ZINC CHLORIDE (ZNCL2): STRUCTURE, PROPERTIES, PRODUCTION, USES - CHEMISTRY - 2025

The zinc chloride is an inorganic compound consisting of zinc or zinc element (Zn) and chlorine (Cl). Its chemical formula is ZnCl ₂. Zinc is in the +2 oxidation state and chlorine has a valence of -1.

It is a colorless or white crystalline solid. It is very soluble in water and absorbs it easily from the environment, which can be seen in the figure of the moistened solid shown below.

Somewhat hydrated solid ZnCl ₂ zinc chloride. User: Walkerma / Public domain. Source: Wikimedia Commons.

The zinc in this compound is biologically very important for humans, animals and plants, as it is involved in basic functions such as protein and fat synthesis.

For this reason, ZnCl ₂ is used as a nutritional supplement for animals and humans in cases of zinc deficiency, and as a micronutrient for plants.

It has bacteriostatic and astringent properties, and is widely used for these purposes in both human and veterinary medicine. It also eliminates pests such as fungi outdoors and is an intermediary for obtaining pesticides.

Among its many uses, it is used to treat cellulose and wool fibers in various processes, as well as to prepare them for coloring or printing. It also slows the combustion of wood.

Structure

ZnCl ₂ is an ionic compound made up of the Zn ²⁺ cation and two Cl ^- chloride anions that are joined by electrostatic forces.

Zinc Chloride. Author: Marilú Stea.

The zinc (II) ion has the following electronic structure:

1s ², 2s ² 2p ⁶, 3s ² 3p ⁶ 3d ¹⁰, 4s ⁰, in which it is observed that it lost both electrons of the 4s shell, so the configuration is stable.

The chloride ion has the following structure:

1s ², 2s ², 2p ⁶, 3s ² 3p ⁶, which is also very stable because it has complete orbitals.

The figure below shows how the ions are arranged in the crystal. The gray spheres represent zinc and the green spheres represent chlorine.

Structure formed by ions in the ZnCl ₂ crystal. CCoil / CC BY-SA (https://creativecommons.org/licenses/by-sa/3.0). Source: Wikimedia Commons.

Nomenclature

• Zinc (II) chloride
• Zinc dichloride

Properties

Physical state

Colorless or white crystalline solid. Hexagonal crystals.

Molecular weight

136.3 g / mol

Melting point

290 ºC

Boiling point

732 ºC

Density

2.907 g / cm ³ at 25 ° C

Solubility

Very soluble in water: 432 g / 100 g H ₂ O at 25 ° C, 614 g / 100 g H ₂ O at 100 ° C. Very soluble in hydrochloric acid (HCl), alcohol and glycerol. Fully miscible with acetone.

pH

Its aqueous solutions are acidic. A solution of 6 moles of ZnCl ₂ / L has a pH of 1.0.

Chemical properties

It is a hygroscopic and deliquescent compound, since in contact with the humidity of the environment it absorbs a lot of water. In water it hydrolyzes and has a tendency to form an insoluble basic zinc oxychloride salt.

It reacts with zinc oxide (ZnO) in water generating zinc oxychlorides that constitute an extremely hard cement-like material.

It is mildly corrosive to metals.

It is not flammable.

Biological role

Biologically, zinc is one of the most important elements. It has been recognized as essential to all forms of life.

In the human body, ZnCl ₂ provides Zn, which is essential for the synthesis of proteins, cholesterol and fats. Zinc in particular is important for the proper functioning of the immune system.

The zinc in ZnCl ₂ is important for cell division in living things. LadyofHats / Public domain. Source: Wikimedia Commons.

More than 25 zinc-containing proteins have been identified, and many of these are enzymes, necessary for cell division and growth, and for the release of vitamin A from the liver.

Zinc deficiency can lead to growth retardation, depressed mental function, anorexia, dermatitis, decreased immunity, diarrhea, and poor night vision, among other conditions.

Obtaining

Commercially, this compound is prepared by reacting aqueous hydrochloric acid with scrap, zinc waste or with the mineral that contains it. In this reaction, hydrogen gas (H ₂) is also produced.

Treating zinc with hydrogen chloride gas at 700 ° C gives high purity zinc chloride.

Zn + HCl → ZnCl ₂ + H ₂ ↑

Applications

In therapeutic treatments

It is a mild antibacterial or bacteriostatic, so it is used in douching to eliminate trichomonas or haemophilus infections. It is also used to treat calluses, as an astringent and in chemosurgery in skin cancer.

It is used as an astringent in some cosmetics such as refreshing skin lotions.

As a nutritional supplement

Due to its importance in various functions of the human body, ZnCl ₂ is administered orally as part of nutritional supplements and also in people who require parenteral nutrition.

ZnCl ₂ supplements are given to treat zinc deficiency in individuals who suffer from inadequate nutrition, have poor intestinal absorption, or a condition that increases the loss of this element from the body.

ZnCl ₂ supplements should be used when zinc is deficient. Author: Moakets. Source: Pixabay.

Healthy individuals acquire it through food.

It should be given at least 1 hour before meals or 2 hours after them, as some foods can prevent their absorption. In patients who have irritation in the stomach after ingesting the supplement, they should take it with meals, but in this way the zinc will be less bioavailable.

