How does a lone pair distort the molecule shape?

A lone pair of electrons occupies space around a central atom in a molecule, contributing to the overall electron repulsion that determines molecular geometry. Unlike bonding pairs, which are shared between atoms, lone pairs exert greater repulsive force due to their localized presence. This increased repulsion can distort the bond angles between the surrounding atoms, often resulting in a molecular shape that deviates from the ideal geometry predicted by the VSEPR (Valence Shell Electron Pair Repulsion) theory. Consequently, the presence of lone pairs can lead to shapes like bent or pyramidal, rather than linear or tetrahedral.