General
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|
|---|---|
| Name | Water |
| Chemical formula | H2O |
| Appearance | Colourless liquid |
Physical
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|
| Formula weight | 18.01528 amu |
| Melting point | 273 K (0 °C) |
| Boiling point | 373 K (100 °C) |
| Critical temperature | 674 K |
| Critical Pressure | 22.1x10^6?? Pa |
| Density | 1.0 ×103 kg/m3 |
Thermochemistry
|
|
| ΔfH0gas | -241.83 kJ/mol |
| ΔfH0liquid | -285.83 kJ/mol |
| ΔfH0solid | -291.83 kJ/mol |
| S0gas, 1 bar | 188.84 J/mol·K |
| S0liquid, 1 bar | 69.95 J/mol·K |
| S0solid | 41 J/mol·K |
Safety
| |
| Ingestion | Necessary to life; excessive consumption can cause headache, confusion, and cramps, and can be fatal in athletes |
| Inhalation | Non-toxic. Can dissolve surfactant of lungs. Suffocation in water is called drowning. |
| Skin | Prolonged immersion may cause flaking (desquamation). |
| Eyes | Not dangerous. |
| SI units were used where possible. Unless otherwise stated, standard conditions were used. | |
O H H <--- a water molecule
The solid state of water is known as (water) ice; the gaseous state is known as steam. The units of temperature (formerly the degree Celsius and now the Kelvin) are defined in terms of the triple point of water, 273.16 K (0.01 °C) and 611.2 Pa, the temperature and pressure at which solid, liquid, and gaseous water coexist in equilibrium.
At temperatures greater than 647 K and pressures greater than 22.064 MPa, a collection of water molecules assumes a supercritical condition, in which liquid-like clusters float within a vapor-like phase.
A body of water is a term for an ocean, sea, lake, river, stream, canal, pond, or the like. See water (resource) for information about fresh water supplies. See also beach, ferry, pier.
Chemists sometimes jokingly refer to water as dihydrogen monoxide or DHMO (see http://www.dhmo.org/),General
An important feature of water is its polar nature. The water molecule forms an angle, with hydrogen atoms at the tips and oxygen at the vertex. Since oxygen has a higher electronegativity than hydrogen, the side of the molecule with the oxygen atom has a partial negative charge, relative to the hydrogen side. A molecule with such a charge difference is called a dipole. The charge differences cause water molecules to be attracted to each other (the relatively positive areas being attracted to the relatively negative areas) and to other polar molecules. This attraction is known as hydrogen bonding.
This relatively weak (relative to the covalent bonds within the water molecule itself) attraction results in physical properties such as a very high boiling point, because a lot of heat energy is necessary to break the hydrogen bonds between molecules. For example, Sulphur is the element below oxygen in the periodic table, and its equivalent compound, hydrogen sulphide (H2S) does not have hydrogen bonds, and though it has twice the molecular weight of water, it is a gas at room temperature. The extra bonding between water molecules also gives liquid water a large specific heat capacity.
Hydrogen bonding also gives water an unusual behaviour when freezing. As with most other materials, the liquid becomes denser with lowering temperature. However, unlike most other materials, when cooled to near freezing point, the presence of hydrogen bonds means that the molecules, as they rearrange to minimise their energy, form a structure that is actually of lower density: hence the solid form, ice, will float in water i.e. water expands as it freezes (most other materials shrink on solidification).
Liquid water reaches its highest density at a temperature of 4 °C. This has an interesting consequence for water life in winter. Water chilled at the surface becomes denser and sinks, forming convection currents that cool the whole water body, but when the temperature of the lake water reaches 4°C, water on the surface, as it chills further, becomes less dense, and stays as a surface layer which eventually forms ice. Since downward convection of colder water is blocked by the density change, any large body of water frozen in winter will have the bulk of its water still liquid at 4°C beneath the icy surface, allowing fish to survive. (this is one of the principal examples of finely-tuned physical properties that support life on Earth that is used as an argument for the Anthropic Cosmological Principle).
Another consequence is that ice will melt if sufficient pressure is applied.
Water is also a good solvent due to its polarity. The solvent properties of water are vital in biology, because many biochemical reactions take place only within aqueous solutions (e.g., reactions in the cytoplasm and blood). In addition, water is used to transport biological molecules.
When an ionic or polar compound enters water, it is surrounded by water molecules. The relatively small size of water molecules typically allows many water molecules to surround one molecule of solute. The partially negative dipoles of the water are attracted to positively charged components of the solute, and vice versa for the positive dipoles.
