Hydrogen bonds in water are found between the hydrogen atom of one water molecule and the oxygen atom of a neighboring water molecule. Specifically, the partially positive hydrogen atom covalently bonded to oxygen in one molecule is attracted to the partially negative oxygen atom in another molecule. This creates a dynamic, electrostatic attraction called a hydrogen bond

. Each water molecule can form up to four hydrogen bonds: two involving its own hydrogen atoms and two involving the lone pairs of electrons on its oxygen atom. These hydrogen bonds arrange themselves roughly tetrahedrally around each water molecule, similar to the structure found in ice, although in liquid water these bonds are constantly bending, stretching, and breaking due to thermal motion

. In summary, hydrogen bonds in water occur between the hydrogen atoms of one water molecule and the oxygen atoms of neighboring water molecules, forming a network that is responsible for many of water's unique properties