Water Chemistry Definition and Properties

Water Chemistry Definition and Properties Of all the molecules in the universe, the one most important to humanity is water: Water Definition Water is a chemical compound consisting of two hydrogen atoms and one oxygen atom. The name water typically refers to the liquid state of the compound. The solid phase is known as ice and gas phase is called steam. Under certain conditions, water also forms a supercritical fluid. Other Names for Water The IUPAC name for water is, actually, water. The alternative name is oxidane. The name oxidane is only used in chemistry as the mononuclear parent hydride to name derivatives of water. Other names for water include: Dihydrogen monoxide or DHMOHydrogen hydroxide (HH or HOH)H2OHydrogen monoxideDihydrogen oxideHydric acidHydrohydroxic acidHydrolHydrogen oxideThe polarized form of water, H OH-, is called hydron hyroxide. The word water comes from the Old English word wà ¦ter  or from the Proto-Germanic watar or German Wasser. All of these words mean water or wet. Important Water Facts Water is the main compound found in living organisms. Approximately 62 percent of the human body is water.In its liquid form, water is transparent and nearly colorless. Large volumes of liquid water and ice are blue. The reason for the blue color is the weak absorption of light at the red end of the visible spectrum.Pure water is flavorless and odorless.About 71 percent of the Earths surface is covered by water. Breaking it down, 96.5 percent of the water in the Earths crust is found in oceans, 1.7 percent in ice caps and glaciers, 1.7 percent in ground water, a small fraction in rivers and lakes, and 0.001 percent in clouds, water vapor, and precipitation.Only about 2.5 percent of the Earths water is fresh water. Nearly all of that water (98.8 percent) is in ice and ground water.Water is the third most abundant molecule in the universe, after hydrogen gas (H2) and carbon monoxide (CO).The chemical bonds between hydrogen and oxygen atoms in a water molecule are polar covalent bonds. Water readily forms hydrogen bonds with other water molecules. One water molecule may participate in a maximum of four hydrogen bonds with other species. Water has an extraordinarily high specific heat capacity [4.1814 J/(g ·K) at 25  Ã‚ °C] and also a high heat of vaporization [40.65  kJ/mol or 2257  kJ/kg at the normal boiling point]. Both of these properties are a result of hydrogen bonding between neighboring water molecules.Water is nearly transparent to visible light and the regions of the ultraviolet and infrared spectrum near the visible range. The molecule absorbs infrared light, ultraviolet light, and microwave radiation.Water is an excellent solvent because of its polarity and high dielectric constant. Polar and ionic substances dissolve well in water, including acids, alcohols, and many salts.Water displays capillary action because of its strong adhesive and cohesive forces.Hydrogen bonding between water molecules also gives it high surface tension. This is the reason why small animals and insects can walk on water.Pure water is an electrical insulator. However, even deionized water contains ions because water unde rgoes auto-ionization. Most water contains trace amounts of solute. Often the solute is salt, which dissociates into ions and increases the conductivity of water. The density of water is about 1 gram per cubic centimeter. Regular ice is less dense than water and floats on it. Very few other substances exhibit this behavior. Paraffin and silica are other examples of substances that form lighter solids than liquids.The molar mass of water is  18.01528  g/mol.The melting point of water is  0.00  Ã‚ °C (32.00  Ã‚ °F; 273.15  K). Note the melting and freezing points of water may be different from each other. Water readily undergoes supercooling. It can remain in liquid state well below its melting point.The boiling point of water is  99.98  Ã‚ °C (211.96  Ã‚ °F; 373.13  K).Water is amphoteric. In other words, it can act as both and acid and as a base. References Braun, Charles L.; Smirnov, Sergei N. (1993-08-01). Why is water blue?. Journal of Chemical Education. 70 (8): 612.  Gleick, P.H., ed. (1993). Water in Crisis: A Guide to the Worlds Freshwater Resources. Oxford University Press.Water in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD).