discuss the properties of water including surface tension, adhesion, cohesion, specific heat, and heat of vapo
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You should be able to find the answers on these web pages:\n\nhttp://www.uni.edu/~iowawet/H2OProperties.html\nhttp://dl.clackamas.cc.or.us/ch106-06/thermal.htm\nhttp://daphne.palomar.edu/jthorngren/latent.htm
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viscosity is the stickness/thickness of liquid. It is a constant for each liquid in relation to its temperature because when you heat stuff up, it flows a little better.\n\nexample: if you heat up honey it goes from being really viscous to flowing better than water at near boling temperatures. You can also look at metals this way too, if you met metal, the hotter the metal, the faster it will flow to where  ever you are trying to get it to go. Lava is a good example as well.
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Off the top of my head:\n\nFlow rate, pressure, viscosity, temperature, rate, calorimetry, optics, nuclear phys., tension, stress & strain, surface tension, acoustics, magnetism, elctricity.
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A water molecule contains two elements: hydrogen and oxygen. Both elements have different electronegativities, which is a fancy word meaning how well they can attract electrons. Since oxygen has a higher electronegativity, it forces the electrons of the water molecule toward itself, giving the oxygen element a slight negative charge and the hydrogen atoms slight positive charges.\nBasically speaking, water itself is somewhat charged. This makes water what is called a polar molecule and allows it to conduct electricity. This also accounts for how well water adheres to itself (cohesion).\nHowever, this polarity is relatively small.
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Water, correct? 2 atoms of oxygen... 1 atom of hydrogen. It's a rare 3 sided molecule.\n\nSurface tension is easily demonstrated by filling a glass of water right to the very top, then adding just a few more drops. You will see the water "rise" above the rim of the glass, yet not spill.\nYou can magnetize a pine needle, by rubbing it with a magnet from one end to the other, over and over, and it will float on the water, never getting wet, and behave as a compass, one end pointing north, the other pointing south.\n\nWithout surface tension,  many forms of life would not exist.
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Vapor Pressure\n\n\n\nOne of the physical properties that we can measure for liquids and solids is vapor pressure. Vapor pressure is defined as the pressure of the vapor of a liquid or solid in equilibrium with the liquid or solid state. Generally liquids have higher vapor pressures than solids. \n\nYou can look at vapor pressure from a molecular view. Let's say that we have a glass of liquid water. The only molecules of water that have the highest probability of escaping into the vapor phase are the surface molecules. Molecules of water below the surface have forces between the molecules called Intermolecular Forces that are stronger then these forces exert on surface molecules. This is simply because there are more molecules surrounding the interior water molecules than what surround the surface molecules. As a result, water molecules can only escape at the surface. The physical process by which vapor pressure occurs is referred to as evaporation. There are several things that could influence the rate at which liquid molecules become vapor. \n\n\nPolar Nature of the molecules \nIf the molecules are non-polar then there will be weaker intermolecular forces keeping them in the liquid state. Non-polar substances like hydrocarbons have weaker forces between them and therefore their vapor pressures are characteristically higher than polar substances. Polar substances have dipolar molecules with positive and negative ends to the molecules. The intermolecular forces are much stronger and the liquid molecules are kept in the liquid state easier. Polar substances tend to have lower vapor pressures at a given temperature. The rate of evaporation for non-polar molecules would be generally greater than polar molecules in comparison. \n\n\nSurface area \nSurface area would play apart since evaporation is a "surface phenomena" as was mentioned above. It stands to reason that if we increase the surface area of a liquid that we will increase the number of surface molecules and therefore more molecules will be able to escape into the vapor state. This is why when we want to evaporate something we place it on a watch glass or in a beaker and not in a test tube where the surface area is much more restricted. Increasing the surface area will increase the rate at which something will evaporate. Unlike the polar nature of the molecules, changing the surface area does not affect the vapor pressure