In general, ionic and polar substances such as acids, alcohols, and salts are easily soluble in water, and nonpolar substances such as fats and oils are not.
Nonpolar molecules stay together in water because it is energetically more favorable for the water molecules to hydrogen bond to each other than to engage in van der Waals interactions with nonpolar molecules.
An example of an ionic solute is table salt; the sodium chloride, NaCl, separates into Na+ cations and Cl- anions, each being surrounded by water molecules.
The ions are then easily transported away from their crystalline lattice into solution.
An example of a nonionic solute is table sugar.
The water dipoles hydrogen bond to the dipolar regions of the sugar molecule and allow it to be carried away into solution.
The strong hydrogen bonds give water a high cohesiveness and, consequently, surface tension. This is evident when small quantities of water are put onto a nonsoluble surface and the water stays together as drops. This feature is important when water is carried through xylem up stems in plants; the strong intermolecular attractions hold the water column together, and prevent tension caused by transpiration pull.
Other liquids with lower surface tension would have a higher tendency to "rip", forming vacuum or air pockets and rendering the xylem vessel inoperative.
Pure water is actually an insulator, meaning that it does not conduct electricity well. Because water is such a good solvent, it often has some solute dissolved in it, most frequently salt.
If water has such impurities, then it can conduct electricity well.
Water can be split into its constituent elements, hydrogen and oxygen, by passing a current through it. This process is called electrolysis.
Water molecules naturally disassociate into H+ and OH- ions, which are pulled toward the cathode and anode, respectively.
At the cathode, two H+ ions pick up electrons and form H2 gas. At the anode, four OH- ions combine and release O2 gas, molecular water, and four electrons. The gases produced bubble to the surface, where they can be collected.
Purified water is needed for many industrial applications, as well as for consumption. Humans require water that does not contain too much salt or other impurities. Common impurities include chemicals or harmful bacteria. Some solutes are acceptable and even desirable for perceived taste enhancement. Water that is suitable for drinking is termed potable water.
Six popular methods for purifying water are:
Wasting water is the abuse of water, i.e. spending it unnecesarily. An example is to dump the river water to the sea and to not allow the use in other places. Also, in homes, water may be wasted if the toilet is flushed unnecessarily.
Water is one of the four classical elements along with fire, earth and air, and was regarded as the ylem, or basic stuff of the universe. Water was considered cold and moist. In the theory of the four bodily humours, water was asssociated with phlegm.
Water was also one of the Chinese five elements along with air, fire, wood, and metal.
In the United States water law is divided between two legal doctrines: riparian water rights, used in the eastern and southern states where there is an abundance of water and the appropriation doctrine (or Colorado doctrine) used in the arid western states.
UNESCO's World Water Development Report (WWDR, 2003) from its World Water Assessment Program indicates that in the next 20 years the world is facing an unprecedented lack of drinking water.
The quantity of water available to everyone is predicted to decrease by 30%.
The causes are contamination, global warming and political problems.
40% of the world's inhabitants have insufficient fresh water for minimal hygiene.
More than 2.2 million people died in 2000 from illnesses related to the consumption of contaminated water.
The report indicates large global disparities in the raw volume of available water: from 10 m³ per person per year in Kuwait to 812.121 [m³?] in French Guiana.
However, richer countries such as Kuwait can more easily cope with low water availability.
The dipolar nature of water
Water as a solvent
Cohesion and surface tension
Conductivity
Electrolysis
Reactivity
Chemically, water is amphoteric: able to act as an acid or base. Occasionally the term hydroxic acid is used when water acts as an acid in a chemical reaction. At a pH of 7 (neutral), the concentration of hydroxide ions (OH-) is equal to that of the hydronium (H3O+) or hydrogen ions (H+) ions. If the equilibrium is disturbed, the solution becomes acidic (higher concentration of hydronium ions) or basic (higher concentration of hydroxide ions).Theoretical vs experience
In theory, pure water has a pH of 7. In practice, pure water is very difficult to produce. Water left exposed to air for any length of time will rapidly dissolve carbon dioxide, forming a solution of carbonic acid, with a limiting pH of ~5.7. (reference: Kendall, J. (1916), Journal of the American Chemical Society, 38(11), 2460-2466)Purifying water
Wasting Water
Mythology
Water rights and development
Body of water
See also
External links