The molecules can interact with each other in three ways, hydrogen-bonding, van der Waals interactions, and electrostatic interactions. These fifth and sixth neighbors may be found when modeling at lower pressures but in smaller amounts. As the pressure is increased (towards 1 GPa) up to two further water molecules are pushed into the first coordination sphere without establishing any extra hydrogen bonds. A locally tetrahedral four-fold hydrogen-bonding pattern (see below left) characterizes ambient water. The hydrogen atoms are slightly positively charged, whereas the oxygen atom has a negative charge. The water molecule is bent (see left), and has two hydrogen atoms and one oxygen atom. On this page, some of its defining properties are described. Its properties are a challenge, particularly as it possesses such a simple molecular formula. Of all liquids, water stands out for its peculiar properties and is the most extraordinary substance. ![]() The significant difference between gases and liquids is the frequency of collisions in the liquid state, causing strong correlations between the positions of the particles. ![]() Among the three fundamental states of matter, gas, liquid, and solid, the liquid state is the most poorly understood far from the better-understood properties of a low-density gas or an ordered crystal. The density of a liquid is similar to but generally less than its solid, but this does not hold for liquid water that is denser than its commonly found solid ice. Over a limited range of temperatures and pressures, the liquid can coexist with the solid or gas phases. It does not have a fixed shape and can flow and conform to the shape of a container, unlike the solid-state. It is much denser than the gas and has a specific volume dependent on its temperature and pressure.
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