What is ice?

Water in nature has three states: gas, solid, and liquid. In the liquid state, we call it water, the gaseous water is called water vapor, and the solid water is called ice.


Water is a special kind of liquid. It has the highest density at 4°C. At temperatures above 4°C, liquid water adheres to normal thermal expansion and contraction laws. Below 4°C, in the condensed molecules that are linearly distributed in the water, there is an ice-like association molecule that resembles an ice crystal structure, called "pseudo-ice crystal." Because the density of ice is lower than that of water, the presence of “pseudo-ice crystals” reduces the density of water, which is why the density of water at 4°C is the greatest and that of density lower than 4°C is reduced.


So far, eight crystals of ice have been made in the laboratory. However, only natural ice can exist under natural conditions. The rest is high-pressure ice and it is not easy to exist in nature.


The association of water molecules in natural ice is based on the rules of the hexagonal system. The simplest example of a so-called crystal lattice is a tightly packed brick. If a hypothetical atom is substituted at the center of these bricks, a crystal lattice is obtained. The lattice of ice is a triangular prism with a top cone, and the oxygen atoms at the six corners are common to the adjacent six cells. The three oxygen atoms on the edges are shared by three adjacent crystal cells. The two axial oxygen atoms are shared by two crystal cells. Only one central oxygen atom is considered unique to the crystal cell.

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