What are some examples of properties of water?
Properties of water:
Properties of water, nature of water and water as an excellent solvent all these properties are listed below:
Water, so commonplace and abundant on Earth, is nevertheless an almost unique substance:
it has very astonishing chemical and physical properties and behaves in bizarre ways. Ice, liquid or water vapor: discover the mysteries of water.
Do you think you know everything about the H 2 O?
However, recent studies have just shown thatwater can coexist in two different states! Have you never seen an bar float on molten iron?
The ice cubes float above the liquid water! In short, water is far from being any.
Ice is less dense than liquid water:
While almost all materials are denser in thestate than in the liquid state, and ice cubes float in a glass.
Usually, when a substance freezes, its molecules come together. But the water presents an: its maximum density is reached at 4 ° C and begins to decrease below. This means that, for the same , there are fewer molecules in an ice cube than in liquid water: it is therefore lighter.
Water is present in nature in its three states: liquid, solid, gas
It is easy to observe ice, liquid water and water vapor in nature. On the other hand, you are unlikely to find gold vapor or– the solid form of (CO 2 ) – while strolling outside!
This strange property comes in particular from the particularly hightemperature of water: alone evaporates for example at -183 ° C, but the between the water molecules oblige to provide much more to switch to the vapor state.
Hot water freezes faster than cold water:
Place an ice cube tray full of hot water in the freezer and your ice cubes will be ready faster than with cold water. This curious phenomenon, called the ”“, could have several explanations.It could be due to evaporation which decreases the of water and consumes , which favors its cooling.
Hot water would also be less sensitive to theeffect which allows a liquid to remain solid even when its temperature has fallen below its threshold .
Other hypotheses are based on heat transfers (currents would be greater in hot water) or the modification of between water molecules (narrowing of betweenoxygen and hydrogen ).
There are two forms of liquid water:
Lately, several studies have suggested that: one at low density, in which molecules form numerous hydrogen bonds with their neighbors, which keeps them away from each other, and another of high density, where the molecules “pile up” on top of each other and can therefore come together.
While it is relatively common to find several forms of solids for the same, it is much rarer for a liquid. The only known case to date is , whose helium II liquid form can crawl along surfaces!
Water is an excellent solvent:
You only have to watch a piece ofmelt in your coffee or powdered salt dissolve in your saucepan to realize it: water is an excellent .
Conversely, it is impossible to dissolve salt in oil or: it will remain solid at the bottom of the container.
This dissolution capacity is explained by the polar nature of water which tends to attract ionic molecules (with positively or negatively charged).
When, for example, salt (NaCl) is put in water, the water molecules will dissociate the chloride ions and theions ; an formsNa + + Cl-.
Likewise, water easily dissolves other polar molecules such as sugars or ethanol.
Water can be both liquid and solid:
Researchers recently demonstrated the existence of ”“, a semi-liquid and solid water that becomes conductive like a .
Under very highand temperature conditions, hydrogen bonds are destroyed, leaving hydrogen ions to circulate freely in the of oxygen atoms, which remain organized as if they were “frozen”.
Water can also be in supercooled form, where it remains liquid down to temperatures of -48 ° C before suddenly freezing upon contact with another surface.
Water shrinks as it melts:
The vast majority of substances occupy more space in the liquid state – when the molecules are disordered – than in the solid state – where the molecules have an organized structure.
Water is a special case:
it occupies about 10% more volume when it freezes. This oddity called “” is explained by the particular structure of the water molecule, where the hydrogen bonds assemble in a hexagonal network, leaving a lot of room between the molecules.
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