Intermolecular vs Intramolecular Forces

Intramolecular forces hold atoms together within a molecule, such as ionic, covalent, and metallic bonds. Intermolecular forces are electrostatic attractions between molecules. Intramolecular forces are much stronger because large charges interact over short distances, while intermolecular forces are weaker due to small or partial charges interacting over larger distances.

Water boils at 100°C because this temperature provides enough thermal energy to overcome intermolecular forces between water molecules, which are separated by about 300 picometers. Breaking the O–H covalent bonds within water molecules requires much more energy and temperatures around 1000°C, demonstrating that intermolecular forces are significantly weaker than intramolecular bonds.

Intermolecular forces include ion–dipole forces between ions and polar molecules, dipole–dipole forces between polar molecules (with hydrogen bonding as a special type), and dispersion forces in all molecules. Dispersion forces are the weakest type, arising from temporary dipoles in both polar and nonpolar molecules.

Intermolecular forces dictate physical properties including melting point, boiling point, and density. Substances with stronger intermolecular forces have higher boiling and melting points. For example, water with strong intermolecular forces boils at 100°C, while hexane with weaker forces boils at 68.73°C, illustrating how intermolecular forces melting point and boiling point are directly related.

The three basic intramolecular bonds are ionic bonds, formed by electron transfer between metals and nonmetals; covalent bonds, formed by electron sharing between nonmetal atoms; and metallic bonds, resulting from interactions between positive metal ions and a shared pool of delocalized valence electrons.

Intermolecular forces are weaker because they involve small or partial charges interacting over relatively large distances between molecules. In contrast, intramolecular forces involve large electrostatic interactions over very short distances within molecules. For example, breaking one mole of HCl covalent bonds requires 430 kilojoules, while overcoming intermolecular forces in liquid HCl requires only 17 kilojoules.

When a liquid is heated, thermal energy overcomes intermolecular forces holding molecules in place, causing the liquid to boil and convert to gas. Melting ice disrupts intermolecular forces between solid water molecules, rearranging them into liquid form, but does not break intramolecular bonds within individual H2O molecules, demonstrating that state changes affect only intermolecular interactions.