As a chemical expert with a deep understanding of molecular structures, I can tell you that the molecular geometry of H2O, or water, is indeed bent, not linear. This is due to the arrangement of electron pairs around the central oxygen atom and the nature of the bonds formed with hydrogen atoms. Let's delve into the details to understand why this is the case. ### Valence Shell Electron Pair Repulsion (VSEPR) Theory The VSEPR theory is a model that helps predict the shapes of molecules. It is based on the principle that electron pairs around a central atom will arrange themselves to minimize repulsion. In the case of water, the central atom is oxygen. ### Electron Pair Geometry Oxygen has six valence electrons. It shares two electrons with each of the two hydrogen atoms, forming two covalent bonds. This leaves four electrons on the oxygen atom that are not involved in bonding, known as lone pairs. These lone pairs, along with the two bonding pairs, make a total of four electron pairs around the oxygen atom. According to VSEPR theory, these four electron pairs will arrange themselves in a tetrahedral geometry to minimize repulsion. However, since we are only considering the shape of the molecule as it appears to the outside (not the lone pairs), we look at the arrangement of the atoms. The tetrahedral geometry of the electron pairs results in a bent or V-shaped molecular geometry when two of the positions are taken up by hydrogen atoms. ### Bond Angles The bond angle between the hydrogen-oxygen-hydrogen atoms in a water molecule is approximately 104.5 degrees. This is less than the 109.5 degrees that would be expected in a perfect tetrahedral geometry, which is occupied by four bonding pairs. The difference is due to the greater repulsion between the lone pairs of electrons compared to the bond pairs. Lone pairs occupy more space and repel the bond pairs more strongly, pushing the hydrogen atoms closer together. ### Molecular Polarity The bent shape of the water molecule also contributes to its polarity. The oxygen atom is more electronegative than hydrogen, meaning it attracts electrons more strongly. This results in a dipole moment, with a partial negative charge on the oxygen and partial positive charges on the hydrogens. The bent shape allows the water molecule to form hydrogen bonds with other polar molecules, which is a significant factor in water's unique properties, such as its high boiling point, high heat capacity, and its role as a universal solvent. ### Conclusion In summary, the water molecule, H2O, has a bent molecular geometry due to the tetrahedral electron pair geometry around the central oxygen atom. The presence of two lone pairs and the repulsion between these lone pairs and the bonding pairs result in a bond angle that is less than that of a perfect tetrahedron. This molecular shape, along with the polarity it creates, is fundamental to many of water's unique and essential properties in nature. read more >>

An example of bent molecular geometry that results from tetrahedral electron pair geometry is H2O. The water molecule is so common that it is wise to just memorize that water is a BENT molecule. The oxygen has 6 valence electrons and thus needs 2 more electrons from 2 hydrogen atoms to complete its octet.read more >>