Water is the true source of life on earth, participating in countless biological processes and being an integral component of them. This is possible thanks to its unique properties such as:
In our blog, we often refer to certain properties of water, but rarely delve into the physics and chemistry of it. Today, we will try to break it out for you in a simple language why water is not only the "source of life on earth", but also a truly special chemical substance.
Physical Properties of Water
Pure water has no taste or odor and is in a liquid state at normal temperature (20°C).
"Water" is a trivial name; the chemical compound is called hydrogen oxide. From the name, we can understand that it contains hydrogen and oxygen ions that are connected by a so-called covalent bond.
The hydrogen atom has a valence (ability to form bonds) of 1, and the oxygen atom has a valence of 2. This is why the formula for water is H2O. Also, each water molecule can form up to four hydrogen bonds (two hydrogen and two oxygen). All anomalies of the physical properties of water are related to these bonds - water has a relatively high boiling point (100°C). If there were no hydrogen bonds, water would boil at a temperature of -80°C and freeze at -100°C. This structure allows us to see water in three states (solid, liquid, gas) in the natural environment. Here, we just briefly described the physical properties of water, if you want to find out more about it, you are welcome to read our previous article where we’ve talked more about how water boils and freezes, as well as the differences between heavy water.
Chemical Properties of Water
Let's delve deeper into the chemical properties of water and how they relate to the indicators of water on Earth.
To understand processes in the environment that involve water as a component of reactions, it is important to be familiar with the main chemical properties of H2O. These properties can be summarized in a short list.
Interaction of water with simple substances
The reaction between alkaline and alkaline-earth metals with water can be quite vigorous, producing heat and occasionally even light. For instance, sodium, potassium, and calcium are able to move and even "jump" on the surface of water.
2Na + 2H2O = H2 + 2NaOH
Less active metals react either upon heating or not at all, for example, iron:
3Fe + 4H2O = 4H2+ Fe3O4 (only upon heating)
These reactions do not occur naturally, but the corrosion reaction that occurs when air is added to water is very common.
4Fe + 3O2 + 6H2O ➝ 4Fe(OH)3.
This equation describes the formation of rust on iron surfaces. Similar processes can also occur with copper, zinc, and their alloys. Reactions with non-metals occur exclusively upon heating or other types of influence.
Reactions with non-oxides
Water in nature often comes into contact with carbon dioxide, as well as sulfur and nitrogen oxides, which are components of exhaust gases, through this mechanism:
SO2 + H2O = H2SO4.
As a result of these processes, acid rain is formed.
Photosynthesis
Photosynthesis is a remarkable reaction that enables plants to convert carbon dioxide and water into nutrients, including starch and glucose, using sunlight as an energy source.
The chemical equation for photosynthesis is:
6nCO2 + 5nH2O → (C6H10O5)n + 6nO2
This equation summarizes the process by which plants use water to create carbohydrates and release oxygen. As such, photosynthesis is a critical process that sustains life on Earth by generating oxygen and providing the foundation for many food chains in ecosystems.
Water as an ideal solvent
Water is a versatile solvent that facilitates many invisible processes, which are often the most fascinating ones. However, it is rare to find water in its purest form in nature, as it typically contains inorganic salts, gases, and a diverse range of organic substances. The natural hardness of water is a result of its movement through rocks, which allows it to become saturated with minerals. Depending on the composition of the rocks, their solubility, and the temperature of the environment, certain concentrations of their ions can dissolve in water. Carbonates, sulfates, nitrates of calcium, magnesium, sodium, potassium, and other cations are commonly found in such rocks. Minerals such as gypsum (CaSO4), dolomite (CaCO3 • MgCO3), and limestone (CaCO3) are likely the primary contributors to water hardness.
Dissolved iron and manganese are typically present in natural borehole waters, as soluble iron salts tend to be found in areas lacking air. Their sources are often magnetic, brown, red iron ores, magnesite, and similar materials. Hydrogen sulfide is also present in groundwater, where it is produced through chemical processes involving organic substances. In the air, it readily oxidizes to elemental sulfur and precipitates, often without being visible to the human eye.
Natural surface waters contain dissolved oxygen and nitrogen-containing components that result from the vital activity of microorganisms, such as ammonia, nitrites, and nitrates, which can easily convert into one another. Proteins and amino acids can also be found in water bodies. Anthropogenic activities introduce the most toxic pollutants into the water, such as heavy metal salts, industrial organic products, and nitrates and phosphates from fertilizers.
Various reactions occur constantly in water, including exchange processes that cause scale consisting of calcium carbonate to precipitate. Additionally, oxidizing-reducing reactions can result in borehole water acquiring rusty iron sludge or sediment.
