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Water Molecules Hydrogen Bonding
Water is the source of all things, and the hydrogen bonding between its molecules is wonderful. Water molecules are composed of hydrogen atoms and oxygen atoms. Hydrogen atoms are slightly positively charged, and oxygen atoms are slightly negatively charged.
Therefore, the hydrogen atom of a water molecule and the oxygen atom of a neighboring water molecule attract each other due to electric charges, thus forming a hydrogen bond. Although this hydrogen bond is weaker than the chemical bond, it has far-reaching effects on the many properties of water.
Because of hydrogen bonds, water has a quite high boiling point. If there are no hydrogen bonds, water is regarded as a gas at room temperature and pressure. It is precisely because of the existence of hydrogen bonds that more energy is required to overcome its binding in order to make the water molecules break free from the liquid phase and turn into a gaseous state, so the boiling point of water can be maintained at 100 degrees Celsius.
Furthermore, the surface tension of water is also closely related to hydrogen bonds. On the surface of water, water molecules attract each other due to hydrogen bonds, forming a layer of elastic film-like structure, which is called surface tension. This property allows water to form water droplets on the surface of small objects without easily spreading out.
And the density change of hydrogen bonds in water also plays a key role. In the liquid state, water molecules are connected to each other due to hydrogen bonds and are arranged relatively tightly. However, when the water temperature drops below the freezing point and water freezes, water molecules form a regular tetrahedral structure due to hydrogen bonds, and the molecular spacing increases, resulting in the density of ice being smaller than that of liquid water. This is also the reason why ice floats on the water surface. In conclusion, hydrogen bonding between water molecules plays an indispensable role in both the natural world and life activities.
Therefore, the hydrogen atom of a water molecule and the oxygen atom of a neighboring water molecule attract each other due to electric charges, thus forming a hydrogen bond. Although this hydrogen bond is weaker than the chemical bond, it has far-reaching effects on the many properties of water.
Because of hydrogen bonds, water has a quite high boiling point. If there are no hydrogen bonds, water is regarded as a gas at room temperature and pressure. It is precisely because of the existence of hydrogen bonds that more energy is required to overcome its binding in order to make the water molecules break free from the liquid phase and turn into a gaseous state, so the boiling point of water can be maintained at 100 degrees Celsius.
Furthermore, the surface tension of water is also closely related to hydrogen bonds. On the surface of water, water molecules attract each other due to hydrogen bonds, forming a layer of elastic film-like structure, which is called surface tension. This property allows water to form water droplets on the surface of small objects without easily spreading out.
And the density change of hydrogen bonds in water also plays a key role. In the liquid state, water molecules are connected to each other due to hydrogen bonds and are arranged relatively tightly. However, when the water temperature drops below the freezing point and water freezes, water molecules form a regular tetrahedral structure due to hydrogen bonds, and the molecular spacing increases, resulting in the density of ice being smaller than that of liquid water. This is also the reason why ice floats on the water surface. In conclusion, hydrogen bonding between water molecules plays an indispensable role in both the natural world and life activities.
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