The molecular geometry of hydrogen sulfide (H2S) is bent or angular.
This shape arises due to the presence of two hydrogen atoms bonded to a central sulfur atom, along with two lone pairs of electrons on the sulfur atom. According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the repulsion between the lone pairs and the bonding pairs results in a bent structure.
In terms of bond angles, the ideal H–S–H angle would be around 104.5 degrees, similar to that of water (H2O), which also has a bent shape. The lone pairs of electrons occupy more space than the bonding pairs, which causes the hydrogen atoms to be pushed closer together, resulting in this angular position.
Overall, the geometry influences the properties of H2S, making it a polar molecule, which has implications for its behavior in different environments.