In veterinary applications

Its solutions have been used in animals as a caustic agent to burn or cauterize fistulas, which are connections between organs that are neither normal nor healthy; In the form of a paste, it is used to treat ulcers and in cancer chemotherapy.

Aqueous solutions of ZnCl ₂ are used to treat infections in the eyes of animals. Author: Mabel Amber. Source: Pixabay.

In eye infections a very dilute solution of this compound acts as an antiseptic and astringent.

It is also used as traces in animal feed or as a food supplement.

In special cements

The reaction between ZnCl ₂ and ZnO in water produces some zinc oxychlorides that make up an extremely hard material or cement. The main constituents are 4ZnO • ZnCl ₂ • 5H ₂ O and ZnO • ZnCl ₂ • 2H ₂ O.

This type of cement resists the attack of acids or boiling water. However, the pentahydrate is very stable and insoluble but not very workable, and the dihydrate is more soluble and can cause fluid drainage.

For these reasons these cements have few applications.

As a catalyst

It serves to speed up some organic chemistry reactions. It acts as a condensing agent. For example, in aldol reactions, amination reactions, and cycle addition reactions. In some of these it acts as a radical initiator.

It is a Lewis acid and catalyzes Diels-Alder reactions. It is also used as a catalyst in Friedel-Crafts reactions, to make dyes and colorants, and in the manufacture of polyester-polyether resins.

A reaction involving this compound is shown below:

Reaction to obtain an alkyl chloride using ZnCl ₂. Author: Walkerma. Source: Wikimedia Commons.

In agricultural activities

It has been used as a herbicide in crops, as a foliar treatment, to eliminate pests such as fungi and moss, and as a micronutrient. It is an intermediary to prepare pesticides.

In dental applications

It is used in mouth washes, however the recommended contact time is very short, so it only acts as an astringent on the oral mucosa. It serves as a desensitizer, is used in toothpastes and is part of dental cements.

In the textile and paper industry

It is an ingredient in the solvent used in the manufacture of rayon or artificial silk from cellulose. It is a crosslinking or bonding agent for finishing resins on textiles. It also serves to treat them and promote their conservation.

It allows curling fabrics, separating silk and wool fibers, and acts as a mordant in printing and coloring textiles.

It is used in the manufacture of parchment paper and to produce crepe paper.

In the preparation of nanoparticles

By reacting zinc chloride with sodium sulfide (Na ₂ S) by a sonochemical method and in the presence of certain organic compounds, zinc sulfide (ZnS) nanoparticles are obtained. Sonochemical methods use sound waves to trigger chemical reactions.

This type of nanomaterials could be used as photocatalytic agents to produce, for example, the division of water into its components (hydrogen and oxygen) through the action of light.

In various applications

• Deodorant, antiseptic and disinfectant of areas. Moss, mold and mildew control in structures and adjacent exterior areas such as sidewalks, patios, and fences. Disinfectant for toilets, urinals, carpets and compressed wood.
• Used in embalming mixtures and in solutions for the conservation of anatomical specimens.
• Flame retardant for wood.
• Primary ingredient in smoke bombs used to disperse crowds of people; they are used by firefighters in fire fighting drills or drills and by military forces for concealment purposes.

Zinc chloride is used in smoke bombs used in military exercises. US Department of Defense Current PhotosCpl. Abraham Lopez / 2nd Marine Division / Public domain. Source: Wikimedia Commons.

• Component of solder fluxes. In recording on metals. For coloring steel, a component of galvanized baths and copper-iron plating.
• In magnesium cements and in cement for metals.
• To break emulsions in oil refining. Agent in the manufacture of asphalt.
• Electrolyte in dry batteries.

ZnCl dry battery ₂. User: 32bitmaschine; edited by User Jaybear / CC BY-SA (https://creativecommons.org/licenses/by-sa/3.0). Source: Wikimedia Commons.

• Rubber vulcanization.
• Dehydrating agent.

Risks

May cause burns to eyes, skin, and mucous membranes.

When heated to decomposition, it emits toxic gases of hydrogen chloride (HCl) and zinc oxide (ZnO).

Warning on its use as a drug

Although conclusive studies are lacking, it is estimated that if this compound is administered to pregnant women it can cause harm to the fetus. But the potential benefits may outweigh the possible risks.

References

1. US National Library of Medicine. (2019). Zinc chloride. Recovered from pubchem.ncbi.nlm.nih.gov.
2. Liska, M. et al. (2019). Special Cements. Zinc Oxychloride Cement. In Lea's Chemistry of Cement and Concrete (Fifth Edition). Recovered from sciencedirect.
3. Pohanish, RP (2017). Zinc Chloride. In Sittig's Handbook of Toxic and Hazardous Chemicals and Carcinogens (Seventh Edition). Recovered from sciencedirect.com.
4. Gedanken, A. and Perelshtein, I. (2015). Power ultrasound for the production of nanomaterials. In Power Ultrasonics. Recovered from sciencedirect.
5. Archibald, SJ (2003). Transition Metal Groups 9-12. Reactions and Catalysis. In Comprehensive Coordination Chemistry II. Recovered from sciencedirect.com.
6. Cotton, F. Albert and Wilkinson, Geoffrey. (1980). Advanced Inorganic Chemistry. Fourth Edition. John Wiley & Sons.
7. Lide, DR (editor) (2003). CRC Handbook of Chemistry and Physics. 85 ^th CRC Press.