Zinc and zinc hydroxide: properties, application and role in nature

It's no secret that zinc and zinc hydroxide are widely used by modern scientists. And the spectrum of their use directly depends on physical and chemical properties.

It is interesting that an alloy of zinc with copper was used by the ancient Egyptians, and later in the Roman Empire. But here zinc in its pure form could not be isolated for many years. Only in 1746 A. Marggraf first received this metal in its pure form. In the seventeenth century, zinc smelting was already carried out on an industrial scale.

Zinc: Chemical properties and brief description

Zinc is a metal of medium hardness. It is interesting that at low temperatures it is rather fragile. But at a temperature of 100 to 150 degrees Celsius the metal becomes plastic - it produces sheets or even foil with a thickness of much less than a millimeter.

From a chemical point of view, zinc is an atom with an oxidation state of +2. This is a fairly active metal, which participates in the reactions as a reducing agent. Interestingly, in air, at a temperature of up to 100 degrees, zinc quickly dims, its surface is covered with a thin film of carbonates. If the air is moist and contains a large amount of carbon dioxide, the metal quickly collapses.

Zinc burns with a blue flame in the presence of oxygen or during heating - in such cases, the combustion process is accompanied by the formation of white smoke (this is metal oxide).

Zinc reacts with both simple elements and acids and some bases, forming salts and zinc hydroxide, respectively.

To date, we know about 66 minerals that contain zinc - they are the main source of industrial metal production. As an example, one can mention calamites, zincites, willemite, frank-lynith and smithsonite.

Zinc hydroside: physical and chemical properties

Zinc (II) hydroxide is also of great importance, as it is used in various branches of the chemical industry. Under normal conditions, this substance is a colorless small crystal, which practically does not dissolve in water. The hydroxide formula is as follows:

Zn (OH) 2

It should also be noted that this substance has relatively strong amphoteric properties. Zinc hydroxide reacts more actively with acids, entering a neutralization reaction and forming salts and water. For example:

Zn (OH) 2 + H2SO4 = ZnSO4 +2H2O

Nevertheless, zinc hydroxide reacts with alkalis, forming complex salts and water. For example:

Zn (OH) 2 + 2 NaOH = Na2ZnO2 + 2H2O

It is worth noting that when heated, the substance decomposes to form oxide and water:

Zn (OH) 2 = ZnO + H2O

As for the field of application, the hydroxide is used in the chemical industry to produce various compounds of zinc, in particular its salts.

Zinc and its application

It's not a secret for anyone that zinc is widely used as an anti-corrosive substance coated with steel and iron. In addition, a huge amount of mined metal is used for the production of brass and bronze.

Interestingly, in dry batteries, zinc is used as an anode, and also serves as a container. In addition, this metal is used during the separation of precious metals (for example, gold) from lead. Some zinc compounds are considered to be common semiconductor materials.

Zinc in the living body

In fact, it is difficult to overestimate the role of zinc in the vital activity of any living organism, including man. Despite its rather low content, it is a part of important enzymes, participates in the process of protein synthesis, cellular respiration, etc. Zinc is also responsible for the development of the skeleton of the fetus. It is proved that in case of insufficient amount of this mineral, a delay in sexual development and the appearance of dwarfism are possible.