Water is a polar molecule composed of one oxygen atom bonded to two hydrogen atoms. It is essential in all forms of life systems. It naturally exists in three states for instance, in a liquid state, solid state and gas state. These states are mainly attributed by temperature difference subjected to this water atom, hence leading to the various water phases. This short paper seeks to elaborate more on the number of bonds made on water phases, their differences and the unique properties of water in general.
As mentioned above there are various phases of water with their respective number of bonds. These include; solid phase, gaseous phase, and the liquid phase. In the solid phase, there are many hydrogen bonds compared to the covalent bonds. There are about four hydrogen bonds in round every oxygen atom. The kinetic energy of the molecules brings about the difference between ice and water. These water molecules are held together by the hydrogen bonds to form a crystal lattice, ice. These crystals are less dense in comparison to the liquids due to the spaces between the molecules hence the ice floating and water sinking.
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In the liquid phase, many of the water molecules have no less than one hydrogen bond to the nearby water molecules with no open molecules in suitable conditions. In the last phase being the gaseous phase, water molecules are not bound together by any bonds, they move about swiftly, water vapor. A water molecule has got an oxygen atom bound together with a hydrogen atom covalently; the two share an electron which results to a polar molecule leading to the formation of hydrogen bonds. It is more of the bond strength as compared to the number that creates the difference between these atoms that vary from one phase to the other.
