Learn how bond enthalpies are used to calculate the enthalpy change (ΔH) of a reaction. Discover how breaking and forming chemical bonds determines whether a reaction is exothermic or endothermic.

This page introduces bond enthalpies (bond energies) and looks at some simple calculations involving them.

Bond enthalpy measures the energy stored in a bond between two atoms. It is the energy required to symmetrically cleave a bond when a compound is in its gaseous phase.

In chemistry, bond energy (BE) is one measure of the strength of a chemical bond.

The bond enthalpy tells you how much heat energy is needed to break one mole of the bond. That is bound to need energy and so bond enthalpies are always positive.

Bond enthalpy (also known as bond energy) is defined as the amount of energy required to break one mole of the stated bond. For example, the bond energy of a O-H single bond is 463 kJ/mol.

Bond enthalpy (which is also known as bond-dissociation enthalpy, average bond energy, or bond strength) describes the amount of energy stored in a bond between atoms in a molecule.

Another term for bond energy is bond enthalpy, or bond dissociation energy. When a chemical reaction occurs, molecular bonds are broken and new bonds are formed to make different molecules.

Bond enthalpy, also known as bond energy, is a quantity that offers insight into the strength of a chemical bond and, by extension, its stability. The bond enthalpy of a chemical bond can be defined …

In the absence of standard formation enthalpies, reaction enthalpies can be estimated using average bond enthalpies. This method is not perfect, but it can be used to get ball-park estimates when more …