Intramoelecular Force and Potential Energy

Intramolecular Forces

Intramolecular forces are the forces of attraction that hold atoms together within a molecule.
These forces are much stronger than intermolecular forces, which exist between molecules.
The three main types of intramolecular forces are ionic bonding, covalent bonding, and metallic bonding.
Ionic bonding occurs between atoms of opposite charges, resulting in the formation of ionic compounds.
In covalent bonding, atoms share electron pairs, most commonly seen in the formation of molecular compounds.
Metallic bonding is characteristic for metal atoms, where electrons are shared among a lattice of cations.

The overall stability of a molecule can be associated with its potential energy.
A molecule’s potential energy is minimised when it reaches a state of equilibrium, or the most stable arrangement.
Changes in potential energy are often associated with changes in the molecule’s physical state or phase.
Potential Energy Diagrams can be used to visualise the energy changes that occur during a reaction. On these diagrams, the y-axis represents potential energy, while the x-axis represents the reaction coordinate.
During a chemical reaction, if the energy of the products is lower than the energy of the reactants, the reaction releases energy, making it exothermic.
If the energy of the products is higher than that of the reactants, the reaction absorbs energy, making it endothermic.

The strength of intramolecular forces in a molecule can be measured by the bond’s dissociation energy, or bond energy.
Bond energy is the amount of energy needed to break a bond between two atoms. A bond’s strength is directly proportional to its bond energy – stronger bonds require more energy to break.
On a potential energy diagram, bond energy can be visualised as the difference in energy between the reactants and the highest point on the potential energy profile, referred to as the transition state or activation energy.
In a reaction, if the sum of the bond energies of the reactants is greater than the products, the resulting reaction will be exothermic. Conversely, if the sum of the bond energies of the products is greater, the reaction will be endothermic.