Final answer:
Nonbonding (lone) pairs repel bonding pairs more strongly than bonding pairs repel each other due to the larger space lone pairs occupy. This is explained by the VSEPR theory, which states electron pairs, both bonding and nonbonding, will orient themselves to minimize repulsion and determine the molecular geometry.
Step-by-step explanation:
The question revolves around the concept of electron pair repulsion in molecular structures. Nonbonding (lone) pairs repel bonding pairs more strongly than bonding pairs repel each other. This is because lone pairs occupy more space around the central atom than bonding pairs, leading to greater electrostatic repulsions. The repulsion strength follows the order of LP-LP (lone pair-lone pair) > LP-BP (lone pair-bonding pair) > BP-BP (bonding pair-bonding pair).
Electron pair repulsion is a central concept in VSEPR (Valence Shell Electron Pair Repulsion) theory, which is used to predict the shapes of molecules. According to the theory, bonding pairs of electrons, located primarily between bonded atoms, and lone pairs will arrange themselves as far apart as possible in three-dimensional space to minimize the repulsive interactions between them. This leads to the observed geometries of molecules.
In molecular geometry, bond lengths and the three-dimensional arrangement of atoms are dictated by these repulsive forces, in conjunction with attractive forces, such that a balanced state is reached at the observed bond distance.