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water (H2O)
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So familiar is water, that we tend to forget how unusual a substance it really is. Of all water's properties, the most significant is its ability to form weak chemical associations, known as hydrogen bonds, with about 5-10% of the strength of covalent bonds. This ability stems from the fact that water consists of polar molecules, in each of which the oxygen atom has a slight negative charge and the two hydrogen atoms slight positive charges. The polarity of water causes it to be attracted to other polar molecules. When these other molecules are also water, the attraction is referred to as cohesion; when they are different, it is known as adhesion. The cohesiveness of water is what allows it to remain a liquid at moderate temperatures (whereas hydrogen sulfide, for example, which is chemically similar, exists as a gas). Water molecules always tend to form the maximum possible number of hydrogen bonds. When nonpolar molecules such as oils, which do not form hydrogen bonds, are placed in water, the water molecules act to exclude them. This forces the nonpolar molecules into association with one another: a tendency to aggregate known as hydrophobic exclusion. Hydrophobic forces arising from the polar nature of water are thought to have been of central importance in the evolution of life. Firstly, they seem to have encouraged the formation of protocells and, in particular, the boundaries which enclosed them (see cell membranes, origin). Secondly, their influence is evident in the fact that some of the exterior portions of many of the molecules on which life came to be based are nonpolar. By forcing the hydrophobic portions of molecules into proximity with one another, water caused such molecules to assume particular shapes.
Whereas water organizes and orchestrates the geometry of nonpolar molecules, it acts as a solvent for substances that consist of ions or polar molecules. It does this by surrounding the charged parts of the substance with a cluster of water molecules known as a hydration shell. Such shells prevent the ions or polar molecules of the solute from reassociating.
Another crucial property of water, which is again a result of its polar nature, is its ability to resist changes in temperature. That is to say, water has a high specific heat. A lot of thermal energy has to be supplied to break the hydrogen bonds between water molecules and cause them to move around faster (resulting in a temperature rise). Even so, only about 20% of the hydrogen bonds are broken in heating water from its freezing point to its boiling point. By the same token, water holds its temperature longer than do most other substances when heat is no longer supplied. Only ammonia, which is more polar than water, has a higher specific heat.
Extensive hydrogen bonding also means that water has a high heat of vaporization. From this it follows that the evaporation of only a small amount of water is sufficient to carry away a great deal of heat, enabling organisms to rid themselves of excess body heat through evaporative cooling.
| Density | 1.00 gm/cm3 |
| Temperature at max. density | 3.98°C |
| Melting point | 0.0°C |
| Boiling point | 100.0°C |
| Specific heat | 1 cal/g/°C |
| Heat of vaporization | 586 cal/g |
Related category
• INORGANIC CHEMISTRY
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