ACS Chemistry Practice Exam 2026 – The All-in-One Guide to Exam Success!

In linear molecular geometry, the shape of the molecule is such that all the atoms involved are arranged in a straight line. This geometric arrangement results in a bond angle of 180 degrees between the bonded atoms. The reason for this specific angle is rooted in the principles of VSEPR (Valence Shell Electron Pair Repulsion) theory, where the electron pairs surrounding a central atom tend to arrange themselves as far apart as possible to minimize repulsion.

In a linear geometry, there are typically two bonded atoms and no lone pairs on the central atom, which allows for the maximum distance between the bonded pairs, achieving a straight line configuration. This results in the characteristic bond angle of 180 degrees, distinguishing linear structures from other molecular geometries like trigonal planar or tetrahedral, which have different angles associated with them.