Bonding: Polarisation and Intermolecular Forces

Electronegativity refers to the power of an atom to attract electrons in a covalent bond.
It is highest at the top right of the Periodic Table.
Electron distribution in covalent bonds between different atoms is uneven, leading to polar covalent bonds.
A permanent dipole can occur unless the polarity is symmetrical.
Polarity is represented by partial charges (δ+ and δ-).
Intermolecular forces are weaker than intramolecular bonds.
These forces include permanent dipole-dipole forces (hydrogen bonding) and London/van der Waals forces (induced dipole-dipole interactions).
The size of these forces affect a molecule’s melting and boiling points.
Water, for example, has strong hydrogen bonding and a higher boiling point compared to similar molecules.