How do the molecules of water evaporate.?
153248
The molecules of water do not actually "change."  They vibrate faster as they get warmer.  If they are vibrating slowly enough, the molecules are packed closely together into the solid form of water we call ice.  As they move faster they become the liquid state we commonly call water.  When they are vibrating fast enough they "evaporate" into the gaseous state.  \nIn any of these 3 states they are still molecules of water, they are just moving around at different speeds.
514471
There is a difference between boiling and evaporating.\nAt 100 degrees water starts boiling. The temperature can not rise because al the energy you put in is used by the molecules to 'escape' and the water to change into gas. That is why damping water cools off. But water kan evaporate also at lower temperatures because molecules can 'escape'. The molecules are not as volatile as at 100 degrees, but they are volatile. Winds helps because the dryer the air, the easier it is to escape. Is the air humid, than the molecules can be caught in the water again. \nSorry I am not a chemist but I think this is it essentially.
771899
When a solid is heated, the molecules become active and the bonds between them come looser, this is how a solid becomes a liquid.\nThe warmer the liquid becomes, the molecular bonds become even less connected and the liquid becomes a gas. (evaporation)\n\nWhen a gas is cooled, the molecular bonds change and they become tighter. or closer together causing the gas to turn back into a liquid (condensation).  And as the molecules become tighter still, then the liquid turns back into a solid.\n\nFreezing and melting points change per molecule.
983710
H2SO4 will dehydrate and remove water.\n\n\n(CH3)2 CH - CH2-CH=CH-(CH3)2
250821
It evaporates.  Remember your body temperature is very warm (98.6 deg).  Your skin is an organ that is designed to protect your body by keeping things out.  You may get a little absorption on the outer most layer, but even it will eventually evaporate.
188359
Water always evaporates no matter what is its temperature. Evaporation is NOT related to heat. Even at 1C it can evaporate. Water boils at 100C but evaporation occurs at every temperature.
119086
The molecules of water are closer together and constantly moving, whereas the molecules of ice are in a crystal lattice, meaning they're in a rigid formation. When water freezes, the molecules spread out a little more to form the crystal lattice. Since density is mass over volume, and ice has takes up more volume than water, the density of ice is lesser than that of water. Which makes ice float on water.
864632
water is poler b/c the hydrogen atoms bond to the oxygen words one side, giving that side a negative charge, while the opposite side has a posative one.\n\nsuger and salt r soluble in water\n\nidk what doesn't desolve in water, sry
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This is a damn good question, and I’m going to do you the credit of assuming it’s your own and not a homework question.\n\nYou’re right, it’s odd that water can evaporate from an ocean at 25oC when by definition water doesn’t have enough energy to vaporise until it hits 100oC. The answer lies in the way that we define and measure temperature.\n\n“Temperature’ as we normally apply it, and as we apply it to ocean water, is simply a measure of the average velocity of the atoms and molecules. Or more simply when we say that water is at 25oC we are really saying that on average they are at 25oC. In reality that probably means something like  25% of the water molecules are at 5oC, 50% at 20oC, 24% at 30oC and the other  1% are at 100oC or even higher.\n\nThat tiny percentage of molecules that are at 100oC or higher, if they are on the surface, can escape the water body and fly ff into the air. That is how water manages to evaporate even when it is well below 100oC.\n\nEven more suprisingly you can see this happening even if the water is frozen. Even when the average temperature is below 0oC some individual molecules will still be at 100oC.Those molecules can evaporate, and you can watch an ice cube slowly shrink and vanish completely over time even though it never melts.
673911
If you could shrink 'way down and look at a single water molecule, you\nwould find that it is made of two hydrogen atoms and one oxygen atom.\nThey are arranged in a V-shape, with the oxygen at the point.  The result\nof this shape is that there is more negative charge at one end of the\nmolecule than the other (oxygen likes to have negative charge).  We call \nthis a POLAR molecule.\n\nOther polar molecules like salt and sugar and Kool-aid will dissolve in\nwater because the water molecule will be attracted to their charged ends.\nThe water molecule likes their charges so much that it will actually\nsurround the salt or sugar molecules, so that each one looks like a ball\nof water molecules.  We call this SOLVATION.  Since the salt molecule\nis surrounded now by water, it can't stick to other salt molecules, so\nit just sort of floats away.
953068
Evaporation is one of the two forms of vaporization. It is the process whereby atoms or molecules in a liquid state (or solid state if the substance sublimes) gain sufficient energy to enter the gaseous state. It is the opposite process of condensation.
883322
To break water molecule, energy is required.To create water molecule, energy is released.The amount of energy will be the same except that one is exothermic and the other is endothermic
942952
Water itself is a polar molecule, with a partial negative charge on the oxygen atom and a partial positive on the hydrogens. It allows water to hydrogen bond with other molecules.
271456
methyl alcohol has all 3 intermolecular forces: dispersion, dipole and hydrogen bonding. the way your question is worded is unusual. molecular forces don't cause liquids to evaporate, they prevent it.
211379
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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It's not actually evaporation.  It's sublimation; the change of phase is directly from solid to gas.
596688
Becaue water is polar and water molecules form hydrogen bonds with each other.