itself. \n\n\nTemperature \nTemperature increases increase the available Kinetic Energy present. The more energy that the surface molecules can absorb the faster they will be able to overcome the intermolecular forces acting upon them and the sooner they will become vapor. Increasing the temperature increases the rate at which something will evaporate. Like the polar nature of molecules it also affects the vapor pressure. Increasing the temperature of a liquid increases the vapor pressure logarithmically. \n\n\nThe concentration of vapor molecules above the liquid \nIncreasing the number of vapor molecules above the liquid will leave less room for further vapor molecules. This has a depressing effect on the rate at which the liquid evaporates. Reducing the concentration of vapor molecules at the surface will increase the rate. That is why we turn on a ventilation fan under the vent hood of a lab when we wish to evaporate something quickly. In addition, clothes hanging on a clothes line dry faster on a windy day then on a still day. \n\n\nThe Vapor Pressure of a liquid at a given temperature is a characteristic property of that liquid. It can be measured by using a pressure instrument known as a manometer. Vapor pressure of a liquid is intimately connected to another physical property known as boiling point, but that will be another topic for discussion. \n\nVapor Pressures are influenced by Temperature logarithmically and this relationship is defined with the Clausius Clapyron Equation: \n\nLog P2 / P1 = Delta H vaporization [ 1 / T1 - 1/T2
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chemical properties:  high electro negativity\nphysical properties:  it's a halogen
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http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/water.html\n\nsee the picture here!
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water-watery\n\ndemon-demonic\n\nevil-evil\n\ngoodness-good\n\nbeauty-beautiful\n\ngrace-graceful\n\nstone-stony\n\nliquid-liquid\n\nnausea-nauseous\n\ncold-cold\n\nheat-hot\n\nelectricity-electric
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air and water vapor\n\ntheir volume depends on temperature and pressure
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http://tigger.uic.edu/~mansoori/Thermodynamic.Data.and.Property_html\nhttp://www.aii-usa.com/proezgc/database.htm\nhttp://theweatherprediction.com/thermo/images/\nhttp://www.lib.utexas.edu/chem/info/thermo.html
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Water is extremely an exceptional molecule consider to it size or molecular weight (18). It has amazing properties such as high in its boiling point (100 oC), high heat capacity, high in heat of evaporation, etc. \n***All of these wonderful properties are due to something called Hydrogen bonding. These bond is like microscopic wire (very strong wire) that ties one water molecule to four other water molecules togather very tightly. Therefore to heat water up is the same thing as loosen these wires. Thus it requires a lot of energy (heat) to do that; that why water, the H2O, has a terrific heat capacity.\n***There are not any other substances that a better heat capacity than water within its size.
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4°C, the temperature of maximum density for water.\n\nBelow that temperature, and the water starts to expand as the crystalline lattice begins to form.  Above that temperature, the density drops because of the increased molecular vibrational activity.
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vapor\n\ngas\n\nliquid\n\nvapor\n\nliquid\n\n\nnot 100% sure but i'm pretty good at science
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X2O\n\nExamples:\nH2O => Water
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Liquid-Gas... water evaporating.  As energy (heat) is added to water molecules, they begin to move more rapidly and break apart from each other with more ease.  They are then able to become completely separate to the point that they can float up into the atmosphere.\n\nLiquid-Solid... water freezing.  As energy (heat) is removed from water molecules, the binding together of two water molecules becomes more frequent.  At water's freezing temperature, the water molecules become binded together so that they are stuck together and don't move nearly as much (they still vibrate, though).
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The mean van der Waals diameter of water has been reported as identical with that of isoelectronic neon (2.82 Å) [112]. Molecular model values and intermediate peak radial distribution data indicates however that it is somewhat greater (~3.2Å). The molecule is clearly not spherical, however, with about a ±5% variation in van der Waals diameter dependent on the axis chosen; approximately tetrahedrally placed slight indentations being apparent opposite the (putative) electron pairs.