Water is composed of hydrogen and oxygen atoms bonded together as H2O molecules. The uneven distribution of charges within water molecules results in polarity, with the oxygen end slightly negative and hydrogen ends slightly positive. This allows opposing charges between molecules to form weak hydrogen bonds. Hydrogen bonding between water molecules absorbs heat energy and requires more energy to change water's state, especially during phase changes. It also results in water having a density of 1g/mL and being less dense as a solid than liquid. Hydrogen bonding and the resulting pockets account for these unique properties.