What type of molecular shape is associated with six bonded pairs of electrons?

The molecular shape associated with six bonded pairs of electrons is octahedral. This geometry arises from the arrangement of six electron pairs around a central atom, where the pairs are distributed as far apart as possible to minimize repulsion according to VSEPR (Valence Shell Electron Pair Repulsion) theory.

In an octahedral arrangement, the six bonding pairs occupy the corners of an octahedron, with 90-degree angles between the bonding pairs. This shape allows for maximum separation between the electron pairs, leading to stability. A common example of an octahedral molecule is sulfur hexafluoride (SF6), where the sulfur atom is at the center, and the six fluorine atoms are positioned at the vertices of the octahedron.

Other molecular shapes mentioned do not correspond to the arrangement of six bonded pairs. For instance, tetrahedral geometry is associated with four bonded pairs, trigonal bipyramidal has five, and trigonal planar features three, which demonstrates that octahedral is the correct and specific configuration for six bonded pairs.