseous states and not in any other state.
Bond enthalpy may be interchangeably used with the terms Bond energy or Bond strength.
It is stated as one of the measures to determine the strength of the bonds. It is often defined as the enthalpy change of homolysis at 0k.
Enthalpy change is a temprature dependent process.
The standard change of enthalpy is encountered at a temprature of 298 k.
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The strength of the chemical bond between any two species can be estimated with the help of bond dissociation enthalpy. Although it is generally measured as the enthalpy change at standard conditions (298K), the bond dissociation energy of a chemical bond is often defined as the enthalpy change of the homolytic fission of the bond at absolute zero (0K).
Some important features of the concept of bond dissociation enthalpy include:
It is the amount of energy which needs to be supplied in order to break a chemical bond between two species.
It is a means of calculating the strength of a chemical bond.
In diatomic molecules specifically, it is equal to the value of bond energy
The bond between silicon and fluorine is said to have the strongest bond dissociation enthalpy.
Covalent bonds between atoms or molecules are said to have weak bond dissociation energies.
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