Bond energy
Bond Energy
Bond energy (pronounced: /bɒnd ˈɛnərdʒi/) is the measure of bond strength in a chemical bond. It is the heat required to break one mole of molecules into their individual atoms.
Etymology
The term "bond energy" is derived from the words "bond", which in this context refers to a lasting attraction between atoms, ions, or molecules, and "energy", which is the capacity for doing work.
Definition
Bond energy, also known as bond dissociation energy, bond enthalpy, and average bond energy, is defined as the standard amount of energy that is required to break a specific type of chemical bond at absolute zero temperature (0 Kelvin). It is usually expressed in units of kilojoules per mole (kJ/mol).
Types of Bond Energy
There are several types of bond energy, including:
- Covalent bond energy: The energy required to break a covalent bond and form neutral atoms.
- Ionic bond energy: The energy required to break an ionic bond and form neutral atoms.
- Metallic bond energy: The energy required to break a metallic bond and form neutral atoms.
Factors Affecting Bond Energy
Several factors can affect bond energy, including:
- Bond length: The distance between the nuclei of two bonded atoms. Shorter bonds are generally stronger and have higher bond energy.
- Bond order': The number of shared electron pairs between two atoms. A higher bond order usually means a stronger bond and higher bond energy.
- Electronegativity: The ability of an atom to attract shared electrons. Bonds between atoms with different electronegativities have higher bond energy.
Related Terms
- Bond dissociation energy: The energy required to break a specific type of chemical bond.
- Bond enthalpy: The enthalpy change associated with breaking a specific type of chemical bond.
- Average bond energy: The average energy required to break a specific type of chemical bond.
External links
- Medical encyclopedia article on Bond energy
- Wikipedia's article - Bond energy
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