The molecular shape of the NO+ ion is linear.
To understand this, we need to consider the electron configuration and the molecular geometry. The NO+ ion is derived from nitric oxide (NO) by removing one electron. In this process, the ion has a total of 11 valence electrons, which impacts its geometry.
According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the arrangement of these electrons around the central nitrogen atom allows for a linear shape. This is because there are two regions of electron density: one from the nitrogen atom and another from the oxygen atom. These regions repel each other and align as far apart as possible, resulting in a linear arrangement.
Additional evidence supporting this linear shape comes from the molecular orbital theory, which shows that the overlap of p-orbitals in NO+ contributes to a stable linear structure, similar to that found in diatomic molecules.
In conclusion, the NO+ ion has a linear molecular shape due to its two regions of electron density creating the least repulsion, hence maximizing stability.