Which molecule has a bent structure due to the presence of lone pairs in its Lewis structure?

The molecule with a bent structure due to the presence of lone pairs in its Lewis structure is water (H2O). In the Lewis structure of water, the oxygen atom has two lone pairs of electrons along with two bonding pairs that are shared with hydrogen atoms. This arrangement results in a tetrahedral electron geometry; however, the molecular shape is defined by the positions of the atoms, leading to a bent structure.

The lone pairs create repulsion that pushes the hydrogen atoms closer together, resulting in an angle of approximately 104.5 degrees between the hydrogen-oxygen-hydrogen atoms. This bent shape is a direct consequence of the VSEPR (Valence Shell Electron Pair Repulsion) theory, which indicates that electron pairs (both bonding and lone pairs) tend to be arranged as far apart from each other as possible.

In contrast, molecules like carbon dioxide (CO2) and methane (CH4) have a linear and tetrahedral structure, respectively, due to the absence of lone pairs on the central atom, allowing all bonding pairs to minimize repulsion without distortion. Ammonia (NH3) does have a trigonal pyramidal shape due to one lone pair, but it is not bent in the same way that water is, as