Question

Define bond enthalpy.

Answer 1

Hint: To be able to define any given terminology that is made up of multiple words, we can make use of the definitions of the individual terms then put together their definitions to draw the meaning of the multiple terms. The given terminologies can be explained with the help of the mole concept.

Complete answer: Let us take the terms ‘bond’ and ‘enthalpy’ individually:
Chemical bonding is when there is a 'chemical bond' formed amongst two or more ions, atoms, or molecules, that results in the construction of a new chemical product. So the chemical ‘bonds’ are responsible for holding the atoms in place and as a result of which forms a stable compound.
Enthalpy is a quantity most commonly used in thermodynamics that represents a system's total heat content. It is proportional to the system's internal energy along with the product of volume and pressure. So enthalpy is in simple terms related to the ‘release of heat’ that brings about an energy change.
Bond Enthalpy together will then be the energy value that is needed to break down one mole of the specified bond.
Previously, the word "bond strength" had been used. Since both words convey the same meaning, they can be used synonymously.
Therefore bond enthalpy, also known as bond energy or bond dissociation energy, can be described to be the amount of energy (or strength) needed to dissociate the covalent bond in consideration for one mole of that molecule (generally in the gaseous state).

Note:
When we talk about bonds, one of the most common forms of bonds available is the covalent bond. A covalent bond is formed when electrons from each interacting atom are shared equally. The electrons are involved in pairs and so this form of bonding is known as a shared pair. Molecular bonds are another name for covalent bonds. When the bonding pairs are shared it would guarantee that the atoms maintain equilibrium in their outer shell, thereby attaining stability.